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Unit Objectives:

Describe the origin of the periodic table

State the modern periodic law

Explain how an element’s electron configuration is related to the element’s placement within a period and a groupon the periodic table.

State the trends of the following properties within periods and groups of elements including:o Ionization energyo Electronegativityo Atomic Radiuso Reactivityo Metallic/Nonmetallic character

Identify and state the properties of the following groups in the periodic table:o Alkali metalso Alkaline earth metalso Halogenso Noble Gaseso Transition elements

Locate within the periodic table and state the properties of the metals, nonmetals, and metalloids (semi-metals)

Define the following vocabulary: Allotrope Nonmetals Ion Metalloids Cation Luster Anion Malleability Electron Ductility Proton Conductivity Neutron Nonmetals Compound Brittleness Element Dull Valence electron Non-conductor Lewis Dot Diagram Noble gas

Mendeleev Period Group(family) Alkali Metals Alkaline Earth Metals Halogens Atomic radius Ionization energy Electronegativity Reactivity Electron configurationStable OctetMetals Periodic Law

Unit 3: Periodic Table Unit Notes & CW

Name: ________________________________ Period: _____

The bold, underlined words are important vocabulary words that you should be able to define and use properly in explanations. This is a study guide for what you will be tested on throughout the year. The objectives are divided into categories of “Knowledge” (what you have to know) and “Application” (what you have to be able to do).

THE PERIODIC TABLE

Knowledge Application

1.

o The placement or location of an element on the Periodic Tablegives an indication of physical and chemical properties of thatelement.

o The elements on the Periodic Table are arranged in order ofincreasing atomic number.

o Explain the placement of anunknown element in the periodictable based on its properties

2.

o The number of protons in an atom (atomic number) identifiesthe element. This goes at the bottom left corner of the symbolfor that element.

o The sum of the protons and neutrons in an atom (massnumber) identifies an isotope. The mass number is placed atthe top left corner of the symbol for an element OR is placedafter the element symbol or name and a dash.Ex: Three different ways to write carbon with a mass number of 14:

C, carbon-14, or C-14

o Interpret and write isotopicnotations.Ex:C-12, C-13, and C-14 are isotopes ofthe element carbon

3.

o Elements are classified by their properties, and located on theperiodic table as metals, metalloids, nonmetals, or noblegases.

o Identify the properties of metals,metalloids, nonmetals and noblegases

o Classify elements as metals,metalloids, nonmetals, or noblegases by their properties

o

4. o An element’s atomic radius, first ionization energy, and electronegativity determine its physical and

chemical properties

5.

o Substances can be differentiated by their physicalproperties.

o Physical properties of substances include melting point, boilingpoint, density, conductivity, malleability, solubility, andhardness.

o Identify and give examples ofphysical properties

o Describe the states of theelements at STP (solid, liquid, orgas). (Table S)

6.

o Substances can be differentiated by chemical properties.o Chemical properties describe how an element behaves during a

chemical reaction and include reactivity, flammability, andtoxicity.

o Identify and give examples ofchemical properties

o Describe the difference betweenphysical and chemical properties ofsubstances

7.

o Some elements exist as two or more forms in the same phase. These forms differ in their molecular orcrystal structure and therefore in their properties. The word to describe this phenomenon isALLOTROPE.

o Ozone and oxygen gases are allotropes of each other. Ozone is O3 and it is very dangerous to our health.Oxygen gas is O2 and we need it to survive.

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o Diamonds and graphite (better known as pencil lead) are both forms of the element carbon. They havedifferent molecular structures and very different properties.

8.

o For Groups (also called families) 1, 2, and 13-18 on the PeriodicTable, elements within the same group have the same number ofvalence electrons (helium is the exception) and therefore similarchemical properties.

o Elements in the same Period (row) have the same number ofprincipal energy levels (shells) which contain electrons.

o Determine the group of anelement, given the chemicalformula of a compoundEx: A compound has the formulaXCl2, element X is in Group 2

o Determine the number of energylevels containing electrons givenan element’s Period and vice versa

9.

o The succession of elements within the same GROUP (top tobottom) demonstrates characteristic trends: differences inatomic radius, ionic radius, electronegativity, first ionizationenergy, and metallic/nonmetallic properties.

o Compare and contrast propertiesof elements within a group or aperiod for groups 1, 2, and 13-18on the periodic table

10.

o The succession of elements across the same PERIOD (left toright) demonstrates characteristic trends: differences in atomicradius, ionic radius, electronegativity, first ionizationenergy, and metallic/nonmetallic properties.

o Understand and be able to explainthe trends in terms of nuclearcharge and electron shielding

Goal setting: Based upon your learning style results and the information above list at least two techniques you plan to use to study during this unit.

1. 2.

What grade would you like to achieve on this unit based on your efforts? _______%

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Activity - Writing Your Name using Chemical Element Symbols

Objective In this activity, you will use your creativity to spell your name (first or middle name and

your last name) using chemical symbols of elements on the periodic table. For example, you can spell Yvonne using the symbols for yttrium (Y), vanadium (V), oxygen (O),

nitrogen (N), and neon (Ne).

Materials

Ruler Pencil

Colored pencils Markers Poster board

8.5 x 11 sheets of copier paper IUPAC Periodic Table of the Elements

Computer or Chrome book

Procedure

Your poster must include: The chemical element symbols used to spell your name (first or middle name and

last name).o If your name has the letter J, use J and the information for Iodine (J was the

former symbol for Iodine).

o If you are only using the first letter of a two-lettered symbol, still include thesecond letter, but fade the letter so it does not appear that it is used in the

spelling (see example at the end of the activity). Box drawings of the symbols as they appear in the IUPAC periodic table of the

elements (including atomic number, atomic mass, symbol, and element’s name).

The following information for at least four of the elements you use (typed andprinted on the copier paper and attached to the bottom of the poster board):

o Physical description of the element: metal, nonmetal, or metalloid; solid,liquid, or gas at room temperature, or synthetic.

o Group number and period number where the element is located in the

periodic table.o Description of the atomic structure of the atoms of the elements:

Number of protons and neutrons in the nucleus, and the number ofelectrons found in the electron cloud.

o At least two chemical and physical properties of the element.o The description of at least two common uses of the element.o When was the element discovered and who discovered it.

Each element’s box should be at least 5.4 cm wide and 6 cm tall on the poster. The poster should be organized neatly and created in color.

Presentation of your poster to the class: The presentation should include sayingwhat elements did you use to spell your name and last name, the element’sproperties and the description of at least two common uses of the element for the

four elements you picked.

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Useful websites: http://www.lenntech.com/periodic/periodic-chart.htm

http://www.webelements.com http://chemicalelements.com/

http://www.rsc.org/periodic-table/ http://www.iupac.org/fileadmin/user_upload/news/IUPAC_Periodic_Table-8Jan16.pdf

Example For example, if your name is Yvonne Wilson, you could write it using the elements Y, V, O, N, Ne, W, I, Li (notice that the i from the Li symbol is shaded grey since it is not part of

the spelling), S, O, and N. Notice that the sizes and shapes of the boxes are different from the instructions given above, in order to fit the space available below

Rubric Element Name (1 point)

Atomic Number (1 point) Atomic Symbol (1 point) Atomic Mass (1 point)

Number of protons, number of neutrons, and number of electrons (3 points) Physical descriptions: metal, non-metal, metalloid, density, physical state at room

temperature (2 points) Uses (at least 2 common uses) (2 points)

Group, period (2 points) At least two chemical or physical properties of the element (2 points) Neatness, spelling, color, creativity (3 points)

List of sources of information (books, websites, magazines, etc. (can be pasted tothe back of poster (4 points)

Year discovered and discoverer (4 points) Your name and date (on back of poster) (4 points) Poster presentation to the class (20 points)

39 Y

ytrium 88.91

23 V

vanadium 50.94

8 O

oxygen 15.99

7 N

nitrogen 14.01

10 Ne

neon 20.18

74 W

tungsten 183.8

53 I

iodine 126.9

3 Li

lithium 6.938

16 S

sulfur 32.05

8 O

oxygen 15.99

7 N

nitrogen 14.01

5

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Lesson 1: The History of the Table &Chemical Periodicity

Objective: To relate the work of chemists to the modern periodic law and the repeating patterns in the periodic table

Watch the following clip: History & structure of the periodic table

Dmitri Mendeleev (Russia)

Between 1868 and 1870, in the process of writing his book, The Principles of Chemistry, Mendeleev created a table or chart that listed the known elements according to increasing order of atomic weights. When he organized the table into horizontal rows, a pattern became apparent--but only if he left blanks in the table. If he did so, elements with similar chemical properties appeared at regular intervals--periodically--in

vertical columns on the table.

Mendeleev was bold enough to suggest that new elements not yet discovered would be found to fill the blank places. He even went so far as to predict the properties of the missing elements. Although many scientists greeted Mendeleev's first table with skepticism, its predictive value soon became clear. The discovery of gallium in 1875, of scandium in 1879, and of germanium in 1886 supported the idea underlying Mendeleev's table. Each of the new elements displayed properties that accorded with those Mendeleev had predicted based on his realization that elements in the same column have similar chemical properties. The three new elements were respectively discovered by French, a Scandinavian, and a German scientist, each of whom named the element in honor of his country or region. (Gallia is Latin for France.) Discovery of a new element had become a matter of national pride--the rare kind of science that people could read about in newspapers, and that even politicians would mention.

Periodic = cyclic; repeating patterns/cycles; similar to monthly/weekly calendar (days of the week) Ex: tired on Mondays, happy on Fridays

Henry Moseley (England) By 1907, when Mendeleev died, chemists were sure that iodine followed tellurium in the Periodic Table and that there was something odd about their relative atomic masses. However no-one was able to measure atomic number, it was just the position of an element in the Periodic Table sequence. For example lithium was known to be the third element but this number three was only because its properties meant that it slotted in

between helium and beryllium. Henry Moseley found and measured a property linked to Periodic Table position. Hence atomic number became more meaningful and the three pairs of elements that seemed to be in the wrong order could be explained. Moseley used what was then brand-new technology in his experiments. A device now called an electron gun had just been developed. He used this to fire a stream of electrons (like machine gun bullets) at samples of different elements. He found that the elements gave off X-rays. (This is how the X-rays used in hospitals are produced.) Moseley measured the frequency of the X-rays given off by different elements. Each element gave a different frequency and he found that this frequency was mathematically related to the position of the element in the Periodic Table – he could actually measure atomic number!

Periodic Law =

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How is the table actually arranged?

Periods =

The period number

The properties of elements change drastically across a period from

. The number of valence electrons increases from left to right (1 à 8)

2. Groups (Families) =

Example: K in Group 1 Let’s look at the electron configuration of elements in the same group…

H = 1 Li = 2-1 Na = 2-8-1 K = 2-8-8-1 Rb = 2-8-18-8-1 Cs = 2-8-18-18-8-1

*Fr = -18-32-18-8-1

What similarities can you observe within the above electron configurations?

Remember… Group # = Period number =

Why do elements in the same group have similar chemical/physical properties?

Reactive elements can bond easily with other elements. They have an incomplete valence electron shell.

All atoms (except hydrogen and Helium) want

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Most elements, except noble gases, combine to form compounds. Compounds are the result of the formation of chemical bonds between two or more different elements. In the formation of a chemical bond, atoms lose, gain or share valence electrons to complete their outer shell and attain a noble gas configuration. This tendency

An ion (charged particle) can be

Isoelectronic: atoms or ions that have the SAME number of ELECTRONS

Ex: F-, Ne, and Na+ all have 10 electrons

Octet =

****KNOW THIS!!!!****

Activity - Make a Periodic Table

Background The periodic table is special way of arranging elements based on their properties and characteristics.

Purpose To create a periodic table using imaginary elements. This periodic table should have appropriate trends across rows and groups of elements.

Materials • One set of element cards• One blank periodic table template

Procedure 1. On the next page, you will see a collection of elements along with their

characteristics. 2. Cut each element card and arrange the elements in order based upon their

characteristics, just like you would see on the periodic table. Use the attached periodic table template. (Note: Not all spaces on the template will be filled – there is a missing element!)

3. When you have finished, have your teacher check your work.

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solid

Ak104.3

light green

gas

Az102.2

light blue

solid

Pa71.7 red

solid

Nj81.2 green

gas

Ia?

blue

brittle solid

Fl99.6

yellow

solid

Tx92.4 pink

solid

Ut16.3

crimson

brittle solid

Cn37.2

orange

liquid

Ma55.9

hunter green

gas

Tn67.8

dark blue

10

11

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Classwork 3-1:

Model: An Electron Dot Diagram of the Elements

Task: Below the symbol for each element, write an electron configuration for the elements in the model. Lithium has been done for you.

Questions:

1.) How are the members of the same column (group) similar in terms of the number of valence electrons?

2.) Which group contains the least number of valence electrons?

3.) Which group contains the largest number of valence electrons?

4.) Which row (period) contains three occupied shells?

5.) How are the members of the same period similar in terms of the number of energy levels (shells)?

6.) Are atoms with a larger radius more likely to be found at the top or bottom of a group (column)? Explain your answer.

7.) In terms of the number of valence electrons, describe one cyclic property that can be observed in the model.

8.) Which group would be considered non-reactive? Why?

9.)When atoms form ions, the electron configuration of the ion resembles the electron configuration of a CERTAIN noble gas. Which Noble Gas will each of these atom’s ions be like? a. Sr c. Br e. Al g. Li______b. O d. Si f. P h. Cs ____ 13

Practice: It’s Elemental

DIRECTIONS: Use the reading below to answer the questions that follow.

We all know by now that the periodic table is arranged according to increasing atomic number. What we’re only beginning to learn is the significance of elements within the same column (vertical) and row (horizontal) on the table.

Every element found within a given row, or period, has the same number of electron shells, or principle energy levels. Despite this one common feature, atoms of one element within a given period do not behave similar to atoms of another element in that same period. In fact, the period in which an element is found really tells you nothing about how the atoms of that element will behave. The only additional thing that we can really say about elements of the same period is that they increase by very little in terms of size (or mass) as we go from left to right on the table since the atomic number( number of protons) only goes up by one. Look at the periodic tables that you labeled and color-coordinated. Look at how much the mass increases as you move from left to right in a given period.

Every element found within a given column, or group, has the same number of valence electrons. This is VERY significant because it’s the number of valence electrons that determines how atoms of any element are going to “behave.” When we say “behave,” what we really mean is how they’re going to react, or bond with atoms of other elements. However, not all columns or groups qualify as “families.” In fact, the only groups that are considered to be families are Group I (Alkalai Metals), Group II (Alkaline Earth Metals), Group XVII (Halogens), and Group XVIII (Noble Gases). The behaviors of the transition metals are very difficult to predict, and the behavior of the elements within the BCNO group varies greatly from one element to another. An element’s family tells you much more about its properties than its period does.

All of the elements in the Halogen family have 7 valence electrons. There’s an easy way to cheat when it comes to determining the number of valence electrons. Just look at the last digit of the group number above the first element in the family. For the first two families (alkali metals and alkaline earth metals) it’s a single digit number, so there’s no confusion. Alkali metals are group 1, which means all elements in that family have 1 valence electron. The halogen family, on the other hand, is group 17, which means they have how many electrons in their valence shell? If you said 7, you’re right. This trick will help you when it comes to drawing Lewis dot diagrams…

Speaking of the Lewis dot diagram, it’s used to show only the valence electrons in a given atom or compound. After all, the valence electrons are the only electrons involved in bonding. There are four basic spots that an electron can occupy in a Lewis dot diagram because the maximum number of valence electrons that an atom of an element can generally hold is eight. If the element symbol was the face of a clock, the spots would be at 12 o’clock, 3 o’clock, 6 o’clock, and 9 o’clock. The first spot is like a taxi cab that can hold two electrons in its single seat. The remaining three spots are like seats on a bus that can also hold electrons. Just as you would do if you got onto a bus, electrons look for empty seats first. Once the taxi cab is full, the remaining electrons in the valence shell occupy empty “seats.” Only after each of the three seats has an electron in it do they begin to pair up. The exceptions to the octet rule are elements that have only one energy level or seek to have one energy level. These elements include hydrogen, helium, lithium, beryllium, and boron. These elements also seek to have a full valence shell, but it will only contain two electrons. Otherwise, there can never be more than 8 valence electrons and, no matter what, there can never be more than 2 electrons in a given “seat.”

All atoms seek to have a full valence shell, and the easiest way to do that is to form bonds with other atoms. We mentioned before that atoms in the family of noble gases already have a full valence shell, and that’s why they rarely ever seek to bond with other atoms. For all other element families, the atoms seek to form bonds in order to complete their valence shell. As a general rule, the number of unpaired valence electrons tells you the number of bonds that atoms of a given element “like” to form. Halogens, like chlorine (Cl), have 7 valence electrons and only one unpaired valence electrons. That means that the halogens have two choices: They can either steal an electron, usually from an atom with only 1 valence electron, like sodium (Na), forming what we call an ionic bond. The other choice an atom like chlorine has is to share an electron with an atom that’s also one short of having a full valence shell, like another chlorine atom. This sharing of electrons is an example of a covalent bond. As we said before, carbon has 4 valence electrons, which means that all of them can occupy a seat unpaired for a maximum of 4 unpaired valence electrons. That’s why

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carbon looks to share each of its 4 single valence electrons in order to end up with 4 pairs instead, giving it the full 8 it needs to fill its valence shell. In other words, carbon will form 4 covalent bonds. A single line is used to illustrate a bond between two atoms, and each single line represents 2 electrons.

1. How is the periodic table arranged?

2. What do we call the horizontal rows of the periodic table? What do all the elements in a given row have in common?

3. What do we call the vertical columns of the periodic table? What do all the elements in a given column have incommon?

4. Which tells us more about an element’s properties, its row or its column? Why is this?

5. Which of the following elements is chlorine (Cl) most similar to?

a. fluorine (F) b. sulfur (S) c. oxygen (O) d. argon (Ar)

6. Does mass increase more as we go from left to right or top to bottom on the periodic table?

7. Are atoms of the elements in the family of noble gases reactive (do they readily form bonds with other atoms)? Whyis this?

8. How are ionic bonds formed?

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9. How are covalent bonds formed?

10. What determines how many bonds an atom will form?

11. What is the easiest way for atoms without a full valence shell to gain a full valence shell?

12. If an atom of an element has four valence electrons, what is the maximum number of unpaired electrons it canhave? Draw a Lewis Dot diagram of an element that fits this description.

13. Draw a Lewis Dot diagram of an element with 6 valence electrons. How many bonds can it form?

14. Why do chlorine (Cl) and sodium (Na) bond so easily with one another?

15. Which element, carbon (C) or fluorine (F) would you expect to be more reactive? Explain your answer. (Hint: Thinkabout which element is closer to its goal.)

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Lesson 2: Key to the Periodic Table

Objective: To define the location and compare and contrast the properties of metals, nonmetals, and metalloids.

Check this out! Interactive Periodic Table

The structure of the periodic table gives us a lot of information. Depending on an element’s position in the table, we can determine a lot of its physical and chemical properties.

1. Metals:

due to

2. Nonmetals:

Metalloids

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3. Metalloids (AKA semi-metals):

The Groups in more detail

Group 2 à

Group 1 à

19

Groups 3-12 à

Found in the MIDDLE of the table (the D block)

Tend to be UNPREDICTABLE will lose electrons or gain them depending on what other METALS are present

Groups 13-16 BCNO groups (not a single group)

MISCELLANEOUS groups

Metals, nonmetals, & metalloids found along the staircase (many different properties)

Group 17 à

Form SALTS/COMPOUNDS called HALIDES

All NONMETALS making up the group

Group 18 à

Most STABLE group; exist ALONE in nature. Non reactive!

Ex: Neon (Ne)

Hydrogen Not officially part of a group

Can be seen as H2(g), H+(aq) or H-(aq)

The Lanthanide/Actinide Series

Two rows on bottom of table (detached) – Elements 58 – 71 & 90 - 103

Actually belong to the TRANSITION METALS

Activity - Organization of the Periodic Table

Directions

Using your computer, tablet or mobile device, navigate to the website: www.ptable.com You will interact with this periodic table to find the answers to the questions below.

*Make sure the “Wikipedia” tab is selected in order to answer the following questions:

1. The vertical columns on the periodic table are called groups, how many groups arethere on the periodic table?

2. The horizontal rows on the periodic table are called periods, how many periods arethere on the periodic table?

3. Using the group and period numbers, identify the elements that are located in eachof the following location.

a. The element in group 10 and period 5 =

b. The element in group 15 and period 4 =

c. The element in group 2 and period 3 =

d. The element in group 18 and period 6=

e. The element in group 1 and period 7 =

4. Are most of the elements on the periodic table classified as a metal or a non-metal?

5. Are the non-metal elements located on the left or right side of the periodic table?

*Elements can also be classified by family, use the color coding at the top of the page tohelp identify the family names and their element members.

6. How many elements belong to the Alkali Metal family? List the member elements by

their symbol.

7. Click on the group number for the Alkali Metals family at the top of the table.

Answer the following about the Alkali metals:a. What are 3 similar properties of these elements?b. Where are these found naturally?

c. What is a common substance that alkali metals react vigorously with?

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8. What type of element does the neon green color indicate? List the element symbolsfor the elements that are designated with neon green below.

9. How many elements belong to the Halogen family? List the member elements bytheir symbol.

10. Click on the group number for the Halogen family at the top of the table. Answerthe following about the Halogen elements:

a. What does the name “halogen” mean?b. What type of molecule is formed when a halogen combines with hydrogen?

11. Group 2 on the periodic table corresponds to what family of elements?

12. What family of elements does arsenic (As) belong?

13. What elements are designated as family members of Arsenic? Click on the name of

this group located in the color coded key at the top of the page, what is the common property of the elements in this family?

14. Tungsten (W), Copper (Cu), and Iron (Fe) all belong to the same family, whose

members are generally used as conductors of electricity. What family is this?

15.In the top right hand corner of your screen check (√) the box next to “Wide.” Thiswill display the periodic table including the Lanthanoid and Actinoid families. Do the

Lanthanoid and Actinoid families have specific group numbers?

16. Click on the word Lanthanoid, what is another common name for this group of

elements?

17. Click on the word Actinoid, this family of elements are known to be radioactive.

What important example, shown in the picture, is given regarding a real-life connection to these elements?

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18. Complete the following table, by finding the atomic numbers and atomic massesfor each element:

Symbol Be O Al Ar K Ca Te I Xe

Atomic number

Atomic Mass

a. Using the data in the table above, is the periodic table is organized by increasingatomic mass? Explain.

b. What property is the periodic table organized by?

*In the top right hand corner of your screen check (√) the box next to “Electrons.” Thiswill make the electron count for each element appear to the right of its symbol in the

periodic table.

19. What electron pattern do you notice for all of the elements belonging to the Alkali

Metal family?

20. Considering your answer above, though we know Hydrogen is a non-metal, why doyou think it is placed on top of the alkali metals?

21. What electron pattern can be observed with the Noble Gases? The Halogens?

*Bohr Models can be used to show, roughly, how electrons are arranged in an atom.Recall that the number of electrons is equal to the number of protons in a neutral atom, which is also the same as the atomic number for the element.

Bohr Models:

The first ring can contain up to 2 electrons The second ring can contain up to 8 electrons The third ring can contain up to 8 electrons

The fourth ring can contain up to 2 electrons The Bohr model is completed for a given atom by filling the inner most ring to

its capacity and moving outward to each subsequent ring, filling each to its

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capacity before moving on. Electrons on the outer most ring are known as VALENCE ELECTRONS. These are

the electrons that participate in chemical bonding. Each dot represents one electron.

22. Identify the elements shown in the Bohr models below and give the number ofvalence electrons in each atom:

a. b. c.

Element= Element= Element=

Valence Valence Valence Electrons = Electrons = Electrons =

23. Draw Bohr models for the elements listed below and state the number of valence

electrons in each.

a. Nitrogen (N) b. Chlorine (Cl) c. Calcium

*At the top of your screen check select the to “properties” tab. Next check (√) the box inthe center next to “Valence,” this will show the valence electron count for each element

appear in the bottom left of its symbol on the periodic table.

24. The transition metal family is very large, which group numbers are included as partof this family? Can you see a pattern for their electron numbers?

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Activity - Periodic Table Scavenger Hunt

Directions

Using your computer, tablet or mobile device, navigate to the website: www.ptable.com You will interact with this periodic table to find the answers to the questions below.

1. What color element symbol designates elements that are a gas at a given

temperature?

2. What family of elements does the light pink color indicate?

3. Hover the cursor over Magnesium, Mg, what type of specific information is givenabout the element in the enlarged information area?

4. Now click on the element symbol for Magnesium, Mg. What information are you

presented with?

5. What are the element symbols for the Metalloid elements?

6. What is the symbol and atomic number of the element with the most protons

according to this periodic table? Click on its symbol to find out what year it wasdiscovered.

7. If an element’s symbol is written in blue, what information does this tell you?

8. Reduce the temperature value to 0K, using the control (shown in the upper righthand side of the screen). How many gaseous elements exist at 0K according to the

table? How many liquid elements exist? List the symbol of any elements that fall inthese categories.

9. Change the temperature value to room temperature, 298K. At the top of the

screen, choose the “Properties” tab. How does this view differentiate between solid,liquid and gas element states?

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10.Using your cursor, choose Iron, Fe. Determine the following values for Iron:

a. Melting Point =

b. Boiling Point =

c. Atomic Radius =

d. Density =

11. A large value for thermal conductivity means that the element is a strongconductor of heat, whereas a small value means the element is a weak conductor.

Find the elements that are the strongest and weakest conductors of heat; List their symbol and conductivity value below. (Select “Thermal Conductivity” to make this easier).

12. By specifically selecting any of the properties at the top of the periodic table, youcan sort the table by individual details. Highlight the “discovered” option from the

list. Can you find an element that was discovered in each of the following years? (Use the slider to help move through time!)

a. 1772 =

b. 1803 =

c. 1900 =

d. 2004 =

13. At the top of the screen, choose the “Orbitals” tab. The periodic table is now

identified by only four specific sections, what do each of the colors represent?

14. As you move the cursor over the elements, you should see the correct orbitaldiagram at the top center of the screen for each element, as well as the electron

configuration for each element displayed at the top right. What is the electron configuration for Selenium, Se, atomic #34?

15. At the top of the screen, choose the “Isotopes” tab. Click on Copper, Cu, atomic#29. How many isotopes are shown for Copper and what are the abundancies of

each?

16. Click on Tellurium, Te, atomic #52. How many isotopes are shown for Tellurium?

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*Click the “Wikipedia” tab in the top left of the screen, it should produce a drop downmenu for you to choose from. Select “Videos.”

17. Choose element #10, neon and watch the short video.

a. What color is a “neon light”?

b. Where would you see neon used this way in your everyday life?

18. Choose element #37, Rubidium and watch the short video.a. What reaction is conducted with Rubidum?

b. What are the results of the reaction?

19.Choose element #16, Sulfur and watch the short video.a. What is the “Barking Dog Experiment?”

b. What was a historical use for this reaction years ago?

20.Choose your favorite element, or the element symbol that appears in your written

name the most often and watch the short video for it.a. What element did you choose?

b. What did you learn about this element?

26

Activity - The Periodic TableStudent Information Sheet

The Periodic Table is a list of all the known elements. It is organized by increasing atomic

number. There are two main groups on the periodic table: metals and nonmetals. The left side of

the table contains the metals with the greatest metallic properties. As you move from the left to

the right, the elements become less metallic with the far right side of the table consisting of the

nonmetals. The elements in the middle of the table are called “transition” elements because their

properties change from metallic properties to nonmetallic properties.

A small group whose members touch the zigzag line between the metals and nonmetals are

called metalloids because they have both metallic and nonmetallic properties.

The table is also arranged in vertical columns called “groups” or “families” and horizontal rows called

“periods.” Each arrangement is significant. The elements in each vertical column or group have

similar properties. The elements in each group have the same number of valence electrons which

determines the elements chemical properties including reactivity. The valence electrons are the

electrons on the outer most energy level of the atom. There are 18 groups (columns) on the

periodic table. They are as follows:

Hydrogen: This element does not match the properties of any other group so it stands alone. It is

placed above group 1 but it is not part of that group. It is a very reactive, colorless, odorless gas at

room temperature. Hydrogen only has one valence electron.

Group 1: Alkali Metals – These metals are extremely reactive. They all have 1 valence electron

(same as the group #). They are shiny and silver in color. Their density is extremely low so that

they are soft enough to be cut with a knife.

Group 2: Alkaline-earth Metals – Slightly less reactive than alkali metals. They all have 2 valence

electrons (same as the group #). They are silver colored and denser than alkali metals.

Groups 3 – 12: Transition Metals – These metals have a moderate range of reactivity and a wide

range of properties. In general, they are shiny and good conductors of heat and electricity. They

also have higher densities and melting points than groups 1 & 2. These elements have 1 or 2 valence

electrons.

Lanthanides and Actinides: These are also transition metals that were taken out and placed at the

bottom of the table so the table wouldn’t be so wide. The elements in each of these two periods

share many properties. The lanthanides are shiny and reactive. The actinides are all radioactive and

are therefore unstable. Elements 95 through 103 do not exist in nature but have been

manufactured in the lab.

Group 13: Boron Group – Contains one metalloid and 4 metals. They are Reactive. These all have 3

valence electrons (group # minus 10)

27

Group 14: Carbon Group – Contains one nonmetal, two metalloids, and two metals. These all have 4

valence electrons (group # minus 10) and have varied reactivity.

Group 15: Nitrogen Group – Contains two nonmetals, two metalloids, and one metal. They have

varied reactivity. These elements have 5 valence electrons (group # minus 10).

Group 16: Oxygen Group – Contains three nonmetals, one metalloid, and one metal. They are a

reactive group. These elements all have 6 valence electrons (group # minus 10).

Group 17: Halogens – All nonmetals. Very reactive. Poor conductors of heat and electricity. Tend

to form salts with metals. Ex. NaCl: sodium chloride also known as “table salt”.) These elements

have 7 valence electrons (group # minus 10).

Group 18: Noble Gases – Unreactive nonmetals. All are colorless, odorless gases at room

temperature. All found in earth’s atmosphere in small amounts. These elements have a full outer

energy level, usually 8 valence electrons except for Helium. Helium only has 2 valence electrons.

Color Coding the Periodic Table

Instructions:

1. Label the groups with 1-18 at the top of each column.

2. Label the periods with 1-7 at the left of each row.

3. Label the groups names (as stated above) at the top of each column.

4. Under each group/family (column), write the number of valence electrons the elements have

in that group.

Note: Do not include groups 3-12. These are the transition metals. They all have 1 or 2

valence electrons.

5. Draw a “G” in the boxes of the elements that exist as a gas at room temperature.

6. Draw an “L” in the boxes of the elements that exist as a liquid at room temperature.

7. Draw a HEAVY BLACK LINE down the staircase that separates the metals from the

nonmetals.

8. Use the following colors to identify the various sections of the periodic table.

a. Alkali Metals = red

b. Alkaline Earth Metals = brown

c. Transition Metals = purple

d. All other metals = orange

e. Metalloids = blue

f. Halogens = green

g. Noble Gases = yellow

i. All other nonmetals = leave white

j. Lanthanide Series = draw a red diagonal line through each element

k. Actinide Series = draw a blue diagonal line through each element

9. Make a legend of your color key in the box labeled “key” of your periodic table

28

KEY

29

Color Coding the Periodic Table

Related Questions

Part 2: Answer the following questions on a separate piece of paper.

1. The vertical columns on the periodic table are called _______________.

2. The horizontal rows on the periodic table are called _______________.

3. Most of the elements in the periodic table are classified as _______________.

4. The elements that touch the zigzag line are classified as _________________.

5. The elements on the right side of the periodic table are classified as________________.

6. Elements in the first group are extremely reactive. They are called ______________

______________.

7. Elements in groups 3 through 12 have many useful properties and are called

_________________ _______________.

8. Elements in group 17 are known as “salt formers”. They are called

_________________.

9. Elements in group 18 are very unreactive. They are said to be “inert”. We call these the

______________ ______________.

10. How many elements are in the lanthanide series? ______________________.

11. What is the name of the element in group 3, period 4? ____________________.

12. Pick any element from the periodic table. List all the information about this element

based on your color-coded periodic table. ELEMENT: ______________

______________________________________________________________________

______________________________________________________________________

30

31

Classwork 3-2:

1. Write in the space, “Group 1 metals”, “Group 2 metals”, “transition metals”, “halogens”, or “noble gases” to

indicate which group each statement is describing

a. Colored solutions

b. Full valence shell

c. Most active metals

d. Most active nonmetals

e. Monatomic gases

f. Diatomic elements

g. Stable and unreactive

h. 7 valence electrons

i. 2 valence electrons

j. Form ions with a +1 charge

2. Describe one chemical property of Group 1 metals that results from the atoms of each metal having only onevalence electron.

3. Given: Samples of Na, Ar, As, RB

a. Which two of the given elements have the most similar chemical properties?

b. Explain your answer in terms of atomic structure.

4. Given: Samples of sulfur, oxygen, and phosphorus

c. Which two of the given elements have the most similar chemical properties?

d. Explain your answer in terms of atomic structure.

5. Based on the Periodic Table, explain why Na and K have similar chemical properties.

32

PERIODIC TABLE – The Basics1. The periodic table was originally arranged according to _______________________

2. Our current periodic table is arranged according to _________________________

3. The periodic table is essentially divided into two types or categories of elements.

Those categories are _________________ and ___________________

4. The dividing line between these two categories of elements is in the shape of a

_________________________

5. The elements that border or touch this dividing line are referred to as

_________________________

6. Explain why the elements from question #5 have this name:

________________________________________________________________

7. The first period on the table in which we see transition metals is period _____

8. The transition metals represent a gradual transition or change from _____________

to ____________________

9. The most metallic elements on the periodic table are found in the

a. upper rightb. lower right

c. upper leftd. lower left

10. The least metallic elements on the periodic table are found in the

a. upper rightb. lower right

c. upper leftd. lower left

11. Which of the following is NOT a Group I metal?

a. Hydrogenb. Lithium

c. Sodiumd. Potassium

12. Name the only four groups on the periodic table that qualify as families.

________________________________________________________________________________________________________________________________

33

34

35

36

37

38

Atomic Radius Exploration

Background 1. Draw a picture to support your written definition of the word “radius.”

2. Let’s assume an atom is shaped like a sphere, what subatomic particles would be

found in the center? What subatomic particles would be found around theperimeter?

3. Keeping in mind your answers to questions 1 & 2, in your own words describe themeaning of “atomic radius”

*Check your answers before moving on to the next portion of the activity.

Directions

Using your computer, tablet or mobile device, navigate to the website: www.ptable.com You will interact with this periodic table to find the answers to the questions below.

Click the “Properties” tab at the top of the page. Next select “Radius” from the properties listed in the top center of the screen.

Finally make sure “Calculated radius” is selected from the options on the right.

1. Complete the following data table:

Group 1 element Calculated Radius Value (pm)

H

Li

Na

K

Rb

Cs

39

2. What trend in the data do you observe as you move from the top of the periodictable to the bottom within this group?

3. Does this periodic trend apply to any other group? Briefly investigate the atomicradii values in another group to support your answer.

4. What ideas do you have about the factors that actually contribute to the atomic

radius trend within a group? (Revisit your background questions to guide you).

5. Complete the following data table:

Period 2 element

Li Be B C N O F Ne

Atomic Radius

Value (pm)

6. What trend in the data do you observe as you move from the left of the periodic

table to the right within this period?

7. Using your knowledge of the Bohr model, as well as considering the atomic radiusdata values collected in question #5, complete the following table. Make sure to

consider comparative sizing of each model.

Period 2 element

Li Be B C N O F Ne

Bohr Model

8. Does this periodic trend apply to any other period? Briefly investigate the atomicradii values in another period to support your answer.

40

9. What ideas do you have about the factors that actually contribute to the atomicradius trend within a period? (Think about subatomic particles)

10. Draw a vertical and horizontal arrow next to the periodic table outline below. Pointthe arrows in the direction that the atomic radius increases.

11.Based on the trend arrows drawn, make a prediction, and place the following

elements in ordering of increasing atomic radius (for smallest to largest): Si, Ca, C,F, Cs

12.Check values on www.ptable.com and record the actual values for atomic radius in

the table below. Was your prediction from question #11 correct?

Element symbol Si Ca C F Cs

Atomic

Radius Value

Rank (1-5) 1=smallest

5=largest

41

13.Read the following descriptions of two important factors that affect the atomic

radius of an atom, then answer the following questions:

Electron Shielding Effect: This is due to inner electrons “shielding” the valence electrons from the positive pulling force of the nucleus. As an atom increases its number of electron shells, the shielding effect will increase in

turn keeping the valence electrons distanced from the nucleus.

Effective Nuclear Charge: This is due to the number of protons in an atom, the more protons the stronger the pulling force of the nucleus will be on the electrons in the atom.

a. Revisit your answers for questions 1-4. Using the vocabulary terms given above

make a statement about the atomic radius trend within a group on the periodictable. Use two specific elements as examples in your response.

b. Revisit your answers for questions 5-9. Using the vocabulary terms given above

make a statement about the atomic radius trend within a period on the periodictable. Use two specific elements as examples in your response.

42

43

Lesson 3: Periodic Table Trends

Objective: To describe and explain the reason for periodic trends

1. Atomic Radius =

a.

Reasons:

SHIELDING electrons from inner energy levels shield/block valence electrons from thenuclear charge of the nucleus

b.

Reasons: NUCLEUS getting HEAVIER (more P & N)

e- (remember they are very LIGHT) are being pulled in TIGHTER

C. Ionic Radius :

44

2. Ionization Energy =(values for each element listed in Table S)

X + energy à X+ + e-

Metals àNonmetals à

a.Reason:

b.

Reason:

45

3. Electronegativity:

GREEDINESS

Electronegativity values range from 0.0 to 4.0

The MOST

The LEAST

a.

Reason:

* Shielding

b.

Reason:

§

46

****YOU NEED TO KNOW THESE TRENDS BUT YOU DO NOT HAVE TO MEMORIZE THEM!!!!! YOU CAN FIGURE THEM OUT USING YOUR PERIODIC TABLE AND TABLE S IN YOUR REFERENCE TABLE

THE TRICK….. Example- If you are looking for the trend in electronegativity going across a group:

Pick 1 element on the left side of the group and 1 element on the right

Look up their values using table S

If the values get larger than the trend is increasing; if smaller than trend is decreasing

Trend is increasing

****This can be done for any trend going across a period or down a group

Practice: What is the trend in ionization energy as you go down a group?

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4. Reactivity =(*Can NOT compare metals to nonmetals)

Metals: (recall: the most reactive metal is FRANCIUM)

a.

Reason:

Increased SHIELDING means VALENCE e- are held less tightly e- LOSTmore easily

b.

Reasons:

increased nuclear CHARGE and MASS pulls more tightly on tiny, negative e- HARDER to remove e-

(magnet vs. car analogy)

Nonmetals: (recall: the most reactive nonmetal is FLUORINE)

a.

Reason:

Increased SHIELDING HARDER for nucleus to attract more valencee-

b.

Reason:

Increased nuclear CHARGE and MASS EASIER for nucleus to attractmore valence e-

5. Metallic & Nonmetallic Character

Metallic Character

b. Nonmetallic Character

a.

Metallic character

Nonmetallic character

Summary of Trends:

B

Si

Ge As

Sb Te

48

To determine the trend in a group and period for the following properties: Atomic radius, Electronegativity and Ionization Energy

Graph paper, pencil, Reference Table S

49

50

51

52

Symbol

[1] Atomic Number . . . . . . . . . __________[2] Atomic Radius . . . . . . . . . . __________[3] Number of Shells . . . . . . . . __________[4] Number of Outer Electrons __________

What are the Trends in the Periodic Table?Below is a portion of the periodic table. In the answer spaces provided in the table, fill in the [1] atomic number,[2] atomic radius, [3] number of shells, and [4] number of outer shell electrons as indicated in the key below. Then,answer the questions that follow.

KEY

H[1]

[2]

[3]

[4]

He[1]

[2]

[3]

[4]

Li[1]

[2]

[3]

[4]

Be[1]

[2]

[3]

[4]

B[1]

[2]

[3]

[4]

C[1]

[2]

[3]

[4]

N[1]

[2]

[3]

[4]

O[1]

[2]

[3]

[4]

F[1]

[2]

[3]

[4]

Ne[1]

[2]

[3]

[4]

Na[1]

[2]

[3]

[4]

Mg[1]

[2]

[3]

[4]

Al[1]

[2]

[3]

[4]

Si[1]

[2]

[3]

[4]

P[1]

[2]

[3]

[4]

S[1]

[2]

[3]

[4]

Cl[1]

[2]

[3]

[4]

Ar[1]

[2]

[3]

[4]

K[1]

[2]

[3]

[4]

Ca[1]

[2]

[3]

[4]

Classwork 3-3:

53

Answer the questions below by referring to the data on the table you filled in on the first page.

1. As you go from left to right across a row of the Periodic Table:

a. What happens to the atomic number and the number of protons?

b. As a result, what happens to the pull on the electrons?

c. Therefore what happens to the atomic radius?

d. Finally, what does this mean about the likelihood of losing electrons? Do the elements become more or less

metallic?

2. As you go from top to bottom down a column of the Periodic Table:

a. What happens to the number of shells?

b. As a result, what happens to the atomic radius?

c. Therefore, what happens to the pull on the electrons?

d. Finally, what does this mean about the likelihood of losing electrons? Do the elements become more or less

metallic?

3. Based on the analysis above, where do metals tend to be located on the Periodic Table?

4. Based on the analysis above, where do nonmetals tend to be located on the Periodic Table?

5. What do the elements at the extreme right of the Periodic Table have in common? What affect does this have

on the chemical properties?

6. Where on the Periodic Table, approximately, is the border between the metals and nonmetals (the metalloids)?

54

55

56

57

58

59

60

61

62

63

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Lesson 4: Allotropes

Objective: To define and recognize an allotrope

Allotropes Elements such as carbon, oxygen, phosphorus, tin and sulfur, display allotropy. The different physical properties displayed by allotropes of an element are explained by the fact that the atoms are arranged into molecules or crystals in different ways. Some allotropes of an element may be more chemically stable than others.

Allotropes of Oxygen

There are

Both allotropes of oxygen are made up only of oxygen atoms,

O2 and O3 have different physical properties such as colour, odour, melting and boiling point, density and solubility. Some properties of the allotropes of oxygen are shown below:

PROPERTY OXYGEN (O2) OZONE (O3)

Structure O=O linear

bent

Color colorless gas pale blue liquid pale blue solid

pale blue gas deep blue liquid deep violet solid

Odor odourless sharp, pungent

Melting Point (oC) -219 -193

Boiling Point (oC) -183 -111

Density (20oC) 1.3 g/L 2.0 g/L

Solubility in Water slightly soluble more soluble that O2

Chemical Stability stable decomposes to O2 easily

Uses common oxidizer sterilizing agent it is poisonous to many living things

Allotropes of Carbon

The two most common,

Both graphite and diamond are made up of carbon atoms, but the arrangement of atoms is different in each allotrope which results in different physical properties. In particular, the presence of delocalized electrons in the structure of graphite results in it being soft and a good electrical conductor whereas diamond is very hard and an electrical insulator.

Some properties of graphite and diamond are shown below:

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PROPERTY GRAPHITE DIAMOND

Structure

Each carbon atom is bonded to 3 other carbon atoms in layers with delocalized electrons between the

layers.

Each carbon atom is bonded to 4 other carbon atoms in a 3-dimensional

covalent network. All valence electrons are used in bonding.

Color black colorless

Melting Point (K)

sublimes at ~3500 sublimes at ~4000

Electrical Conductivity

good delocalized electrons between the layers allow an electric current to pass through

poor (an insulator) no delocalized electrons to allow for the flow of electrical current

Hardness (Mohs Scale)

1-2 (soft) delocalized electrons allow the sheets to move over each other

10 (hardest known natural mineral)

Chemical Stability

stable decomposes slowly over time

Uses lubricant because it is soft

abrasive because it is so hard

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Periodic Table Activity - Atoms and Elements

INTRODUCTIONPrimary substances, called elements, build all the materials around you. There are more than 109different elements known today. The elements are composed of atoms, the smallest units that arecharacteristic of a particular element. Some elements occur in different forms, such as graphite anddiamond for the element carbon. But whatever the form of the element, it is composed of itscharacteristic atoms.

In this experiment, you will be looking at some elements in the laboratory display. Some look differentfrom each other, while others look similar. Elements can be categorized in several ways. In thisexperiment, you are going to group elements by similarities in their physical properties. Elements thatappear shiny or lustrous are called metals. Metals are usually good conductors of heat and electricity,somewhat soft and ductile, and can be molded into a shape. Some of the metals you will see such assodium or calcium may have an outer coating of a white oxide formed due to combination with oxygen inthe air. If cut, you would see the fresh shiny metal underneath. Other elements called nonmetals are notgood conductors of heat and electricity, are brittle, and appear dull (not shiny).

Atoms are made of even smaller particles of matter called subatomic particles. A large number ofsubatomic particles are now known, but we are primarily interested in the protons (p), neutrons (n), andelectrons (e). Protons are positively charged particles (+1), electrons are negatively charged particles (–1),and neutrons are neutral (charge = 0). The charge is often included with the symbol: p+, n0, and e–.

Within the atom, the protons and neutrons are tightly packed together in the nucleus and are collectivelycalled “nucleons.” Moving electrons outside of the nucleus occupy the rest of the atom, which is mostlyempty space. Electrons are so small that their mass is almost negligible compared to the mass of theprotons and neutrons in the nucleus.

Atoms of a particular element have one feature in common: the number of protons in the nucleus. Thenumber of protons, called the atomic number (Z) is unique for each element. Atoms of the elementhydrogen always have one proton in their nuclei, while atoms of the next element, helium, always havetwo protons in their nuclei. Atoms of the element carbon similarly contain six protons, and atoms of ironhave 26 protons.

The sum of the number of protons and neutrons in the nucleus of an atom is called the mass number (A)of the atom (remember A for “all”):

Mass Number = Number of Protons + Number of Neutrons

Protons attract the electrons because they have opposite charges. In a neutral atom, the number ofprotons is equal to the number of electrons. This is the normal situation in atoms. However, throughchemical reactions, an imbalance in the number of protons and electrons can result. For example, whenthe element sodium (11p+, 11e–) reacts with the element chlorine (17p+, 17e–) the compound sodiumchloride, NaCl, is formed. Sodium chloride is an ionic compound composed of sodium ions, Na+, with +1charges, and an equal number of chloride ions, Cl–, with –1 charges. In the reaction, each sodium atomloses one electron and each chlorine atom gains one electron, so the number of protons and electrons arenow 11p+, 10e– in the Na+ ion and 17p+, 18e– in the Cl– ion.

Classwork 3-4: Unit Reviews

67

All neutral atoms of the same element have the same number of protons and electrons, but interestingly,they often differ in the number of neutrons. This means that atoms of the same element while having thesame atomic number can have different mass numbers. The atoms of an element that have differentnumbers of neutrons are called isotopes of that element. In the complete chemical symbol or atomicnotation of an element, the mass number and atomic number are indicated next to the symbol. Forexample, the isotope of the element sodium that has 12 neutrons has the following symbol:

The number of protons in an atom (and the number of electrons if the atom is neutral) is given by theatomic number. To determine the number of neutrons, the mass number of the atom is needed. Thenumber of neutrons is determined by subtracting the atomic number from the mass number, A – Z.

The Periodic TableThe periodic table is a listing, in chart form, of the known elements. It has gone through many revisionsand sometimes appears in alternate forms, but with the discovery of atomic numbers in the early 20th

century, this has been the basis for the order of the elements in the table. But even before this time, it waslong recognized that certain elements shared similar properties, and when the property, such as density,was plotted against atomic mass, a repeating, or “periodic” pattern was observed. Beginning with DmitriMendeleev in 1869, chemists began organizing the elements in rows and columns in an attempt to explainthe periodic nature of various physical and chemical properties of the elements. Below are shown anearly table of Mendeleev’s and a modern periodic table:

The modern periodic table is arranged in horizontal rows (also called periods) and vertical columnscalled groups or families. The rows are numbered from 1 to 7. The groups have not always beennumbered consistently, but are usually numbered 1A, 2A, 3A, etc., from left to right, excluding the groupsof the transition elements in the middle, which have a different numbering. Because of this confusion,most modern tables have the groups numbered 1 through 18, excluding the lower, separate rows ofelements (the lanthanides and actinides) below the main table.

68

Below is a table with the common names of different sections and columns given:

The alkali metals, found in Group 1 (or 1A) of the periodic table are very reactive metals and as such donot occur freely in nature. They are the elements Li, Na, K, Rb, Cs, and Fr.

The alkaline earth elements are metallic elements found in the second group of the periodic table. Theyare not as reactive as the alkali metals, but are so reactive that they are likewise never found free in nature.These are the elements Be, Mg, Ca, Sr, Ba, and Ra.

The elements of Group 17 (7A) are called the halogens, which mean "salt formers." These are theelements F, Cl, Br, I, and At.

The noble gases are found in group 18 of the periodic table. These elements were considered to bechemically inert until the 1960's when their first compounds were characterized.

The representative elements occur in Groups 1-2 and 13-18 and exclude the transition metals and innertransition metals.

The term "transition elements" most commonly refers to the "d-block" elements in which the delectronic sublevel is being filled with electrons.

The "inner transition elements" are the "f-block" elements in which the f-sublevel is being filled withelectrons. The inner transition metals are further divided into the lanthanide series and the actinideseries. They are normally separated from the rest of the elements in the periodic table in order to savespace.

69

For this experiment a laboratory display of the elements and a wall periodic table is required.

Part I. Comparison of Physical Properties of Elements

Complete the table in the report form by writing the name and atomic number for each element. Observethe elements in the laboratory display. Describe their properties (color and luster). From yourobservations, describe each type of element as a metal or a non-metal

Part II. Predicting Properties Based on Location in the Periodic Table

Use the location of the given elements in the periodic table to predict whether the elements listed wouldbe a metal or non-metal and shiny or dull.

After you have completed your predictions, observe those same elements in the posted periodic table todetermine if you predicted their properties correctly.

Part III. Subatomic Particles and Chemical Symbols

(a) Complete the table given in the report form with the correct atomic numbers, mass numbers, andnumber of protons, electrons, and neutrons for the neutral atom of each element.

(b) Complete the table with the number of protons, electrons, neutrons, and complete chemicalsymbol (showing the mass number and atomic number) for each neutral atom.

Part IV. Graphing a Periodic Property

For this part of the experiment you will make a graph of a periodic property vs. atomicnumber. The property chosen is atomic radius, given in pm (1 pm = 10–12 m). The atomicradius, r, is related to the volume of the atom by the formula of a sphere, V = 4/3 π r3.

In Table 1 below, the atomic radii of the first 54 elements are given. Plot the points on the accompanyinggraph paper. Label selected “tick mark” values on each axis to make each scale clear. For the atomicradius scale (the Y-axis), 10 pm per mark will work well.

Connect the points and note where the high and low parts of your pattern occur in the periodic table.Does your graph indicate a reason for beginning and ending each row of the periodic table at certainelements? Why are the rows of the periodic table called “periods”?

70

Table 1. Atomic Radii of the First 54 ElementsFrom http://www.periodictable.com/Properties/A/AtomicRadius.an.html

AtomicNumber

ElementAtomic

Radius, pmAtomicNumber

ElementAtomic

Radius, pm1 H 53 28 Ni 1492 He 31 29 Cu 1453 Li 167 30 Zn 1424 Be 112 31 Ga 1365 B 87 32 Ge 1256 C 67 33 As 1147 N 56 34 Se 1038 O 48 35 Br 949 F 42 36 Kr 8810 Ne 38 37 Rb 26511 Na 190 38 Sr 21912 Mg 145 39 Y 21213 Al 118 40 Zr 20614 Si 111 41 Nb 19815 P 98 42 Mo 19016 S 88 43 Tc 18317 Cl 79 44 Ru 17818 Ar 71 45 Rh 17319 K 243 46 Pd 16920 Ca 194 47 Ag 16521 Sc 184 48 Cd 16122 Ti 176 49 In 15623 V 171 50 Sn 14524 Cr 166 51 Sb 13325 Mn 161 52 Te 12326 Fe 156 53 I 11527 Co 152 54 Xe 108

71

Name ______________________________ Date _________________

Part I

Symbol Element Atomic Number Color Shiny/Dull Metal/Nonmetal

Zn ………….. …….. …….. …….. ……….

Al ………….. …….. …….. …….. ……….

Mg ………….. …….. …….. …….. ……….

Pb ………….. …….. …….. …….. ……….

O ………….. …….. …….. …….. ……….

C ………….. …….. …….. …….. ……….

Sn ………….. …….. …….. …….. ……….

I ………….. …….. …….. …….. ……….

Fe ………….. …….. …….. …….. ……….

S …………… …….. …….. …….. ……….

Hg ………….. …….. …….. …….. ……….

Ca ………….. …….. …….. …….. ……….

Cu ………….. …….. …….. …….. ……….

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Part II

Element Metal/Nonmetal Shiny/Dull

Osmium (Os) ………. ……….

Cadmium (Cd) ………. ……….

Phosphorus (P) ………. ……….

Radium (Ra) ………. ……….

Seaborgium (Sg) ………. ………. (predicted)

Part III (a)

Element Atomic MassSymbol Number Number Protons Electrons Neutrons

F …….. 19 …….. …….. ……..

…….. …….. …….. …….. 19 20

Br …….. 80 …….. …….. ……..

…….. 79 197 …….. …….. ……..

…….. …….. 127 …….. 53 ……..

Part III (b)

Chemical Symbol Protons Electrons Neutrons

19 K39

…….. …….. ……..

16 S32

…….. …….. ……..

…….. 20 …….. 20

…….. …….. 19 22

…….. 17 …….. 20

73

Part IV

74

1. Define the following terms:

a) Nucleon

b) Transition Element

2. Compare mass, charge, and location of the subatomic particles in the atom.

Particle Mass Charge Location

Proton ____________ ______ _____________________

Neutron ____________ ______ _____________________

Electron ____________ ______ _____________________

3. Describe the location (group and period) of the following metals and nonmetals on the periodic table.

Element Group Period

I _____ _____

Fr _____ _____

Kr _____ _____

4. Write the complete chemical symbol (including the mass number, atomic number, and charge if any)of the element that corresponds to the following subatomic particles:

a) p =1, e = 1, and n = 0 b) p = 36, e = 36, and n = 48

c) p = 26, e = 23, and n = 30 d) p = 35 , e = 36, and n = 44

75

1. Define the following terms:

a) Isotopes

b) Subatomic particle

2. Compare the physical properties of metals and nonmetals (at least four properties).

3. Use the periodic table to categorize the following elements as metals (M) or nonmetals (NM).

S …….. P …….. Cr …….. Ni …….. Sr …….. I ……..

4. A neutral atom has a mass number of 58 and contains 30 neutrons. Write its complete chemicalsymbol (showing the mass number and atomic number).

5. Determine the number of protons, electrons, and neutrons in the following atoms:

Aluminum-27 Bromine-80 Uranium-238

76

A) nonmetal with a high electronegativityB) nonmetal with a low electronegativityC) metal with a high electronegativityD) metal with a low electronegativity

1 A diatomic element with a high first ionization energywould most likely be a

A) N B) P C) As D) Bi

2 The metalloids that are included in Group 15 areantimony (Sb) and

A) 2-3 B) 2-5 C) 2-8-5 D) 2-8-6

3 Which represents the electron configuration of ametalloid in the ground state?

A) atomic mass B) atomic radiusC) number of protons D) number of neutrons

4 The elements of the Periodic Table are arranged inhorizontal rows according to each successive element'sgreater

A) 1 B) 2 C) 3 D) 4

5 How many Group 17 elements are in Period 3 of thePeriodic Table?

A) 19, 23, 30, 36 B) 9, 16, 33, 50C) 3, 12, 21, 40 D) 4, 20, 38, 88

6 Which sequence of atomic numbers represents elementswhich have similar chemical properties?

A) 1, 2, and 18 B) 2, 13, and 17C) 1, 2, and 14 D) 1, 2, and 17

7 Alkali metals, alkaline earth metals, and halogens areelements found respectively in Groups

A) bromine B) argonC) sulfur D) rubidium

8 Which element exists as a diatomic molecule at STP?

A) a halogenB) a noble gasC) an alkali metalD) an alkaline earth metal

9 The element in Period 2 with the largest atomic radius is

A) Ar B) Si C) Mg D) S

10 Which of the following elements in Period 3 has thegreatest metallic character?

A) Group 1 metal B) Group 2 metalC) Group 1 nonmetal D) Group 2 nonmetal

11 In the formula XF2, the element represented by X can beclassified as a

A) metal B) metalloidC) noble gas D) nonmetal

12 A solid element that is malleable, a good conductor ofelectricity, and reacts with oxygen is classified as a

A) electrons and neutronsB) electrons and protonsC) positrons and neutronsD) positrons and protons

13 An atom of lithium-7 has an equal number of

A) tantalum B) rheniumC) osmium D) hafnium

14 Which element has the highest melting point?

A) gain electrons and form negative ionsB) gain electrons and form positive ionsC) lose electrons and form negative ionsD) lose electrons and form positive ions

15 Atoms of metallic elements tend to

A) gold B) hydrogenC) sulfur D) radon

16 Which element is considered malleable?

A) Iron can be flattened into sheets.B) Iron conducts electricity and heat.C) Iron combines with oxygen to form rust.D) Iron can be drawn into a wire.

17 Which statement describes a chemical property of iron?

A) S B) Si C) Ge D) Au

18 Which element is malleable and ductile?

A) 2-8-2 B) 2-8-8-2C) 2-8-18-8-2 D) 2-8-18-18-2

19 The least active metal of those represented below has anelectron configuration abbreviated as

A) silver B) mercuryC) barium D) bromine

20 Which element is a liquid at STP and has low electricalconductivity?

A) They are malleable and have metallic luster.B) They are malleable and lack metallic luster.C) They are brittle and have metallic luster.D) They are brittle and lack metallic luster.

21 Which characteristics describe most nonmetals in thesolid phase?

A) N2 B) O2 C) Cl2 D) F2

22 Which gaseous element has the greatest density at STP?

Unit 3 Practice Test

77

A) A B) B C) C D) D

23 The table below shows some properties of elements A, B, C, and D.

Which element is most likely a nonmetal?

A) Neon is a gas at STP.B) Neon has a low melting point.C) Neon atoms have a stable valence electron

configuration.D) Neon atoms have two electrons in the first shell.

24 Which statement explains why neon is a Group 18element?

A) hydrogen B) chlorineC) oxygen D) helium

25 Which of the following gases is monatomic at STP?

A) is malleable and ductileB) is an excellent conductor of heat and electricityC) exhibits metallic and nonmetallic propertiesD) none of the above

26 Pure silicon is chemically classified as a metalloidbecause silicon

A) 1 B) 2 C) 3 D) 4

27 Which period contains elements that are all gases atSTP?

A) B) C) D)

28 An atom in the ground state contains a total of 5electrons, 5 protons, and 5 neutrons. Which Lewiselectron-dot diagram represents this atom?

A) B)

C) D)

29 Which Lewis electron-dot diagram is correct for a S2–

ion?

A) mass numberB) atomic numberC) number of electron shellsD) number of valence electrons

30 Lithium and potassium have similar chemical propertiesbecause the atoms of both elements have the same

A) 5 B) 2 C) 3 D) 4

31 An atom of an element has 28 innermost electrons and 7outermost electrons. In which period of the PeriodicTable is this element located?

A) They have the same number of valence electrons.B) They have similar chemical properties.C) They have electrons occupying the same number of

principal energy levels.D) They have completely filled principal energy

levels.

32 Which is a common characteristic of the elements Rb,Te, I, and Xe in the ground state?

A) RbCl B) CaCl2 C) NiCl2 D) ZnCl2

33 Which compound forms a green aqueous solution?

A) alkali metalsB) alkaline earth metalsC) noble gasesD) transition elements

34 Which elements contain atoms that form colored ionsand have more than one positive oxidation state?

A) fluoride ion B) sodium ionC) neon atom D) argon atom

35 Which particle has the same electron configuration as apotassium ion?

78

A) The Cd atom gains two electrons and its radiusdecreases.

B) The Cd atom gains two electrons and its radiusincreases.

C) The Cd atom loses two electrons and its radiusdecreases.

D) The Cd atom loses two electrons and its radiusincreases.

36 Which changes occur as a cadmium atom, Cd, becomesa cadmium ion, Cd2+?

A) positively charged and gains a small amount ofmass

B) positively charged and loses a small amount ofmass

C) negatively charged and gains a small amount ofmass

D) negatively charged and loses a small amount ofmass

37 When an atom loses an electron, the atom becomes anion that is

A) number of protons increases, and the number ofshells of electrons remains the same

B) number of protons increases, and the number ofshells of electrons increases

C) number of protons decreases, and the number ofshells of electrons remains the same

D) number of protons decreases, and the number ofshells of electrons increases

38 As the elements in Period 2 of the Periodic Table areconsidered in succession from left to right, there is adecrease in atomic radius with increasing atomicnumber. This may best be explained by the fact that the

A) atomic numberB) mass numberC) the number of protons occupying the nucleusD) the number of occupied electron shells

39 As the elements of Group 16 are considered in orderfrom top to bottom, the covalent radius of eachsuccessive element increases. This increase is primarilydue to an increase in

A) decrease in size as it forms a positive ionB) increase in size as it forms a positive ionC) decrease in size as it forms a negative ionD) increase in size as it forms a negative ion

40 An atom with the electron configuration2-8-2 would most likely

A) aluminum B) chlorineC) silicon D) sodium

41 Atoms of which of the following elements have thestrongest attraction for electrons?

A) Na B) P C) Si D) S

42 Atoms of which element have the weakest attraction forelectrons?

A) lithium atom B) potassium atomC) rubidium atom D) sodium atom

43 Which atom in the ground state requires the least amount of energy to remove its valence electron?

A) decreasing atomic massB) decreasing electronegativityC) increasing atomic radiusD) increasing first ionization energy

44 Which general trend is found in Period 2 on the PeriodicTable as the elements are considered in order ofincreasing atomic number?

A) H ® Li ® Na ® KB) I ® Br ® Cl ® FC) O ® S ® Se ® TeD) H ® Be ® Al ® Ga

45 Which sequence correctly places the elements in orderof increasing ionization energy?

A) nuclear charge is decreasingB) number of neutrons is increasingC) number of principal energy levels is decreasingD) distance between the valence electron and the

nucleus is increasing

46 As the Group 1 elements of the Periodic Table areconsidered from top to bottom, the first ionizationenergy of each successive element decreases. Onereason for this is that the

A) He B) As C) Xe D) Cs

47 Which element has an atom in the ground state with themost loosely bound electron?

A) 17 B) 2 C) 12 D) 7

48 In which group of the Periodic Table do most of theelements exhibit both positive and negative oxidationstates?

79

A) A B) B C) D D) E

49 The graph below represents the relationship betweenatomic radii, in picometers, and increasing atomicnumber for elements in Group 15.

Which element is most metallic

A) a higher melting point and a higher boiling pointB) a higher melting point and a lower boiling pointC) a lower melting point and a higher boiling pointD) a lower melting point and a lower boiling point

50 When the elements in Group 1 are considered in orderfrom top to bottom, each successive element at standardpressure has

80

Unit Review:

Periodic Table Place a checkmark next to each item that you can do! If a sample problem is given, complete it as evidence.

_____1. I can still do

everything from Unit 1A.

_____2. I can still do

everything from Unit 1B.

_____3. I can still do

everything from Unit 2.

_____4. I can classify elements

as metals, nonmetals, or

metalloids based on their

placement on the Periodic

Table.

Classify each of the following elements as metals (M), nonmetals (NM),

or metalloids (MTLD).

_______B ________K ________Li ________C _______Ar

_______Sb ________H ________Fe ________Au _______S

_______F ________Si ________Fr ________He _______Rn

_______Ge ________Al ________As ________Bi _______I

_____5. I can state the group

names for elements in groups

1, 2, 17, and 18.

Group 1 is called the ____________________________________.

Group 2 is called the ____________________________________.

Group 17 is called the ____________________________________.

Group 18 is called the ____________________________________.

_____6. I can explain why

elements in the same group

have similar chemical

properties.

Elements in the same group have similar chemical properties because

_____7. I can explain why the

elements in Group 18 don’t

usually react with other

elements.

Elements in Group 18 don’t usually react with other elements because

_____8. I can state the

meaning of “STP” and the

Reference Table on which it

can be found.

STP stands for

____________________________________________________.

The values can be found on Reference Table______________.

_____9. I can state the

names/symbols for the two

elements on the Periodic Table

that are liquids at STP.

The two elements that are liquids at STP are:

________________________ and __________________

_____10. I can state the

names/symbols of the 11

elements that are gases at STP.

The 11 elements that are gases at STP are:

_____________________________,

_______________________________,

_____________________________,

_______________________________,

_____________________________,

_______________________________,

_____________________________,

_______________________________,

_____________________________,

_______________________________,

and _____________________________

_____11. I can state how the

elements on the Periodic Table

are arranged.

The elements on the Periodic Table are arranged by increasing

_______________ ____________________.

_____12. I can list the 7

diatomic elements.

The seven diatomic elements are:

_____13. I can define

electronegativity, first

ionization energy, atomic

radius, ionic radius, metallic

character, and

activity/reactivity.

Definitions:

electronegativity

first ionization energy

atomic radius

ionic radius

metallic character

activity/reactivity

81

82

_____14. I can state the

periodic trend for

electronegativity and explain

why it occurs.

As one reads down a group from top to bottom, electronegativity

______________________ because

__________________________________

______________________________________________________________.

As one reads across a period from left to right, electronegativity

______________________ because

__________________________________

______________________________________________________________.

_____17. I can state the

periodic trend for first

ionization energy and explain

why it occurs.

As one reads down a group from top to bottom, first ionization energy

______________________ because

__________________________________

______________________________________________________________.

As one reads across a period from left to right, , first ionization energy

______________________ because

__________________________________

_____________________________________________________________.

_____15. I can state the

periodic trend for atomic

radius and explain why it

occurs.

As one reads down a group from top to bottom, atomic radius

______________________ because

__________________________________

______________________________________________________________.

As one reads across a period from left to right, atomic radius

______________________ because

__________________________________

______________________________________________________________.

_____16. I can state the

periodic trend for metallic

character and explain why it

occurs.

As one reads down a group from top to bottom, metallic character

______________________ because

__________________________________

______________________________________________________________.

As one reads across a period from left to right, metallic character

______________________ because

__________________________________

______________________________________________________________.

83

_____17. I can state the trend

for melting points and boiling

point for METALS as one

reads down a group.

As one reads down a group from top to bottom, the melting points and boiling

points for METALS ______________________.

_____18. I can state the trend

for melting points and boiling

point for NONMETALS as

one reads down a group.

As one reads down a group from top to bottom, the melting points and boiling

points for NONMETALS ______________________.

84

_____19. I can state the trend

for activity/reactivity for

METALS as one reads down a

group.

As one reads down a group from top to bottom, the activity/reactivity of

METALS ____________________.

_____20. I can state the trend

for activity/reactivity for

NONMETALS as one reads

down a group.

As one reads down a group from top to bottom, the activity/reactivity of

NONMETALS ____________________.

_____21. I can explain how loss

or gaining of electrons affects

the radius of an element.

Metals tend to lose electrons (get oxidized). This loss of electrons causes

cations to be __________________ than the original atom.

Nonmetals tend to gain electrons (get reduced). This gain of electrons

causes

anions to be __________________ than the original atom.

_____22. I can list the

properties of metals.

Properties of metals are:

_____23. I can list the

properties of nonmetals.

Properties of non metals are: