unit 3: periodic table lab packet

Unit 3: Periodic Table

Lab Packet

DO NOT LOSE THIS PACKET.

IT WILL BE SUBMITTED AT THE END OF THE

UNIT FOR ALL LAB CREDIT.

Please keep track of when each lab is assigned and

the due date by which it should be completed.

Periodicity of Elements

Why?

Within musical scales the notes form a series that repeats every eighth note. Eight notes

up from a C note is another C note. Each interval or series is referred to as an octave since it

contains eight notes. Elements also form an eight step series. The purpose of this activity is to

explore how valence electrons generate an eight step series that repeats itself within the periodic

table.

Learning Objectives

• Associate groups on the periodic table with a number of valence electrons in an electron

configuration.

• Associate periods on the periodic table with a number of principle energy levels (shells)

in an electron configuration.

Success Criteria

• Assign a group number for the elements in groups 1, 2 and 13-18 based upon the number

of ground-state valence electrons in their atoms.

• Assign a period number for the elements in groups 1, 2 and 13-18 based upon the number

of occupied shells in a ground-state electron configuration for the element.

Prerequisites

• Electron Configuration

• Nuclear Charge

Information

Periodic Table is a grid made up of:

• Rows (or periods) that proceed horizontally (from side to side) across the table.

• Columns (or groups) that proceed vertically (up and down) on the table.

Resources

• Periodic Table

Model: An Electron Dot Diagram of the Main Group Elements

Task

Below the symbol for each element, write an electron configuration for the elements in the

model. Lithium has been done for you.

Key Questions

1. How are 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 period (row) contains three occupied shells?

5. Within a group, which period, top or bottom is likely to contain atoms with the larger radius?

Explain your answer.

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

the model.

7. Refer to a Periodic Table and write the number of protons in the nucleus for the period 2

elements listed below:

Li _____ Be _____ B _____ C _____ N _____ O _____ F _____

8. Which of the above elements within period 2 contains the greatest nuclear charge? Explain.

9. The atomic radius for an atom is the distance from the center of the nucleus to the outermost

principle energy level.

Refer to Table S in your reference tables and write the atomic radius for the period 2 elements

listed below. Please include units:

Li ________ Be ________ B ________ C ________ N ________ O ________ F ________

10. Which of the above elements has the strongest pull on its valence electrons and electron shells?

Explain.

11. Which element within period 2 generates the greatest force of attraction between its nucleus and

its valence electrons? Explain in terms of atomic structure.

Exercise

Complete all of the information below for each of the atoms with the following ground state electron configurations:

Electron configuration 2-8-3 2-8-8-1 2-6 2-8-18-7 2-8-18-32-18-8

Element symbol

Group number

Period or Row number

Nuclear charge

# of valence electrons

Electron dot diagram

(atom)

Ion’s charge (oxidation

state)

Ion’s symbol including

charge

# of electrons lost or

gained. Indicate if lost or

gained.

Questions:

1 a. Which of the above elements have fewer than 4 valence electrons?

b. What type of ions do these elements form? Explain how these ions form in terms of valence electrons.

c. Are these elements metals or nonmetals?

2 a. Which of the above elements have greater than 4 valence electrons?

b. What type of ions do these elements form? Explain how these ions form in terms of valence electrons.

c. Are these elements metals or nonmetals?

METALS NONMETALS METALLOIDS

1. Have luster 1. Are dull 1. Have luster

2. Are malleable and ductile 2. Are brittle 2. Are brittle

3. Conduct heat and electricity 3. Do not conduct heat or electricity very well. 3. Semi-conductors

4. Lose electrons to form ions 4. Prefer to gain electrons to form an ion. 4. Can gain or lose electrons

5. Low electronegativity and ionization 5. High electronegativity and ionization energies to form an ion.

energies. 5. Moderate electronegativities and

ionization energies.

Name: ____________________________________________ Date: _____________________ Lab # _____: Metals, Nonmetals and Metalloids

Background: More than 75% of the elements on the Periodic Table are metals. They are recognizable by certain characteristics. You will examine several different elements and determine if they are metals or nonmetals based on the properties observed.

Procedure: 1. At each of the stations, record the name of the element into your data table. 2. Using your reference tables look up the atomic symbol and draw the Lewis dot diagram of the atom. 3. Observe the color of the element and record it. 4. Rub the sample of the element with steel wool to see if you can make it shiny and lustrous. Record

your result as shiny or dull. 5. Use the conductivity tester to see if the sample conducts electricity (Make sure the tester is switched

“on” and put both ends of the tester to a sample, but do not let the two metal prongs touch each other). If the light goes on, it conducts electricity. Record your result.

6. Try to bend the sample gently. If it bends, record it as malleable. If it does not bend, record it as brittle.

Data Table: Name Symbol Lewis Dot

Diagram

Color Luster Conducts electricity

Malleable/

Brittle

1

2

3

4

5

6

7

8


Teacher Demonstration Elements (at the front desk):

Station # Name Symbol Lewis Dot Diagram

Color Luster Conducts electricity

Phase at Room

Temperature

9 Iodine

NO NO

10 Bromine

NO NO

11 Mercury

YES YES

Analysis Questions: 1. From your notes, what are the properties of metals?

2. Using the information from Question # 1, which samples that you tested were metals? Explain why you classified these elements as metals using your observations from the lab.

3. Where are metals and nonmetals located on the Periodic Table with respect to the Boron “staircase”?

4. Are there more metals or nonmetals on the Periodic Table?

5. Where are the metalloids located on the periodic table? Name the metalloids.

6. Using your notes, what are the characteristics of a metalloid?

7. In terms of the number of valence electrons, how do the electron dot diagrams of metals compare to the electron dot diagrams of nonmetals?

8. What type of ion does Sodium, Magnesium and Aluminum form? A cation or an anion? Support your answer with evidence from the periodic table.

9. Which type of ion does Fluorine, Oxygen, and Chlorine form? A cation or an anion? Support your answer with evidence from the periodic table.


USING THE CLASS SET OF TEXTBOOKS OR YOUR PRENTICE HALL REVIEW BOOK, DEFINE EACH OF THE TERMS BELOW AND THEN USE THESE TERMS TO ANSWER QUESTIONS 10 and 11.

Electronegativity: _______________________________________________________________________

______________________________________________________________________________________

First Ionization energy: ___________________________________________________________________

______________________________________________________________________________________

Elements with high ionization energy and high electronegativity tend to gain electrons while elements with low ionization energy and low electronegativity tend to lose electrons. Metal atoms prefer to lose electrons while nonmetal atoms prefer to gain electrons in order to achieve a “stable octet” or a full valence shell. The noble gases are inert or unreactive nonmetal gaseous elements. The noble gases are unreactive because they all have a full valence shell making them very stable. They exist as monatomic elements and do not want to lose or gain valence electrons.

10. Explain, in terms of electronegativity values, why Fluorine forms a -1 ion by gaining an electron and why sodium forms a +1 ion by losing an electron.

11. Explain, in terms of electrons, why the noble gases have no electronegativity values and very high ionization energies.

Name: ______________________________________ Date: __________________ Lab #____: Trends of the Periodic Table

Purpose: To graph several properties of selected elements and observe the trend as you move across a period or

down a group within the periodic table.

Materials: Reference Table for Chemistry, pencil, pen

Pre-lab Questions:

Define each of the following terms: a. Atomic Radius:

b. First Ionization Energy:

c. Electronegativity:

d. Nuclear charge:

Procedure: 1) On the graphs provided, graph the properties listed for the elements in Group 16 (Oxygen, Sulfur, Selenium,

Tellurium and Polonium) and then again for those in Period 3 (Sodium, Magnesium, Aluminum, Silicon, Phosphorus, Sulfur, Chlorine and Argon).

2) The x-axis has been completed for you. Please label an appropriate y-axis before plotting.

3) Graphs to plot: a) atomic radius b) first ionization energy c) electronegativity. Find information on Table S.

4) For each graph, circle and connect the points. You will then answer questions about the observed trend for each graph and explain why this trend occurs.

Atomic Radius Trends

Ato

mic

Rad

ius

(pm

)

Ato

mic

Rad

ius

(pm

)

Na Mg Al Si P Cl Ar Elements in Period 3

O S Se Te Po Elements in Group 16

First Ionization Energy Trends

Electronegativity Trends


Firs

t Io

niz

atio

n E

ner

gy (

kJ/m

ol)

Firs

t Io

niz

atio

n E

ner

gy (

kJ/m

ol)

Elec

tro

neg

ativ

ity

Ele

ctro

neg

ativ

ity




Questions and Conclusions

1) State the Periodic Law:

2) What keeps the valence electrons tethered to an atom and prevents them from easily escaping? (Hint: Use your knowledge of atomic structure and subatomic particles)

Looking at your graphs, state the change in each property as you go down a group and across a period. 3) Atomic Radius Graph Analysis

a. Observed trend down a group:

b. Observed trend across a period:

c. Explain, in terms of atomic structure, why the atomic radius increases down a group.

d. Explain, in terms of atomic structure, why the atomic radius decreases across a period.

4) First Ionization Energy Graph Analysis a. Observed trend down a group:


c. Explain, in terms of atomic structure, why the ionization energy decreases down a

group.

d. Explain, in terms of atomic structure, why the ionization energy increases across a period.

5) Electronegativity Graph Analysis a. Observed trend down a group:


c. Explain, in terms of atomic structure, why the electronegativity decreases down a group.

d. Explain, in terms of atomic structure, why the electronegativity increases across a period.

6) Explain why the transition metals were skipped for the period 3 graphs showing trends in ionization energy, electronegativity and atomic radius.

7) Why does having a low first ionization energy and low electronegativity cause a metal to be very reactive?

8) Why does having a high first ionization energy and high electronegativity cause a nonmetal to be very reactive?

Name___________________________________________________ Date:______________

Activity: What can be determined by examining the Periodic Table of Elements? Background: By the mid-1800s, 60 elements were known. Scientists had quite a bit of information about these elements, but the information was not organized, so it was not very useful. In 1869, a Russian scientist named Dmitri Mendeleev made a chart of the know elements. Since that time, more elements have been discovered and added to the chart. The chart is called the PERIODIC TABLE OF ELEMENTS, which is used worldwide. In the periodic table, elements are arranged in order of their atomic numbers. With a couple of exceptions, atomic numbers are in the same order as atomic masses. That is, the lightest element has the lowest atomic number and the heaviest element has the highest atomic number. ** Each row is called a _________________ ** Each column is called a ________________________ **Each group is identified by a number ** Elements can be divided into two main types ______________and ________________ There are more metals than nonmetals, and metals are located to the left of the “stair-step” line. Hydrogen can behave as a metal or nonmetal, depending on the situation, but is considered a nonmetal. ANSWER THE QUESTIONS ABOUT THE PERIODIC TABLE. USE YOUR TABLE AS A REFERENCE

1. List the periods by number______________________________________

2. List the groups by number ______________________________________

A). Fill in the following table using elements from Period 3.

ELEMENT NAME SYMBOL ATOMIC NUMBER EN Atomic Radius

3. Explain, in terms of nuclear charge, why the electronegativity increases across a period.

4. Explain, in terms of nuclear charge, why the ionization energy increases across a period.

5. Explain, in terms of nuclear charge, why the atomic radius decreases across a period.

Name___________________________________________________ Date:______________

Activity: What can be determined by examining the Periodic Table of Elements? B) List the name, symbol and atomic number of each element in Group 13

ELEMENT NAME SYMBOL ATOMIC NUMBER EN Atomic Radius

6. Why does atomic radius increase going down a group?

7. Why does electronegativity decrease going down a group?

8. Why does ionization energy decrease going down a group? C) Find the element:

Period Group Element Symbol Atomic Number

2 16

3 1

4 8

1 18

6 12

9. Which one of these elements is the lightest?

10. You know it is the lightest because it has the (highest / lowest) atomic number and the mass of an atom is found

in the (nucleus / electron shells)

11. Which one is in the noble gas group? D) Finding the periods and groups

Period Group Element Symbol Atomic Number

Chlorine

Potassium

Neon

Tin

Krypton

12. Which of these elements are metals? Which are nonmetals?

13. Two of these elements have properties that are similar: _________________ and_______________.

14. We know they are alike because they are in the same (Period / group) and have the same number of (principle energy levels / valence electrons)

15. Name four elements that have properties similar to Chlorine. _________________________________________

Name: ________________________________________________________ Date: ___________ Lab #: ________________; Periodicity of Metals Lab

Background: The ability of metals to react with air and water is a function of their electronegativity. Iron railings must be

painted to prevent them from rusting since iron reacts with both air and water to form rust (iron (II) oxide). Gold and

platinum on the other hand, are used in jewelry and for coins because they are relatively less reactive for metals. They do

not tarnish when exposed to air or water. To compare the reactivity of different metals, see Table J, the “Activity Series”.

The terms “active” and “reactive” are synonymous in Chemistry. During this experiment, you will determine the relative

reactivity of 3 metals (Calcium, Magnesium and Aluminum) and predict the trend for reactivity of 3 other metals (Lithium,

Sodium and Potassium) prior to a video demonstration. PUT ON YOUR GOGGLES BEFORE BEGINNING THE LAB!

Materials:

• Calcium metal • Water • 150-mL beaker • Forceps • Test tube rack

• Magnesium metal • 2 test tubes • Graduated cylinder • Aluminum metal • Phenolphthalein

Procedure:

1. Add approximately 10 ml of water to the 2 test tubes using the graduated cylinder. Add 3 drops of phenolphthalein to each test tube.

2. Using a small watch glass, obtain 1 piece of Al and Mg from the back counter and bring to your lab table.

3. Place the Al metal into test tube 1 and the Mg metal into test tube 2. Compare the reactions of water with magnesium and aluminum.

4. Record your observations in the data table; you should check for the vigor of the reaction and the degree of the change in the color of the reaction solution.

5. Using a graduated cylinder, pour 20 ml of water into the 150 mL beaker. Add 3 drops of phenolphthalein indicator.

6. Ask your teacher for a piece of calcium metal to be placed in the beaker. Note how vigorous the reaction is and record your observations in the data table.

7. CLEAN UP: KEEP YOUR GOGGLES ON FOR CLEANUP. Fill the calcium reaction beaker with water, pour down the drain and rinse the beaker thoroughly with excess water.

8. Pour the aluminum metal and excess water in the waste beaker on the back counter. Use the squirt bottle of water to help get the metal out of the test tube if needed. Do the same for the magnesium ribbon and excess water.

9. After removing the metals, rinse both test tubes using the lab sink and place both, INVERTED on the wooden dowels of the test tube racks to dry.

10. Complete all sections of the data table using your observations and reference tables.

Metal Group number

Period Reaction in H2O observations

Color of solution after reaction

Lewis Dot Diagram

Electronegativity

Ca

Mg

Al

Name: ________________________________________________________ Date: ___________ Lab #: ________________; Periodicity of Metals Lab

Data: (Video Demonstration): Reactivity of Group 1 metals

Metal 1: _____________; Period: _____; Observations: ____________________________________________





Analysis Questions:

1. What is the trend for the reactivity of metals down a group? Explain the reason for this trend.

2. Based on your observations, which metal was more reactive; Magnesium or Calcium? How does this compare to your answer to question 1.

3. What is the trend for the reactivity of metals across a period? Explain the reason for this trend.

4. Based on your observations, which metal was more reactive; Magnesium or Aluminum? How does this

compare to your answer to question 3.

5. Look up the electronegativity values for each of the metals demonstrated during the video:

a. Li= _________ b. Na= _________ c. K= _________ d. Rb= _________ e. Cs= __________

6. Is high or low electronegativity associated with increased metal activity?

7. In chemical bonding, metals tend to lose electrons when forming an ionic compound. What is the connection with the electronegativity of metals?

8. After watching the video demonstration, which metal was the most reactive? Support your answer with your observations and electronegativity.

9. In chemical bonding, nonmetals tend to gain electrons when forming an ionic compound. The more readily a nonmetal can gain electrons, the more reactive it is. Which nonmetal is the most reactive? Support your answer in terms of electronegativity.

Name: ___________________________________________ Classifying Elements as Metals, Nonmetals, Metalloids and Noble Gases

Electronegativity: The attraction a nucleus has for electrons in a chemical bond.

• Metal elements have electronegativity’s lower than 1.9. This is a weak attraction for electrons which is why when metals form ions and bond they lose electrons, resulting in an overall positive charge.

• Nonmetal elements have electronegativity’s greater than 2.1. This is a stronger attraction for electrons which is why when nonmetals form ions and bond, they prefer to gain electrons, resulting in an overall negative charge.

• Metalloids have an electronegativity that falls on the borderline between 1.9-2.2. These elements can behave as both a metal or nonmetal. This depends on what type of element they form a bond with. There are 6 metalloids and they lie on the bold staircase found on the periodic table. This is the dividing line between the metals and nonmetals.

• The nonmetal elements are found to the right of the staircase while the metal elements are found to the left of the staircase.

• There is one element to the left of the stair case but it is a NONMETAL. This element has 1 proton. What is the name of this element? __________________

Determining the Metalloid Elements The number of electrons in the 6 metalloids are listed below, please determine the identity of each metalloid using your periodic tables.

Metalloid Name Metalloid Symbol

a. 5 electrons: ______________________ ___________

b. 14 electrons: ______________________ ___________

c. 32 electrons: ______________________ ___________

d. 33 electrons: ______________________ ___________

e. 51 electrons: ______________________ ___________

f. 52 electrons: ______________________ ___________

Identifying the Noble Gas Elements The noble gases are found in Group 18 on the periodic table. Please list their name and symbol below.

a. ______________________ d. _______________________

b. ______________________ e. _______________________

c. ______________________ f. ________________________

Name: ___________________________________________ Classifying Elements as Metals, Nonmetals, Metalloids and Noble Gases

Using Electronegativity to Classify Elements as Metals or Nonmetals. The elements below are either a metal or nonmetal. Please look up their electronegativity values and then determine if they are a metal or nonmetal. As mentioned in the beginning of the packet, elements with an electronegativity greater than 2.0 are nonmetals and less than 2.0 are metals.

Name Symbol Electronegativity Metal/Nonmetal

a. Cobalt Co ______________ ______________

b. Nitrogen N ______________ ______________

c. Carbon C ______________ ______________

d. Phosphorus P ______________ ______________

e. Copper Cu ______________ ______________

f. Zinc Zn ______________ ______________

g. Potassium K ______________ ______________

h. Sulfur S ______________ ______________

i. Fluorine F ______________ ______________

j. Cesium Cs ______________ ______________

k. Rubidium Rb ______________ ______________

l. Manganese Mn ______________ ______________

m. Bromine Br ______________ ______________

n. Chlorine Cl ______________ ______________

o. Selenium Se ______________ ______________

p. Strontium Sr ______________ ______________

q. Barium Ba ______________ ______________

r. Iodine I ______________ ______________

s. Oxygen O ______________ ______________

t. Iron Fe ______________ ______________

u. Chromium Cr ______________ ______________

v. Radium Ra ______________ ______________

w. Silver Ag ______________ ______________

x. Nickel Ni ______________ ______________

y. Francium Fr ______________ ______________

Please complete the coloring sheet using the color indicated for each type of element.

unit 3: periodic table lab packet

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