periodic table tutorial chapter 5.4 chapter 14 periodic table periodic table scientists &...

Periodic Table Periodic Table TutorialTutorialChapter 5.4Chapter 5.4

Chapter 14Chapter 14

Periodic TablePeriodic Table

Scientists Scientists & Definitions& Definitions

Periodic Periodic TrendsTrends

QuestionsQuestions

Click on a region of the table to learn more about Click on a region of the table to learn more about that region.that region.

Alkali MetalsAlkali Metals• The alkali metals are the Group 1 The alkali metals are the Group 1

metals & include lithium, sodium, metals & include lithium, sodium, potassium and the others in the group. potassium and the others in the group. All the alkali metals have an sAll the alkali metals have an s11 e e-- configuration. They are very reactive & configuration. They are very reactive & want to lose 1 electron to obtain a want to lose 1 electron to obtain a noble gas configuration. They are part noble gas configuration. They are part of the s-block.of the s-block.

Back to Periodic TableBack to Periodic Table

Alkaline Earth MetalsAlkaline Earth Metals• The alkaline earth metals are the Group The alkaline earth metals are the Group

2 metals & include beryllium, 2 metals & include beryllium, magnesium, calcium, etc. These metals magnesium, calcium, etc. These metals have an shave an s22 e e-- configuration. They are configuration. They are reactive & want to lose 2 electrons to reactive & want to lose 2 electrons to obtain a noble gas configuration.obtain a noble gas configuration. They They are part of the s-block.are part of the s-block.


Transition MetalsTransition Metals• The transition metals make up the d-The transition metals make up the d-

block. Iron, copper, zinc, mercury, gold block. Iron, copper, zinc, mercury, gold & silver are all transition metals. & silver are all transition metals. Their Their ee-- configurations all end in a d sublevel. configurations all end in a d sublevel. They are not part of the representative They are not part of the representative elements and are considered Group B. elements and are considered Group B.


Inner-Transition MetalsInner-Transition Metals• The inner-transition metals make up The inner-transition metals make up

the f-block. Uranium is an inner-the f-block. Uranium is an inner-transition metals. transition metals. Their eTheir e-- configurations all end in an f sublevel. configurations all end in an f sublevel. The are not part of the representative The are not part of the representative elements & actually belong in the 6elements & actually belong in the 6thth and 7and 7thth periods, not below the Table. periods, not below the Table.


Other MetalsOther Metals• The other metals include aluminum & The other metals include aluminum &

lead. They are all in the p-block & their lead. They are all in the p-block & their ee- - configurations therefore end in a p configurations therefore end in a p sublevel. Like the rest of the metals, sublevel. Like the rest of the metals, they are good conductors of both heat they are good conductors of both heat and electricity. and electricity.


Semi-Metals (Metalloids)Semi-Metals (Metalloids)• The semi-metals or metalloids are not The semi-metals or metalloids are not

metals & are not non-metals. They are metals & are not non-metals. They are all in the p-block so their eall in the p-block so their e-- configurations end in a p sublevel. configurations end in a p sublevel. Their properties are in between those Their properties are in between those of metals & nonmetals. Silicon and of metals & nonmetals. Silicon and germanium are metalloids. germanium are metalloids.


Other NonmetalsOther Nonmetals• The other non-metals include The other non-metals include

hydrogen, oxygen & carbon – some of hydrogen, oxygen & carbon – some of the most abundant elements on earth & the most abundant elements on earth & in the universe! Some, like nitrogen, in the universe! Some, like nitrogen, are gases & some, like carbon, are are gases & some, like carbon, are solids. Hydrogen is the only non-metal solids. Hydrogen is the only non-metal not in the p-block. not in the p-block.


HalogensHalogens• The halogens are some of the most The halogens are some of the most

reactive elements on earth. They reactive elements on earth. They include: fluorine & chlorine (gases), include: fluorine & chlorine (gases), bromine (a liquid) and iodine (a solid). bromine (a liquid) and iodine (a solid). They are not found alone in nature and They are not found alone in nature and commonly form salts with metals such commonly form salts with metals such as sodium (i.e. NaCl) They all end in a as sodium (i.e. NaCl) They all end in a pp5 5 configuration. configuration.


Noble GasesNoble Gases• The noble gases include helium, neon The noble gases include helium, neon

& argon. Helium has a 1s& argon. Helium has a 1s22 e e-- configuration & all the others end in a configuration & all the others end in a pp66 configuration. This makes them configuration. This makes them completely stable & unreactive with all completely stable & unreactive with all the other elements. They are also the other elements. They are also called the inert gases. called the inert gases.


ScientistsScientists• There were two scientists who designed There were two scientists who designed

the periodic table – Mendeleev arranged the periodic table – Mendeleev arranged the elements in order of atomic mass. the elements in order of atomic mass. Later, Moseley used atomic number – this Later, Moseley used atomic number – this is the table we use today! They were able is the table we use today! They were able to predict properties of the missing to predict properties of the missing elements based on where they were in the elements based on where they were in the table. table.

Groups & PeriodsGroups & Periods• The modern periodic table is arranged in The modern periodic table is arranged in

familiesfamilies or or groupsgroups (vertical columns), & (vertical columns), & periodsperiods (horizontal rows). The period (horizontal rows). The period number corresponds to the main energy number corresponds to the main energy level being filled with electrons. Groups level being filled with electrons. Groups are numbered 1 - 18. Groups 1, 2, & 13-are numbered 1 - 18. Groups 1, 2, & 13-17 are the 17 are the representative elementsrepresentative elements. .

BlocksBlocks• There are 4 blocks of the periodic table. There are 4 blocks of the periodic table.

The The s-blocks-block consists of the first two consists of the first two groups. All the s-block elements have groups. All the s-block elements have an s sublevel ean s sublevel e-- configuration. The configuration. The p-p-blockblock is made of groups 13-18. They is made of groups 13-18. They end in a p sublevel eend in a p sublevel e-- configuration. configuration.

BlocksBlocks• The The transition metalstransition metals make up the make up the d-d-

blockblock. These elements end in a d sub-. These elements end in a d sub-level configuration. Finally, the level configuration. Finally, the f-blockf-block consists of the consists of the inner-transition metalsinner-transition metals. . They end in an f sub-level They end in an f sub-level configuration. The d-block and f-block configuration. The d-block and f-block are the group B elements. are the group B elements.

Metals vs. Non-MetalsMetals vs. Non-Metals• There are 3 main categories for the There are 3 main categories for the

elements. elements. MetalsMetals are found on the left are found on the left side of the table, have a luster & side of the table, have a luster & conduct heat and electricity. conduct heat and electricity. NonmetalsNonmetals are on the right hand corner, are dull & are on the right hand corner, are dull & are not good conductors. The final are not good conductors. The final designation is designation is metalloidmetalloid or or semi-metalsemi-metal. .

MetalloidsMetalloids• MetalloidsMetalloids have intermediate have intermediate

properties between metals and non-properties between metals and non-metals. They are semi-conductors, metals. They are semi-conductors, which makes them great for use in which makes them great for use in computer technology. There are only computer technology. There are only 7 metalloids.7 metalloids.

Periodic TrendsPeriodic Trends• As you move across a period, the As you move across a period, the

chemical & physical properties of the chemical & physical properties of the elements change in a predictable way. elements change in a predictable way. Each period repeats this change. This is Each period repeats this change. This is the the Periodic LawPeriodic Law. We can determine the . We can determine the properties of the elements based on properties of the elements based on where they are in the table. There are 3 where they are in the table. There are 3 trends to analyze. trends to analyze.

Atomic RadiusAtomic Radius• Atomic radiusAtomic radius is the size (length) of an is the size (length) of an

atom. As you go down, the radius atom. As you go down, the radius increases due to an increase in the increases due to an increase in the energy levels. As you go across, the energy levels. As you go across, the size decreases because of the increased size decreases because of the increased nuclear charge pulling on the electrons nuclear charge pulling on the electrons without adding an energy level. without adding an energy level.

Atomic RadiusAtomic Radius• The largest atoms are on the bottom The largest atoms are on the bottom

left of the periodic table, and the left of the periodic table, and the smallest atoms are on the top right. For smallest atoms are on the top right. For instance, sodium (Na) is larger than instance, sodium (Na) is larger than sulfur (S), but potassium (K) is larger sulfur (S), but potassium (K) is larger than sodium. than sodium.

Ionization EnergyIonization Energy• Ionization energyIonization energy is the amount of is the amount of

energy required to take 1 electron away energy required to take 1 electron away from an atom. The more an atom wants from an atom. The more an atom wants to keep its electrons, the larger the to keep its electrons, the larger the ionization energy will be. Ionization ionization energy will be. Ionization energy increases as you go across a energy increases as you go across a period and decreases as you go down a period and decreases as you go down a group.group.

Ionization EnergyIonization Energy• As you go across, the elements want to As you go across, the elements want to

keep their electrons more, so it is keep their electrons more, so it is harder to take an electron away. As you harder to take an electron away. As you go down, the atoms get bigger & it go down, the atoms get bigger & it becomes easier for the atom to lose 1 becomes easier for the atom to lose 1 electron because they are farther away electron because they are farther away from the nucleus. from the nucleus.

Ionization EnergyIonization Energy• Noble gases have very high ionization Noble gases have very high ionization

energies. Metals have low ionization energies. Metals have low ionization energies. Calcium (Ca) has a lower energies. Calcium (Ca) has a lower ionization energy than Bromine (Br) ionization energy than Bromine (Br) and Chlorine (Cl) has a higher and Chlorine (Cl) has a higher ionization energy than Bromine. ionization energy than Bromine.

ElectronegativityElectronegativity• ElectronegativityElectronegativity is the ability of an is the ability of an

atom to attract an electron to itself atom to attract an electron to itself during bonding. Nonmetals have high during bonding. Nonmetals have high electronegativities because they want to electronegativities because they want to gain electrons to complete their outer gain electrons to complete their outer energy levels. Metals have low energy levels. Metals have low electronegativities because they want to electronegativities because they want to lose electrons. lose electrons.

ElectronegativityElectronegativity• As you go down a group, As you go down a group,

electronegativity will decrease because electronegativity will decrease because the atoms are getting bigger and there is the atoms are getting bigger and there is less attraction from the nucleus. Across less attraction from the nucleus. Across a period, electronegativity increases – a period, electronegativity increases – the elements are smaller and become the elements are smaller and become more stable by gaining electrons. more stable by gaining electrons.

ElectronegativityElectronegativity• The most electronegative element is The most electronegative element is

Fluorine (F) (electronegativity = 4). The Fluorine (F) (electronegativity = 4). The noble gases do not have noble gases do not have electronegativities. Oxygen (O) and electronegativities. Oxygen (O) and Chlorine (Cl) are similar to Fluorine. All Chlorine (Cl) are similar to Fluorine. All the metals have a very low the metals have a very low electronegativity and will not want to electronegativity and will not want to attract electrons at all. attract electrons at all.

Question 1Question 1• Which of the following describes Which of the following describes

sodium (Na)? sodium (Na)?

Alkaline Earth Metal

Alkali Metal

Transition Metal


calcium (Ca)? calcium (Ca)?


Alkali Metal

Transition Metal

Question 3Question 3• Which of the following describes Silver Which of the following describes Silver

(Ag)? (Ag)?


Alkali Metal

Transition Metal


Oxygen (O)? Oxygen (O)?

Other Non-Metal

Halogen

Noble Gas


Fluorine (F)? Fluorine (F)?

Other Non-Metal

Halogen

Noble Gas

Question 6Question 6• Which of the following describes Argon Which of the following describes Argon

(Ar)? (Ar)?

Other Non-Metal

Halogen

Noble Gas


Hydrogen (H)? Hydrogen (H)?

Alkali Metal


Non-Metal

Question 8Question 8• Which of the following describes Silicon Which of the following describes Silicon

(Si)? (Si)?

Other Metal

Halogen

Metalloid

Question 9Question 9• Which of the following contains Which of the following contains onlyonly s- s-

block elements?block elements?

Na, Ca, Li, H

Na, Mg, B, Si

He, Sr, Cu, Al

Question 10Question 10• Which of the following contains Which of the following contains onlyonly p- p-


He, C, O, Ag

C, Ar, Si, Po

Cu, Fe, Au, Y

Question 11Question 11• Which of the following contains Which of the following contains onlyonly d- d-


He, C, O, Ag

C, Ar, Si, Po

Cu, Fe, Au, Y

Question 12Question 12• Which of the following contains Which of the following contains onlyonly

representative elements?representative elements?

He, C, O, Ag

C, Na, Si, Po

U, Kr, F, Be


Noble gases?Noble gases?

F, Cl, O, N

H, He, Br, Hg

Ar, Rn, Kr, He


halogens?halogens?

F, Cl, O, N

F, Cl, Br, I

Be, Mg, Ca, Sr


period 2 elements?period 2 elements?

Fe, Cu, Zn, Co

B, C, N, O

Be, Mg, Ca, Sr

Question 16Question 16• Mendeleev arranged the periodic table Mendeleev arranged the periodic table

according to what?according to what?

Atomic Number

Atomic Mass

Number of Electrons

Question 17Question 17• Moseley arranged the periodic table Moseley arranged the periodic table


Atomic Number

Atomic Mass

Number of Electrons

Question 18Question 18• The modern periodic table is arranged The modern periodic table is arranged


Atomic Number

Atomic Mass

Number of Electrons

Question 19Question 19• A group or family on the periodic table A group or family on the periodic table

is:is:

A Horizontal Row

A Vertical Column

A Block

Question 20Question 20• The elements in the same group or The elements in the same group or

family on the periodic table have:family on the periodic table have:

Different Properties

Similar Properties

A Constant Atomic Mass

Question 21Question 21• The elements in the same period on the The elements in the same period on the

periodic table have:periodic table have:

Different Properties

Similar Properties

A Constant Atomic Mass

Question 22Question 22• The ability of an atom to attract an The ability of an atom to attract an

electron during bonding is:electron during bonding is:

Electronegativity

Ionization Energy

Atomic Radius

Question 23Question 23• The size or length of an atom is known The size or length of an atom is known

as: as:

Electronegativity

Ionization Energy

Atomic Radius

Question 24Question 24• The amount of energy required to The amount of energy required to

remove 1 electron from an atom is: remove 1 electron from an atom is:

Electronegativity

Ionization Energy

Atomic Radius

Question 25Question 25• As you go across a period, As you go across a period,

electronegativity will: electronegativity will:

Increase

Decrease

Vary Randomly

Question 26Question 26• As you go across a period, ionization As you go across a period, ionization

energy will: energy will:

Increase

Decrease

Vary Randomly

Question 27Question 27• As you go across a period, atomic As you go across a period, atomic

radius will: radius will:

Increase

Decrease

Vary Randomly

Question 28Question 28• As you go down a group, atomic radius As you go down a group, atomic radius

will: will:

Increase

Decrease

Vary Randomly

Question 29Question 29• As you go down a group, As you go down a group,

electronegativity will: electronegativity will:

Increase

Decrease

Vary Randomly

Question 30Question 30• As you go down a group, ionization As you go down a group, ionization

energy will: energy will:

Increase

Decrease

Vary Randomly

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periodic table tutorial chapter 5.4 chapter 14 periodic table periodic table scientists &...

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alkali metals

innertransition metals

inner transition metals

alkaline earth metals

semimetals metalloids

e configurations end

d block

p sublevel