Periodic Table PropertiesMetals vs. Nonmetals

Electron Configurations Valence Electrons

Metals vs. Nonmetals

AppearanceConductivity

of heat & electricity

State of Matter Other

Metals shiny good tend to be solids

malleable (can be hammered)

ductile (can be drawn into

a wire)

Nonmetals dull poorgases,

solids, and a liquid

brittle

Metals

melting point of gallium is 85.6 ℉ antimony

sodium can be cut with a butter knife

Nonmetals

sulfur

carbon

Electron Configurations

• The PT can be divided into s,p,d,f blocks corresponding to the predictions made by quantum mechanics.

• Knowing the location of an element on the PT can easily give the electron configuration.

Blocks

Practice electron configurations: Ti: Br: Ba: S: Pb:

Practice electron configurations: Ti: [Ar]4s23d2

Br: Ba: S: Pb:

Practice electron configurations: Cu: [Ar]4s23d9

Br: [Ar]4s23d104p5 Ba: S: Pb:

Practice electron configurations: Cu: [Ar]4s23d9

Br: [Ar]4s23d104p5 Ba: [Xe]6s2 S: Pb:

Practice electron configurations: Cu: [Ar]4s23d9

Br: [Ar]4s23d104p5 Ba: [Xe]6s2 S: [Ne]3s23p4 Pb:

Practice electron configurations: Cu: [Ar]4s23d9

Br: [Ar]4s23d104p5 Ba: [Xe]6s2 S: [Ne]3s23p4 Pb: [Xe]6s24f145d106p2

Valence Electrons

• Valence electrons are responsible for an element’s chemical properties.

• Valence electrons - electrons in the outermost energy levels (highest energy levels) that are gained, lost, or shared to form chemical bonds.

Mg 1s22s22p63s2

ValenceElectrons(electrons in the highest energy level)

12

Mg 1s22s22p63s212

Valence ShellThe region of space occupied by the valence e-

Core ElectronsInterior e-

Valence Electrons• Must always be in the s and p orbitals

which means there is a maximum of 8 valence electrons for any element.

• Valence shell - the region of space occupied by the valence electrons

• Core electrons - electrons interior to the valence electrons (lower energy levels)

Determine Valence Electrons

Ti: [Ar]4s23d2

Br: [Ar]4s23d104p5 Ba: [Xe]6s2 S: [Ne]3s23p4 Pb: [Xe]6s24f145d106p2

Valence ElectronsElectron Configuration

Determine Valence Electrons

Ti: [Ar]4s23d2

Br: [Ar]4s23d104p5 Ba: [Xe]6s2 S: [Ne]3s23p4 Pb: [Xe]6s24f145d106p2

Valence ElectronsElectron Configuration

6

72

4

4

How many valence electrons do all transition metals have?

Family Valence Electrons

1A 1

2A 2

3A 3

4A 4

5A 5

6A 6

7A 7

8A 8

The 1A-8A naming system indicates the numberof valence electrons in a family!

Transition metals have 2 valence electrons from the s sublevel.

They never make it to the p sublevel of their period.

4s14s2 4p14p23d1

The energy level drops when you move to d or f blocks!

4f1

But the energy level goes back up when you move to the p block!

Dot StructuresValence e- can be represented with dots around the chemical symbol.

Think north, south, east, west. Fill in each direction before doubling up!

F CB7 valence e- 3 valence e- 4 valence e-

Practice Dot StructuresMg

S

Ar

Li

He

Mg

S

Ar

Li

He

Octet Rule• Atoms tend to gain, lose, or share

electrons to have a stable octet and have the same electron configuration as the nearest noble gas!

• Usually that equals 8 valence electrons (unless near helium then it equals 2 valence electrons).

Ionic Charge

• Metals tend to lose electrons and become positively charged to form an octet

• The charged metal is a “cation”

CationsNa+ now has same e- config

as neon! (10 e-)

Ca2+ has the same e- configas argon! (18 e-)

Ionic Charge

• Nonmetals tend to gain electrons and become negatively charged to have a stable octet

• The charged nonmetal is an “anion”

Anions

F + e- F-

S + 2e- S2-

F- now has the same e- configas neon! (10 e-)

S2- now has the same e- configas argon! (18 e-)

fluorine fluorine anion

sulfur sulfur anion

Ionic Charge TrendFamily Ionic Charge Trend

alkali metals +1

alkaline earth metals +2

boron family +3

carbon family (nonmetals) -4

nitrogen family (nonmetals) -3

oxygen family (nonmetals) -2

halogens -1

noble gases no charge