Objectives19-1 Distinguish periods and rows on the periodic

table.19-2 Identify an element as a metal, nonmetal or

metalloid.19-3 Identify the valence electrons for elements in

groups 1-2, 13-18.19-4 Create electron dot structures for elements in

groups 1-2, 13-18.19-5 Identify an element’s properties based on the

group it belongs to.19-6 Compare and contrast elements based on their

placement on the table.

• Atomic Number• Symbol• Name• Average Atomic

Mass

You Know This!!!!1

HHydrogen

1.008

Periods• DEF: Horizontal rows

–Elements gain one proton and one electron as you go from left to right across the periods.

–Change properties• Numbered 1-7

Groups• DEF: Vertical columns

–AKA: Families• Numbered 1 through 18.• Elements in each group have

similar properties

• Same valence electrons–DEF: electrons in outermost

energy level used for bonding

Group number1 2 13 14 15 16 17 18

1 2 3 4 5 6 7 8Valence electrons

• Groups 3-12 and the 2 pull out sections–No set pattern–Varies even within the group

Electron or Lewis Dot Structures• DEF: uses symbols and dots to

show valence electrons• Used to show how elements will

bond–Will they gain or lose electrons

Pattern to use

X 1

2

3

4

56

7

8

Group 1

Group 2

Group 13

Group 14

Li Mg B C

Group 15

Group 16

Group 17

Group 18

As S F Ne

Bonding with Lewis Structures• Middle atom is usually atom

with the most open spots• Octet Rule

–DEF: Elements want 8 VE–Bonding accomplishes this

Periodic Table Groups

Metals• State of matter at room temperature

–All but one are solid• Valence electrons

–Easily lose • Group Numbers

–1, 2, 3-12, pull outs and parts of 13, 14 and 15

Characteristics• Good conductors of heat and

electricity• High densities• High melting points• Luster• Malleable• Ductile

Nonmetals• State of matter at room temperature

–Gases, liquids or brittle solids• Valence electrons

–Most gain • Group Numbers

–All of 18, parts of 14, 15, 16, 17–Plus Hydrogen

Characteristics• Are not shiny, do not conduct.• Low densities• Low melting points

Metalloids• State of matter at room temperature

– All solids• Valence electrons

– Varies• Group Numbers

– Follows the stair steps

Characteristics• Conduct better than nonmetals,

but not as good as metals.–AKA: semiconductors.

• They contain properties of both metals and nonmetals.

• Group 1 – Alkali metals __VE–Most reactive of metals–Exists as compounds, not

elements–Lower metallic densities–Used in batteries, drugs,

fertilizers

• Group 2 – Alkaline Earth Metals __ VE–Don’t occur free in nature–Mg only used on a large scale

•Used in fireworks and building materials

–Ca VERY important to bones

• Groups 3-12 – Transition metals–VE varies–Exists as elements in nature–High MP, BP and densities–VERY conductive–Uses: wires, pipes, cast iron,

coloring glass and paint•Cu, Fe, Cr, Co, Cd

Inner Transition Elements• Lanthanides

–Atomic #’s 57 – 71–Rare earth metals–Uses: lamps, lasers, magnets,

motion picture projectors, and X-ray intensifying screens.

AKA: Synthetic Elements

Inner Transition Elements• Actinides

–Atomic #’s 89 – 103–Actinides do not occur in nature–Radioactive–Tarnish readily–Very dense

AKA: Synthetic Elements

Elements 93 & above found only in laboratories.

• Group17 – Halogens ___ VE–Most reactive of the nonmetals!

•Same reactivity value as Alkali metals

–Many uses•Toothpaste, disinfectant, glass etching

–Form salts

• Group18 – Noble Gases __ VE–Do not readily bond at all–No naturally occurring

compounds exist.–Colored signs, light bulbs,

windows, balloons

Mixed Groups• Group 13

–Boron Group ____ VE• Group 14

–Carbon Group ____VE• Group 15

–Nitrogen Group ____VE• Group 16

–Oxygen Group ____VE