Periodic Table Unit IV. I History A. Mendeleev Arranged elements by their masses Arranged elements by their masses B. Moseley Arranged elements by their.

Periodic TableUnit IV

I H

isto

ry

A.Mendeleev• Arranged elements by

their massesB.Moseley• Arranged elements by

their atomic number• Modern periodic table

II A

rrangem

ent

of

the P

eri

odic

Ta

ble

A.Groups• Columns on the table• Contain the same

number of valence electronsB.Periods• Rows on the table

• Use the same energy

levels

Groups

Peri

od

s

III Types of Elements

A. M

eta

ls

1. Locationa) Lower left side of the table

2. Propertiesa) Metals are malleable and

ductileb) Metals are solids at room

temperature except mercury

c) Metals have lusterd) Metals are good conductors

e) Metals have low ionization

energy and low electronegativity

f) Metals lose electrons and

form positive ions

B. N

onm

eta

ls

1. Locationa) Upper right side of the table

2. Propertiesa) Nonmetals are brittle

b) Nonmetals are gases or

molecular solids at room

temperature except bromine

which is a liquidc) Nonmetals are dulld) Nonmetals are insulators

e) Nonmetals have high ionization

energy and high electronegativity

f) Nonmetals gain electrons and

form negative ions

C. Tr

ansi

tion

Meta

ls

1.Locationa)Groups 3 through 12

2. Propertiesa)Series of elements that

fill the d-sublevelb)Transition metals have

multiple oxidation statesc)Transition metals form

colored ions

D. M

eta

lloid

s

1. Locationa) On the “stairs” plus Ge and Sb

2. Propertiesa) Metalloids are brittleb) Metalloids are solid at room

temperaturec) Metalloids have luster

d) Metalloids are semi-conductorse) Metalloids have middle

ionization energy and

electronegativity values

f) Metalloids gain or lose

electrons

E. N

oble

Gase

s

1.Locationa)Noble Gases are in Group 182. Propertiesa)Noble gases are inert

which means they do

not reactb)Noble gases are monatomicc)Noble gases have filled

outer energy levels

IV P

ropert

ies

of

Ele

ments

Ionization Energy (IE)• Amount of energy to remove an

electronAtomic Radius• ½ distance between two nuclei

Ionic Radius• Metals decrease in size

• Nonmetals increase in size

Electronegativity (EN)• Attraction for electrons

Reactivity• Metal activity increases as you go left

and down• Nonmetallic activity increases as you go

up and to the right

V G

roups

HydrogenAlkali Metals• Group 1• Explosive in waterAlkaline Earth Metals• Group 2Halogens• Group 17• All nonmetals• All phases of matter

• F2 and Cl2 (gas) Br

2 (liquid) I2 (solid)

Noble Gases• Group 18• Do not react except the largest

members

VI Tre

nds

As you go

down a group

• Atomic number

increases

• Mass increases

• Valence electrons

remain the same

• Energy levels

increase

• Metallic character

increases

• Nonmetallic

character decreases

• Radius increases

• IE and EN decrease

As you go

across a period

• Atomic number

increases

• Mass increases

• Valence electrons

increase

• Energy level is

constant

• Metallic character

decreases

• Nonmetallic

character increases

• Radius decreases

• IE and EN increase

Notable

Observations

s-electrons

d-electronss

p-electrons

f-ele

ctr

on

s

METAL SIDE

NONMETAL SIDE

Metalloids

s-electrons

2s

3s

4s

5s

6s

7s

2p

3p

4p

5p

6p

7p

p-electrons

d-electrons

4d

6d

5d

3d

f-electrons

4f

5f