Bellringer1. Draw a model for the following elements:

A. SodiumB. Chlorine

2. How many valence electrons does sodium have?

3. If sodium lost its valence electrons, what would its charge be?

4. How many valence electrons does chlorine have?

5. If chlorine gained an electron, what would its charge be?

Sodium

P: 11N: 12

XX

X XX

X X

XXXX

Chlorine

P: 17N: 18

X

XX X

X

X X

XXXX

X

X X

XX

X

2. One3. +1

1 A. 1 B.

4. Seven5. -1

I. Bonding Atoms

A. Atoms bond because their valence electrons interact

1. Bonding occurs so that atoms will have stable outer energy levels

a. What is a stable outer energy level? How many electrons?

i. 1st Energy level: 2e-

ii. 2nd, 3rd, 4th, etc…Energy level: 8e-

Example: Hydrogen

Valence electrons: 1Energy levels: 1

X X

The valence electron in each hydrogen is shared, giving each atom

a stable outer energy level.

II. Ionic Bonds

A. Ionic Bonds – Formed between oppositely charged ions

1. Metals form positive ions

2. Nonmetals form negative ions

B. When one atom loses an electron, another atom gains that same electron

1. Salt is formed from positively charged sodium ions and negatively charged chlorine ions

Example:

Na - [Na]+

Cl + [ Cl ]-

Sodium Ion (positive)

Chloride Ion (negative)

C. The chemical formula, NaCl, tells the ratio of sodium to chloride ions

D. Characteristics of ionic compounds:

1. Conduct electricity when dissolved

2. Metallic bonds – the attraction between a nucleus of one atom and the electrons from another atom

i. Causes atoms to pack close to each other

III. Covalent Bonds

A. Covalent Bond – Molecules, made when electrons are shared between atoms

Example: ChlorineSeven Valence Electrons

XXXXX

X

XX X

X XXX

X XX X

XXXXX

X

XXX

X XX X

X XX X

Cl ClThe line indicates shared electrons

1. Elements can form double or triple bonds

O O N Na. The compounds above share electrons

equally, so they form nonpolar covalent bonds

2. Not all covalent bonds are nonpolar

a. Water is a polar covalent molecule

Groups of covalently bonded atoms that have either gained or lost electrons

A. Polyatomic Ions –

IV. Polyatomic Ions

NH4+ ammonium

PO33- phosphite

NO2- nitrite

NO3- nitrate

OH- hydroxide

Polyatomic Ion Examples:

B. A polyatomic ion that is bonded with another atom is often indicated with parentheses

(NH4)2SO4

1. But not always

NH4NO3

Ammonium sulfate

Ammonium nitrate

C. Polyatomic ions usually end in -ate or -ite

1. -ate indicates one additional oxygen atom than the polyatomic ion with -ite

ClO3- chlorate

ClO2- chlorite

____ 1. SO42- A. sulfite

B. sulfate

____ 4. AsO33-

_____ 3. AsO43- C. arsenate

D. arsenite

Quiz: Match the polyatomic ion with its name

____ 2. SO32-A

D

C

B