Ionic Bonds

Non-metal elements have a strong hold on their electrons as a result of having a high electron affinity. Instead, they easily gain electrons.

Metal elements have a weak hold on electrons and so are easily able to lose them.

Draw the Bohr model for the following:

Natural: Na Cl State

Stable: Na Cl State

Ionic Bonds form between molecules with opposite charges (cations and anions). Electrostatic attraction between positive/negative atoms holds ionic molecules together.

Made up of metal and non-metal atoms. The atoms DO NOT share electrons. Total charge is always 0.

Electrostatic forces are strong, which gives ionic compounds a high melting temperature. Many form a crystalline structure, with hard/straight breaks.

Practice

Identify the charge the following atoms would need to be stable:– Na– S– Br– Sr

If you were to combine Sodium and Bromine, what would be the resulting compound?

Swap & Drop Method for Ionic BondingAn atom’s oxidation state is an atom’s charge when it is a stable ion.

Identify the oxidation state for the following

– H–Mg– B– Al– O– Ne

Swap & Drop Method for Ionic Bonding

Identify the oxidation state for each atom.

Ca Cl Mg O

Al Cl Al O

Naming Ionic Compounds

Generally, the name for compounds can be obtained by using the following convention:

Name = [Metal] + [Non-Metal] + ide

What would the name for NaCl?

What would the compound for Calcium Bromide be?

Naming Ionic Compounds

Some metals are able to form multiple ions.

For example, copper can form Cu+ or Cu+2.

You must say which one in naming:– Using Cu+1 :Cu2O

Copper (I) Oxide– Using Cu+2 :CuO

Copper(II)Oxide

Question• Manganese (Mn) can form the ions

+2, +3, +4, +6, and +7.

• Determine the formula & name for:– Oxygen molecules and Mn+3 and Mn+7

Identify and name the resulting ionic compound

• Na + F Al + O

• Al + Cl Mg + Cl

• Cu+ + O

• Cu2+ + O

• Fe+3 + S