Ionic bonds

1

3

5

7

Yes

No, too many electrons

No, not enough electrons

No, dots are in wrong places

$$N^{+3}\ \longrightarrow N^{-3}\ +\ 3\ e$$

$$N\ +3e\ \longrightarrow N^{-3}$$

$$N\ +\ 2\ e\ \longrightarrow N^{-2}\$$

$$N^{+3}\ \ +\ 3\ e\longrightarrow N^{-3}\$$

High melting points

Ability to lose valence electrons easily

Ability to gain electrons easily

Low density

Lanthanoids

Actinoids

s- block elements

d-block elements

noble gas configurations

pseudo-noble gas configurations

octet configurations

stable gas configurations

Group 15

Group 16

Group 17

Group 14

Dialuminum oxide

Aluminum oxygen

Oxygen Aluminide

Aluminum oxide

Each outer shell electron in Cl is represented by a cross.

In Na, the total charge is -2.

Na+ and Cl- are held together by electrostatic attraction.

Na+ has a full outer shell of electrons.

Their ions are free to move.

Their ions are held in fixed positions.

They have many strong bonds which require a large amount of heat energy to overcome these strong bonds.

They have weak bonds which require a little amount of heat energy to overcome these weak bonds.

Cl cation

Cl anion

Na cation

Na anion

Crystal

Crystal System

Crystal Lattice

Cube

Smaller ionic radius leads to greater lattice energy

Larger ionic radius leads to greater lattice energy

Ionic radius has no effect on lattice energy

Lattice energy is only affected by charge