Chemical Bonding and Structure

$MgO$ is lower because ions are smaller

$MgO$ is higher because the ions have higher charges

$NaF$ is higher because fluorine is more electronegative

$NaF$ is lower because it is a liquid at room temperature

$SO_4^{2-}$

$SO_3^{2-}$

$S^{2-}$

$HSO_4^-$

Nitrogen

Oxygen

Aluminum

Carbon

$NaCl$

$MgBr_2$

$SiO_2$

$K_2O$

1

1.5

2

3

It is formed by the sideways overlap of p orbitals.

It is formed by the head-on overlap of orbitals along the internuclear axis.

It is weaker than a pi bond.

It can only be formed between two s orbitals.

Dipole-dipole interaction

London dispersion forces

Hydrogen bonding

Covalent bonding

$CF_{4}$

$CCl_{4}$

$CBr_{4}$

$CI_{4}$

London dispersion forces

Dipole-dipole forces

Hydrogen bonding

Ionic bonding

Ionic lattice

Molecular lattice

Giant covalent lattice

Metallic lattice

They are lower than their melting points

They are very low compared to non-metals

They are generally high due to strong metallic bonds

They increase as the metallic bond gets weaker

Larger cations lead to higher melting points

Smaller cations lead to higher melting points

Cation size has no effect on melting point

Smaller cations lead to lower melting points

$sp^3$

$sp^3d$

$sp^3d^2$

$sp^2$

Hexagonal

Octahedral

Trigonal bipyramidal

Square pyramidal

90°

107°

109.5°

120°

$sp$

$sp^2$

$sp^3$

$sp^3d$

Four orbitals arranged at $120^\circ$ to each other

Four orbitals arranged at $109.5^\circ$ to each other

Three orbitals arranged at $120^\circ$ to each other

Two orbitals arranged at $180^\circ$ to each other

$sp$

$sp^2$

$sp^3$

$sp^2d$