Molecular and Ionic Bonding

Covalent bond

Ionic bond

Metallic bond

Hydrogen bond

Volatility

Electrical conductivity in the solid state

Melting point

Solubility in nonpolar solvents

NaCl

H₂O

Cl₂O

NaH

The point at which atoms repel each other strongly.

The optimal distance for bond formation with the lowest potential energy.

The point at which atoms are too far apart to interact.

The highest potential energy of the system.

Increases bond strength and decreases melting point.

Decreases bond strength and increases melting point.

Increases both bond strength and melting point.

Decreases both bond strength and melting point.

Increasing the ionic radii and decreasing the charge of the ions.

Decreasing the ionic radii and decreasing the charge of the ions.

Increasing the ionic radii and increasing the charge of the ions.

Decreasing the ionic radii and increasing the charge of the ions.

$NaCl$

$MgO$

They would be approximately the same.

Cannot be determined without knowing the exact ionic radii.

Ionic Alloy

Substitutional Alloy

Interstitial Alloy

Covalent Alloy

Interstitial alloys are generally more ductile and less hard than pure metals.

Interstitial alloys are generally more conductive and less strong than pure metals.

Interstitial alloys are generally more malleable and less dense than pure metals.

Interstitial alloys are generally harder and less ductile than pure metals.

H-O-H (no lone pairs)

H-O-H (one lone pair on O)

H-O-H (two lone pairs on O)

H-O-H (three lone pairs on O)