Bonding Review

Write the formula for sodium oxide.

Na2O

State the name for FePO4.

Iron (III) phosphate

Identify the bonding type in each of the following as ionic, covalent or metallic: magnesium and chlorine;

ionic

carbon and oxygen;

covalent

tin and copper;

metallic

silver

metallic

What is the charge on each ion of the following: SnI2;

Sn = +2 I = -1

What is the charge on each ion of the following: NiCO3;

Ni = +2 CO3 = -2

Al2O3;

Al = +3 O = -2

AuBr3

Au = +3 Br = -1

Explain why metals conduct electricity.

The delocalized electrons can travel past all the cations and carry the electric current from one end of the metal to the other end.

State the shapes of each of the substances and identify whether each substance is polar or non-polar. State the intermolecular force for each.  HI

Linear Polar Dipole -dipole

N2

Linear Non-polar London dispersion forces

CH3Cl

Tetrahedral Polar Dipole-dipole

CO2

Linear Non-polar London dispersion forces

H2S

Bent Polar Dipole-dipole

PH3

Trigonal pyramid Polar Dipole-dipole

HCN

Linear Polar Dipole-dipole

Identify the strongest type of intermolecular force for each of the following: HCl;

Dipole-dipole

Identify the strongest type of intermolecular force for each of the following:NH3

Hydrogen bonding

Identify the strongest type of intermolecular force for each of the following: CHCl3

Dipole-dipole

Identify the strongest type of intermolecular force for each of the following: OCl2

Dipole-dipole

Identify the strongest type of intermolecular force for each of the following: SiH4

London dispersion forces

Identify the strongest type of intermolecular force for each of the following: N2

London dispersion forces

Identify the strongest type of intermolecular force for each of the following:NBr3

Dipole-dipole

This is the end of the review for the test on Tuesday 12/13/16.

List the following bonds in order from weakest to strongest: I. permanent dipole-dipole bonds between SO2 molecules II. covalent bonds between carbon and hydrogen in CH4 III. London dispersion forces between atoms of helium IV. Permanent hydrogen bonds between HF molecules V. Covalent bonds between nitrogen atoms in N2 molecules VI. London dispersion forces between molecules of carbon dioxide

III, VI, I, IV, II, V

Identify which molecule in the pair has the higher boiling point and explain: HF and HBr

HF – has hydrogen bonding

Identify which molecule in the pair has the higher boiling point and explain: NH3 and AsH3

NH3 because of hydrogen bonding

Identify which molecule in the pair has the higher boiling point and explain: CH4 and CH3Cl

CH3Cl because of dipole-dipole instead of only London dispersion forces