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