Module 2 - Bonding practice Page 1 of 5

1) Use the ion puzzle to find formulas for the following:

Fluoride F1-

Oxide O2-

Nitride N3-

Carbide C4-

Potassium K1+

Calcium Ca2+

Aluminum Al3+

Germanium Ge4+

2) Show the electron transfer and write the formula unit for the following sets of ions:

Lithium and Sulfur Aluminum and Oxygen

Magnesium and Phosphorus Calcium and Nitrogen

Barium and Oxygen Aluminum and Arsenic

3) Which pair of atoms would not form an ionic compound, and why?1

a) Magnesium & Florine or Calcium & Barium

b) Oxygen & Sulfur or Calcium & Oxygen

1 Adapted from Science Perspectives (Nelson) p.195

Module 2 - Bonding practice Page 2 of 5

4) Element M has 2 valence electrons. Element X has 5 valence electrons.2

a) What charge will M take on? b) Is M a metal or non-metal? Why? c) What charge will X take on?

d) Is X a metal or non-metal? Why? e) What is the formula of the compound formed from M and X?

5) Write formulas for the following ionc compounds:

Potassium chloride Osmium silicide Calcium nitride Zirconium chloride

Cerium phosphide Hafnium arsenide Yttrium telluride Thorium oxide

Indium carbide Scandium fluoride Beryllium bromide Tungsten telluride

Rubidium carbide Strontium silicide Sodium sulfide Lithium nitride

Magnesium selenide Molybdenum arsenide Tungsten carbide Cesium chloride

2 Adapted from Science Perspectives (Nelson) p.195

Module 2 - Bonding practice Page 3 of 5

6) Determine the formula for the following compounds containing polyatomic ions:

Zirconium sulfate Zirconium sulfide Zirconium sulfite Calcium nitride

Barium nitrate Tungsten arsenite Tungsten arsenate Tungsten arsenide

Magnesium nitrate Ammonium carbonate Hydrogen peroxide Ammonium carbide (carbide = C4-)

7) Determine the name for the following compounds containing polyatomic ions:

Th(SO3)2 Th(SO4)2

ThS2 Ba(ClO3)2

Ba(ClO2)2 BaCl2

Zn(BrO3)2 ZnBr2

Zn3(BO3)2 Sc2(CO3)3

8) Write the formula for the following ionic compounds:

Lead (IV) sulfate Scandium phosphate Ammonium chloride Tin (II) nitrate

Ammonium sulfate Cobalt (III) oxide Calcium hydroxide Molybdenum oxide

Ammonium chlorate Lithium oxide Cobalt (II) oxide Ammonium sulfide

Module 2 - Bonding practice Page 4 of 5

9) Name the following compounds containing multivalent metals:

Pb(SO3)2 Co(NO3)2 UO3

Cu3N2 FePO4 MnS2

10) Draw Lewis Diagrams for the following molecules:3

H2S H2

HCN CHCl3

PBr3 N2H2

C2H2 SO3

11) Determine the formula for the following covalent compounds:

Dinitrogen pentoxide Boron trichloride Dioxygen difluoride

Tetraphosphorus trisulfide Silicon carbide Bromine

12) Determine the name of the following compounds:

SeI2 H2O2 NI3

P2I5 SF6 I2

3 Adapted from http://misterguch.brinkster.net/PRA017.pdf

Module 2 - Bonding practice Page 5 of 5

13) Determine if the compound is ionic or covalent, and then name the compound:

Compound Ionic / Covalent Name

CaS Ionic / Covalent

SO2 Ionic / Covalent

(NH4)I Ionic / Covalent

NH4OH Ionic / Covalent

P2O5 Ionic / Covalent

FeO Ionic / Covalent

N2 Ionic / Covalent

NO Ionic / Covalent

Ca(OH)2 Ionic / Covalent

CCl4 Ionic / Covalent

Ti(SO4)2 Ionic / Covalent

14) Determine if the compound is ionic or covalent, and then determine the formula for the compound:

Compound Ionic / Covalent Formula

Ammonium iodide Ionic / Covalent

Platinum (IV) sulfate Ionic / Covalent

Lithium peroxide Ionic / Covalent

Ammonium sulfide Ionic / Covalent

Iron (II) selenide Ionic / Covalent

Ammonium hydroxide Ionic / Covalent

Ruthenium (III) chlorite Ionic / Covalent

Calcium nitrate Ionic / Covalent

Silicon monoxide Ionic / Covalent

Nitrogen dioxide Ionic / Covalent

Diphosphorus monosulfide Ionic / Covalent

Diarsenic trioxide Ionic / Covalent