CHEM 130
PROBLEM SET Ch.2
Key begins on page 5.
1. Rubidium has two naturally occuring isotopes of mass 85.0 and 87.0 amu. What percent of Rubidium-85 is
normally present given that its reported atomic mass is 85.47 amu?
______________
2. Balance the following equations.
a) ____UO2 + ____HF -----> ____UF4 + ____H2O
b) ____H3BO3 ---------> ____B2O3 + ____ H2O
c) ____B2O3 + ____HF -------> ____BF3 + ____H2O
d) ____C2H3Cl + ____O2 ------> ____CO2 + ____H2O + ____HCl
e) ____PH3 + ____O2 -------> ____P4O10 + ____H2O
3. Indicate whether the following compounds are ionic or covalent.
a) CCl4 _______________________
c) NaF ________________________
_______________________
d) PF3 ________________________
b) CO2
4. Give names for the following ionic compounds.
a) Na2CO3 ____________________
b) AlP
____________________
c) Ba(ClO3)2 ______________________
d) Cu2CrO4
______________________
5. Give formulas for each of the following ionic compounds.
a) zinc sulfate _________________ c) aluminum phosphate ______________
b) silver nitrate ________________ d) magnesium nitride ______________
6. Give names for the following covalent compounds.
a) PCl3 ____________________
c) CS2 ___________________________
b) SO2 ____________________
d) N2O5 ___________________________
7. Give formulas for the following covalent compounds.
a) nitrogen triiodide ____________ c) phosphorus trifluoride __________
b) oxygen difluoride ____________ d) diphosphorus tetroxide __________
8. Indicate the "pet" name associated with each of the following.
a) Mg
____________________
c) K _______________________
b) Ar
____________________
d) Cl _______________________
9. Briefly distinguish between homogeneous and heterogeneous mixtures.
10. Briefly distinguish between periods and groups on the periodic table.
11. Briefly describe the difference betwween anions and cations.
Naming Ionic and Covalent Compounds
Give the names of the following ionic compounds
Write the formulas for the following ionic compounds
Al(NO3)3
calcium hydroxide
HgI2
magnesium nitride
Fe2(CrO4)3
copper(I) cyanide
NH4NO2
silver nitrate
Li2CO3
potassium bromide
SrO
lead(IV) bromide
Ba(OH)2
tin(II) sulfide
Mg3P2
potassium phosphate
CoF3
mercury(I) iodide
Ca(C2H3O2)2
ammonium hydroxide
PbCl4
potassium dichromate
Cu2S
lead(II) carbonate
KMnO4
barium sulfite
Na2HPO4
lithium phosphide
Give the name the following covalent compounds
Write the formula for the following covalent
compounds
SeBr4
carbon monoxide
F2O2
nitrogen triiodide
IBr2
tetraphosphorus decasulfide
OF2
disulfur dichloride
N2S5
dichlorine heptoxide
Br3O8
diphosphorus tetraoxide
CS2
dinitrogen monoxide
S4N4
selenium hexafluoride
Valences of Some Common Ions
Cations
(positive charge)
Anions
+1
H+
Li +
Na +
K+
Ag +
Cu +
NH4 +
hydrogen
lithium
sodium
potassium
silver
copper(I)
ammonium
–1
H3O + hydronium
Hg + mercury(I)
H–
F–
Cl –
Br –
I–
OH –
NO2 –
NO3 –
CN –
hydride
fluoride
chloride
bromide
iodide
hydroxide
nitrite
nitrate
cyanide
+2
Mg 2+
Ca 2+
Sr 2+
Ba 2+
Zn 2+
Cu 2+
Fe 2+
Hg 2+
magnesium
calcium
strontium
barium
zinc
copper(II)
iron(II)
mercury(II)
Cr 2+
Co 2+
Mn 2+
Cd 2+
Sn 2+
Pb 2+
Ni 2+
aluminum
iron(III)
Cr 3+
Co 3+
+4
Sn 4+
Pb 4+
tin(IV)
lead(IV)
MnO4 –
ClO –
ClO2 –
ClO3 –
ClO4 –
HCO3 –
C2H3O2 –
HSO3 –
HSO4 –
H2PO4 –
permanganate
hypochlorite
chlorite
chlorate
perchlorate
hydrogen carbonate
acetate
hydrogen sulfite
hydrogen sulfate
dihydrogen phosphate
–2
chromium(II)
cobalt(II)
magnanese(II)
cadmium
tin(II)
lead(II)
nickel(II)
O 2–
S 2–
CO3 2–
SO3 2–
SO4 2–
CrO4 2–
Cr2O7 2–
oxide
sulfide
carbonate
sulfite
sulfate
chromate
dichromate
+3
Al 3+
Fe 3+
(negative charge)
C2O4 2–
S2O3 2–
HPO4 2–
O22–
oxalate
thiosulfate
monohydrogen phosphate
peroxide
–3
chromium(III) N 3–
cobalt(III)
P 3–
nitride
phosphide
PO4 3–
phosphate