Exam 3 SI Review
1) Indicate whether the following bonds are polar or non-polar. If the bond is polar, show
the polarity of the bond with an arrow (
) and indicate + and – on the atoms.
F-F
H-Br
N-O
S-O
2) What is a dipole moment and what unit is it measured in?
3) Draw the 3-D structure of each of the following molecules and state show the dipole moment using
CH4
CH3Cl
PF3
NOCl
CSO
4) What is the difference between an intramolecular force and an intermolecular force?
5) True or False. A higher molecular dipole means a higher boiling point.
6) Convert:
a) 16.78 g Cu to moles Cu and Cu atoms
b) Convert 12.98 g hydrogen gas to moles hydrogen gas, molecules hydrogen gas and hydrogen
atoms
c) Convert 5.790 x 1026 chlorine atoms to chlorine molecules, to moles chlorine gas and grams
chlorine
7) Complete and balance the following chemical equation and determine phases
Na2CO3 +
MgCl2
→
a) How many moles of precipitate will be produced if 25.67 g sodium carbonate is combined
with excess magnesium chloride?
b) How many grams of precipitate?
8) Balance and state the reaction type for the following reactions:
a)
CaO (s) +
b)
C3H8 (g)+ O2 (g) →
c)
Ba(OH)2 (aq) + CuBr2 (aq) →
d)
Li (s)+
H2O (l)
→
Ca(OH)2
CO2 (g) + H2O (g)
BaBr2 (aq) +
CoF2 (aq) →
LiF (aq) +
O2(g) →
SO3(g)
e)
SO2 (g) +
f)
KClO3 (s) →
KCl (s) +
O2 (g)
Co (s)
Cu(OH)2 (s)
9) 42.35 g silver acetate was reacted with 34.67 g of Tin (III) Chloride in the following reaction:
a) Complete and balance the following double displacement reaction (include phases):
AgC2H3O2 (aq) +
SnCl3 (aq)
→
b) Write the ionic equation showing charges and phases:
c) Write the net ionic equation showing charges and phases:
d) What were the spectator ions in this chemical reaction?
e) What is the limiting reactant?
f) What is the theoretical yield of this reaction?
g) What is the percent yield if 16.04 g of precipitate is recovered following this
reaction?
h) How much excess reactant remains following this reaction?
10) What is the mass percent composition of chlorine in MgCl2?
11) Ethylene glycol, used for antifreeze, has the molecular formula C2H6O. Calculate the mass
percent of each element in ethylene glycol.
12) What is the empirical formula of the compound that is 43.2% by mass K, 39.1% by mass Cl,
and also contains oxygen.
13) Determine the oxidation state of each element in each of the following compounds and
molecules
a) F2
b) PO43-
c) Cr2O72-
d) Mg2+
e) NH3
g) KCl
h) P2O5
i) Na2O
j) SO2
k) NaH
f) SnBr4
14) Is the following reaction a redox reaction?
4 Fe (s) + 3 O2 (g) → 2 Fe2O3 (s)
15) Which reactions are redox reactions? (Circle all that apply)
Precipitation
16)
Combustion
Corrosion
Acid/Base Rxns
Combination/decomposition
a) Determine the oxidation states of the elements of the following redox reaction.
CH4 + O2 →
CO2
b) What is being oxidized? What is being reduced?
c) What is the oxidizing agent? The reducing agent?
+ H2O