1
Unit #2 (Chapters 5,6,7,8,16)
1.
2.
3.
NAME
Write names for the ions
a.
HCO3-1
bicarbonate or hydrogen carbonate
b.
CrO4-2
chromate
c.
Sn+4
tin (IV)
d.
S-2
sulfide
For the following pairs of ions, predict the formula of the compound that the ions will form and
give its name?
a)
ions
Pb+4, Cr2O7-2
b)
PO4 , K
-3
+1
formula
Pb(Cr2O7)2
name of compound
lead (IV) dichromate
K3PO4
potassium phosphate
Identify the following electrolytes as an acid, base, salt or identify as nonelectrolyte
a) HI (aq)
acid
b) CoCl3 (aq)
salt
c) PbCl2 (s)
nonelectrolyte salt
d) NaOH (aq)
base
4.
What net charge will all molecules and ionic compounds have?
5.
Write the names for each of the following compounds:
Ca(NO3)2
calcium nitrate
(NH4)2SO3
ammonium sulfite
FeBr3
iron (III) bromide
N2O3
dinitrogen trioxide
HClO3 (aq)
chloric acid
H2O
water
C8H18
octane
zero
2
6.
7.
Write the formula for each of the following compounds:
sulfur hexafluoride
SF6
sulfurous acid
H2SO3
nickel (III) carbonate
Ni2(CO3)3
zinc hydroxide
Zn(OH)2
hydrobromic acid
HBr (aq)
magnesium oxide
MgO
nickel (II) acetate
Ni(C2H3O2)2
Determine the charge (oxidation number) of the indicated species:
Fe
=
+3
in Fe2O3
Cu =
+2
V
=
+5
in VCl5
Au = +1
in CuCl2
in AuNO3
Solubility Rules for ionic compounds: (fill in the blanks)
Compounds containing the following ions are generally soluble in water:
Write out the solubility Rules for Soluble ionic compounds and there exceptions
1.
Group 1A (Li+1, Na+1, K+1) and NH4+1 cations
2.
Nitrates (NO3-1) anion or acetates (C2H3O2-1) anion
3.
Most halide ions Cl-1 , Br-1 , I-1 are soluble (except Ag+1, Pb+2, and Hg2+2 are
insoluble)
Most SO4-2 anions are soluble (CaSO4, SrSO4, BaSO4, Ag2SO4, Hg2SO4, and PbSO4
are insoluble)
4.
Compounds containing the following ions are generally insoluble in water:
8.
5.
Most CO3-2 are insoluble (see rule 1 exceptions, which are soluble)
6.
Most CrO4-2 are insoluble (see rule 1 exceptions, which are soluble)
7.
Most PO4-3 are insoluble (see rule 1 exceptions, which are soluble).
8.
Most S-2 are insoluble (CaS, SrS, BaS, and rule 1 exceptions are soluble)
9.
Most hydroxides are insoluble (except for NH4OH and the strong bases which are in group 1A (LiOH,
NaOH, KOH, RbOH, CsOH, FrOH) and in group IIA (Ca(OH) 2, Sr(OH)2, Ba(OH)2, Ra(OH)2)
List information that can be obtained from a balanced chemical equation?
Identity of reactants, products, phases, relative stoichiometric amounts, above the arrow
you may see reaction conditions or catalyst.
3
9.
Zn(NO3)2 (aq) will react with Al (s) but no reaction with Fe (s).
Ni(NO3)2 (aq) will react with Fe (s)
a)
Write the four metals in order of decreasing activity, (highest activity first).
Highest Al < Zn < Fe < Ni Lowest
b)
Write the balanced equation for the reaction, for Ni(NO3)2 (aq) and
Al (s), if no reaction write NR.
2 Al (s) + 3 Ni(NO3)2 (aq) 3 Ni (s) + 2 Al(NO3)3 (aq)
10.
Balance, identify driving force, and classify and in as many ways possible the following
reactions.
Possible classifications:
(R) redox or oxidation-reduction
(Syn)synthesis or combination
(P) precipitation
a)
2 Al(HCO3)3 (s) 
(SR) single replacement
(D) decomposition
(C) combustion
(D-D)double displacement
(N) neutralization (acid- base)
Al2(CO3)3 (s) + 3 CO2 (g)+
Driving force(s)formation of gas and liquid Classifications:
b)
2 HCl (aq) + Mg (s)

MgCl2 (aq)
Driving force(s)transfer of electrons, form gas Classifications:
c)
2 N2 (g) +
3 O2 (g)

2 Bi(NO3)3 (aq)
+ 3 K2S (aq)
Driving force(s) formation of solid
e)
D, G
+
SR, R, G

Bi2S3 (s) +
Classifications:
Ba(OH)2 (aq) + (NH4)2SO4(aq) 
2 NH3 (g) +
Syn, R, G
6 KNO3 (aq)
DD, P
BaSO4(s)
Driving force(s)formation of gas, solid, and water Classifications:
f)
H2 (g)
2 N2O3 (g)
Driving force(s) transfer of electrons, form gas Classifications:
d)
3 H2O (l)
4 C2H7N (s) + 19 O2 (g) 4 NO2 (g) + 14 H2O (l)
+ 2 H2O (l)
DD, G, P
+ 8 CO2 (g)
Driving force(s)transfer electrons, form gas, water Classifications:
C, R, G
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11.
Complete and balance the reactions. Indicate states of matter in products and the driving force(s)
of the reaction. If there are no driving forces balance anyway and write NR for no reaction.
a & b are double displacement; c is decomposition; d is combustion.
DRIVING FORCE(S)
PRODUCTS
form gas, water
a)
2 HCl (aq) + Na2SO3 (aq)
No Reaction
b)
3 LiNO3 (aq) + Na3PO4 (aq)
Transfer e-1, form gas c)
 2 NaCl (aq) + H2O (l) + SO2 (g)
 3 Li3PO4 (aq) + 3 NaNO3 (aq)
 2 KCl (s) + 3 O2 (g)
2 KClO3 (s)
Transfer e-1, form gas, water d) 2 CH3OH (l) + 3 O2 (g)  2 CO2 (g) + 4 H2O (g)
12.
Complete and Balance the following chemical reactions.
Include the state that the substances are in, (s), (l), (g), or (aq).
Identify the driving force for each reaction, if no driving force, write No reaction, but balance it
anyway.
a)
a)
Combustion reaction, redox, G:
Driving Force(s) Transfer e-1, form gas, water
2 C8H18S (s) +
 16 CO2 (g) + 18 H2O (g) + 2 SO2 (g)
Single replacement reaction, R:
Driving Force(s)
(Mg > Cu, magnesium is more active than copper)
Solid magnesium is added to aqueous copper (II) nitrate
Cu(NO3)2 (aq)
c)
27 O2 (g)
+
Mg (s) 
Mg(NO3)2
Decomposition reaction, G: Driving Force(s)
Transfer electrons
(aq)
+Cu (s)
form gas
Co2(CO3)3 (s)  Co2O3 (s) + 3 CO2 (g)
d)
Double Displacement, N:
Driving Force(s)
form water
aqueous nitric acid is added to aqueous strontium hydroxide
2 HNO3 (aq) + Sr(OH)2 (aq)  Sr(NO3)2 (aq) + 2 H2O (l)
e)
Synthesis reaction:
NH3 (g)
Driving Force(s)form weak electrolyte
+ H2O (l)  NH4OH (aq)
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13.
A sample of lysine, one of the alpha amino acids found in protein, is found to contain 49.3%
carbon, 9.6% hydrogen, 19.3% nitrogen and 21.9% oxygen. The molecular weight of lysine is
146 g/mol. Calculate the empirical formula and the molecular formula of lysine.
Change % to grams, divide by atomic mass to get moles, divide by smallest # moles
49.3 g C  4.105 mole C  3 C
9.6 g H  9.52 mole H  7 H
19.3 g N  1.38 mole N  1 N
21.9 g O  1.37 mol O  1 O
Empirical formula C3H7NO
Empirical weight = 73.0 g/mol
=n
Molecular Formula = C6H14N2O2
= 2
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14.
a)
Calculate the molar mass of aluminum dichromate, Al2(Cr2O7)3
702.0 g/mol
b)
Determine the mass percent composition of only the O in Al2(Cr2O7)3
47.9% O
c)
Calculate the number of moles in 35.4 g of Al2(Cr2O7)3
0.0504 mol
d)
Calculate the number of formula units in 35.4 g of Al2(Cr2O7)3
3.04 x 1022 molecules
e)
Calculate the number of oxygen atoms in 35.4 g of Al2(Cr2O7)3
6.34 x 1023 atoms O
f)
24
Calculate the mass of 2.51 x 10 molecules of Al2(Cr2O7)3
2926 g  2.93 x 103 g
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15.
a) Balance the following unbalanced equation:
C3H8 (g)
+
5 O2 (g) 
3 CO2 (g)
+
4 H2O (l)
a) Calculate the theoretical mass in grams of CO2 produced from 5.00 grams C3H8 and 8.00 g
oxygen.
Limiting reactant problem
Molar masses: C3H8 = 44.09 g/mol, O2 = 32.00 g/mol, CO2 = 44.01 g/mol
5.00 g C3H8 can produce 15.0 g CO2
8.00 g O2 can produce 6.60 g CO2
The maximum CO2 is the lowest theoretical value, 6.60 g CO2
b) What is the limiting reactant in the reaction above?
O2
c) What is the % yield of the reaction above if 4.22 grams of CO2 were experimentally produced
in a lab starting with the given amounts above?
63.9% yield
16.
For the following double-displacement reaction:
a)
Complete the whole equation by including the products and balance the equation.
Include the physical states in all the equations.
K2CO3 (aq) +
b)
NiF2 (aq)

2 KF (aq) + NiCO3 (s)
Write the balanced total ionic equation for the above reaction. Include charges on ions
and states of matter.
2 K+1(aq) + CO3-2 (aq) + Ni+2(aq) + 2F-1 (aq)  2 K+1(aq) + 2F-1 (aq) + NiCO3 (s)
c) Circle the spectator ions in part b?
d) Write the balanced net ionic equation for this reaction. Include charges on ions and states of
matter.
Ni+2(aq) + CO3-2 (aq)  NiCO3 (s)
e) What is/are the driving force(s) for this reaction?
Formation of solid