CHEMISTRY WKST KEY: POST TEST REVIEW #2
1)
a) vaporization
b) freezing
c) melting
d) sublimation
e) condensation
2)
a)
b)
c)
d)
e)
f)
g)
h)
3)
a) 1000
b) 100
c) 1000
d) 1000
4)
a) physical
b) physical
c) chemical
d) physical
e) physical
f) chemical
deci
centi
milli
micro
nano
kilo
mega
giga
5)
pure / mixture
elements /
compounds
# elements
pure
mixture
mixture
pure
element
elements
element, compound
compound
1
2
3
2
6)
a) pure substance
b) mixture
c) pure substance
d) pure substance
7)
- precipitate forms
- gas given off
- temperature change
- color change
- energy given off
8)
a) 7A or 17
b) 1A or 1
c) 8A or 18
d) 2A or 2
9)
a) 2+
b) 1−
c) 3+
d) 2+ and 4+
e) 2+
f) 2−
10)
a) metal
b) metal
c) nonmetal
g) 1+
h) 1+ and 2+
i) 3−
d) nonmetal
e) metal
f) metal
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11)
a) single replacement
b) acid-base
c) synthesis
d) decomposition
e) combustion
f) double replacement
12)
a) CH
b) H2SO4
c) CH2O
d) P2O5
13)
CH2O  30.03 g
e) NO3
f) C5H20N16O2
2
3 3
(CH2O)8 = C8H16O8
14)
1 mol
molar mass and 1 mol
Avo adro’s Number of items
Answer: 28.02 g N2
23
6.022 x 10 N2 molecules
mol solute
soln
15)
2
mol
32
N
3
16)
HCl (hydrochloric acid)
HBr (hydrobromic acid)
HI (hydroiodic acid)
HNO3 (nitric acid)
HClO3 (chloric acid)
HClO4 (perchloric acid)
H2SO4 (sulfuric acid)
17)
a) Na2CO3
b) Al2O3
c) PbCrO4
d) (NH4)3PO4
18)
a) Na2CO3 → soluble (all alkali metal compounds are soluble in water)
b) NH3 → soluble (polar molecules will dissolve in water which is also polar)
c) (NH4)2S → soluble (all ammonium compounds are soluble in water)
d) CH3CH2CH2CH3 → insoluble (nonpolar molecules will not dissolve in water which is polar)
e) Zn3(PO4)2 → insoluble (phosphate compounds are only soluble if with an alkali metal or ammonium)
SF4 → soluble (polar molecules will dissolve in water which is also polar)
f)
1−
19)
Cl
(It’s the only ion found on both sides of the arrow )
20)
a) increase
b) increase
c) stay the same
d) increase
21)
a) stay the same
b) increase
c) increase
d) increase
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22)
NUCLEAR
SYMBOL
3
1
33As
ATOMIC
NUMBER
MASS
NUMBER
NUMBER
+
OF p
NUMBER
OF n°
NUMBER
F e‾
CHARGE
l
17
36
17
19
17
0
3
33
75
33
42
36
3-
37
86
37
49
36
1+
52
127
52
75
54
2-
23)
a) red
b) violet
c) red
ROY G BIV
 λ↑
ν↑ 
E↑ 
24)
similar → The 3s and s orbitals have the same shape and can hold a maximum of 2 electrons
different → The s orbital is lar er and has more ener y than the 3s orbital
25)
a) 1
b) 5
c) 7
d) 3
26)
a) 2
b) 6
c) 10
d) 14
27)
a) 2
[ e]
b) 3
[Ar]
c) 0
[Ar]
28)
a) HB
b) LF
c) LF
d) HB
29)
a) Cl
b) Sb
c) Ba
d) F
30)
a) no
b) yes
c) yes
d) yes
↑
2s
↑
↑ ↑ ↑
2p
↑ ↑ ↑
s
↑
3d
↑ ↑ ↑ ↑ ↑
s
3d
e) DD
f) LF
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31)
The expression puts the products over the reactants with the coefficients in the chemical equation as the
substances’ exponent
a)
2SO3(g) ⇄ 2SO2(g) + O2(g)
S
2
S
b)
2
3
2NH3(g) ⇄ N2(g) + 3H2(g)
N2
N
c)
2
2
3
2
2
3
2KClO3(s) ⇄ 2KCl(s) + 3O2(g)
2
3
32)
a) HNO3
b) HCl
c) H2SO4
d) HC2H3O2
33)
Nonmetals have a high electronegativity so they easily attract electrons and therefore can become negative ions.
Metals have a low electronegativity so they don’t attract electrons Instead, metals have a low ionization ener y and
will easily lose electrons to become positive ions.
34)
a) distill the mixture—the water will boil off and the steam can be collected while the NaCl remains in the vessel.
b) filter the mixture—the water will pass through the filter paper but the charcoal does not
35)
a) quantized → exist with only specific amounts of ener y
b) ground state → the lowest possible ener y state of an atom
c) node → part of a wave with zero amplitude
d) activation energy → ener y needed for a reaction to take place
e) ionization energy → ener y needed to remove an electron from an atom
f)
exothermic → process that ives off ener y
g) endothermic →process that absorbs energy
h) limiting reactant → the reactant that is used up first in a chemical reaction and thus stops the reaction
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