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Which of the following is a physical observation?
1. burns in oxygen
2. melts at 76 oC
3. forms a white precipitate
4. decomposes in air
5. cooks at high temperature
In the presence of aqueous I-, Pb2+
forms a yellow precipitate, PbI2
Which of the following is a physical observation?
1. burns in oxygen
2. melts at 76 oC
3. forms a white precipitate
4. decomposes in air
5. cooks at high temperature
In the presence of aqueous I-, Pb2+
forms a yellow precipitate, PbI2
Which of the following is an observation of a
chemical property?
1. orange crystal
2. boils at 112 oC
3. smells like mint
4. ignites in water
5. shatters when hammered
Magnesium metal burns in air to
produce magnesium oxide.
Which of the following is an observation of a
chemical property?
1. orange crystal
2. boils at 112 oC
3. smells like mint
4. ignites in water
5. shatters when hammered
Magnesium metal burns in air to
produce magnesium oxide.
Solutions containing 3.2 g and 3.3 g of
Hg(NO3)2 and KI, respectively (which
amounts to 10 mmol and 20 mmol,
respectively). The two components were
separated and dried. The mass of KNO3
was determined to be 2.0 g (ie. 20 mmol).
What mass of HgI2 was produced?
Hg(NO3 )2 (aq) + 2KI(aq)  HgI 2 (aq) + 2KNO3 (aq)
1. 9.0 g
4. 2.8 g
2. 4.5 g
5. 1.4 g
3. 4.0 g
Two solutions contain 3.2 g and 3.3 g of
Hg(NO3)2 and KI, respectively (which
amounts to 10 mmol and 20 mmol,
respectively). The two components were
separated and dried. The mass of KNO3
was determined to be 2.0 g (ie. 20 mmol).
What mass of HgI2 was produced?
Hg(NO3 )2 (aq) + 2KI(aq)  HgI 2 (aq) + 2KNO3 (aq)
1. 9.0 g
4. 2.8 g
2. 4.5 g
5. 1.4 g
3. 4.0 g
Red phosphorus is an allotrope of
phosphorus which can be made by heating
white phosphorus to temperatures above
240 oC. The most common isotope of
phosphorus can be represented by
31
15
How many protons, electrons and neutrons
does this isotope have?
P
1. 16, 16, 15
2. 15, 15, 1
4. 16, 16, 31
3. 15, 15, 16
5. 16, 16, 1
Red phosphorus is an allotrope of
phosphorus which can be made by heating
white phosphorus to temperatures above
240 oC. The most common isotope of
phosphorus can be represented by
31
15
How many protons, electrons and neutrons
does this isotope have?
P
1. 16, 16, 15
2. 15, 15, 1
4. 16, 16, 31
3. 15, 15, 16
5. 16, 16, 1
Bromine is a reddish-brown liquid. The atoms
are composed of two isotopes with abundances
and masses given below the figure.
The
average atomic mass of bromine is
1. 79.90
4. 79.99
2. 79.92
5. 78.91
3. 79.93
isotope
mass / amu
abundance / %
79
35
Br
78.9183
50.69
81
35
Br
80.9163
49.31
Bromine is a reddish-brown liquid. The atoms
are composed of two isotopes with abundances
and masses given below the figure.
The
average atomic mass of bromine is
1. 79.90
4. 79.99
2. 79.92
5. 78.92
3. 79.93
isotope
mass / amu
abundance / %
79
35
Br
78.9183
50.69
81
35
Br
80.9163
49.31
Depicted to the right is the reaction of calcium with
water to form calcium hydroxide and hydrogen. If one
mole of calcium is reacted with one mole of water, how
many moles of calcium hydroxide will be formed?
1. 0.25 moles
4. 1.0 moles
2. 0.33 moles
5. 1.5 moles
3. 0.50 moles
Depicted to the right is the reaction of calcium with
water to form calcium hydroxide and hydrogen. If one
mole of calcium is reacted with one mole of water, how
many moles of calcium hydroxide will be formed?
1. 0.25 moles
4. 1.0 moles
2. 0.33 moles
5. 1.5 moles
3. 0.50 moles
250.0 mL of 0.100 M HCl is required for a particular experiment. A 2.50 M stock
solution is available. What volume of stock solution is needed to prepare the
required HCl solution?
1. 1.00x10-3 mL
2. 10.0 mL
3. 12.5 mL
4. 100 mL
5. 6250 mL
250.0 mL of 0.100 M HCl is required for a particular experiment. A 2.50 M stock
solution is available. What volume of stock solution is needed to prepare the
required HCl solution?
1. 1.00x10-3 mL
2. 10.0 mL
3. 12.5 mL
4. 100 mL
5. 6250 mL
It was found that 10.0 mL of 0.100 M HCl was
required to titrate a 20.0 mL aliquot of NaOH.
What is the concentration of the sodium
hydroxide solution?
1. 0.0500 M
4. 0.200 M
2. 0.100 M
5. 0.250 M
3. 0.150 M
It was found that 10.0 mL of 0.100 M HCl was
required to titrate a 20.0 mL aliquot of NaOH.
What is the concentration of the sodium
hydroxide solution?
1. 0.0500 M
4. 0.200 M
2. 0.100 M
5. 0.250 M
3. 0.150 M
A compound is found to consist of C, H
and O in abundances, by mass, of 40.0,
6.7, and 53.3 percent respectively. A
mass spectrum revealed that the
compound’s molecular mass was 90.08
amu. What is the molecular formula of
the compound?
1. CH2O
4. C3H6O3
2. C2H4O2
5. C4H10O2
3. C2H2O4
relative intensity
100
80
60
40
20
0
20
30
40
50
60
m/z
70
80
90
100
A compound is found to consist of C, H
and O in abundances, by mass, of 40.0,
6.7, and 53.3 percent respectively. A
mass spectrum revealed that the
compound’s molecular mass was 90.08
amu. What is the molecular formula of
the compound?
1. CH2O
4. C3H6O3
2. C2H4O2
5. C4H10O2
3. C2H2O4
relative intensity
100
80
60
40
20
0
20
30
40
50
60
m/z
70
80
90
100
Which of the following pairs of solutions, when mixed,
will form a precipitate?
1. NaCl(aq) + KNO3(aq)
2. NH3Br(aq) + CaSO4(aq)
3. BaCl2(aq) + NaOH(aq)
4. AgNO3(aq) + LiClO4(aq)
5. MgBr2(aq) + AlCl3(aq)
Which of the following pairs of solutions, when mixed,
will form a precipitate?
1. NaCl(aq) + KNO3(aq)
2. NH3Br(aq) + CaSO4(aq)
3. BaCl2(aq) + NaOH(aq)
4. AgNO3(aq) + LiClO4(aq)
5. MgBr2(aq) + AlCl3(aq)
When methane is burned in oxygen the
product containing the carbon atom is carbon
dioxide. The oxidation numbers of the carbon
atoms in methane and carbon dioxide,
respectively, are
1. +4, -4
4. -2, +4
2. +2, -2
5. -4, +4
3. -1, +2
When methane is burned in oxygen the
product containing the carbon atom is carbon
dioxide. The oxidation numbers of the carbon
atoms in methane and carbon dioxide,
respectively, are
1. +4, -4
4. -2, +4
2. +2, -2
5. -4, +4
3. -1, +2
The rusting of iron is a redox reaction where iron is
oxidized and changes oxidation states from 0 to 3.
Which of the following reactions is not an
oxidation reaction?
1. Mg(s) + 2H2O(g)  Mg(OH)2 (s) + H 2 (g)
2. CH4 (g) + 2O2 (g)  CO2 (g) + 2H2O(g)
3. SnO2 (s) + 2C(s)  S(s) + 2CO(g)
Fe(s) + 3O2 (g)  Fe2O3 (g)
4. 2Ag+ (aq) + Cu(s)  Cu2+ (aq) + 2Ag(s)
5. 2NaOH(aq) + H2SO4 (aq)  2Na + (aq) + SO4 (aq) + 2H2O(l)
The rusting of iron is a redox reaction where iron is
oxidized and changes oxidation states from 0 to 3.
Which of the following reactions is not an
oxidation reaction?
1. Mg(s) + 2H2O(g)  Mg(OH)2 (s) + H 2 (g)
2. CH4 (g) + 2O2 (g)  CO2 (g) + 2H2O(g)
3. SnO2 (s) + 2C(s)  S(s) + 2CO(g)
Fe(s) + 3O2 (g)  Fe2O3 (g)
4. 2Ag+ (aq) + Cu(s)  Cu2+ (aq) + 2Ag(s)
5. 2NaOH(aq) + H 2SO4 (aq)  2Na + (aq) + SO4 (aq) + 2H 2O(l)
strongly
reducing
Silver cation will oxidize copper becoming
solid silver and liberating copper (II) ions.
Looking at the diagram to the left, which
one of the four reactions below will occur?
1. Pt(s) + 2H+ (aq)  Pt 2+ (aq) + H2 (g)
2. Ni(s) + 2H+ (aq)  Ni2+ (aq) + H2 (g)
weakly
reducing
3. Sn2+ (aq) + H2 (g)  Sn(s) + 2H+ (aq)
4. 3Ni2+ (aq) + 2Au(s)  3Ni(s) + 2Au3+ (aq)
strongly
reducing
Silver cation will oxidize copper becoming
solid silver and liberating copper (II) ions.
Looking at the diagram to the left, which
one of the four reactions below will occur?
1. Pt(s) + 2H+ (aq)  Pt 2+ (aq) + H2 (g)
2. Ni(s) + 2H + (aq)  Ni 2+ (aq) + H 2 (g)
weakly
reducing
3. Sn2+ (aq) + H2 (g)  Sn(s) + 2H+ (aq)
4. 3Ni2+ (aq) + 2Au(s)  3Ni(s) + 2Au3+ (aq)
The reaction occurring during the titration of oxalic acid
(H2C2O4) with permanganate ion (MnO4-) is as follows,
5H2C2O4 + 2MnO4 + 6H+ (s)  10CO2 + 2Mn2+ + 8 H2O
In the titration of 0.0117 mol of the oxalic acid primary
standard it was found that 18.5 mL of permanganate
solution was required to reach the light purple endpoint.
What is the concentration of the permanganate solution?
1. 2.53x10-4 M
3. 0.253 M
2. 6.32x10-4 M
4. 0.632 M
5. 1.58 M
The reaction occurring during the titration of oxalic acid
(H2C2O4) with permanganate ion (MnO4-) is as follows,
5H2C2O4 + 2MnO4 + 6H+ (s)  10CO2 + 2Mn2+ + 8 H2O
In the titration of 0.0117 mol of the oxalic acid primary
standard it was found that 18.5 mL of permanganate
solution was required to reach the light purple endpoint.
What is the concentration of the permanganate solution?
1. 2.53x10-4 M
3. 0.253 M
2. 6.32x10-4 M
4. 0.632 M
5. 1.58 M
Hydrocarbons are composed of just
the elements carbon and hydrogen.
Which of the following compounds
has all single bonds?
•
naphthalene, C10H8
•
propane, C3H8
•
ethyne, C2H2
•
ethene, C2H4
Hydrocarbons are composed of just
the elements carbon and hydrogen.
Which of the following compounds
has all single bonds?
•
naphthalene, C10H8
•
propane, C3H8
•
ethyne, C2H2
•
ethene, C2H4
How many neutrons
are in 1000 atoms of
Cl-37?
•
•
•
•
•
37
37,000
20
20,000
cannot be determined
How many neutrons
are in 1000 atoms of
Cl-37?
•
•
•
•
•
37
37,000
20
20,000
cannot be determined
shown below. The atomic mass of Ga is
69.7 amu. Which of the following
c) The atomic mass of Ga will
•statements
All Ga atoms weigh
69.7
is correct?
amu.
• The atomic mass of Ga is the
average of 68.9 and 71.9.
be closer to 69 than 71
because there are more atoms
that weigh 68.9 amu.
Relative Abundance (%)
Gallium Mass Spectrum
70
68.9 amu, 60.1 %
60
50
71.9 amu, 39.9 %
40
30
20
10
0
67
68
69
70
Mass (amu)
71
72
shown below. The atomic mass of Ga is
69.7 amu. Which of the following
c) The atomic mass of Ga will
•statements
All Ga atoms weigh
69.7
is correct?
Relative Abundance (%)
be closer to 69 than 71
amu.
because there are more
• The atomic mass of Ga is
atoms that weigh 68.9 amu.
the average of 68.9 and
71.9.
Gallium Mass Spectrum
70
68.9 amu, 60.1 %
60
50
71.9 amu, 39.9 %
40
30
20
10
0
67
68
69
70
Mass (amu)
71
72
Which weighs more, a pea or a
marble?
a) Pea
b) Marble
Which weighs more, a pea or a
marble?
a) Pea
b) Marble
Which has more atoms, 10.0 g Mg or
10.0 g Ca?
a) Magnesium
b) Calcium
c) Both have the same number
of atoms.
24.30
40.08
Which has more atoms, 10.0 g Mg or
10.0 g Ca?
a) Magnesium
b) Calcium
c) Both have the same number
of atoms.
24.30
40.08
Aqueous solutions of which of the
following would conduct electricity?
•
•
•
•
•
•
AgNO3
C11H22O11 (sucrose: table sugar)
CH3CH2OH (ethanol)
O2
All of the above
None of the above
Aqueous solutions of which of the
following would conduct electricity?
•
•
•
•
•
•
AgNO3
C11H22O11 (sucrose: table sugar)
CH3CH2OH (ethanol)
O2
All of the above
None of the above
Determine the oxidation number of the red element in
each of the following compounds:
H2PO4–
•
•
•
•
•
+6
+5
+5
+5
+6
+6
+2
+4
+4
+4
+4
+4
+4
+8
+4
SO32–
N2O4
Determine the oxidation number of the red element in
each of the following compounds:
H2PO4–
•
•
•
•
•
+6
+5
+5
+5
+6
+6
+2
+4
+4
+4
+4
+4
+4
+8
+4
SO32–
N2O4

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