1) In which compound does chlorine have the highest oxidation ...

Name: ____________________________________________
1) In which compound does chlorine have the highest
oxidation number?
A) NaClO 3
C) NaClO 4
B) NaClO
D) NaClO 2
2) In which substance does chlorine have an oxidation number
of +1?
A) Cl 2
B) HCl
C) HClO 2
D) HClO
3) What is the oxidation number assigned to manganese in
KMnO 4
?
A) +4
B) +3
C) +7
D) +2
4) What is the oxidation state of nitrogen in NaNO 2
?
A) +1
B) +2
C) +3
D) +4
5) The transfer of which particle is required for a redox reaction
to occur?
A) electron
B) ion
6) Given the redox reaction:
Cr 3+ + Al ‚ Cr + Al 3+
C) neutron
D) proton
As the reaction takes place, there is a transfer of
A) protons from Al to Cr 3+
B) electrons from Al to Cr 3+
C) protons from Cr 3+ to Al
D) electrons from Cr 3+ to Al
7) Which reaction is an example of an oxidation-reduction
reaction?
A) 2KOH + H 2 SO 4
‚ K 2 SO 4 + 2H 2 O
B) Cu + 2AgNO 3
‚ Cu(NO 3 ) 2 + 2Ag
C) AgNO 3 + KI ‚ AgI + KNO 3
D) Ba(OH) 2 + 2HCl ‚ BaCl 2 + 2H 2 O
8) As a Ca atom undergoes oxidation to Ca 2+ , the number of
neutrons in its nucleus
A) increases
C) remains the same
B) decreases
9) Given the reaction:
Mg + CuSO 4
‚ MgSO 4 + Cu
Which equation represents the oxidation that takes place?
A) Mg 2+ + 2e - ‚ Mg C) Cu ‚ Cu 2+ + 2e -
B) Mg ‚ Mg 2+ + 2e - D) Cu 2+ + 2e - ‚ Cu
D) Al 3+ B) Fe
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10) Given the reaction:
Mg(s) + 2H + (aq) + 2Cl - (aq) ‚
Mg 2+ (aq) + 2Cl - (aq) + H 2 (g)
Which species undergoes oxidation?
A) H + (aq)
C) Mg(s)
B) H 2 (g)
D) Cl - (aq)
11) Given the balanced ionic equation:
Zn(s) + Cu 2+ (aq) ‚ Zn 2+ (aq) + Cu(s)
Which equation represents the oxidation half-reaction?
A) Zn(s) + 2e - ‚ Zn 2+ (aq)
B) Cu 2+ (aq) + 2e - ‚ Cu(s)
C) Cu 2+ (aq) ‚ Cu(s) + 2e -
D) Zn(s) ‚ Zn 2+ (aq) + 2e -
12) Given the reaction:
Zn(s) + 2HCl(aq) ‚ ZnCl 2 (aq) + H 2 (g)
Which statement correctly describes what occurs when this
reaction takes place in a closed system?
A) There is a net loss of mass.
B) Atoms of Zn(s) gain electrons and are reduced.
C) Atoms of Zn(s) lose electrons and are oxidized.
D) There is a net gain of mass.
13) In an oxidation-reduction reaction, reduction is defined as
the
A) gain of electrons
C) gain of protons
B) loss of protons
D) loss of electrons
14) In any redox reaction, the substance that undergoes
reduction will
A) gain electrons and have an increase in oxidation
number
B) lose electrons and have a decrease in oxidation number
C) gain electrons and have a decrease in oxidation number
D) lose electrons and have an increase in oxidation number
15) Given the reaction:
2Al(s) + Fe 2 O 3 (s) Al 2 O 3 (s) + 2Fe(s)
Which species undergoes reduction?
A) Fe 3+
C) Al

16) Which change in oxidation number indicates oxidation?
A) +2 to -3
B) -1 to -2
C) +3 to +2
D) -1 to +2
17) According to the Activity Series chemistry reference table,
which of these metals will react most readily with 1.0 M HCl
to produce H 2
(g)?
A) Zn
B) K
C) Ca
D) Mg
18) Which metal reacts spontaneously with a solution
containing zinc ions?
A) silver
B) nickel
C) copper
D) magnesium
C) Fe ‚ Fe 2+ + 2e -
19) In a redox reaction, how does the total number of electrons
lost by the oxidized substance compare to the total number
of electrons gained by the reduced substance?
A) The number lost is always greater than the number
gained.
B) The number lost is always equal to the number gained.
C) The number lost is sometimes equal to the number
gained.
D) The number lost is sometimes less than the number
gained.
20) Which equation shows conservation of charge?
A) Fe + 2e - ‚ Fe 3+
B) Fe ‚ Fe 2+ + e - D) Fe + 2e - ‚ Fe 2+
21) Which equation shows conservation of both mass and
charge?
A) Ni + Pb 2+ ‚ Ni 2+ + Pb
B) Cl 2 + Br - ‚ Cl - + Br 2
C) Cu + 2Ag + ‚ Cu 2+ + Ag
D) Zn + Cr 3+ ‚ Zn 2+ + Cr
22) A voltaic cell spontaneously converts
A) chemical energy to electrical energy
B) electrical energy to nuclear energy
C) electrical energy to chemical energy
D) nuclear energy to electrical energy
23) Which statement is true for any electrochemical cell?
A) Reduction occurs at both the anode and the cathode.
B) Oxidation occurs at both the anode and the cathode.
C) Oxidation occurs at the anode, only.
D) Reduction occurs at the anode, only.
24) A diagram of a chemical cell and an equation are shown
below.
When the switch is closed, electrons will flow from
A) the Pb 2+ (aq) to the Pb(s)
B) the Cu 2+ (aq) to the Cu(s)
C) the Cu(s) to the Pb(s)
D) the Pb(s) to the Cu(s)
25) All organic compounds must contain the element
A) nitrogen
B) carbon
C) phosphorus
D) oxygen
26) Which element must be present in an organic compound?
A) oxygen
B) hydrogen
C) nitrogen
D) carbon
27) Which element has atoms that can bond with each other to
form long chains or rings?
A) nitrogen
B) fluorine
C) oxygen
D) carbon
28) An unknown substance, liquid X, is tested in the laboratory.
The chemical and physical test results are listed below.
d Nonconductor of electricity
d Insoluble in water
d Soluble in hexane
d Low melting point as a solid
d Combustion produces only CO 2 and H 2 O
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Based on these results, a student should conclude that
liquid X is
A) covalent and organic
B) ionic and organic
C) covalent and inorganic
D) ionic and inorganic

29) Which structural formula is incorrect?
A)
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34) What is the IUPAC name of the compound having the
following structural formula?
B)
A) 3-pentene
B) 3-pentyne
C) 2-pentene
D) 2-pentyne
35) Which structural formula correctly represents a
hydrocarbon molecule?
C)
A)
C)
D)
B)
D)
30) Molecules of 2-methyl butane and 2,2-dimethyl propane
have different
A) numbers of covalent bonds
B) molecular formulas
C) structural formulas
D) numbers of carbon atoms
31) Which compound is classified as a hydrocarbon?
A) chloroethane
B) ethanol
32) Which formula represents a hydrocarbon?
C) ethanoic acid
D) ethane
36) The empirical formula of a compound is CH 2 . Which
molecular formula is correctly paired with a structural
formula for this compound?
A) C 2 H 4 ,
B) C 3 H 8 ,
A) CH 3 CH 2 CH 2 CH 3
B) CH 3 CH 2 COOCH 3
C) CH 3 CH 2 CH 2 CHO
D) CH 3 CH 2 CH 2 COOH
C) C 3 H 8 ,
33) Given the structural formula:
D) C 2 H 4 ,
What is the IUPAC name of this compound?
A) propene
B) propanone
C) propane
D) propanal
37) Given the reaction: 4Al(s) + 3O 2
(g) ‚ 2Al 2
O 3
(s)
(a)
Write the balanced oxidation half-reaction for this
oxidation-reduction reaction.
(b) What is the oxidation number of oxygen in Al 2 O 3 ?

Questions 38 and 39 refer to the following:
The equation below represents an unbalanced redox reaction.
__Cu(s) + __AgNO 3
(aq) ‚ __Cu(NO 3
) 2
(aq) + __Ag(s)
38) Write the reduction half-reaction for the given redox
reaction.
39) Balance the given redox equation using the smallest wholenumber
coefficients.
Questions 40 and 41 refer to the following:
6118 - 1 - Page 4
42) On the given diagram, indicate with one or more arrows the
direction of electron flow through the wire.
43) Write an equation for the half-reaction that occurs at the
zinc electrode in the given diagram.
44) Explain the function of the salt bridge in the given diagram.
Questions 45 and 46 refer to the following:
The diagram below represents a voltaic cell and a balanced ionic
equation.
The redox reaction below occurs spontaneously in an
electrochemical cell.
Zn + Cr 3+ ‚ Zn 2+ + Cr
40) Which species loses electrons and which species gains
electrons?
41) State what happens to the number of protons in a Zn atom
when it changes to Zn 2+ as the redox reaction occurs.
Questions 42 through 44 refer to the following:
45) What is the total number of moles of electrons needed to
completely reduce 6.0 moles of Ni 2+ (aq) ions in the ionic
equation shown?
46) Identify one metal from the Activity Series chemistry
reference table that is more easily oxidized than Mg(s).
47) How is the bonding between carbon atoms different in
unsaturated hydrocarbons and saturated hydrocarbons?
48) Identify the homologous series of hydrocarbons to which
CH 3 CHCH 2 belongs.