Chem 051 - Fundamentals of Chemistry » Winter 2021 » Final Exam
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Question #1
Which particle has the smallest mass?
A.
electron
B.
helium nucleus
C.
proton
D.
neutron
Question #2
Which of the following elements is most similar to chlorine?
A.
He
B.
H
C.
Br
D.
Hg
E.
Na
Question #3
Identify the type of organic compound shown: (CH3)3N
A.
ketone
B.
ester
C.
amine
D.
aldehyde
Question #4
In the reaction 2Cs(s) + Cl2(g) → 2CsCl(s), the chlorine is ______________.
A.
synthesized
B.
reduced
C.
electrolyzed
D.
oxidized
Question #5
Calculate the heat given off when 101.4 g of copper cools from 155.0oC to 23.0oC. The specific heat of copper is 0.385 J/g oC.
A.
5.15 × 103 J
B.
3.48 × 104 J
C.
6.05 × 103 J
D.
8.98 × 102 J
E.
none of these
Question #6
Heat is typically measured in
A.
joules
B.
grams
C.
°C
D.
°F
Question #7
1s22s22p63s23p64s23d7 is the electron configuration for which of the following atoms?
A.
Ca
B.
Ar
C.
Co
D.
Fe
E.
Cr
Question #8
A 2.2-mol sample of KClO3 was decomposed according to the equation 2KClO3(s) → 2KCl(s) + 3O2(g) How many moles of O2 are formed?
A.
1.1 mol
B.
1.8 mol
C.
2.2 mol
D.
1.5 mol
E.
3.3 mol
Question #9
The formula for potassium carbonate is
A.
P2CO3.
B.
K2CO3.
C.
P2C.
D.
Po2CO3.
E.
K2C.
Question #10
A.
In an acidic solution, [H+] > [OH-]
B.
In a neutral solution, [H+] = [OH-]
C.
In a basic solution,[OH-] > [H+]
D.
In an acidic solution, [H+] > [OH-], In a basic solution,[OH-] > [H+], and In a neutral solution, [H+] = [OH-] .
E.
None of the above statements are correct.
Question #11
True or false? The equation N2(g) + 3H2(g) → 2NH3(g) can be interpreted by saying that 1 mol of N2 reacts with 3 mol of H2 to form 2 mol of NH3.
A.
FALSE
B.
TRUE
Question #12
Oxidation of a primary alcohol results in a(n) __________ and oxidation of a secondary alcohol results in a(n) _________.
A.
ketone, aldehyde
B.
amine, carboxylic acid
C.
ester, ether
D.
aldehyde, ketone
E.
carboxylic acid, amine
Question #13
3.03 mol of CO2 at STP will occupy
A.
67.9 L
B.
8.93 × 10–2 L
C.
74.1 L
D.
33.9 L
E.
67.9 g
Question #14
The chemical formula for iron(III) sulfide is
A.
Fe2(SO3)3.
B.
Fe2S3.
C.
Fe3(SO3)2.
D.
Fe2(SO4)3.
Question #15
True or false? CH4 has ionic bonds.
A.
FALSE
B.
TRUE
Question #16
True or false? Arrhenius postulated that acids produce hydrogen ions in aqueous solution, whereas bases produce hydroxide ions.
A.
FALSE
B.
TRUE
Question #17
There are three isotopes of carbon differing with respect to
A.
B.
nuclear charge.
C.
number of protons.
D.
electron configuration.
E.
neutrons.
F.
atomic number.
Question #18
H2CCHCH2N(CH3)2 is
A.
an alkene and a primary amine.
B.
an alkyne and a tertiary amine.
C.
an alkene and a tertiary amine.
D.
an alkyne and a secondary amine.
Question #19
How many protons, electrons, and neutrons, respectively, does 127I have?
A.
74, 53, 127
B.
53, 127, 74
C.
53, 74, 53
D.
53, 53, 74
E.
53, 53, 127
Question #20
A substance that, when dissolved in water, produces a solution that conducts electric current very efficiently is called
A.
a strong ion
B.
none of these
C.
a weak electrolyte
D.
a strong electrolyte
E.
an electrical solute
Question #21
Chemical reactions involving alkanes in which hydrogen atoms are removed and the product is an unsaturated hydrocarbon are called
A.
addition reactions.
B.
combustion reactions.
C.
dehydrogenation reactions.
D.
polymerization reactions.
E.
substitution reactions.
Question #22
Which of the following will yield a carboxylic acid upon oxidation?
A.
an aldehyde
B.
tertiary alcohol
C.
a secondary alcohol
D.
a cycloalkane
E.
a ketone
Question #23
The elements chlorine and iodine have similar chemical properties because they
A.
have the same number of stable isotopes
B.
none of these
C.
have the same number of electrons in their outer energy levels
D.
are both metals
E.
are in the same chemical period
Question #24
Which of the following compounds contains one or more covalent bonds?
A.
CO2
B.
BaBr2
C.
Cs2O
D.
CaO
E.
NaCl
Question #25
The total mass of a solution is 171.5 g. The solvent mass is 125.2 g. What is the mass percent of the solute?
A.
Not enough information is given.
B.
73.0%
C.
38.0%
D.
18.1%
E.
27.0%
Question #26
The best answer to report for 131.00 – 31.9904 is
A.
99.0.
B.
99.010.
C.
99
D.
99.01.
E.
99.0096.
Question #27
The complete combustion of heptane, C7H16, which is a volatile hydrocarbon, yields carbon dioxide and water: __ C7H16 + __ O2 → __ CO2 + __ H2O The coefficient of oxygen in the balanced equation is
A.
13
B.
11
C.
8
D.
15
E.
9
Question #28
When an electron in the ground state absorbs energy, it goes to a(n) ______________ state.
A.
stable
B.
frenetic
C.
excited
D.
lower
E.
ionic
Question #29
The oxidation product of a secondary alcohol is
A.
an aldehyde.
B.
an acid.
C.
an ester.
D.
a ketone.
E.
a tertiary alcohol.
Question #30
Which of the following compounds contains an ionic bond?
A.
O2
B.
SO2
C.
NaCl
D.
CCl4
E.
HCl(g)
Question #31
True or false? N2 is an example of a covalent bond.
A.
FALSE
B.
TRUE
Question #32
The reaction HCl(aq) + KOH(aq) → H2O(l) + KCl(aq) is a(n) ______________ reaction.
A.
single-replacement
B.
acid-base
C.
precipitation
D.
none of these
E.
oxidation-reduction
Question #33
True or false? The calorie is defined as the amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius.
A.
FALSE
B.
TRUE
Question #34
Name the following: CH3C ≡ CCH2CH2Cl
A.
2-chloro-5pentyne
B.
5-chloro-2pentyne
Question #35
A solution with a pH of 2 is how many times more acidic as a solution with a pH of 3?
A.
0.7
B.
5
C.
10
D.
100
E.
2
Question #36
A solution has [OH–] = 2.8 X 10–7 M. The [H+] in this solution is
A.
2.8X 107 M
B.
3.6 X 10–8 M
C.
3.6 X 107 M
D.
2.8 X 107 M
Question #37
The number of unpaired electrons in a nitrogen atom is
A.
3
B.
6
C.
7
D.
5
E.
4
Question #38
If you were to heat pentanoic acid and 2-butanol with a strong acid, you would most likely discover in your flask:
A.
an amine
B.
an alkane
C.
a ketone
D.
an ester
E.
an aldehyde
Question #39
Choose the state of water in which the water molecules are farthest apart on average.
A.
ice (solid)
B.
liquid
C.
steam (vapor)
D.
all the same
Question #40
The air in the inner tube of the tire of a racing bike has a pressure of 110.2 psi. Convert this pressure to atm.
A.
1620 atm
B.
7.497 atm
C.
1.088 atm
D.
110.2 atm
E.
0.1450 atm
Question #41
The number of significant figures in 0.074100 × 10–4 is
A.
5
B.
7
C.
4
D.
3
E.
6
Question #42
A given set of d orbitals consists of ______________ orbital(s).
A.
6
B.
5
C.
1
D.
3
Question #43
An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride. Identify the solid in the balanced equation.
A.
There is no solid formed when the two solutions are mixed.
B.
CaCl2
C.
Na2CO3
D.
NaCl
E.
CaCO3
Question #44
The number of protons in a given nucleus determines the
A.
number of electrons.
B.
number of isotopes.
C.
atomic number.
D.
number of protons.
E.
mass number.
Question #45
A solution with a pH of 2.17 is
A.
neutral
B.
basic
C.
acidic
Question #46
The state of matter for an object that has a definite volume but not a definite shape is
A.
elemental
B.
gaseous
C.
solid
D.
liquid
E.
mixed
Question #47
Which of the following has a double C-O bond and a single C-O bond?
A.
aldehyde
B.
alcohol
C.
ester
D.
ketone
E.
amine
Question #48
True or false? The law of conservation of enery states that energy can be converted from one form to another but can be neither created nor destroyed.
A.
TRUE
B.
FALSE
Question #49
The alkaline earth metals have how many valence electrons?
A.
7
B.
3
C.
2
D.
8
E.
1
Question #50
You have 25.00 mL of a 0.1000 M sugar solution. How much water must be added to make a 0.01042 M solution?
A.
26.1 mL
B.
214.9 mL
C.
239.9 mL
D.
2.61 mL
E.
22.4 mL
Question #51
If you mix 20.0 mL of a 3.00 M sugar solution with 30.0 mL of a 5.30 M sugar solution, you will end up with a sugar solution of ________.
A.
10.95 M
B.
0.166 M
C.
4.15 M
D.
7.30 M
E.
4.38 M
Question #52
True or false? Reduction is a gain of electrons.
A.
TRUE
B.
FALSE
Question #53
Which of the following is an incorrect designation for an atomic orbital?
A.
1s
B.
2p
C.
2d
D.
4f
E.
3s
Question #54
Perform the indicated conversion: 2.63 X 103 cal = _______________ J
A.
629 J
B.
1.59 x 10–3 J
C.
11.0 J
D.
1.10 X 104 J
E.
6.29 X 105 J
Question #55
At 1 atm of pressure and a temperature of 0°C, which phase(s) of H2O can exist?
A.
water only
B.
water vapor only
C.
ice and water
D.
ice only
E.
ice and water vapor
Question #56
How many electrons are in the third principal energy level (n = 3) of one atom of Fe?
A.
none of these
B.
18
C.
2
D.
14
E.
8
Question #57
If temperature and pressure are held constant, the volume and number of moles of a gas are
A.
equal
B.
directly proportional
C.
inversely proportional
D.
not enough information given
E.
independent of each other
Question #58
The most characteristic reaction of the alkenes is
A.
substitution.
B.
reduction.
C.
addition.
D.
oxidation.
E.
addition and elimination.
Question #59
The oxidation product of a primary alcohol is
A.
a tertiary alcohol.
B.
an alkene.
C.
an acid.
D.
an ether.
E.
a ketone.
Question #60
Which represents the greatest mass?
A.
1.0 mol Al
B.
1.0 mol Zn
C.
1.0 mol Cu
D.
all the same
E.
1.0 mol Fe
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