The size of metal atoms

generally increases progressively from top to bottom in a group

All gases approach ideal behavior under conditions of

low density and high temperature

What is the best procedure to prepare 0.500 L of a 0.200 M solution of Li3PO4? (LiPO4=115.8 g/mol)

Weigh 11.6 g of solute and add water to obtain a final volume of 0.500 L

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CHEM 120 ACS Review

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The ACS final consists of 70 multiple-choice questions; you have 110 minutes to complete them. These questions are taken from the ACS study guide, and you will have 2 minutes per question (the suggested amount of time per question). You may not have learned how to answer some of these questions, it is alright to guess!

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Questions 167

Answers

1
What are the coefficients for each substance in the chemical reaction when balanced? _CH₄ + _O₂ -> _CO₂ + _H₂O
1, 3, 1, 2
2, 4, 2, 4
4, 2, 2, 2
1, 2, 1, 2
2
The speed of light is 3.0x10⁸ m/s. What is the speed in nm/ms?
3.0x10-4 nm/ms
3.0x102 nm/ms
3.0x1020 nm/ms
3.0x1014 nm/ms
3
A sample of ethanol (C₂H₆O) contains 3.024g hydrogen. How many moles of carbon are in the sample? (ethanol=46.07 g/mol)
0.1667
8.333x10-2
0.2500
0.09980
4
Which element contains a Group 14 metal?
GeF4
SnCl2
ZnCl2
CCl4
5
If a nanoparticle has a density of 12.0g/cm³, what is the mass of a nanoparticle with a volume of 1.84x10^-21cm³?
2.21x10-20 g
1.63x10-20 g
1.53x10-22 g
6.52x10-21 g
6
If gallium combines with selenium what is the most likely formula based on your knowledge of periodic table elements?
GaSe
GaSe2
Ga2Se
Ga2Se3
7
Which ground state electron configuration is possible for an atom in the second period?
1s22p4
1s22s22d1
1s22s1
1s21s12p1
8
What mass of nitrogen is in 7.43x10^-4 moles of 3TC (C₈H₁₁N₃O₃S)? (Molar mass C₈H₁₁N₃O₃S=229.26 g/mol)
3.12x10-2 g
1.70x10-1 g
5.11x10-1 g
3.47x10-3 g
9
What is the coefficient for ZnO when the reaction is balanced? _ZnS + _O₂ -> _ZnO + _SO₂
2
3
4
1
10
What is the wavelength of a photon with an energy of 6.51x10^-19 J
1.00x1015 nm
3.05x10-9 nm
4.52x1026 nm
305 nm
11
When 1.0 M aqueous solutions of KI, NaC₂H₃O₂, and Pb(NO₃)₂ are mixed together, what precipitate forms?
PbI2
NaNO3
KC2H3O2
Pb(C2H3O2)2
12
What are the coefficients for each substance in the chemical reaction when balanced? _NaBr + _Cl₂ -> _NaCl + _Br₂
1, 2, 2, 2
1, 1, 2, 2
2, 1, 2, 1
2, 4, 2, 4
13
Which set of quantum numbers is correct and consistent with n=4?
l=4, ml= +2, ms= -1/2
l= 2, ml= +3, ms= +1/2
l= 3, ml= -3, ms= +1
l= 3, ml= -3, ms= +1/2
14
Which sample has the largest volume? Densities: Al 2.7g/cm³ and Cu 9.0 g/cm³
1.0 g Al
5.0 g Al
1.0 g Cu
5.0 g Cu
15
Which compound contains the largest percent by mass of oxygen?
NO2
CO2
SiO2
SO2
16
Which element is more electronegative than arsenic and less electronegative then sulfur?
chlorine
tin
phosphorous
oxygen
17
What is an example of an oxidation-reduction reaction?
2H2O2(aq) -> O2(g) + 2H2O(l)
NaHCO3(s) + HCl(aq) -> NaCl(aq) + CO2(g) + H2O(l)
CaCO3(s) -> CaO(s) + CO2(g)
2Pb2+(aq) + Cr2O72-(aq) + H2O(l) -> 2PbCrO4(s) + 2H+(aq)
18
What molecule contains carbon with a negative formal charge?
H2CO-
CO2
CH4
CO
19
How many atoms are in 1.50g of Al?
2.44x1025
0.0556
3.35x1022
18.0
20
What volume (in mL) of a 0.0557 M Sr(OH)₂ solution is needed to neutralize 36.4 mL of a 0.0750 M HNO₃ solution?
98.0 mL
36.4 mL
24.5 mL
49.0 mL
21
How many neutrons are in ¹⁴₆C
7
8
6
20
22
What is the maximum mass of NO₂ (46.0 g/mol) formed when 7.5g of N₂O₅ (108.0 g/mol) are consumed? 2N₂O₅ -> 4NO₂ + O₂
3.2 g
1.6 g
6.4 g
15 g
23
Lithium has 2 isotopes, ⁶Li and ⁷Li, with masses of 6.015 amu and 7.016 amu. What is the relative abundance of each?
6Li=46.16% and 7Li=53.84%
6Li=25.31% and 7Li=74.69%
6Li=92.51% and 7Li=7.49%
6Li=7.49% and 7Li=92.51%
24
Which compound has the highest percent composition by mass of oxygen?
CaSO3
Li2CO3
CaCO3
Li2SO3
25
Arrange LiF, HCl, HF, and F₂ in order of increasing normal boiling point.
F2 < HF < HCl < LiF
F2 < HCl < LiF < HF
HF < LiF < HCl < F2
F2 < HCl < HF < LiF
26
Under the same conditions of temperature and pressure, hydrogen (H₂) diffuses _________ than oxygen (O₂).
eight times slower
sixteen times faster
two times slower
four times faster
27
Alkaline earth metals form
+1 ions
+2 ions
-1 ions
+3 ions
28
Which of these species (is/are) paramagnetic? Ti⁴⁺Fe²⁺ Zn
Fe2+ and Zn only
Ti4+ and Fe2+ only
Zn only
Fe2+ only
29
What amount of excess reagent remains when 4.0 g zinc reacts with 2.0 g phosphorus? 2Zn + 3P -> Zn₃P₂
1.3 g P
0.22 g Zn
4.2 g Zn
0.70 g P
30
The size of metal atoms
are smaller than those of the corresponding ions
generally increases progressively from top to bottom in a group
generally increases progressively from left to right in a period
do not change upon losing electrons
31
How much heat is required to convert 10.5 g of iron into Fe₂O₃? 2Fe + 3CO -> Fe₂O₃ + 3CO₂ ΔH=26.6 kJ/mol
5.04 kJ
2.52 kJ
1.76 kJ
13.4 kJ
32
Aluminum metal crystallizes in a face-centered cubic unit cell. How many aluminum atoms are in one unit cell?
7
2
4
14
33
A central atom has two lone pairs and three single bonds. What is the molecular geometry?
trigonal pyramidal
T-shaped
trigonal planar
tetrahedral
34
What is/are the spectator ion(s) in this reaction? HC₂H₃O₂(aq) + NaOH(aq) -> NaC₂H₃O₂(aq) + H₂O(l)
C2H3O2- only
H+ and OH-
Na+ only
Na+ and C2H3O2-
35
What is the mass percent of oxygen in Fe₂(SO₄)₃?
18.76%
30.80%
15.40%
48.01%
36
What amount of the excess reagent remains when 0.30 mol NH₃reacts with 0.40 mol O₂? 4NH₃ + 5O₂ -> 4NO + 6H₂O
0.10 mol NH3
0.025 mol NH3
0.10 mol O2
0.025 mol O2
37
All gases approach ideal behavior under conditions of
low density and high temperature
high density and low temperature
high density and high temperature
low density and low temperature
38
What is the mass percent of carbon in isooctane (C₈H₁₈), a common component of gasoline?
92.26%
84.12%
7.743%
15.88%
39
Which statement about this redox reaction is correct? 2MnO₄^-(aq) + 5H₂O₂(aq) + 6H⁺(aq) -> 2Mn²⁺(aq) + 5O₂(g) + 8H₂O(l)
only oxidation has taken place
H2O2 acts as a reducing agent
H2O2 acts as an oxidizing agent
O2 acts as the oxidant in this reaction
40
What is a weak acid in water?
HF
HBr
HI
HCl
41
How many sodium ions are in 25.0g of Na₂CO₃? (Molar mass Na₂CO₃=105.99 g/mol)
2.84x1023 ions
1.13x1020 ions
1.42x1023 ions
7.10x1020 ions
42
What is the name of Ti₃(PO₄)₄?
titanium phosphate
titanium (IV) phosphate
titanium tetraphosphate
titanium (III) phosphate
43
What is the correctly reported mass of water? Mass of water and beaker=29.62 g and mass of beaker=28.3220 g
1.298 g
1.30 g
1.3 g
1.2980 g
44
What is the final concentration when 28.2 mL of an 11.8 M solution is diluted to 100.0 mL?
4.18 M
0.333 M
3.33 M
2.82 M
45
THC contains 80.16% carbon, 9.63% hydrogen, and 10.17% oxygen by mass. What is the empirical formula of THC?
C8HO
C21H30O2
C30H3O5
C7H10O
46
What is the best procedure to prepare 0.500 L of a 0.200 M solution of Li₃PO₄? (LiPO₄=115.8 g/mol)
Weigh 11.6 g of solute and add 0.500 L of water
Weigh 23.2 g of solute and add 0.500 L of water
Weigh 11.6 g of solute and add water to obtain a final volume of 0.500 L
Weigh 23.2 g of solute and add water to obtain a final volume of 0.500 L
47
How many neutrons are in ³⁷₁₇Cl^-?
21
20
37
17
48
Which sample has the largest mass?
1 mole of Pb atoms
1 mole of marshmallows
1 mole of CO2 molecules
all of these have the same mass
49
What pure substance has the lowest vapor pressure at 25 °C?
H2O
CO2
H2S
O2
50
Which electronic transition in a hydrogen atom is associated with the largest emission of energy?
n=2 to n=1
n=2 to n=4
n=3 to n=2
n=2 to n=3
51
Which ionic compound has the largest magnitude lattice energy?
CaO
NaF
KBr
MgO
52
What is the work done if a system's internal energy increases 250 kJ after adding 375 kJ of heat?
125 kJ
-625 kJ
-125 kJ
625 kJ
53
What is the energy of a photon with a wavelength of (λ) of 656 nm?
3.03x10-19 J
3.03x10-28 J
4.35x10-40 J
4.35x10-31 J
54
Which element is an actinide?
Rb
Mo
U
Ga
55
Magnesium forms an ionic compound with an element with the formula MgX. Which ion could be X?
C4-
S2-
P3-
Br-
56
What mass of oxygen does 25.5g of Al₂(CO₃)₃ contain? (MM Al₂(CO₃)₃=233.99 g/mol)
1.74g
1.59g
15.7g
5.23g
57
The most abundant isotope (50.69%) of bromine is ⁷⁹₃₅Br of mass 78.9183 amu. What is the other isotope?
7936Br
8135Br
8136Br
8035Br
58
What is the maximum number of electrons that can occupy an orbital labeled d_xy?
4
1
2
3
59
In which compound does vanadium have the lowest oxidation state?
V2O3
VO2
V2O5
VO
60
What is the empirical formula for a compound that is comprised of 54.0% sodium, 8.50% boron, and 37.5% oxygen by mass?
Na3B2O2
Na4BO4
Na2B2O3
Na3BO3
61
Which combination will result in a precipitate forming?
Zn(s) and HCL(aq)
NaOH(aq) and HCl(aq)
NaNO3(aq) and FeCl3(aq)
NaOH(aq) and FeCl3(aq)
62
Which equation corresponds to the electron affinity of chlorine?
Cl(g) -> Cl+(g) + e-
Cl(g) + e- -> Cl-(g)
Cl2(g) + e- -> Cl2-(g)
Cl- (g) -> Cl(g) + e-
63
Which statement is true?
The atomic number of an element is the number of protons in one atom
The nucleus of an atom contains neutrons and electrons
The number of electrons is the same as the number of neutrons
The mass number is the number of protons plus the number of electrons
64
How many water molecules are produced if 0.34 mol of C₃H₈ combusts in excess oxygen? C₃H₈ + 5O₂ -> 3CO₂ + 4H₂O
2.1x1023
5.1x1022
8.2x1023
2.4x1024
65
Which compound contains a +1 ion?
KCl
NO
MgO
AlP
66
Which term best described the relation of hydrogen (¹H) to deuterium (²H)
allotropes
isomers
polymers
isotopes
67
Which molecule is polar?
PH3
PF5
CS2
CCl4
68
What is the oxidation number of chromium in Na₂Cr₂O₇?
+6
+12
+3
-2
69
Which of these atoms will be the smallest?
Si (Z=14)
Ge (Z=32)
P (Z=15)
As (Z=33)
70
What is the molar concentration of the chloride ion in a 3.0 M CaCl₂ solution?
1.5 M
6.0 M
1.0 M
3.0 M
71
Which ion has the same number of electrons as an argon atom?
Na+
Ne
Cl-
Mg2+
72
How many covalent bonds are represented in the formula NH₄Cl?
4
1
5
0
73
What is the density of F₂(g) at 1.00 atm and 25.0 °C
1.55 g/L
0.776 g/L
0.850 g/L
1.70 g/L
74
Which compound below contains a transition metal?
BF3
AlCl3
VO2
NaF
75
The halogens are found in group
15
1
17
18
76
A 3.41x10^-6 g sample is known to contain 4.67x10¹⁶ molecules. What is this compound?
H2O
CO2
NH3
CH4
77
Arrange CsBr, NaCl, and RbBr in increasing magnitude of lattice energy.
NaCl < RbBr < CsBr
CsBr < RbBr < NaCl
RbBr < CsBr < NaCl
CsBr < NaCl < RbBr
78
The formula of strontium hexafluorosilicate is SrSiF₆. What is the formula of aluminum hexafluorosilicate?
Al3(SiF6)2
Al2(SiF6)3
Al3SiF6
AlSiF6
79
Which molecular equation would give this net ionic equation? H⁺(aq) + OH^-(aq) -> H₂O(l)
H2SO4(aq) + 2NH3(aq) -> (NH4)2SO4(aq)
2HClO4(aq) + Ba(OH)2(aq) -> 2H2O(l) + Ba(ClO4)2(aq)
HCN(aq) + KOH(aq) -> H2O(l) + KCN(aq)
3HBr(aq) + Fe(OH)3(s) -> 3H2O(l) + FeBr3(aq)
80
Which element has the highest electronegativity?
oxygen
lithium
cesium
iodine
81
2 isotopes of element X exist with abundance of 30.00% ¹⁰⁰X and 70.00% ¹⁰¹X. What is the approximate atomic mass of X?
100.5 amu
100.7 amu
100.3 amu
101.0 amu
82
Which is an example of an oxidation-reduction reaction?
Pb(s) + PbO2(s) + 2H2SO4(aq) -> 2PbSO4(s) + 2H2O(l)
(NH4)2CO3(s) -> 2NH3(g) + CO2(g) + H2O(g)
Pb(NO3)2(aq) + Na2SO4(aq) -> PbSO4(s) + 2NaNO3(aq)
HCl(aq) + RbOH(aq) -> H2O(l) + RbCl (aq)
83
What is the correct name for N₂O₅
dinitrogen oxide
dinitrogen pentoxide
nitrogen (V) oxide
nitrogen (II) oxide
84
What is the formula for the compound formed when an aluminum ion, Al³⁺, combines with an oxide ion, O^2-?
Al2O3
AlO2
Al3O2
AlO
85
What happens when a bromine atom becomes a bromide ion?
The atomic number of bromine is decreased by one.
The bromide ion is then larger than the bromine atom.
A positive ion is formed.
The bromine nucleus acquires a negative charge.
86
What intermolecular forces are present in a pure sample of ethanol (C₂H₅OH)?
dispersion and dipole-dipole
hydrogen bonding and ion-dipole
dispersion, dipole-dipole, and hydrogen bonding
dispersion and ion-dipole
87
Which is NOT named correctly?
MnO2 - manganese (II) oxide
CaF2 - calcium fluoride
CuSO4 - copper (II) sulfate
Na3PO4 - sodium phosphate
88
What mass of FeS (87.92 g/mol) is needed to form 1.08 g Fe₂O₃ (159.7 g/mol) with excess O₂? 4FeS + 7O₂ -> 2Fe₂O₃ + 4SO₂
2.16 g
0.0136 g
1.19 g
0.298 g
89
How many moles of Ba₃N₂ are necessary to react with 1.5 mol of water? Ba₂N₂ + 6H₂O -> 3Ba(OH)₂ + 2NH₃
0.25 mol
9 mol
1 mol
6 mol
90
How many moles of hydrogen atoms are in six moles of Ca(OH)₂?
12
2
8
6
91
Which element is represented by ⁵⁶₂₄X_?
germanium
barium
chromium
iron
92
In a compound (NH₄)₂S₂O₃, which element is present in the largest percent by mass?
O
N
H
S
93
What is the ground-state electron configuration of the manganese atom, Mn?
1s22s22p63s23p63d7
1s22s22p63s23p64s24p5
1s22s22p63s23p63d54s2
1s22s22p63s23p64s24d5
94
What amount of excess reagent remains when 0.500 mol Li reacts with 0.350 mol N₂? 6Li + N₂ -> 2Li₃N
0.267 mol N2
0.417 mol Li
0.150 mol Li
0.0833 mol N2
95
A cup of coffee contains 95.0g caffeine, C₈H₁₀N₄O₂. How many caffeine molecules are in one cup? (C₈H₁₀N₄O₂=194.2 g/mol)
1.11x1025 molecules
2.95x1020 molecules
1.23x1027 molecules
3.06x10-23 molecules
96
A 0.152 mol sample of CH₂O₂is reacted and 38.7 kJ was released. What is the ΔH°? 2CH₂O₂ + O₂ -> 2CO₂ + 2H₂O
-509 kJ/mol
509 kJ/mol
254 kJ/mol
-254 kJ/mol
97
When excited, a Na atom emits a photon of frequency 5.090x10¹⁴ s^-1. What is the energy associated with this emission?
3.90x10-50 J
3.90x10-48 J
3.37x10-19 J
3.37x10-28 J
98
25.0g of carbon dioxide contains ___ oxygen atoms. (Molar mass CO₂=44.0 g/mol)
6.80x1023
3.40x1023
1.00x1024
6.02x1023
99
What is the mass of 1.75 moles of Zn?
114g
65.4g
0.0268g
37.4g
100
What happens to the volume of a fixed amount of gas if both the pressure and absolute temperature are doubled?
doubles
quadruples
no change
halved
101
Which species has this ground-state electron arrangement? 1s²2s²2p⁶3s²3p⁶3d¹⁰
Zn
Ni
Ni2+
Zn2+
102
As intermolecular forces increase, enthalpy of vaporization ________ and vapor pressure __________.
decreases, increases
decreases, decreases
increases, increases
increases, decreases
103
What is the formula of sulfur trioxide?
SO3
SO2
SO3 2-
SO4 2-
104
Which reaction represents ΔH°_f for Al₂O₃(s)?
2Al(s) + 3O(g) -> Al2O3(s)
4Al(s) + 3O2(g) -> 2Al2O3(s)
Al2(s) + O3(g) -> Al2O3(s)
2Al(s) + 3/2O2(g) -> Al2O3(s)
105
What is the oxidation number of chlorine in NaClO₂?
+5
-1
+1
+3
106
Which statement best describes ionic bonding in lithium fluoride?
A lithium atom shared one electron with a fluorine atom
The positive and negative charges of the ions cancel out
An electrostatic attraction exists between lithium ions and fluoride ions
An electron is transferred from a lithium atom to a fluorine atom
107
A silicon chip has a mass of 2.3x10^-4g. Assuming the chip is pure silicon, how many silicon atoms are in the chip?
3.9x1021
1.4x1020
2.6x1027
4.9x1018
108
Which sample deviates most from ideal gas behavior?
Xe at 200 atm and -50 °C
Xe at 1 atm and -50 °C
Xe at 200 atm and 1000 °C
He at 200 atm and -50 °C
109
In all neutral atoms, there are equal numbers of
neutrons and electrons
electrons and protons
positrons and electrons
protons and neutrons
110
A pair of isotopes has
the same number of neutrons and the same number of electrons
the same number of protons and a different number of neutrons
the same number of protons and the same number of neutrons
the same number of protons and neutrons but a different number of electrons
111
The standard enthalpy of formation, ΔH°_f, for NO₂(g) is the enthalpy change for which reaction?
N(g) + 2O(g) -> NO2(g)
1/2 N2(g) + O2(g) -> NO2(g)
NO(g) + 1/2 O2(g) -> NO2(g)
1/2 N2O4(g) -> NO2(g)
112
The limiting reagent for a given reaction can be recognized because it is the reagent that
would be used up first
has the smallest coefficient in the balanced equation of the reaction
has the smallest mass in the reaction mixture
is present in the smallest molar quantity
113
What amount of Al₂O₃ is produced from the reaction of 3.0 mol Al with 2.0 mol Fe₂O₃? 2Al + Fe₂O₃ -> Al₂O₃ + 2Fe
1.5 mol
3.0 mol
6.0 mol
2.0 mol
114
What volume of 0.100 M HCl is needed to neutralize 25.0 mL of 0.100 M Ba(OH)₂? 2HCl + Ba(OH)₂ -> BaCl₂ + 2H₂O
25.0 mL
0.250 mL
50.0 mL
12.5 mL
115
What is the valence electron configuration for the element in Period 5, Group 3A?
3s23p5
5s25p1
3s23p3
5s25p3
116
Suppose a gas mixture contains equal moles of He(g) and O₂(g). Which is true?
The partial pressure of each gas is the same
The partial pressure of He(g) is four times the partial pressure of O2(g)
The partial pressure of O2(g) is eight times the partial pressure of He(g)
The partial pressure O2(g) is two times the partial pressure of He(g)
117
Which pair of particles has the same number of electrons?
Ne, Ar
Al3+, P3-
F-, Mg2+
Br-, Se
118
Which statement below is correct?
Sodium is a metalloid
Chlorine is a transition metal
Oxygen is a metal
Phosphorous
119
The best Lewis structure of N₂H₂ shows
a nitrogen-nitrogen single bond
a nitrogen-nitrogen triple bond
each nitrogen with one nonbonding electron pair
each nitrogen with two nonbonding electron pairs
120
How many valence electrons are in the carbonate ion, CO₃^2-?
20
32
24
22
121
Which compound contains the greatest percentage of nitrogen?
KNO2
KNO3
NaNO2
NaNO3
122
What is the percent by mass of oxygen in Ca(NO₃)₂?
47.1%
29.3%
58.5%
94.1%
123
The species F^-, Mg²⁺, and Na⁺ all have the same number of electrons. Arrange them in order of decreasing size.
Mg2+ > F- > Na+
Na+ > Mg2+ > F-
F- > Mg2+ > Na+
F- > Na+ > Mg2+
124
Which ion has the largest radius?
F-
K+
Cu2+
Cl-
125
What is the oxidizing agent in this reaction? Pt²⁺(aq) + CH₃CH₂OH(aq) -> CH₃CHO(aq) + Pt(s) + 2H⁺(aq)
Pt(s)
Pt2+(aq)
H+(aq)
CH3CH2OH(aq)
126
What mass of NO₂ is formed by the reaction of 2 mol O₃ with excess NO? O₃ + NO -> O₂ + NO₂
46.0g
23.0g
96.0g
92.0g
127
Which element is an alkali metal?
K
V
Mg
Fe
128
A molecule of a compound has a mass of 2.4x10^-22g. Which value comes closest to the mass of a mole of this compound?
100 g/mol
150 g/mol
50 g/mol
200 g/mol
129
The number of atoms in 9.0g of aluminum is the same as the number of atoms in
9.0g of Mg
18.0g of Mg
12.1g of Mg
8.1g of Mg
130
When this equation is balanced, what is the coefficient for N₂? _N₂H₄ + _N₂O₄ -> _N₂ + _H₂O
2
1
4
3
131
A 2.32 g sample of Na₂SO₄*nH₂O yields 1.42 g Na₂SO₄ (142 g/mol). What is the value of n? Na₂SO₄*nH₂O -> Na₂SO₄ + nH₂O
5
2
3
10
132
A 10.000g sample of water contains 11.19% H by mass. What should by the %H in a 20.000g sample of water?
22.38%
5.560%
88.81%
11.19%
133
A 14.0 g sample of N₂(g) occupies what volume at 0 °C and 1.00 atm?
11.2 L
22.4 L
14.0 L
5.60 L
134
Which ion is the smallest?
Al3+
F-
Na+
O2-
135
Which emission line in the hydrogen spectrum occurs at the highest frequency?
n=10 to n=8
n=3 to n=1
n=4 to n=2
n=7 to n=5
136
In a 10.0 L vessel at 100.0 °C, 10.0 grams of an unknown gas exert a pressure of 1.13 atm. What is the gas?
NH3; MW= 17 g/mol
HCN; MW=27 g/mol
NO2; MW= 46 g/mol
NO; MW= 39 g/mol
137
How many moles of water are needed to react with 8.0 mol PCl₅? PCl₅ + 4H₂O -> H₃PO₄ + 5HCl
2.0 mol
16 mol
32 mol
8.0 mol
138
What particles would be present in NH₃(aq)?
water molecules, NH4+ ions and OH- ions
water molecules, H3O+ ions and NH2- ions
water molecules, NH3 molecules and a small number of NH4+ ions and OH- ions
water molecules and NH3 molecules
139
Which substance has the lowest boiling point?
CCl4
CI4
CH4
CBr4
140
How many moles of iron are necessary to react completely with 1.75 mol of oxygen gas? 3O₂(g) + 4Fe(s) -> 2FeO₃(s)
2.33 mol
1.31 mol
5.25 mol
1.75 mol
141
What is a main group element?
Fe
Mg
Pu
Sc
142
A sample of gas occupies 3.00 L at 1.00 atm. What volume will it occupy at 1.45 atm and the same temperature?
4.35 L
2.07 L
2280 L
1572.4 L
143
What mass of oxygen is in 200. mg dose of Guaifenesin (C₁₀H₁₄O₄)? (Molar mass C₁₀H₁₄O₄=198.2 g/mol)
3.20 g
0.0161 g
0.0646 g
0.00403 g
144
Which ion has 26 electrons?
Ni2+
Fe2+
Cu2+
Cr2+
145
An atom of Fe has two 4s electrons and six 3d electrons. How many unpaired electrons would there be in a Fe²⁺ ion?
4
3
2
1
146
Which gas is most dense at 2 atm and 400K?
O2
F2
N2
Ne
147
What are the coefficients for each substance in the chemical reaction when balanced? _C₇H₁₄O₂+ _O₂-> _CO₂+ _H₂O
1, 10, 7, 7
2, 19, 14, 14
2, 19, 7, 7
2, 21, 14, 14
148
What is the amount of ammonia that can be produced when 0.35 mol N₂ reacts with 0.90 mol H₂? N₂ + 3H₂ -> 2NH₃
1.4 mol NH3
0.18 mol NH3
0.70 mol NH3
0.60 mol NH3
149
A 10g sample of which substance contains the greatest number of hydrogen atoms?
10g of PH3
10g of H2
10g of HCl
10g of Mg
150
What mass of Sn is formed by the reaction of 1.75 mol H₂ with excess SnO₂? SnO₂ + H₂ -> Sn + 2H₂O
151 g
301 g
104 g
527 g
151
Which electron configuration is impossible?
1s22s22p62d2
1s22s22p63s23p64s24d5
1s22s22p63s23p6
1s22s22p53s1
152
Which group contains nonmetals, metalloids, and metals?
18
1
13
15
153
Which atom has the most neutrons?
neon-20
phosphorous-32
chlorine-35
sulfur-35
154
What is the balanced net ionic equation for the reaction of CuCl₂(aq) and H₂(g)?
CuCl2(aq) + H2(g) -> Cu(s) + 2HCl(aq)
Cu2+(aq) + 2Cl-(aq) + H2(g) -> Cu(s) + 2H+(aq) + 2Cl-(aq)
Cu2+(aq) + H2(g) -> Cu(s) + 2H+(aq)
Cu2+(aq) + Cl2(aq) + H2(g) -> Cu(s) + 2H+(aq) + 2Cl-(aq)
155
Which of these elements has the smallest atomic radius?
bromine
chlorine
fluorine
iodine
156
SCl₂ has __________ bonds and overall the molecule is ________.
nonpolar, polar
polar, nonpolar
polar, polar
nonpolar, nonpolar
157
What is the empirical formula of a compound of carbon (51.56%), hydrogen (14.09%), and oxygen?
C8H13O2
C2H7O
C7H2O5
C4H13O2
158
What is the name of HBrO₄(aq)?
bromic acid
bromous acid
perbromic acid
hydrobromic acid
159
A sodium ion differs from a sodium atom in that the sodium ion
has fewer electrons
exists only in solution
has a negative charge on its nucleus
is an isotope of sodium
160
What is the molar concentration of a solution when 7.00 mL of a 3.25 M aqueous solution is diluted to 25.00 mL?
2.15 M
0.280 M
1.10 M
0.910 M
161
In which reaction is carbon reduced?
CO(g) + O2(g) -> CO2(g)
CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)
CO2(g) + H2O(l) -> H2CO3(aq)
C2H2(g) + H2(g) -> C2H4(g)
162
Why is the boiling point of Br₂ higher than that of Cl₂?
Br2 has greater molar mass and is therefore easier to vaporize
Br is more electronegative and therefore has greater dipole-dipole forces
Br2 is more polarizable and therefore has greater London dispersion forces
Br is less electronegative and therefore its bonding is more ionic
163
What is the strongest electrolyte in dilute aqueous solution?
HF
HCN
HClO4
HNO2
164
What mass of SbF₃ (179g/mol) is needed to produce 1.00 g CCl₂F₂ (121 g/mol)? 3CCl₄ + 2 SbF₃ -> 3CCl₂F₂ + 2SbCl₃
0.986 g
0.667 g
1.48 g
2.22 g
165
The density of helium is 0.164 kg/m³. What is this density in lb/ft³? 1 kg=2.20 lb and 1 m=3.28 ft
0.0102 lb/ft3
1.18 lb/ft3
12.7 lb/ft3
0.110 lb/ft3
166
What molecule has a 120° bond angle?
NH3
CO2
SO3
IF3
167
What solution volume is needed to prepare a 0.110 M solution of MgSO₄ using 10.3 g of the compound? (MgSO₄=120.36 g/mol)
1.11 L
0.778 L
9.41x10-3 L
93.6 L

CHEM 120 ACS Review Flashcards | StudBud

CHEM 120 ACS Review

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Questions 167

Answers

1
What are the coefficients for each substance in the chemical reaction when balanced? _CH₄ + _O₂ -> _CO₂ + _H₂O
1, 3, 1, 2
2, 4, 2, 4
4, 2, 2, 2
1, 2, 1, 2
2
The speed of light is 3.0x10⁸ m/s. What is the speed in nm/ms?
3.0x10-4 nm/ms
3.0x102 nm/ms
3.0x1020 nm/ms
3.0x1014 nm/ms
3
A sample of ethanol (C₂H₆O) contains 3.024g hydrogen. How many moles of carbon are in the sample? (ethanol=46.07 g/mol)
0.1667
8.333x10-2
0.2500
0.09980
4
Which element contains a Group 14 metal?
GeF4
SnCl2
ZnCl2
CCl4
5
If a nanoparticle has a density of 12.0g/cm³, what is the mass of a nanoparticle with a volume of 1.84x10^-21cm³?
2.21x10-20 g
1.63x10-20 g
1.53x10-22 g
6.52x10-21 g
6
If gallium combines with selenium what is the most likely formula based on your knowledge of periodic table elements?
GaSe
GaSe2
Ga2Se
Ga2Se3
7
Which ground state electron configuration is possible for an atom in the second period?
1s22p4
1s22s22d1
1s22s1
1s21s12p1
8
What mass of nitrogen is in 7.43x10^-4 moles of 3TC (C₈H₁₁N₃O₃S)? (Molar mass C₈H₁₁N₃O₃S=229.26 g/mol)
3.12x10-2 g
1.70x10-1 g
5.11x10-1 g
3.47x10-3 g
9
What is the coefficient for ZnO when the reaction is balanced? _ZnS + _O₂ -> _ZnO + _SO₂
2
3
4
1
10
What is the wavelength of a photon with an energy of 6.51x10^-19 J
1.00x1015 nm
3.05x10-9 nm
4.52x1026 nm
305 nm
11
When 1.0 M aqueous solutions of KI, NaC₂H₃O₂, and Pb(NO₃)₂ are mixed together, what precipitate forms?
PbI2
NaNO3
KC2H3O2
Pb(C2H3O2)2
12
What are the coefficients for each substance in the chemical reaction when balanced? _NaBr + _Cl₂ -> _NaCl + _Br₂
1, 2, 2, 2
1, 1, 2, 2
2, 1, 2, 1
2, 4, 2, 4
13
Which set of quantum numbers is correct and consistent with n=4?
l=4, ml= +2, ms= -1/2
l= 2, ml= +3, ms= +1/2
l= 3, ml= -3, ms= +1
l= 3, ml= -3, ms= +1/2
14
Which sample has the largest volume? Densities: Al 2.7g/cm³ and Cu 9.0 g/cm³
1.0 g Al
5.0 g Al
1.0 g Cu
5.0 g Cu
15
Which compound contains the largest percent by mass of oxygen?
NO2
CO2
SiO2
SO2
16
Which element is more electronegative than arsenic and less electronegative then sulfur?
chlorine
tin
phosphorous
oxygen
17
What is an example of an oxidation-reduction reaction?
2H2O2(aq) -> O2(g) + 2H2O(l)
NaHCO3(s) + HCl(aq) -> NaCl(aq) + CO2(g) + H2O(l)
CaCO3(s) -> CaO(s) + CO2(g)
2Pb2+(aq) + Cr2O72-(aq) + H2O(l) -> 2PbCrO4(s) + 2H+(aq)
18
What molecule contains carbon with a negative formal charge?
H2CO-
CO2
CH4
CO
19
How many atoms are in 1.50g of Al?
2.44x1025
0.0556
3.35x1022
18.0
20
What volume (in mL) of a 0.0557 M Sr(OH)₂ solution is needed to neutralize 36.4 mL of a 0.0750 M HNO₃ solution?
98.0 mL
36.4 mL
24.5 mL
49.0 mL
21
How many neutrons are in ¹⁴₆C
7
8
6
20
22
What is the maximum mass of NO₂ (46.0 g/mol) formed when 7.5g of N₂O₅ (108.0 g/mol) are consumed? 2N₂O₅ -> 4NO₂ + O₂
3.2 g
1.6 g
6.4 g
15 g
23
Lithium has 2 isotopes, ⁶Li and ⁷Li, with masses of 6.015 amu and 7.016 amu. What is the relative abundance of each?
6Li=46.16% and 7Li=53.84%
6Li=25.31% and 7Li=74.69%
6Li=92.51% and 7Li=7.49%
6Li=7.49% and 7Li=92.51%
24
Which compound has the highest percent composition by mass of oxygen?
CaSO3
Li2CO3
CaCO3
Li2SO3
25
Arrange LiF, HCl, HF, and F₂ in order of increasing normal boiling point.
F2 < HF < HCl < LiF
F2 < HCl < LiF < HF
HF < LiF < HCl < F2
F2 < HCl < HF < LiF
26
Under the same conditions of temperature and pressure, hydrogen (H₂) diffuses _________ than oxygen (O₂).
eight times slower
sixteen times faster
two times slower
four times faster
27
Alkaline earth metals form
+1 ions
+2 ions
-1 ions
+3 ions
28
Which of these species (is/are) paramagnetic? Ti⁴⁺Fe²⁺ Zn
Fe2+ and Zn only
Ti4+ and Fe2+ only
Zn only
Fe2+ only
29
What amount of excess reagent remains when 4.0 g zinc reacts with 2.0 g phosphorus? 2Zn + 3P -> Zn₃P₂
1.3 g P
0.22 g Zn
4.2 g Zn
0.70 g P
30
The size of metal atoms
are smaller than those of the corresponding ions
generally increases progressively from top to bottom in a group
generally increases progressively from left to right in a period
do not change upon losing electrons
31
How much heat is required to convert 10.5 g of iron into Fe₂O₃? 2Fe + 3CO -> Fe₂O₃ + 3CO₂ ΔH=26.6 kJ/mol
5.04 kJ
2.52 kJ
1.76 kJ
13.4 kJ
32
Aluminum metal crystallizes in a face-centered cubic unit cell. How many aluminum atoms are in one unit cell?
7
2
4
14
33
A central atom has two lone pairs and three single bonds. What is the molecular geometry?
trigonal pyramidal
T-shaped
trigonal planar
tetrahedral
34
What is/are the spectator ion(s) in this reaction? HC₂H₃O₂(aq) + NaOH(aq) -> NaC₂H₃O₂(aq) + H₂O(l)
C2H3O2- only
H+ and OH-
Na+ only
Na+ and C2H3O2-
35
What is the mass percent of oxygen in Fe₂(SO₄)₃?
18.76%
30.80%
15.40%
48.01%
36
What amount of the excess reagent remains when 0.30 mol NH₃reacts with 0.40 mol O₂? 4NH₃ + 5O₂ -> 4NO + 6H₂O
0.10 mol NH3
0.025 mol NH3
0.10 mol O2
0.025 mol O2
37
All gases approach ideal behavior under conditions of
low density and high temperature
high density and low temperature
high density and high temperature
low density and low temperature
38
What is the mass percent of carbon in isooctane (C₈H₁₈), a common component of gasoline?
92.26%
84.12%
7.743%
15.88%
39
Which statement about this redox reaction is correct? 2MnO₄^-(aq) + 5H₂O₂(aq) + 6H⁺(aq) -> 2Mn²⁺(aq) + 5O₂(g) + 8H₂O(l)
only oxidation has taken place
H2O2 acts as a reducing agent
H2O2 acts as an oxidizing agent
O2 acts as the oxidant in this reaction
40
What is a weak acid in water?
HF
HBr
HI
HCl
41
How many sodium ions are in 25.0g of Na₂CO₃? (Molar mass Na₂CO₃=105.99 g/mol)
2.84x1023 ions
1.13x1020 ions
1.42x1023 ions
7.10x1020 ions
42
What is the name of Ti₃(PO₄)₄?
titanium phosphate
titanium (IV) phosphate
titanium tetraphosphate
titanium (III) phosphate
43
What is the correctly reported mass of water? Mass of water and beaker=29.62 g and mass of beaker=28.3220 g
1.298 g
1.30 g
1.3 g
1.2980 g
44
What is the final concentration when 28.2 mL of an 11.8 M solution is diluted to 100.0 mL?
4.18 M
0.333 M
3.33 M
2.82 M
45
THC contains 80.16% carbon, 9.63% hydrogen, and 10.17% oxygen by mass. What is the empirical formula of THC?
C8HO
C21H30O2
C30H3O5
C7H10O
46
What is the best procedure to prepare 0.500 L of a 0.200 M solution of Li₃PO₄? (LiPO₄=115.8 g/mol)
Weigh 11.6 g of solute and add 0.500 L of water
Weigh 23.2 g of solute and add 0.500 L of water
Weigh 11.6 g of solute and add water to obtain a final volume of 0.500 L
Weigh 23.2 g of solute and add water to obtain a final volume of 0.500 L
47
How many neutrons are in ³⁷₁₇Cl^-?
21
20
37
17
48
Which sample has the largest mass?
1 mole of Pb atoms
1 mole of marshmallows
1 mole of CO2 molecules
all of these have the same mass
49
What pure substance has the lowest vapor pressure at 25 °C?
H2O
CO2
H2S
O2
50
Which electronic transition in a hydrogen atom is associated with the largest emission of energy?
n=2 to n=1
n=2 to n=4
n=3 to n=2
n=2 to n=3
51
Which ionic compound has the largest magnitude lattice energy?
CaO
NaF
KBr
MgO
52
What is the work done if a system's internal energy increases 250 kJ after adding 375 kJ of heat?
125 kJ
-625 kJ
-125 kJ
625 kJ
53
What is the energy of a photon with a wavelength of (λ) of 656 nm?
3.03x10-19 J
3.03x10-28 J
4.35x10-40 J
4.35x10-31 J
54
Which element is an actinide?
Rb
Mo
U
Ga
55
Magnesium forms an ionic compound with an element with the formula MgX. Which ion could be X?
C4-
S2-
P3-
Br-
56
What mass of oxygen does 25.5g of Al₂(CO₃)₃ contain? (MM Al₂(CO₃)₃=233.99 g/mol)
1.74g
1.59g
15.7g
5.23g
57
The most abundant isotope (50.69%) of bromine is ⁷⁹₃₅Br of mass 78.9183 amu. What is the other isotope?
7936Br
8135Br
8136Br
8035Br
58
What is the maximum number of electrons that can occupy an orbital labeled d_xy?
4
1
2
3
59
In which compound does vanadium have the lowest oxidation state?
V2O3
VO2
V2O5
VO
60
What is the empirical formula for a compound that is comprised of 54.0% sodium, 8.50% boron, and 37.5% oxygen by mass?
Na3B2O2
Na4BO4
Na2B2O3
Na3BO3
61
Which combination will result in a precipitate forming?
Zn(s) and HCL(aq)
NaOH(aq) and HCl(aq)
NaNO3(aq) and FeCl3(aq)
NaOH(aq) and FeCl3(aq)
62
Which equation corresponds to the electron affinity of chlorine?
Cl(g) -> Cl+(g) + e-
Cl(g) + e- -> Cl-(g)
Cl2(g) + e- -> Cl2-(g)
Cl- (g) -> Cl(g) + e-
63
Which statement is true?
The atomic number of an element is the number of protons in one atom
The nucleus of an atom contains neutrons and electrons
The number of electrons is the same as the number of neutrons
The mass number is the number of protons plus the number of electrons
64
How many water molecules are produced if 0.34 mol of C₃H₈ combusts in excess oxygen? C₃H₈ + 5O₂ -> 3CO₂ + 4H₂O
2.1x1023
5.1x1022
8.2x1023
2.4x1024
65
Which compound contains a +1 ion?
KCl
NO
MgO
AlP
66
Which term best described the relation of hydrogen (¹H) to deuterium (²H)
allotropes
isomers
polymers
isotopes
67
Which molecule is polar?
PH3
PF5
CS2
CCl4
68
What is the oxidation number of chromium in Na₂Cr₂O₇?
+6
+12
+3
-2
69
Which of these atoms will be the smallest?
Si (Z=14)
Ge (Z=32)
P (Z=15)
As (Z=33)
70
What is the molar concentration of the chloride ion in a 3.0 M CaCl₂ solution?
1.5 M
6.0 M
1.0 M
3.0 M
71
Which ion has the same number of electrons as an argon atom?
Na+
Ne
Cl-
Mg2+
72
How many covalent bonds are represented in the formula NH₄Cl?
4
1
5
0
73
What is the density of F₂(g) at 1.00 atm and 25.0 °C
1.55 g/L
0.776 g/L
0.850 g/L
1.70 g/L
74
Which compound below contains a transition metal?
BF3
AlCl3
VO2
NaF
75
The halogens are found in group
15
1
17
18
76
A 3.41x10^-6 g sample is known to contain 4.67x10¹⁶ molecules. What is this compound?
H2O
CO2
NH3
CH4
77
Arrange CsBr, NaCl, and RbBr in increasing magnitude of lattice energy.
NaCl < RbBr < CsBr
CsBr < RbBr < NaCl
RbBr < CsBr < NaCl
CsBr < NaCl < RbBr
78
The formula of strontium hexafluorosilicate is SrSiF₆. What is the formula of aluminum hexafluorosilicate?
Al3(SiF6)2
Al2(SiF6)3
Al3SiF6
AlSiF6
79
Which molecular equation would give this net ionic equation? H⁺(aq) + OH^-(aq) -> H₂O(l)
H2SO4(aq) + 2NH3(aq) -> (NH4)2SO4(aq)
2HClO4(aq) + Ba(OH)2(aq) -> 2H2O(l) + Ba(ClO4)2(aq)
HCN(aq) + KOH(aq) -> H2O(l) + KCN(aq)
3HBr(aq) + Fe(OH)3(s) -> 3H2O(l) + FeBr3(aq)
80
Which element has the highest electronegativity?
oxygen
lithium
cesium
iodine
81
2 isotopes of element X exist with abundance of 30.00% ¹⁰⁰X and 70.00% ¹⁰¹X. What is the approximate atomic mass of X?
100.5 amu
100.7 amu
100.3 amu
101.0 amu
82
Which is an example of an oxidation-reduction reaction?
Pb(s) + PbO2(s) + 2H2SO4(aq) -> 2PbSO4(s) + 2H2O(l)
(NH4)2CO3(s) -> 2NH3(g) + CO2(g) + H2O(g)
Pb(NO3)2(aq) + Na2SO4(aq) -> PbSO4(s) + 2NaNO3(aq)
HCl(aq) + RbOH(aq) -> H2O(l) + RbCl (aq)
83
What is the correct name for N₂O₅
dinitrogen oxide
dinitrogen pentoxide
nitrogen (V) oxide
nitrogen (II) oxide
84
What is the formula for the compound formed when an aluminum ion, Al³⁺, combines with an oxide ion, O^2-?
Al2O3
AlO2
Al3O2
AlO
85
What happens when a bromine atom becomes a bromide ion?
The atomic number of bromine is decreased by one.
The bromide ion is then larger than the bromine atom.
A positive ion is formed.
The bromine nucleus acquires a negative charge.
86
What intermolecular forces are present in a pure sample of ethanol (C₂H₅OH)?
dispersion and dipole-dipole
hydrogen bonding and ion-dipole
dispersion, dipole-dipole, and hydrogen bonding
dispersion and ion-dipole
87
Which is NOT named correctly?
MnO2 - manganese (II) oxide
CaF2 - calcium fluoride
CuSO4 - copper (II) sulfate
Na3PO4 - sodium phosphate
88
What mass of FeS (87.92 g/mol) is needed to form 1.08 g Fe₂O₃ (159.7 g/mol) with excess O₂? 4FeS + 7O₂ -> 2Fe₂O₃ + 4SO₂
2.16 g
0.0136 g
1.19 g
0.298 g
89
How many moles of Ba₃N₂ are necessary to react with 1.5 mol of water? Ba₂N₂ + 6H₂O -> 3Ba(OH)₂ + 2NH₃
0.25 mol
9 mol
1 mol
6 mol
90
How many moles of hydrogen atoms are in six moles of Ca(OH)₂?
12
2
8
6
91
Which element is represented by ⁵⁶₂₄X_?
germanium
barium
chromium
iron
92
In a compound (NH₄)₂S₂O₃, which element is present in the largest percent by mass?
O
N
H
S
93
What is the ground-state electron configuration of the manganese atom, Mn?
1s22s22p63s23p63d7
1s22s22p63s23p64s24p5
1s22s22p63s23p63d54s2
1s22s22p63s23p64s24d5
94
What amount of excess reagent remains when 0.500 mol Li reacts with 0.350 mol N₂? 6Li + N₂ -> 2Li₃N
0.267 mol N2
0.417 mol Li
0.150 mol Li
0.0833 mol N2
95
A cup of coffee contains 95.0g caffeine, C₈H₁₀N₄O₂. How many caffeine molecules are in one cup? (C₈H₁₀N₄O₂=194.2 g/mol)
1.11x1025 molecules
2.95x1020 molecules
1.23x1027 molecules
3.06x10-23 molecules
96
A 0.152 mol sample of CH₂O₂is reacted and 38.7 kJ was released. What is the ΔH°? 2CH₂O₂ + O₂ -> 2CO₂ + 2H₂O
-509 kJ/mol
509 kJ/mol
254 kJ/mol
-254 kJ/mol
97
When excited, a Na atom emits a photon of frequency 5.090x10¹⁴ s^-1. What is the energy associated with this emission?
3.90x10-50 J
3.90x10-48 J
3.37x10-19 J
3.37x10-28 J
98
25.0g of carbon dioxide contains ___ oxygen atoms. (Molar mass CO₂=44.0 g/mol)
6.80x1023
3.40x1023
1.00x1024
6.02x1023
99
What is the mass of 1.75 moles of Zn?
114g
65.4g
0.0268g
37.4g
100
What happens to the volume of a fixed amount of gas if both the pressure and absolute temperature are doubled?
doubles
quadruples
no change
halved
101
Which species has this ground-state electron arrangement? 1s²2s²2p⁶3s²3p⁶3d¹⁰
Zn
Ni
Ni2+
Zn2+
102
As intermolecular forces increase, enthalpy of vaporization ________ and vapor pressure __________.
decreases, increases
decreases, decreases
increases, increases
increases, decreases
103
What is the formula of sulfur trioxide?
SO3
SO2
SO3 2-
SO4 2-
104
Which reaction represents ΔH°_f for Al₂O₃(s)?
2Al(s) + 3O(g) -> Al2O3(s)
4Al(s) + 3O2(g) -> 2Al2O3(s)
Al2(s) + O3(g) -> Al2O3(s)
2Al(s) + 3/2O2(g) -> Al2O3(s)
105
What is the oxidation number of chlorine in NaClO₂?
+5
-1
+1
+3
106
Which statement best describes ionic bonding in lithium fluoride?
A lithium atom shared one electron with a fluorine atom
The positive and negative charges of the ions cancel out
An electrostatic attraction exists between lithium ions and fluoride ions
An electron is transferred from a lithium atom to a fluorine atom
107
A silicon chip has a mass of 2.3x10^-4g. Assuming the chip is pure silicon, how many silicon atoms are in the chip?
3.9x1021
1.4x1020
2.6x1027
4.9x1018
108
Which sample deviates most from ideal gas behavior?
Xe at 200 atm and -50 °C
Xe at 1 atm and -50 °C
Xe at 200 atm and 1000 °C
He at 200 atm and -50 °C
109
In all neutral atoms, there are equal numbers of
neutrons and electrons
electrons and protons
positrons and electrons
protons and neutrons
110
A pair of isotopes has
the same number of neutrons and the same number of electrons
the same number of protons and a different number of neutrons
the same number of protons and the same number of neutrons
the same number of protons and neutrons but a different number of electrons
111
The standard enthalpy of formation, ΔH°_f, for NO₂(g) is the enthalpy change for which reaction?
N(g) + 2O(g) -> NO2(g)
1/2 N2(g) + O2(g) -> NO2(g)
NO(g) + 1/2 O2(g) -> NO2(g)
1/2 N2O4(g) -> NO2(g)
112
The limiting reagent for a given reaction can be recognized because it is the reagent that
would be used up first
has the smallest coefficient in the balanced equation of the reaction
has the smallest mass in the reaction mixture
is present in the smallest molar quantity
113
What amount of Al₂O₃ is produced from the reaction of 3.0 mol Al with 2.0 mol Fe₂O₃? 2Al + Fe₂O₃ -> Al₂O₃ + 2Fe
1.5 mol
3.0 mol
6.0 mol
2.0 mol
114
What volume of 0.100 M HCl is needed to neutralize 25.0 mL of 0.100 M Ba(OH)₂? 2HCl + Ba(OH)₂ -> BaCl₂ + 2H₂O
25.0 mL
0.250 mL
50.0 mL
12.5 mL
115
What is the valence electron configuration for the element in Period 5, Group 3A?
3s23p5
5s25p1
3s23p3
5s25p3
116
Suppose a gas mixture contains equal moles of He(g) and O₂(g). Which is true?
The partial pressure of each gas is the same
The partial pressure of He(g) is four times the partial pressure of O2(g)
The partial pressure of O2(g) is eight times the partial pressure of He(g)
The partial pressure O2(g) is two times the partial pressure of He(g)
117
Which pair of particles has the same number of electrons?
Ne, Ar
Al3+, P3-
F-, Mg2+
Br-, Se
118
Which statement below is correct?
Sodium is a metalloid
Chlorine is a transition metal
Oxygen is a metal
Phosphorous
119
The best Lewis structure of N₂H₂ shows
a nitrogen-nitrogen single bond
a nitrogen-nitrogen triple bond
each nitrogen with one nonbonding electron pair
each nitrogen with two nonbonding electron pairs
120
How many valence electrons are in the carbonate ion, CO₃^2-?
20
32
24
22
121
Which compound contains the greatest percentage of nitrogen?
KNO2
KNO3
NaNO2
NaNO3
122
What is the percent by mass of oxygen in Ca(NO₃)₂?
47.1%
29.3%
58.5%
94.1%
123
The species F^-, Mg²⁺, and Na⁺ all have the same number of electrons. Arrange them in order of decreasing size.
Mg2+ > F- > Na+
Na+ > Mg2+ > F-
F- > Mg2+ > Na+
F- > Na+ > Mg2+
124
Which ion has the largest radius?
F-
K+
Cu2+
Cl-
125
What is the oxidizing agent in this reaction? Pt²⁺(aq) + CH₃CH₂OH(aq) -> CH₃CHO(aq) + Pt(s) + 2H⁺(aq)
Pt(s)
Pt2+(aq)
H+(aq)
CH3CH2OH(aq)
126
What mass of NO₂ is formed by the reaction of 2 mol O₃ with excess NO? O₃ + NO -> O₂ + NO₂
46.0g
23.0g
96.0g
92.0g
127
Which element is an alkali metal?
K
V
Mg
Fe
128
A molecule of a compound has a mass of 2.4x10^-22g. Which value comes closest to the mass of a mole of this compound?
100 g/mol
150 g/mol
50 g/mol
200 g/mol
129
The number of atoms in 9.0g of aluminum is the same as the number of atoms in
9.0g of Mg
18.0g of Mg
12.1g of Mg
8.1g of Mg
130
When this equation is balanced, what is the coefficient for N₂? _N₂H₄ + _N₂O₄ -> _N₂ + _H₂O
2
1
4
3
131
A 2.32 g sample of Na₂SO₄*nH₂O yields 1.42 g Na₂SO₄ (142 g/mol). What is the value of n? Na₂SO₄*nH₂O -> Na₂SO₄ + nH₂O
5
2
3
10
132
A 10.000g sample of water contains 11.19% H by mass. What should by the %H in a 20.000g sample of water?
22.38%
5.560%
88.81%
11.19%
133
A 14.0 g sample of N₂(g) occupies what volume at 0 °C and 1.00 atm?
11.2 L
22.4 L
14.0 L
5.60 L
134
Which ion is the smallest?
Al3+
F-
Na+
O2-
135
Which emission line in the hydrogen spectrum occurs at the highest frequency?
n=10 to n=8
n=3 to n=1
n=4 to n=2
n=7 to n=5
136
In a 10.0 L vessel at 100.0 °C, 10.0 grams of an unknown gas exert a pressure of 1.13 atm. What is the gas?
NH3; MW= 17 g/mol
HCN; MW=27 g/mol
NO2; MW= 46 g/mol
NO; MW= 39 g/mol
137
How many moles of water are needed to react with 8.0 mol PCl₅? PCl₅ + 4H₂O -> H₃PO₄ + 5HCl
2.0 mol
16 mol
32 mol
8.0 mol
138
What particles would be present in NH₃(aq)?
water molecules, NH4+ ions and OH- ions
water molecules, H3O+ ions and NH2- ions
water molecules, NH3 molecules and a small number of NH4+ ions and OH- ions
water molecules and NH3 molecules
139
Which substance has the lowest boiling point?
CCl4
CI4
CH4
CBr4
140
How many moles of iron are necessary to react completely with 1.75 mol of oxygen gas? 3O₂(g) + 4Fe(s) -> 2FeO₃(s)
2.33 mol
1.31 mol
5.25 mol
1.75 mol
141
What is a main group element?
Fe
Mg
Pu
Sc
142
A sample of gas occupies 3.00 L at 1.00 atm. What volume will it occupy at 1.45 atm and the same temperature?
4.35 L
2.07 L
2280 L
1572.4 L
143
What mass of oxygen is in 200. mg dose of Guaifenesin (C₁₀H₁₄O₄)? (Molar mass C₁₀H₁₄O₄=198.2 g/mol)
3.20 g
0.0161 g
0.0646 g
0.00403 g
144
Which ion has 26 electrons?
Ni2+
Fe2+
Cu2+
Cr2+
145
An atom of Fe has two 4s electrons and six 3d electrons. How many unpaired electrons would there be in a Fe²⁺ ion?
4
3
2
1
146
Which gas is most dense at 2 atm and 400K?
O2
F2
N2
Ne
147
What are the coefficients for each substance in the chemical reaction when balanced? _C₇H₁₄O₂+ _O₂-> _CO₂+ _H₂O
1, 10, 7, 7
2, 19, 14, 14
2, 19, 7, 7
2, 21, 14, 14
148
What is the amount of ammonia that can be produced when 0.35 mol N₂ reacts with 0.90 mol H₂? N₂ + 3H₂ -> 2NH₃
1.4 mol NH3
0.18 mol NH3
0.70 mol NH3
0.60 mol NH3
149
A 10g sample of which substance contains the greatest number of hydrogen atoms?
10g of PH3
10g of H2
10g of HCl
10g of Mg
150
What mass of Sn is formed by the reaction of 1.75 mol H₂ with excess SnO₂? SnO₂ + H₂ -> Sn + 2H₂O
151 g
301 g
104 g
527 g
151
Which electron configuration is impossible?
1s22s22p62d2
1s22s22p63s23p64s24d5
1s22s22p63s23p6
1s22s22p53s1
152
Which group contains nonmetals, metalloids, and metals?
18
1
13
15
153
Which atom has the most neutrons?
neon-20
phosphorous-32
chlorine-35
sulfur-35
154
What is the balanced net ionic equation for the reaction of CuCl₂(aq) and H₂(g)?
CuCl2(aq) + H2(g) -> Cu(s) + 2HCl(aq)
Cu2+(aq) + 2Cl-(aq) + H2(g) -> Cu(s) + 2H+(aq) + 2Cl-(aq)
Cu2+(aq) + H2(g) -> Cu(s) + 2H+(aq)
Cu2+(aq) + Cl2(aq) + H2(g) -> Cu(s) + 2H+(aq) + 2Cl-(aq)
155
Which of these elements has the smallest atomic radius?
bromine
chlorine
fluorine
iodine
156
SCl₂ has __________ bonds and overall the molecule is ________.
nonpolar, polar
polar, nonpolar
polar, polar
nonpolar, nonpolar
157
What is the empirical formula of a compound of carbon (51.56%), hydrogen (14.09%), and oxygen?
C8H13O2
C2H7O
C7H2O5
C4H13O2
158
What is the name of HBrO₄(aq)?
bromic acid
bromous acid
perbromic acid
hydrobromic acid
159
A sodium ion differs from a sodium atom in that the sodium ion
has fewer electrons
exists only in solution
has a negative charge on its nucleus
is an isotope of sodium
160
What is the molar concentration of a solution when 7.00 mL of a 3.25 M aqueous solution is diluted to 25.00 mL?
2.15 M
0.280 M
1.10 M
0.910 M
161
In which reaction is carbon reduced?
CO(g) + O2(g) -> CO2(g)
CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)
CO2(g) + H2O(l) -> H2CO3(aq)
C2H2(g) + H2(g) -> C2H4(g)
162
Why is the boiling point of Br₂ higher than that of Cl₂?
Br2 has greater molar mass and is therefore easier to vaporize
Br is more electronegative and therefore has greater dipole-dipole forces
Br2 is more polarizable and therefore has greater London dispersion forces
Br is less electronegative and therefore its bonding is more ionic
163
What is the strongest electrolyte in dilute aqueous solution?
HF
HCN
HClO4
HNO2
164
What mass of SbF₃ (179g/mol) is needed to produce 1.00 g CCl₂F₂ (121 g/mol)? 3CCl₄ + 2 SbF₃ -> 3CCl₂F₂ + 2SbCl₃
0.986 g
0.667 g
1.48 g
2.22 g
165
The density of helium is 0.164 kg/m³. What is this density in lb/ft³? 1 kg=2.20 lb and 1 m=3.28 ft
0.0102 lb/ft3
1.18 lb/ft3
12.7 lb/ft3
0.110 lb/ft3
166
What molecule has a 120° bond angle?
NH3
CO2
SO3
IF3
167
What solution volume is needed to prepare a 0.110 M solution of MgSO₄ using 10.3 g of the compound? (MgSO₄=120.36 g/mol)
1.11 L
0.778 L
9.41x10-3 L
93.6 L