Download Final Exam Practice Problems Set 2

1.
1
When the following operation is performed, the answer to the correct number of significant figures
(assuming no number shown is exact) is
(1.0 + 12.01) / (12 – 1.2)
1) 1.2
2.
The active ingredient in many antacids is CaCO3. Suppose that the average dose of CaCO3 in an antacid
tablet is 500.0 mg, and that a bottle of antacid tablets contains 250 tablets. What mass of Ca is present
in 4 bottles of antacid tablets? CaCO3 is 40.0% Ca by mass.
2) 1.38
3) 134
4) 7.48
5) none of these
What is the molar mass of (NH4)2CO3?
2) 87 g
3) 78 g
4) 69 g
The hypothetical element studentium (Sd) has two isotopes: Sd-88; natural abundance 66.7% with
atomic mass 88.1 amu; and Sd-91; natural abundance 33.3% with atomic mass 91.1 amu. What is the
average atomic mass of Sd?
1) 90.1 amu
8.
4) 200. g
the number of protons in a nucleus.
the coefficient preceding a substance in a balanced equation.
the subscript following an element’s symbol in a formula.
the number of nucleons in an atom.
the number of atoms in an isomer.
1) 96 g
7.
3) 120. g
Atomic number refers to
1)
2)
3)
4)
5)
6.
2) 40.0 g
An object will sink in a liquid if the density of the object is greater than that of the liquid. The mass of a
sphere is 9.83 g. If the volume of this sphere is less than _____ cm3, then the sphere will sink in liquid
mercury (density = 13.6 g/cm3).
1) 0.723
5.
4) 1.2046
Its surface turns black when first exposed to air.
It is a solid at 25 ˚C and changes to a liquid when heated to 98 ˚C.
When placed in water it sizzles and a gas is formed.
When placed in contact with chlorine it forms a compound that melts at 801 ˚C.
1) 2.00 g
4.
3) 1.205
All of the following are properties of sodium. Which one is a physical property of sodium?
1)
2)
3)
4)
3.
2) 1.20
2) 89.1 amu
3) 91.1 amu
How many protons, neutrons, and electrons are in one ion of 35Cl–?
protons
neutrons
electrons
1)
18
17
19
2)
18
17
18
3)
17
18
17
4)
17
18
18
5)
35
35
36
4) 88.1 amu
5) 89.6 amu
2
9.
What is the name of CuCl2?
1) cupric bichlorine
2) copper(II) chloride
10.
3) copper(I) chloride
4) copper dichloride
The name of PCl3 is
1) potassium chloride
2) phosphorus trichloride
3) phosphorus(III) chloride
11.
How many oxygen atoms are there in 52.06 g of carbon dioxide?
1) 1.424  1024
12.
2) 6.022  1023
2) Cr2(SO4)3
5) 1.018  1024
3) Cr3S2
4) Cr2(SO3)3
4) mass
5) all are extensive properties
The formula for magnesium nitrate is
1) MgNO3
15.
4) 5.088  1023
Which of the following is an extensive property?
1) density
2) boiling point
3) color
14.
3) 1.204  1024
What is the formula of chromium(III) sulfate?
1) Cr3SO4
13.
4) phosphorus chloride
5) trichloro potassium
2) Mg(NO3)2
3) Mg2NO3
4) Mg2NO4
5) MgNO
Balance the equation using the smallest set of whole numbers. What is the coefficient for H2O?
_____PCl3() + _____H2O()  _____H3PO3(aq) + _____HCl(aq)
1) 1
16.
3) 3
4) 5
3) 1.5  102 L
4) 1.5  104 L
Convert 15 m3 to liters.
1) 1.5  10–2 L
17.
2) 2
2) 1.5 L
Precision refers to ___________.
1)
2)
3)
4)
5)
how close a measured number is to other measured numbers
how close a measured number is to the true value
how close a measured number is to the calculated value
how close a measured number is to zero
how close a measured number is to infinity
5) none of these
3
18.
To the correct number of significant figures, what is the temperature reading on the Celsius
thermometer at the right?
1)
2)
3)
4)
21 ˚C
21.7 ˚C
21.70 ˚C
22 ˚C
Questions 19 and 20 refer to the following diagram.
a)
19.
2) drawing b)
3) drawing c)
2) drawing b)
3) drawing c)
4) drawing d)
An element cannot
1) be part of a heterogeneous mixture.
2)
3) be separated into other substances by chemical means.
4) interact with other elements to form compounds.
5)
22.
4) drawing d)
If shaded and unshaded spheres represent atoms of different elements, which of the above drawings
most likely represents a molecular compound at room temperature and a pressure of 1 atm?
1) drawing a)
21.
d)
c)
If shaded and unshaded spheres represent atoms of different elements, which of the drawings below
most likely represents an ionic compound at room temperature and a pressure of 1 atm?
1) drawing a)
20.
b)
be part of a homogeneous mixture.
be a pure substance.
Which one of the following is not one of the postulates of Dalton’s atomic theory?
1) Atoms are composed of protons, neutrons, and electrons.
2) All atoms of a given element are identical; the atoms of different elements are different and have
different properties.
3) Atoms of an element are not changed into different types of atoms by chemical reactions; atoms are
neither created nor destroyed in chemical reactions.
4) Compounds are formed when atoms of more than one element combine; a given compound always
has the same relative number and kind of atoms.
5) Each element is composed of extremely small particles called atoms.
23.
When 0.387 g of Cr is heated in an atmosphere of Cl2 gas, a combination reaction occurs and 1.178 g of
a solid compound is formed. Assuming that all of the chromium reacts, what is the mass of chlorine that
reacted?
1) 0.387 g
2) 1.178 g
3) 0.791 g
4) 0.396 g
5) 1.565 g
4
24.
The correct name for H2SO3 is ________.
1) sulfuric acid
4) hydrosulfic acid
25.
2) sulfurous acid
5) sulfur hydroxide
Which is a chemical property of chlorine?
1) It is yellowish green.
3) It has a density of 3.2 g•L–1 at STP.
5) It boils at -34 ˚C.
26.
2)
4)
2) 2.15 mol
3) 1.10 mol
3) Sr2N3
4) SrN2
5) SrN3
2) 55.1 amu
3) 78.1 g
4) 78.1 amu
5) 6.022  1023
2) 1.5
4) 0.36
5) 184
3) 2.8
In accordance with the solubility rules, which of the following is true when solutions of CuSO4(aq) and
BaCl2(aq) are mixed?
1)
2)
3)
4)
5)
2.
2) Sr3N2
How many grams of hydrogen are in 46 g of CH4O?
1) 5.8
1.
2) the law of constant composition
4) the law of conservation of energy
What is the mass of 1 mole of Na2S?
1) 55.1 g
30.
5) 0.421 mol
What is the formula of the compound formed between strontium ions and nitrogen ions?
1) SrN
29.
4) 0.466 mol
A molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement of _____.
1) the law of multiple proportions
3) the law of conservation of mass
5) none of the above
28.
It burns in sodium vapor.
It dissolves in carbon tetrachloride.
Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of
electrical insulators. Calculate the number of moles in 47.51 g of Al2O3.
1) 2.38 mol
27.
3) hydrosulfuric acid
CuCl2 will precipitate, and Ba2+ and SO42– are spectator ions.
CuSO4 will precipitate, and Ba2+ and Cl– are spectator ions.
BaSO4 will precipitate, and Cu2+ and Cl– are spectator ions.
BaCl2 will precipitate, and Cu2+ and SO42– are spectator ions.
No precipitate will form.
How many of the following are oxidation-reduction reactions?
a) NaOH + HCl  NaCl + H2O
b) Cu + 2 AgNO3  2 Ag + Cu(NO3)2
1) 1
2) 2
3) 3
c) Mg(OH)2  MgO + H2O
d) 2 Na + Cl2  2 NaCl
4) 4
5) zero
5
3.
Which of the following is the balanced net ionic equation for the reaction between Al(OH)3(s) and
HNO3(aq)? HNO3 is a strong acid.
1)
2)
3)
4)
4.
Al(OH)3(s) + 3HNO3(aq)  Al(NO3)3(aq) + 3H2O()
Al(OH)3(s) + 3H+(aq)  Al3+(aq) + 3H2O()
Al3+(aq) + 3OH–(aq) + 3H+(aq) + 3NO3–(aq)  Al3+(aq) + 3NO3–(aq) + 3H2O()
H+(aq) + OH–(aq)  H2O()
How many grams of KOH are required to prepare 250.0 mL of 2.0 M KOH solution?
1) 0.5 g
5.
2) 14 g
3) 28 g
4) 56 g
5) 112 g
When 48.0 g of nitrogen gas reacts with an excess amount of hydrogen gas to give an actual yield of
5.90 g of ammonia gas, NH3(g), what is the percentage yield for this reaction?
N2(g) + 3 H2(g)  2 NH3(g)
1) 82.3%
2) 60.7%
3) 58.3%
4) 20.2%
5) 10.1%
The following statement and diagrams refer to problems 6 and 7.
Consider a representation of a small volume of a reaction flask before the start of a reaction between nitrogen
gas and oxygen gas to give dinitrogen pentoxide,
.
____N2(g) + ____O2(g) 
N2 =
N2O5(g)
O2 =
10
?
10
initial
6.
after
Which of the following represents this same small volume after the reaction occurs?
4
2
10
4
6
8
1)
2)
3)
4)
6
7.
What is the limiting reagent in the above problem?
1) N2O5
8.
2) N2
3) O2
4) both N2 and O2
5) none of these
The amount of chloride ion in a water supply can be determined by reaction with aqueous silver nitrate.
AgNO3(aq) + Cl–(aq)  AgCl(aq) + NO3–(aq)
What mass of chloride ion is present in a 100.0 g sample of aqueous solution if 40.8 mL of
0.100 M AgNO3 is required to react with all the chloride ion in the sample?
1) 4.08  10–3 g
2) 0.144 g
3) 0.585 g
4) 0.693 g
5) 4.08 g
9.
When 25.0 mL of H2SO4 solution was completely neutralized in a titration with 0.0500 M NaOH
solution, 18.3 mL of the base was required. What was the molarity of the H2SO4 solution? The reaction was
H2SO4 + 2 NaOH  Na2SO4 + 2 H2O
1) 0.0366 M
10.
2) 0.0100 M
3) 0.0148 M
4) 0.200 M
5) 0.0183 M
Write a balanced net ionic equation for the reaction of NiBr 2(aq) with (NH4)2S(aq).
1) NiBr2(aq) + (NH4)2S(aq)  NiS(s) + 2 NH4Br(aq)
2) Ni2+(aq) + 2 Br – (aq) + 2 NH4+(aq) + S2–(aq)  NiS(s) + 2 NH4+(aq) + 2 Br – (aq)
3) Ni2+(aq) + 2 Br – (aq) + 2 NH4+(aq) + S2–(aq)  NiS(s) + 2 NH4Br(s)
4) Ni2+(aq) + S2–(aq)  NiS(s)
11.
What type of reaction will take place when NH3(aq) and H2SO4(aq) are mixed?
1) precipitation
2) oxidation-reduction
12.
3) acid-base
4) NH3(aq) and H2SO4(aq) do not react.
Which of the following compounds is a weak electrolyte?
1) HCl
2) CH3COOH (acetic acid)
3) C6H12O6 (glucose)
13.
Identify the major ionic species present in an aqueous solution of Na2CO3
1) Na2+, CO32–
14.
4) O2
5) NaCl
2) Na2+, C2–, O3
3) Na+, C4+, O32–
4) Na+, C+, O2–
5) Na+, CO32–
What element is reduced in the following chemical reaction?
Cu + 2 H2SO4  CuSO4 + SO2 + 2 H2O
1) Cu
2) H
3) S
4) O
5) H2O
7
15.
What is the oxidation state of the C atom in C2O42–?
1) +4
16.
2) +3
1) a and d
2) a, b, c, and d
5) c and d
A2Y
A2Z
The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12H22O11) (MW = 342) in 35.5 mL
of solution is
2) 1.85  10–3
3) 1.85
4) 3.52
5) 0.104
The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500 mL is
1) 57.2
2) 0.0044
3) 0.438
4) 0.0879
5) 0.870
3) HF
4) HBr
5) HCl
Which of the following is a weak acid?
1) H2SO4
21.
4) b, c, and d
A2X is the strongest electrolyte and A2Y is the weakest electrolyte.
A2Y is the strongest electrolyte and A2X is a nonelectrolyte.
A2Y is the strongest electrolyte and A2Z is a nonelectrolyte.
A2Z is the strongest electrolyte and A2Y is the weakest electrolyte.
1) 0.0657
20.
3) a, c, and d
Three different substances, A2X, A2Y, A2Z, were dissolved in water with the following results. (Water
molecules are omitted for clarity.) Which of the substances is the strongest electrolyte, and which is the
weakest?
1)
2)
3)
4)
19.
5) none of these
CH4(g) + O2(g)  CO2(g) + H2O()
CaO(s) + CO2(g)  CaCO3(s)
PbCO3(s)  PbO(s) + CO2(g)
CH3OH() + O2(g)  CO2(g) + H2O()
A2X
18.
4) +1
Which of the following are combustion reactions?
a)
b)
c)
d)
17.
3) +2
2) HNO3
The concentration of iodide ions in a 0.193 M solution of barium iodide, BaI2(aq), is
1) 0.193 M
2) 0.386 M
3) 0.0965 M
4) 0.579 M
5) 0.0643 M
8
22.
Ethylene glycol, used as a coolant in automotive engines, has a specific heat capacity of 2.42 J/(g•K).
Calculate q when 3.65 kg of ethylene glycol is cooled from 132 ˚C to 85 ˚C.
1) -1900 kJ
23.
3) -99 kJ
4) -0.42 kJ
5) -4.2  10–6 kJ
A 275-g sample of nickel at 100.0 ˚C is placed in 100.0 mL of water at 22.0 ˚C. What is the final
temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat
capacity of nickel = 0.444 J/(g•K)
1) 39.6 ˚C
24.
2) -420 kJ
2) 40.8 ˚C
3) 61.0 ˚C
4) 79.2 ˚C
5) 82.4 ˚C
A sample of baking soda dissolves in water. The initial temperature of the water is 23 ˚C. The temperature
of the resultant solution is 18 ˚C.
NaHCO3(s)
H2O
Na+(aq) + HCO3–(aq)
For the dissolving process described above, the reaction shown is _____ and heat is _____.
1)
2)
3)
4)
5)
25.
exothermic, given off by the reaction.
exothermic, taken in (absorbed) by the reaction.
endothermic, given off by the reaction.
endothermic, taken in (absorbed) by the reaction
cannot tell without knowing the mass of water and the specific heat of the resultant solution
A 13.8 mL aliquot of 0.176 M H3PO4(aq) is to be titrated with 0.110 M NaOH(aq). What volume (mL)
of base will it take to reach the equivalence point?
H3PO4(aq) + 3 NaOH(aq)  Na3PO4(aq) + 3 H2O()
1) 7.29
26.
2) 22.1
3) 199
4) 66.2
5) 20.9
Lithium and nitrogen react in a combination reaction to produce lithium nitride.
6 Li(s) + N2(g)  2 Li3N(g)
In a particular experiment, 3.50 g samples of each reagent are reacted. The theoretical yield of lithium
nitride is _____ g.
1) 3.52
27.
3) 17.6
4) 5.85
5) 8.70
What are the spectator ions in the reaction between KOH(aq) and HNO3(aq)?
1) K+ and H+
28.
2) 2.93
2) H+ and OH–
3) K+ and NO3–
4) H+ and NO3–
5) OH– only
A gas expands against an external pressure while in thermal isolation from the surroundings. For this
expansion
1) ∆E increases
2) ∆E does not change
3) ∆E decreases
4) ∆E = q
9
29.
A nitrogen oxide is 63.65% by mass nitrogen. The molecular formula could be _______.
1) NO
30.
5) either NO2 or N2O4
Which sketch represents an orbital that can have a principal quantum number of 2?
1) I
II
2) II & III
III
IV
3) I, II, & III
V
4) IV & V
5) I, II, III, IV, & V
The wavelength of light associated with an electronic transition from n = 3 to n = 2 in a hydrogen atom is
1) 306 nm
3.
4) N2O4
The system loses heat and does work on the surroundings.
The system gains heat and does work on the surroundings.
The system loses heat and has work done on it by the surroundings.
The system gains heat and has work done on it by the surroundings.
None of the above is correct.
I
2.
3) N2O
Which one of the following conditions would always result in an increase in the internal energy of a
system?
1)
2)
3)
4)
5)
1.
2) NO2
2) 361 nm
3) 434 nm
4) 656 nm
The electronic configuration of cadmium (Z = 48) is
1) 1s22s22p62d103s23p63d104s25d10
2) 1s22s22p63s23p64s23d104p65s24d10
3) 1s22s22p62d103s23p63d104s24p64d2
4) 1s21p62s22p62d103s23p63d104s24p2
5) 1s22s22p63s23p63d104s24p65s25p65d4
4.
Which is isoelectronic with N3–?
1) C4+
5.
3) Na
4) Ne
Which one of the following configurations depicts an excited oxygen atom?
1) 1s22s22p2
6.
2) F
2) 1s22s22p23s2
3) 1s22s22p1
4) 1s22s22p4
5) [He]2s22p4
Elements with the outermost electron configuration ns2np3 are found in which portion of the periodic
table?
1) s
2) t
3) u
4) v
10
7.
Which of the following is true?
1) Fe3+ is larger than Fe2+
2) Na is larger than Na+
8.
The energy of a photon of light is _____ proportional to its frequency and _____ proportional to its
wavelength.
1) directly, directly
2) inversely, inversely
3) inversely, directly
9.
4) directly, inversely
5) indirectly, not
Which of the following is the correct electron configuration for the ground state of a Mn atom?
1) 1s22s22p63s33p63d7
2) 1s22s22p63s23p64s24d5
10.
3) O– is larger than O2–
4) K+ is larger than Cl–
3) 1s21p62s22p63s23p63d5
4) 1s 2s22p63s23p64s23d5
2
Which of the following is a correct orbital diagram for the valence electrons in a S atom?
1)
2)
3s
3p
3s
3p
3)
4)
3s
3p
3s
3p
Use the following diagram to answer Q-11. Two electromagnetic waves are represented below.
11.
Wave (a) has the
1)
2)
3)
4)
12.
longer wavelength and higher frequency than wave (b).
longer wavelength and lower frequency than wave (b).
shorter wavelength and higher frequency than wave (b).
shorter wavelength and lower frequency than wave (b).
What is the frequency of blue light that has a wavelength of 400 nm?
1) 2.65  10–31 Hz
13.
2) 1.3  10–6 Hz
3) 7.5  105 Hz
4) 2.5  106 Hz
5) 7.5  1014 Hz
What is the energy in joules of a mole of photons associated with red light of wavelength 7.00  102
nm?
1) 256 kJ
2) 1.71  105 J
3) 4.72  10–43 J
4) 12.4 kJ
5) 2.12  1042 J
11
14.
Which has the highest Zeff for its valence electrons?
1) K
15.
2) Rb
3) Ge
Which experiment caused Bohr to invoke an explanation that quantized the energy levels of electrons in
atoms?
1) The discovery of isotopes by mass spectrometry
3) The Mulliken oil-drop experiment
5) The placing of Mentos in 2 L bottles of Diet Coke.
16.
2) 1
3) 2
Of the following, which gives the correct increasing order for atomic radius for Mg, Na, P, Si and Ar?
[start with small one first]
4) Ar < P < Si < Mg < Na
5) Na < Mg < Si < P < Ar
The spheres below represent atoms of Sb, As, P, and N (not necessarily in that order).
A, r = 75 pm
B, r = 110 pm
C, r = 120 pm
D, r = 140 pm
Which one of these spheres represents an atom of Sb?
1) sphere A
20.
5) 4
matter and energy are really the same thing.
it is impossible to know anything with certainty.
it is impossible to know both the exact position and momentum of an electron.
there can only be one uncertain digit in a reported number.
it is impossible to know how many electrons there are in an atom.
1) Mg < Na < P < Si < Ar
2) Si < P < Ar < Na < Mg
3) Ar < Si < P < Na < Mg
19.
4) 3
The uncertainty principle states that
1)
2)
3)
4)
5)
18.
2) The Rutherford gold foil experiment
4) The discovery of atomic line spectra
There are _____ unpaired electrons in a ground state phosphorus atom.
1) 0
17.
4) Br
2) sphere B
3) sphere C
4) sphere D
Within a given shell of a multielectron atom, the lower  for an orbital, the
1)
2)
3)
4)
higher the orbital energy and the higher Zeff for the electron.
higher the orbital energy and the lower Zeff for the electron.
lower the orbital energy and the higher Zeff for the electron.
lower the orbital energy and the lower Zeff for the electron.
12
1.
For the fourth-shell orbital shown below, what are the principal quantum numbers, n, and the angular
momentum quantum number, ?
1) n = 4 and  = 0
22.
2) [Ar]3d4
4) n = 4 and  = 3
3) [Ar]3d6
4) [Ar]3d104s1
2) temperature, pressure
3) volume, pressure
4) pressure, volume
When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown
in the net ionic equation below. The initial temperature of both solutions is 21.0 ˚C. Assuming that the
reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of
4.18 J/(g•˚C), calculate the final temperature of the solution.
Ca2+(aq) + 2 F–(aq)  CaF2(s)
1) 20.45 ˚C
25.
5) [Ar]3d3
Heat transferred in a chemical reaction or physical change is expressed as ∆E when the heat is
transferred under constant _____and is expressed as ∆H when heat is transferred under constant _____
conditions.
1) pressure, temperature
24.
3) n = 4 and  = 2
Fe+2 ions are represented by __________.
1) [Ar]3d1
23.
2) n = 4 and  = 1
2) 21.55 ˚C
∆Ho = –11.5 kJ
3) 22.10 ˚C
Given the data in the table, ∆H orxn for the reaction
2 CO(g) + O2(g)  2 CO2(g)
is __________ kJ.
1) –566.4

2) –283.2
3) 283.2
4) 22.65 ˚C
Substance
CO(g)
CO2(g)
CaCO3(s)

∆H of (kJ/mol)
–110.5
–393.7
–1207.0
4) –677.0
5) The ∆H of of O2(g) is needed for the calculation
26.
Hydrogen peroxide can decompose to water and oxygen by the following reaction:
2 H2O2(l)  2 H2O(l) + O2(g)
H = 196 kJ

Calculate the value of q when 5.00 g of H2O2(l) decomposes at constant pressure.
[Molar mass of H2O2 = 34.0 g]
1) 14.4 kJ
27.
2) 490 kJ
3) 98 kJ
4) +98 kJ
5) 28.8 kJ
Which of the following is a valid set of four quantum numbers? (n, , m, ms)
1) 2, 1, 0, +1/2
2) 2, 2, 1, –1/2
3) 1, 0, 1, +1/2
4) 2, 1, +2, +1/2
5) 1, 1, 0, –1/2
13
28.
The de Broglie wavelength of a _____ will have the shortest wavelength when traveling at 30 cm/s.
1) marble
29.
2) B, Si, As
3) N, As, Bi
2) K; In
3) Br; Al
1) +2
(II) Al, Ga, In
4) Br; In
2) +1
1
_
3) 0
4) –1
5) –2
2) O=PCl
3) O=P=Cl
4) PCl=O
Based on valence bond theory, the bond order of the N–N bond in the N2 molecule is _____.
1) 0
4.
4) He, Ne, F
Which one of the following is the best Lewis electron-dot formula for POCl?
1) P=OCl
3.
5) hydrogen atom
What is the formal charge on the oxygen atom in OCN- ion. The correct Lewis structure is shown.
OC–N
2.
4) uranium atom
Which atom in each group (I and II) has the smallest atomic radius? (I) K, Zn, Br
1) K; Al
1.
3) planet
Which of the following have the same number of valence electrons?
1) K, As, Br
30.
2) car
2) 1
3) 2
4) 3
5) 5
4) sodium
5) magnesium
Consider the following properties of an element:
(i) It is solid at room temperature.
(ii) It easily forms an oxide when exposed to air.
(iii) When it reacts with water, hydrogen gas evolves.
(iv) It must be stored submerged in oil.
Which element fits the above description the best?
1) sulfur
5.
2) copper
Which is not generally considered to be a chemical reaction of the alkaline earth metal calcium?
1) Ca(s) + Cl2(g)  CaCl2(s)
3) 6 Ca(s) + 2 N2(g)  2 Ca3N2(s)
6.
3) mercury
2) 2 Ca(s) + 2 H2O()  2 Ca(OH)2(aq) + H2(g)
4) Ca(s) + O2(g)  CaO2(s)
What is the general trend in ionization energy and electron affinity values?
1)
2)
3)
4)
Both decrease as one traverses a period from left to right and both decrease as one descends a group.
Both decrease as one traverses a period from left to right and both increase as one descends a group.
Both increase as one traverses a period from left to right and both decrease as one descends a group.
Both increase as one traverses a period from left to right and both increase as one descends a group.
14
7.
Select the best Lewis structure for P2I4.
1)
I
8.
I
I
P
P
P
P
I
I
I
I
P
P
I
I
3) Al
2) bent
2) Si
X(g)
X+(g)
X+(g) + e–
X(g) + e–
X+(g) + Y–(g)





P
I
5) Na
3) trigonal planar
4) tetrahedral
3) Br2
5) see-saw
4) S8
5) Cr
X+(g) + e–
X+(aq)
X(g)
X–(g)
XY(s)
4) see-saw
5) octahedral
F
F
_
F
Si
For the SF4, the number of electron pairs (regions of electron density) around S is
molecular geometry is described as _______.
2) 5, seesaw
5) 5, trigonal bipyramidal
2
F
What is the molecular shape of SiF62– as predicted by the VSEPR theory?
1) 4, tetrahedral
4) cannot be determined
F
, and its
3) 4, seesaw
Which one of the following is a polar molecule?
1) PBr5
15.
P
Which one of the following equations correctly represents the process involved in the electron affinity of X?
1) trigonal bibyramidal
2) hexagonal
3) tetrahedral
14.
I
4) Si
F
13.
I
In which of these substances are the atoms held together by metallic bonding?
1)
2)
3)
4)
5)
12.
I
According to VSEPR theory, a molecule with the general formula AX2E2 will have a _____ molecular
shape.
1) CO2
11.
I
2) Mg
1) linear
10.
I
I
4)
An element M reacts with chlorine to form MCl2, with oxygen to form MO, and with nitrogen to form
M3N2. The most likely candidate for the element is.
1) Li
9.
3)
2)
2) CCl4
3) BrF5
4) XeF2
5) XeF4
Choose the incorrect statement about molecular geometries (shapes).
1) PCl5 is trigonal bipyramidal.
2) SO32– is tetrahedral.
3) XeF2 is linear.
4) The O–C–O angle in CH3COH is about 120˚ (sp2)
O
15
16.
For which molecule can the bonding be described in terms of sp3 hybrid orbitals of the central atom?
1) SF6
17.
2) BF3
3) PCl5
4) NH3
5) BeH2
Which bond in the Lewis structure shown is the most polar?
H
O
C
N
The electronegativities of the elements are: H = 2.1; O = 3.5; C = 2.5; N = 3.0
1) H–O
2) O–C
3) CN
4) They are equally polar.
Questions 18 and 19 refer to the Lewis structure for ozone that is shown.
O
18.
2) bent
2) bent
3) trigonal planar
4) trigonal pyramidal
O
S
O
2) O
S
O
3)
O
S
O
4)
O
S
O
Element A has an electronegativity of 2.8 and element B has an electronegativity of 3.5. Which
statement best describes the bonding in A3B?
1)
2)
3)
4)
22.
4) trigonal pyramidal
Which of the following is a correct Lewis structure for SO2?
1)
21.
3) trigonal planar
Based on the VSEPR model, what is the molecular geometry for ozone?
1) linear
20.
O
Based on the VSEPR model, what is the electronic geometry for ozone?
1) linear
19.
O
The AB bond is largely covalent with a – on A.
The AB bond is largely covalent with + on A.
The compound is largely ionic with A as the cation.
The compound is largely ionic with A as the anion.
What are the bond angles in the molecule model of PF5 at the right?
1) some less than 90˚ and one less than 180˚
2) 90˚ and 180˚
3) some less than 90˚ and some less than 120˚ but greater than 90˚, one less than
180˚ but greater than 120˚
4) 90˚, 120˚, and 180˚
23.
Which of the following molecules or ions will exhibit delocalized bonding?
SO2
1) SO2, SO3, and SO32–
4) SO3 and SO32–
SO3
SO32–
2) SO32– only
3)
SO2 and SO3
5)
None of the above will exhibit delocalized bonding.
16
24.
How many lone pairs of electrons are on the iodine atom of IF4+?
1) 0
25.
2) 1
4) 3
2) 5 π and 1 
3) 4  and 1 π
H
H
C
N
H
2) H
C
N
3) H
H
28.
4) 5  and 1 π
H
H
C
C
N
H
4) All are equal.
H
Which of the following has the bonds correctly arranged in order of increasing polarity?
1) Be–F, Mg–F, N–F, O–F
2) O–F, N–F, Be–F, Mg–F
4) N–F, Be–F, Mg–F, O–F
5) Mg–F, Be–F, N–F, O–F
3) O–F, Be–F, Mg–F, N–F
Using the table of bond dissociation energies, the ∆H for the following reaction is ____ kJ.
Bond
H–Cl
F–F
H–F
Cl–Cl
2 HCl(g) + F2(g)  2 HF(g) + Cl2(g)
1) -359
29.
2) -223
3) 359
4) 223
5) 208
D (kJ/mol)
431
155
567
242
A reactive element with a relatively low electronegativity would be expected to have a relatively
1)
2)
3)
4)
30.
5) 4  and 2 π
Which compound contains the longest carbon-to-nitrogen bond?
1) H
27.
5) 4
According to modern bonding theory the number of sigma () and pi (π) bonds in the ethylene molecule
H2C=CH2.
1) 4 π and 1 
26.
3) 2
small negative electron affinity and a relatively low ionization energy.
small negative electron affinity and a relatively high ionization energy.
large negative electron affinity and a relatively low ionization energy.
large negative electron affinity and a relatively high ionization energy.
Which of the following are allowed resonance forms of NCS–?
1) only I
_
I
N
C
S
II
N
C
S
III
N
C
S
2) only II
_
_
_
and
N
C
S
and
N
C
S
and
S
C
N
3) only III
_
_
4) I and III
17
18
B19. How many nitrogen atoms are there in 60.0 g of ammonium nitrate sample?
19
20
B14. Using standard enthalpy of formation data given in Appendix-C (at the end of the book),
calculate H for the combustion of Octane.
B15. How many molecules of oxygen is needed to completely burn 275 mL of Octane
[density = 0.703 g/cm3]?
B18. Based on the picture giving in B17, if you have 8.0 moles of A and 6.0 moles of B2,
how many moles of A3B4 will be formed?
(A) 5.3 mol
(B) 6.8 mol
(C) 2.7 mol
(D) 1.8 mol
21
22