EXAMINATION TEST
SECTIONS:
1, Multiple Choice (60 problems);
ANY CHEATING WILL BE PENALIZED!
Do Your Best.
Name: _____________________________
SECTION 1: Multiple Choice (60 problems)
1) Based on molecular orbital theory, the bond orders of the H—H bonds in
H2, H2 +, and H2
– are _________, respectively
A) 1, 0, and 0 B) 1, ½, and 0 C) 1, 0, and ½ D) 1, ½, and ½ E) 1, 2, and 0
2) Sodium hydride reacts with excess water to produce aqueous sodium
hydroxide and hydrogen gas:
NaH (s) + H2O (l) → NaOH (aq) + H2 (g)
A sample of NaH weighing ______ g will produce 982 mL of gas at 28oC
and 765 torr, when the hydrogen is collected over water. The vapor pressure
of water at this temperature is 28 torr.
A) 2.93 B) 0.960 C) 0.925 D) 0.0388 E) 925
3) Of the following transitions in the Bohr hydrogen atom, the _______
transition results in the emission of the highest-energy photon.
A) n = 1 → n = 6 B) n = 6 → n = 1 C) n = 6 → n = 3 D) n = 3 → n = 6 E) n = 1 → n = 4
4) Of the molecules below, only ______ is polar.
A) CCl4 B) CH4 C) SeF4 D) SiCl4
5) The ground state configuration of fluorine is ________ .
A) [He]2s22p2 B) [He]2s22p3 C) [He]2s22p4 D) [He]2s22p5 E) [He]2s22p6
6) The volume of HCl gas required to react with excess magnesium metal to
produce 6.82 L of hydrogen gas at 2.19 atm and 35.0oC is _______ L.
A) 6.82 B) 2.19 C) 13.6 D) 4.38 E) 3.41
7) Which of the following is a statement of the first law of thermodynamics?
A) Ek = 0.5 m v 2
B) A negative ΔH corresponds to an exothermic process C) ΔE = Efinal – Einitial D) Energy lost by the system must be gained by the surroundings. E) 1 cal = 4.184 J (exactly)
8) How many p-orbitals are occupied in a B atom?
A) 5 B) 6 C) 0 D) 1 E) 3
9) Using the VSEPR model, the molecular geometry of the central atom is
NCl3 is ________ .
A) linear B) trigonal planar C) tetrahedral bent D) bent E) trigonal pyramidal
10) The elements in the _______ period of the periodic table have a core-
election configuration that is the same as the electron configuration of neon.
A) first B) second C) third D) fourth E) fifth
11) What is the maximum number of double bonds that a hydrogen atom can
form?
A) 0 B) 1 C) 2 D) 3 E) 4
12) The density of ammonia gas in a 4.32 L container at 837 torr and 45.0oC
is _______ g/L.
A) 3.86 B) 0.719 C) 0.432 D) 0.194 E) 4.22*10-2
13) In which of the molecules below is the carbon-carbon distance the
shortest?
A) H2C=CH2 B) H-C≡C-H C) H3C-CH3 D) H2C=C=CH2 E) H3C-CH2-CH3
14) PCl5 has _____ electron domains and a _______ molecular arrangement.
F) 6, trigonal bipyramidal G) 6, tetrahedral H) 5, square pyramidal I) 5, trigonal bipyramidal J) 6, seesaw
15) The oxidation number of phosphorus in PF3 is _______.
A) -2 B) +1 C) +3 D) +2 E) -3
16) The temperature of a sample of CH4 gas (10.34 g) in a 50.0 L vessel at
1.33 atm is _________ .
A) 984 B) -195 C) 195 D) 1260 E) -1260
17) Which one of the following is a weak acid?
A) HNO3 B) HCl C) HI D) HF E) HClO4
18) The ion ICl4 – has _____ valence electrons.
A) 34 B) 35 C) 36 D) 28 E) 8
19) Of the atoms below, ______ is the most electropositive.
A) Be B) Mg C) Ca D) Sr E) Ba
20) The mass of nitrogen dioxide contained in a 4.32 L vessel at 48oC and
141600 Pa is ________ g.
A) 5.35*104 B) 53.5 C) 10.5 D) 70.5 E) 9.46*10-2
21) The molecular geometry of the SiH2Cl2 molecule is _________ .
A) trigonal planar B) tetrahedral C) trigonal pyramidal D) octahedral E) T-shaped
22) ________ -orbitals are spherically symmetrical.
A) s
B) p
C) d
D) f
E) g
23) Calculate the kinetic energy in joules of an automobile weighing 4345 lb
and traveling at 75 mph. (1 mile = 1.6093 km, 1 lb = 453.59 g)
A) 5.5*105 B) 5.5*10-5 C) 1.1*106 D) 2.2*106 E) 2.2*10-6
24) Of the possible bonds between carbon atom (single, double, and triple),
___________.
A) a triple bond is longer than a single bond B) a double bond is stronger than a triple bond C) a single bond is stronger than a triple bond D) a double bond is longer than a triple E) a single bond is stronger than a double bond
25) The volume of an ideal gas is zero at _______ .
A) 0oC B) -45oF C) -273 K D) -363 K E) -273oC
26) Of the following, ΔHf o is not zero for _________ .
A) O2 (g) B) C (graphite) C) N2 (g) D) F2 (s) E) Cl2 (g)
27) With which of the following will the potassium ion form an insoluble
salt?
A) chloride B) sulfate C) carbonate D) sulfate and carbonate E) none of the above
28) The correct name for HClO3 is .
A) hydrochloric acid
B) perchloric acid
C) chloric acid
D) chlorous acid
E) hydrochlorous acid
29) Of the following, is the largest mass.
A) 25 kg
B) 2.5*10-2 mg
C) 2.5*1015 pg
D) 2.5*109 fg
E) 2.5*1010 ng
30) How many moles of gas are there in a 50.0 L container at 22.0oC and
825 torr?
A) 2.29*104 B) 1.70*103 C) 2.23 D) 0.603 E) 18.4
31) Of the choices below, which would be the best for the lining of a tank
intended for use in storage of hydrochloric acid?
A) copper B) zinc C) nickel D) iron E) tin
32) The correct name for CCl4 is .
A) carbon chloride
B) carbon tetrachlorate
C) carbon perchlorate
D) carbon tetrachloride
E) carbon chlorate
33) Expressing a number in scientific notation .
A) changes its value
B) removes ambiguity as to the significant figures
C) removes significant zeros
D) allows to increase the number’s precision
E) all of the above
34) The total number of π bonds in the H-C≡C-C≡C-C≡N molecule is ____ .
A) 3 B) 4 C) 6 D) 9 E) 12
35) A mole of red photons of wavelength 725 nm has _______ kJ of energy.
A) 2.74*10-19 B) 4.56*10-46 C) 6.05*10-3 D) 165 E) 227
36) A molecular orbital can accommodate a maximum of _____ electron(s).
A) one B) two C) four D) six E) twelve
37) How many grams of CH3OH must be added to water to prepare 150 mL
of a solution that is 1.0 M CH3OH?
A) 0.15 B) 430 C) 2.4 D) 4.8 E) 4.3
38) Which species is an isotope of 39Cl?
A) 40Ar+
B) 34S2-
C) 36Cl-
D) 80Br
E) 39Ar
39) How many carbon atoms are there in 52.06 g of carbon dioxide?
A) 5.206*1024
B) 3.134*1025
C) 7.122*1023
D) 8.648*10-23
E) 1.424*1024
40) Of the reactions below, which one is not a combination reaction?
A) C + O2 → CO2
B) 2Mg + O2 → 2MgO
C) 2N2 + 3H2 → 2NH3
D) CaO + H2O → Ca(OH)2
E) 2CH4 + 4O2 → 2CO2 + 4H2O
41) The formula for aluminum hydroxide is _______ .
A) AlOH B) Al3OH C) Al2(OH)3 D) Al(OH)3 E) Al2O3
42) The sp3d2 atomic hybrid orbital set accommodates ______ electron
domains.
A) 2 B) 3 C) 4 D) 5 E) 6
43) The combustion of ammonia in the presence of oxygen yields NO2 and
H2O:
4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O (g).
The combustion of 43.9 g of ammonia with 258g of oxygen produces
_______ g of NO2.
A) 212 B) 178 C) 119 D) 0.954 E) 43.9
44) The net ionic equation for the dissolution of zinc metal in aqueous
hydrobromic acid is ______________ .
A) Zn (s) + 2 Br- (aq) → ZnBr2 (aq) B) Zn (s) + 2 HBr (aq) → ZnBr2 (aq) + 2H
+ (aq)
C) Zn (s) + 2 HBr (aq) → ZnBr2 (s) + 2H + (aq)
D) Zn (s) + 2 H+ (aq) → Zn2+ (aq) + H2 (g) E) 2Zn (s) + H+ (aq) → 2Zn2+ (aq) + H2 (g)
45) _______ is the chemical symbol for elemental sodium.
A) S B) W C) So D) Na E) Sn
46) When a hydrocarbon burns in air, a component produced is?
A) oxygen
B) nitrogen
C) carbon
D) water
E) argon
47) Which formula/name pair is incorrect?
A) FeSO4 iron(II) sulfate
B) Fe2(SO3)3 iron(III) sulfite
C) FeS iron(II) sulfide
D) FeSO3 iron(II) sulfite
E) Fe2(SO4)3 iron(III) sulfide
48) Round the number 3456.5 to two significant figures.
A) 3400.0 B) 3400 C) 3000 D) 3500 E) 3000.0
49) One side of a cube measures 1.55 m. The volume of this cube is ______
cm3.
A) 2.40*104 B) 3.72*106 C) 2.40 D) 3.72 E) 155
50) What is the volume (in cm3) of a 63.4g piece of metal with a density of
12.86 g/cm3?
A) 4.93 B) 19.5 C) 0.425 D) 6.65 E) none of the above
51) The volume of 1.20 mol of gas at 61.3 kPa and 25.0oC is ________ L.
A) 135 B) 48.5 C) 52.4 D) 108 E) 55.7
52) Of the bonds below, _______ is the least polar.
A) C, O B) N, O C) C, F D) S, O E) K, Br
53) For which one of the following reactions is the value of ΔHorxn equal to
ΔHof for the product?
A) 2C (s, graphite) + 2 H2 (g) → C2H4 (g) B) N2 (g) + O2 (g) → 2 NO (g) C) 2H2 (g) + O2 (g) → 2 H2O (l) D) 2H2 (g) + O2 (g) → 2 H2O (g) E) H2O (l) + 0.5 O2 (g) → H2O2 (l)
54) The name of the binary compound N2O4 is _______ .
A) nitrogen oxide B) nitrous oxide C) nitrogen (IV) oxide D) dinitrogen tetraoxide E) oxygen nitride
55) Of the molecules below, only _____ is polar.
A) SbF5 B) AsH3 C) I2 D) SF6 E) CH4
56) Lead (II) carbonate decomposes to give lead (II) oxide and carbon
dioxide:
PbCO3 (s) → PbO (s) + CO2 (g)
If the reaction yield is 95.7%, how many grams of lead (II) oxide will be
produced by the decomposition of 2.50 g of lead (II) carbonate?
A) 1.04 B) 1.55 C) 2.09 D) 4.00 E) 5.55
57) 420 pm is the same as ________ Angstroms.
A) 4200 B) 42 C) 420 D) 4.2 E) 0.42
58) The element _______ is the most similar to chlorine in chemical and
physical properties.
A) Li B) Rb C) O D) Br E) Ba
59) The density (in g/L) of CO2 at 1140 torr and 60.0 oC is ______ .
A) 2.42 B) 16.2 C) 5.70 D) 44.0 E) 10.9
60) The hybrid orbital set used by the central atom in NO3 – is _________ .
A) sp B) sp2 C) sp3 D) sp3d E) sp3d2
