MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1) The possible values of the orbital quantum
... [Show More] number of a 3p electron are:
A) 0, 1, 2
B) +1/2, -1/2
C) 1, 2, 3
D) -1, 0, +1
E) none of these
1)
2) Determine the oxidation state of Sn in Sn(SO4)2.
A) +6 B) -2 C) +2 D) +4 E) 0
2)
3) An interpretation of the results of many tests is called
A) a theory. B) a hypothesis. C) an experiment. D) a prediction.
3)
4) Which one of the following compounds is soluble in water?
A) CuS B) ZnCO3 C) Ag3PO4 D) Pb(NO3)2
4)
5) Consider the following balanced reaction. How many grams of water are required to form
75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows:
H2O = 18.02 g/mol, HNO3 = 63.02 g/mol.
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
A) 10.9 g H2O
B) 21.7 g H2O
C) 38.0 g H2O
D) 43.4 g H2O
E) 26.5 g H2O
5)
6) Calculate the energy of the orange light emitted by a neon sign with a frequency of 4.89 × 1014
Hz.
A) 5.11 × 10-19 J
B) 3.24 × 10-19 J
C) 3.09 × 10-19 J
D) 1.63 × 10-19 J
E) 6.14 × 10-19 J
6)
7) How many electrons does magnesium lose and nitrogen need to form Mg3N2?
A) magnesium loses 2 and nitrogen gains 3 B) magnesium loses 3 and nitrogen gains 2
C) magnesium loses 3 and nitrogen gains 3 D) magnesium loses 2 and nitrogen gains 2
7)
1
8) How many moles are in 1.50 g of ethanol, CH3CH2OH?
A) 0.0326 mol B) 69.0 mol C) 30.7 mol D) 0.0145 mol
8)
9) What is the molar concentration of sodium ions in a 0.350 M Na3PO4 solution?
A) 0.350 M B) 1.40 M C) 1.05 M D) 0.117 M
9)
10) Balance the chemical equation given below, and determine the number of grams of MgO
needed to produce 15.0 g of Fe2O3.
________ MgO(s) + ________ Fe(s) → ________ Fe2O3(s) + ________ Mg(s)
A) 0.0877 g B) 1.26 g C) 11.4 g D) 3.78 g
10)
11) To the correct number of significant figures, what is the temperature reading on the following
Celsius thermometer?
A) 21.7°C B) 22°C C) 21.70°C D) 21°C
11)
12) The ions ClO4-, ClO3-, ClO2-, and ClO- are named respectively
A) hypochlorite, chlorite, chlorate, perchlorate.
B) hypochlorate, chlorate, chlorite, perchlorite.
C) perchlorite, chlorite, chlorate, hypochlorate.
D) perchlorate, chlorate, chlorite, hypochlorite.
12)
13) Which of the following reactions gives a positive value for the electron affinity?
A) O(g) + e- → O-(g) B) S-(g) + e- → S2-(g)
C) S(g) + e- → S-(g) D) Br(g) + e- → Br-(g)
13)
2
14) Give the set of four quantum numbers that represent the electron lost to form the Rb ION from
the Rb atom.
A) n = 4, l = 1, ml = 0, ms = - 1
2
B) n = 4, l = 1, ml = 1, ms = - 1
2
C) n = 5, l = 0, ml = 0, ms = + 1
2
D) n = 5, l = 1, ml = 0, ms = + 1
2
E) n = 5, l = 0, ml = 0, ms = - 1
2
14)
15) What is the chemical formula for strontium hydride?
A) SrH2 B) Sr(OH)2 C) SrOH2 D) SrOH
15)
16) What is the ground-state electron configuration of Co?
A) [Ar]4s23d7 B) [Ar]4s24p64d1 C) [Ar]4s13d8 D) [Ar]3d9
16)
17) What is the oxidation number of the chromium atom in K2Cr2O7?
A) +6 B) -2 C) +7 D) +2
17)
18) Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO3.
A) eg=trigonal pyramidal, mg=bent, nonpolar
B) eg=trigonal planar, mg=trigonal planar, nonpolar
C) eg=tetrahedral, mg=tetrahedral, nonpolar
D) eg=tetrahedral, mg=trigonal pyramidal, polar
E) eg= trigonal bipyramidal, mg=trigonal planar, polar
18)
19) What are the coefficients in front of NO3-(aq) and Zn(s) when the following equation is
balanced in a basic solution:
___ NO3-(aq) + ___ Zn(s) → ___ Zn2+(aq) + ___ NO(g)?
A) 3, 2 B) 2, 3 C) 3, 4 D) 2, 5
19)
20) Place the following in order of decreasing metallic character.
P As K
A) K > As > P
B) P > As > K
C) As > P > K
D) As > K > P
E) K > P > As
20)
3
21) How many of the following species are diamagnetic?
Cs Zr2⁺ Al3⁺ Hg2⁺
A) 1 B) 3 C) 0 D) 4 E) 2
21)
22) Which of the following is NOT a strong electrolyte?
A) NaC2H3O2
B) LiOH
C) Li2SO4
D) CaCl2
E) MgCO3
22)
23) Determine the number of protons, neutrons and electrons in the following:
65
29
X
A) p+ = 36 n° = 29 e- = 36
B) p+ = 29 n° = 36 e- = 36
C) p+ = 29 n° = 29 e- = 36
D) p+ = 36 n° = 36 e- = 29
E) p+ = 29 n° = 36 e- = 29
23)
24) What is the identity of substance X if 0.380 mol of X weighs 17.5 g?
A) N2O4 B) N2O C) NO3 D) NO2
24)
25) For a process at constant pressure,
A) ΔE = q and w = 0. B) ΔE = ΔH.
C) ΔE = w and q = 0. D) ΔH = q.
25)
26) Given the reaction:
2 KMnO4 + 10 KI + 8 H2SO4 → 6 K2SO4 + 2 MnSO4 + 5 I2 + 8 H2O
How many moles of I2 are produced by reacting 28.0 g KMnO4, 18.0 g KI and 46.0 g H2SO4?
A) 0.108 mol
B) 0.0542 mol
C) 0.293 mol
D) 0.443 mol
E) 0.886 mol
26)
27) What element is undergoing oxidation (if any) in the following reaction?
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
A) H
B) C
C) O
D) both C and H
E) None of the elements is undergoing oxidation.
27)
4
28) Which of the following drawings depicts a chemical reaction consistent with Daltonʹs atomic
theory?
A) drawing a) B) drawing b) C) drawing c) D) drawing d)
28)
29) Which of the following molecules contains polar bonds but has a zero dipole moment?
A) NH3 B) CO2 C) CH3Cl D) BrCl E) N2
29)
30) Of the following elements, which has the highest electronegativity?
A) As B) S C) P D) Sc
30)
31) The observation that 15.0 g of hydrogen reacts with 120.0 g of oxygen to form 135.0 g of water
is evidence for the law of
A) definite proportions. B) energy conservation.
C) multiple proportions. D) mass conservation.
31)
32) What is the charge on the Cr in the ionic compound Cr2O3?
A) 2- B) 2+ C) 1+ D) 3+ [Show Less]