Practice pre-exam 4 Th
1) Accuracy refers to ______.
A) how close a measured number is to zero
B) how close a measured number is to the calculated value
C) how close a measured number is to other measured numbers
D) how close a measured number is to the true value
E) how close a measured number is to infinity
Answer: D
Diff: 1
Page Ref: Sec. 1.4
2) An unknown element is found to have three naturally occurring isotopes with atomic masses of 35.9675 (0.337%), 37.9627 (0.063%), and 39.9624 (99.600%). Which of the following is the unknown element?
A) Ar
B) K
C) Cl
D) Ca
E) None of the above could be the unknown element.
Answer: A
Diff: 2
Page Ref:
3) In the symbol shown below, x = ______.
A) 7
B) 13
C) 12
D) 6
E) not enough information to determine
Answer: D
Diff: 1
4) Of the choices below, which one is not an ionic compound?
A) NBr3
B) CuCl2
C) RbCl
D) Pb(NO3)2
E) KBr
Answer: A
Diff: 1
Page Ref: Sec. 2.6
5) Chromium and chlorine form an ionic compound whose formula is. The name of this compound is ______.
A) chromium chlorine
B) chromium(III) chloride
C) monochromium trichloride
D) chromium(III) trichloride
E) chromic trichloride
Answer: B
Diff: 1
Page Ref: Sec. 2.8
6) The name of the binary compound is ______.
A) nitrogen oxide
B) nitrous oxide
C) nitrogen(IV) oxide
D) dinitrogen tetroxide
E) oxygen nitride
Answer: D
Diff: 2
Page Ref: Sec. 2.8
7) Predict the empirical formula of the ionic compound that forms from magnesium and fluorine.
A)
B) MgF
C)
D)
E)
Answer: E
Diff: 1
Page Ref: Sec. 2.7
8) What is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass?
A)
B)
C) NaSO
D)
E)
Answer: A
Diff: 3
Page Ref: Sec. 3.5
9) When the following equation is balanced, the coefficient of is ______.
A) 1
B) 2
C) 3
D) 5
E) 4
Answer: B
Diff: 1
Page Ref: Sec. 3.1
10) Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:
In a particular experiment, a 9.27-g sample of reacts completely. The mass of Mg consumed is ______g.
A) 8.04
B) 24.1
C) 16.1
D) 0.92
E) 13.9
Answer: B
Diff: 3
Page Ref: Sec. 3.6
11) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:
How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?
A) 0.41
B) 2.50
C) 0.00936
D) 2.09
E) 2.61
Answer: D
Diff: 3
Page Ref: Sec. 3.6
12) A 30.5 gram sample of glucose (C6H12O6) contains ______atoms of carbon.
A)
B)
C)
D)
E)
Answer: B
Diff: 3
Page Ref: Sec 3.4
13) The balanced net ionic equation for precipitation of when aqueous solutions of are mixed is ______.
A)
B)
C)
D)
E)
Answer: D
Diff: 3
Page Ref: Sec. 4.2
14) When aqueous solutions of and KI are mixed, AgI precipitates. The balanced net ionic equation is ______.
A) )
B)
C)
D)
E)
Answer: A
Diff: 3
Page Ref: Sec. 4.2
15) The spectator ions in the reaction between aqueous hydrofluoric acid and aqueous barium hydroxide are ______.
A)
B)
C)
D)
E)
Answer: B
Diff: 2
Page Ref: Sec. 4.2
16) The net ionic equation for formation of an aqueous solution of via mixing solid and aqueous nitric acid is ______.
A)
B)
C)
D)
E)
Answer: D
Diff: 4
Page Ref: Sec. 4.2
17) The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ______.
A)
B)
C)
D)
E)
Answer: D
Diff: 2
Page Ref: Sec. 4.3
18) How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.175 M NaOH solution?
A)
B) 114
C) 14.0
D) 3.50
E)
Answer: D
Diff: 3
Page Ref: Sec. 4.5
19) What are the respective concentrations (M) of and afforded by dissolving 0.500 mol in water and diluting to 1.33 L?
A) 0.665 and 0.665
B) 0.665 and 1.33
C) 1.33 and 0.665
D) 0.376 and 0.752
E) 0.752 and 0.376
Answer: E
Diff: 4
Page Ref: Sec. 4.5
19) A 17.5 mL sample of an acetic acid solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of acetic acid was ______M.
A) 0.158
B) 0.423
C) 134
D) 6.88
E) 0.214
Answer: B
Diff: 3
Page Ref: Sec. 4.6
20) The complete electron configuration of gallium, element 31, is ______.
A)
B)
C)
D)
E)
Answer: B
Diff: 1
Page Ref: Sec. 6.8
21) The ground state configuration of tungsten is ______.
A) [Ar]4s23d3
B) [Xe]6s24f145d4
C) [Ne]3s1
D) [Xe]6s24f7
E) [Kr]5s24d105p5
Answer: B
Diff: 2
Page Ref: Sec. 6.8
22) Which electron configuration represents a violation of Hund's rule for an atom in its ground state?
A)
B)
C)
D)
E)
Answer: B
Diff: 1
Page Ref: Sec. 6.8
23) Which one of the following configurations depicts an excited oxygen atom?
A)
B)
C)
D)
E)
Answer: B
Diff: 2
Page Ref: Sec. 6.8
24) A mole of red photons of wavelength 725 nm has ______kJ of energy.
A)
B)
C)
D) 165
E) 227
Answer: D
Diff: 3
Page Ref: Sec. 6.2
25) Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The frequency of this light is ______.
A)
B)
C)
D)
E)
Answer: A
Diff: 1
Page Ref: Sec. 6.1
26) If an electron has a principal quantum number (n) of 3 and an azimuthal quantum number (l) of 2, the subshell designation is ______.
A) 3p
B) 3d
C) 4s
D) 4p
E) 4d
Answer: B
Diff: 1
Page Ref: Sec. 6.7
27) Which one of the following is an incorrect subshell notation?
A) 4f
B) 2d
C) 3s
D) 2p
E) 3d
Answer: B
Diff: 1
Page Ref: Sec. 6.5
28) A tin atom has 50 electrons. Electrons in the ______subshell experience the lowest effective nuclear charge.
A) 1s
B) 3p
C) 3d
D) 5s
E) 5p
Answer: E
Diff: 2
Page Ref: Sec. 7.2
29) The ______have the most negative electron affinities.
A) alkaline earth metals
B) alkali metals
C) halogens
D) transition metals
E) chalcogens
Answer: C
Diff: 1
Page Ref: Sec. 7.4
30) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?
A) Mg > Na > P > Si > Ar
B) Ar > Si > P > Na > Mg
C) Si > P > Ar > Na > Mg
D) Na > Mg > Si > P > Ar
E) Ar > P > Si > Mg > Na
Answer: D
Diff: 1
Page Ref: Sec. 7.2
31) ______is isoelectronic with argon and ______is isoelectronic with neon.
A)
B)
C)
D)
E)
Answer: A
Diff: 1
Page Ref: Sec. 7.3
32) Of the choices below, which gives the order for first ionization energies?
A) Cl > S > Al > Ar > Si
B) Ar > Cl > S > Si > Al
C) Al > Si > S > Cl > Ar
D) Cl > S > Al > Si > Ar
E) S > Si > Cl > Al > Ar
Answer: B
Diff: 1
Page Ref: Sec. 7.4
…………………………….
33) Of the atoms below, ______is the most electronegative.
A) Si
B) Cl
C) Rb
D) Ca
E) S
Answer: B
Diff: 1
Page Ref: Sec. 8.4
34) Of the molecules below, the bond in ______is the most polar.
A) HBr
B) HI
C) HCl
D) HF
E)
Answer: D
Diff: 1
Page Ref: Sec. 8.4
35) Which of the following has the bonds correctly arranged in order of increasing polarity?
A)
B)
C)
D)
E)
Answer: B
Diff: 1
Page Ref: Sec. 8.4
36) In the nitrite ion , ______.
A) both bonds are single bonds
B) both bonds are double bonds
C) one bond is a double bond and the other is a single bond
D) both bonds are the same
E) there are 20 valence electrons
Answer: D – assuming the resonance
Diff: 2
Page Ref: Sec. 8.6
37) The central atom in ______does not violate the octet rule.
A)
B)
C)
D)
E)
Answer: C
Diff: 2
Page Ref: Sec. 8.7
38) How many equivalent resonance forms can be drawn for without expanding octet on the sulfur atom (sulfur is the central atom)?
A) 0
B) 2
C) 3
D) 4
E) 1
Answer: B
Diff: 1
Page Ref: Sec. 8.6
39) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ______.
A) 0
B) +1
C) -1
D) +2
E) -2
Answer: B
Diff: 1
Page Ref: Sec. 8.6
39) The Lewis structure of shows that the central phosphorus atom has ______nonbonding and ______bonding electron pairs.
A) 2, 2
B) 1, 3
C) 3, 1
D) 1, 2
E) 3, 3
Answer: B
Diff: 1
Page Ref: Sec. 8.5
…………………………………………..
…………………………..
40) The hybrid orbital set used by the central atom in is ______.
A) sp
B)
C)
D)
E)
Answer: C
Diff: 1
Page Ref: Sec. 9.5
41) The hybridization of nitrogen in the molecule is ______.
A) sp
B)
C)
D)
E)
Answer: A
Diff: 1
Page Ref: Sec. 9.6
42) The hybrid orbitals used for bonding by the sulfur atom in the molecule are ______orbitals.
A) sp
B)
C)
D)
E)
Answer: D
Diff: 1
Page Ref: Sec. 9.5
43) The molecular geometry of the molecule is ______, and this molecule is ______.
A) linear, nonpolar
B) linear, polar
C) bent, nonpolar
D) bent, polar
E) trigonal planar, polar
Answer: A
Diff: 1
Page Ref: Sec. 9.3
44) The atomic hybrid orbital set accommodates ______electron domains.
A) 2
B) 3
C) 4
D) 5
E) 6
Answer: B
Diff: 1
Page Ref: Sec. 9.5
45) The electron-domain geometry of the molecule is trigonal bipyramidal. The hybrid orbitals used by the As atom for bonding are ______orbitals.
A)
B)
C)
D)
E)
Answer: D
Diff: 1
Page Ref: Sec. 9.5
46) A balloon originally had a volume of 4.39 L at 44 °C and a pressure of 729 torr. The balloon must be cooled to ______°C to reduce its volume to 3.78 L (at constant pressure).
A) 38
B) 0
C) 72.9
D) 273
E) 546
Answer: B
Diff: 2
Page Ref: Sec. 10.3
47) Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation:
.
What mass (g) of is required to provide 40.0 L of at 25.0 °C and 763 torr?
A) 1.64
B) 1.09
C) 160
D) 71.1
E) 107
Answer: D
Diff: 4
Page Ref: Sec. 10.5
48) A vessel contained, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was ______torr.
A) 42.4
B) 521
C) 19.4
D) 239
E) 760
Answer: D
Diff: 2
Page Ref: Sec. 10.6
49) A sample of He gas (2.0 mmol) effused through a pinhole in 53 s. The same amount of an unknown gas, under the same conditions, effused through the pinhole in 248 s. The molecular mass of the unknown gas is ______g/mol.
A) 0.19
B) 5.5
C) 88
D) 19
E) 350
Answer: C
Diff: 4
Page Ref: Sec. 10.8
50) A sample of gas (2.0 mmol) effused through a pinhole in 5.5 s. It will take ______s for the same amount of to effuse under the same conditions.
A) 7.3
B) 5.5
C) 3.1
D) 4.2
E) 9.6
Answer: D
Diff: 4
Page Ref: Sec. 10.8
51) The kinetic-molecular theory predicts that pressure rises as the temperature of a gas increases because ______.
A) the average kinetic energy of the gas molecules decreases
B) the gas molecules collide more frequently with the wall
C) the gas molecules collide less frequently with the wall
D) the gas molecules collide more energetically with the wall
E) both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall
Answer: E
Diff: 2
Page Ref: Sec. 10.7
52) According to kinetic-molecular theory, in which of the following gases will the root-mean-square speed of the molecules be the highest at 200 °C?
A) HCl
B)
C)
D)
E) None. The molecules of all gases have the same root-mean-square speed at any given temperature.
Answer: C
Diff: 3
Page Ref: Sec. 10.7
53) Arrange the following gases in order of increasing average molecular speed at 25 °C.
He,, ,
A) He < < <
B) He < < <
C) < < < He
D) < < < He
E) < He < <