CHEM 1411-050 Chapter 8-13

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1) The hybridization of the carbon atom in carbon dioxide is ________. A) sp B) sp2 C) sp3 D)sp3d E) sp3d2

102) How may lone pair electrons are found on the central atom in a ClF3 molecule which has a ʺT-shapedʺ geometry? A) 2 B) 4 C) 0 D) 3 E) 1

103) The heating curve shown was generated by measuring the heat flow and temperature of a solid as it was heated. The heat flow into the sample in the segment D-E will yield the value of the ________ of this substance. A) ΔHvap B) ΔHrxn C) ΔHmelting D) ΔHsub E) ΔHfusion

105) The hybridizations of iodine in IF3 and IF5 are ________ and ________, respectively. A) sp3d, sp3d2 B) sp3d2, sp3d2 C) sp3, sp3d D) sp3d2, sp3d E) sp3d, sp3

113) CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO in the container was ________ atm. A) 6.29 B) 4.02 C) 10.3 D) 0.292 E) 1.60

116) Gaseous mixtures ________. A) are all homogeneous B) can only contain isolated atoms C) can only contain molecules D) are all heterogeneous . E) must contain both isolated atoms and molecules

122) What is the molality (m) of a solution containing 5.16 g of C6H12O6 in 183 mL of water? The density of water is 1.00 g/mL. A) 0.156 B) 0.00524 C) 0.0782 D) 28.2 E) 0.313

132) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ________. A) +1 B) -1 C) +2 D) -2 E) 0

136) If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy ________ L at STP. A) 25.5 B) 50.8 C) 12.9 D) 3.92 E) 5.08

142) The molecular geometry of the PF4+ ion is ________. A) tetrahedral B) octahedral C) trigonal planar D) trigonal bipyramidal E) trigonal pyramidal

144) The phase diagram of a substance is given above. The region that corresponds to the solid phase is ________. A) w B) x C) y D) z E) x and y

17) Calcium hydride (CaH2) reacts with water to form hydrogen gas: CaH2 (s) + 2H2O (l) → Ca(OH)2 (aq) + 2H2 (g) How many grams of CaH2 are needed to generate 48.0 L of H2 gas at a pressure of 0.995 atm and a temperature of 32 °C? A) 40.1 B) 0.954 C) 80.3 D) 161 E) 56.8

20) Which of the following does not have eight valence electrons? A) Ca+ B) Xe C) Br- D)Rb+ E) All of the above have eight valence electrons.

26) The phase diagram of a substance is shown above. The area labeled ________ indicates the solid phase for the substance. A) w B) x C) y D) z E) y and z

4) Which one of the following is least soluble in water? A) CH3CH2CH2CH2CH2OH B) CH3CH2CH2CH2OH C) CH3CH2OH D) CH3OH E) CH3CH2CH2OH

41) Using the VSEPR model, the electron-domain geometry of the central atom in O3 is ________. A) linear B) trigonal planar C) tetrahedral D) trigonal bipyramidal E) octahedral

70) The bond angle marked a in the following molecule is about ________. A) 120 B) 90 C) 109.5 D) 180 E) 60

101) Which of the following molecules would be expected to be attracted to a magnetic field? F2 N2 O2 . A) O2 only B) N2 and O2 C) N2 only D) F2 and N2 E) F2 and O2

104) The heating curve shown was generated by measuring the heat flow and temperature of a solid as it was heated. The heat flow into the sample in the segment ________ will yield the value of the ΔH fusion of this substance. A) AB B) BC C) CD D) DE E) EF

107) The sp2 atomic hybrid orbital set accommodates ________ electron domains. A) 2 B) 3 C) 4 D) 5 E) 6

109) To convert from one resonance structure to another, ________. A) neither electrons nor atoms can be moved B) only electrons can be moved C) only atoms can be moved D) electrons and atoms can both be moved E) electrons must be added

110) How many unhybridized p atomic orbital(s) are found in an sp-hybridized carbon atom? A) 0 B) 2 C) 4 D) 1 E) 3

112) The predominant intermolecular force in water is ________. A) London dispersion forces B) hydrogen bonding C) ionic bonding D) dipole-dipole forces E) ion-dipole forces

117) The Lewis structure of the CO32- ion is ________. A) B) C) D) E)

119) What mass (g) of carbon dioxide is contained in a 5.33 L vessel at 48 °C and 1.44 atm? A) 151 B) 12.8 C) 44.0 D) 6.62 × 10-3 E) 0.291

123) Using the VSEPR model, the electron-domain geometry of the central atom in ClF3 is ________. A) linear B) trigonal planar C) tetrahedral . D) trigonal bipyramidal E) octahedral

145) A 0.325 L flask filled with gas at 0.851 atm and 19 °C contains ________ mol of gas. A) 80.7 B) 0.0116 C) 0.0148 D) 12.4 E) 9.42

148) According to MO theory, overlap of two p atomic orbitals produces ________. A) one π MO and one σ* MO B) one π MO and one π* MO or one σ MO and one σ* MO C) one π+ MO and one σ* MO D) two π MOs, two π+ MOs, one σ MO, and one σ* MO E) one π MO and one σ MO

42) Using the VSEPR model, the molecular geometry of the central atom in PCl3 is ________. A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal

51) Bond enthalpy is ________. A) sometimes positive, sometimes negative B) always positive C) always negative D) always zero E) unpredictable

52) A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is ________ L at 469 K and 1.00 atm. A) 41.1 B) 90.5 C) 1.41 D) 57.9 E) 0.709

55) Of the bonds below, ________ is the least polar. A) C-F B) N-O C) K-Br D) C-O E) S-O

56) The concentration of lead nitrate (Pb(NO3)2) in a 0.926 M solution is ________ molal. The density of the solution is 1.202 g/mL. A) 0.770 B) 1.03 C) 0.819 D) 0.650 E) 2.13

81) An antibonding π orbital contains a maximum of ________ electrons. A) 1 B) 2 C) 4 D) 6 E) 8

87) The hybridization and molecular shape of the carbon atom in carbon dioxide is ________. A) sp2d2 and linear B) sp and linear C) sp2d and bent D) sp2 and linear E) sp3 and bent

88) Molecular Orbital theory correctly predicts diamagnetism of fluorine gas, F2. This is because ________. A) the FF bond enthalpy is very low B) all electrons in the MO electron configuration of F2 are paired C) there are more electrons in the bonding orbitals than in the antibonding orbitals D) the bond order in F2 can be shown to be equal to 1 E) the energy of the π2pMOs is higher than that of the σ2p MO

89) Of the following, ________ is a valid statement of Charlesʹ law. A) P/T = constant B) V = constant × P C) PV = constant D) V = constant × n E) V/T = constant

91) In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges ________ and the radii ________. A) decreases, increase, increase B) increases, increase, decrease C) increases, decrease, decrease D) increases, decrease, increase E) increases, increase, increase

78) On the phase diagram shown above, segment ________ corresponds to the conditions of temperature and pressure under which the solid and the gas of the substance are in equilibrium. A) AB B) BC C) AC D) CD E) AD

79) Of the bonds C-N, CN, and C≡N, the C-N bond is ________. A) strongest/shortest B) weakest/shortest C) weakest/longest D) strongest/longest E) intermediate in both strength and length

85) A gas mixture of Xe, Ne, and Ar has a total pressure of 12.20 atm. What is the mole fraction of Xe if the partial pressures of Ne and Ar are 2.10 and 4.50 atm, respectively? A) 0.848 B) 2.18 C) 0.459 D) 5.60 E) 1.18

98) Electropositivity ________ from left to right within a period and ________ from top to bottom within a group. A) increases, decreases B) stays the same, increases C) decreases, increases D) increases, stays the same E) increases, increases

12) One significant difference between gases and liquids is that ________. A) a gas may consist of both elements and compounds B) gases are always mixtures C) a gas is made up of molecules D) a gas expands to fill its container E) All of the above answers are correct.

121) The molecular geometry of the H3O+ ion is ________. A) tetrahedral B) linear C) octahedral D) trigonal pyramidal E) bent

125) The electron-domain geometry of a sulfur-centered compound is trigonal bipyramidal. The hybridization of the central sulfur atom is ________. A) sp B) sp2 C) sp3 D) sp3d E) sp3d2

126) Electronegativity ________ from left to right within a period and ________ from top to bottom within a group. A) increases, increases B) stays the same, increases C) increases, stays the same D) increases, decreases E) decreases, increases

127) A fixed amount of gas at 25.0 °C occupies a volume of 8.66 L when the pressure is 629 torr. Use Charlesʹs law to calculate the volume (L) the gas will occupy when the temperature is increased to 112 °C while maintaining the pressure at 629 torr. A) 6.70 B) 1.93 C) 9.26 D) 11.2 E) 38.8

129) What is the total pressure (atm) in a 10.0 L vessel that contains 2.34 mol of carbon dioxide, 1.73 mol of sulfur dioxide, and 4.50 mol of argon at standard temperature? A) 0.192 B) 192 C) 0.0192 D) 19.2 E) 1.92

135) The phase diagram of a substance is given above. This substance is a ________ at 30 °C and 0.5 atm. A) supercritical fluid B) crystal C) liquid . D) gas E) solid

137) The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H 2O is ________ molal. A) 96 B) 6.3 C) 0.68 D) 6.8 E) 0.11

138) 13.3 g of benzene (C6H6) is dissolved in 282 g of carbon tetrachloride. What is the molal concentration of benzene in this solution? A) 0.0851 B) 0.0450 C) 6.04 × 10-4 D) 0.604 E) 4.50

139) In a saturated solution of a salt in water, ________. A) addition of more water causes massive crystallization . B) the rate of dissolution > the rate of crystallization C) seed crystal addition may cause massive crystallization D) the rate of crystallization = the rate of dissolution E) the rate of crystallization > the rate of dissolution

14) A solution is prepared by dissolving 15.8 g of MgCl2 in 255 g of water. What is the mole fraction of Cl- in this solution? A) 0.00583 B) 0.977 C) 0.0116 D) 0.0232 E) 0.988

140) What is the molecular weight (g/mol) of an unknown gas that has a density of 3.59 g/L at STP? A) 87.9 B) 8.15 × 103 C) 0.0879 D) 80.5 E) 7.37

141) In liquids, the attractive intermolecular forces are ________. A) very weak compared with kinetic energies of the molecules B) strong enough to keep the molecules confined to vibrating about their fixed lattice points C) strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other D) not strong enough to keep molecules from moving past each other E) strong enough to hold molecules relatively close together

147) What is the molal concentration of KCl in a solution prepared by adding 2.11 mol of KCl to 889 g of water? A) 0.421 B) 421 C) 2.37 × 10-3 D) 2.37 E) 1.88 × 103

150) When four atomic orbitals are mixed to form hybrid orbitals, how many hybrid orbitals are formed? A) six B) five C) one D) four E) three

23) As the number of covalent bonds between two atoms increases, the distance between the atoms ________ and the strength of the bond between them ________. A) increases, increases B) decreases, decreases C) increases, decreases D) decreases, increases E) is unpredictable, is unpredictable

25) According to the phase diagram shown above, what is the normal melting point ( °C)? A) 10 B) 38 C) -13 D) 0 E) 29

3) The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the ________. A) strength of the covalent bond in NaCl B) strong solvent-solvent interactions C) hydrogen bonding in C6H6 D) weak solvation of Na+ and Cl- by C6H6 E) increased disorder due to mixing of solute and solvent

37) What is the mole fraction of nitric acid in a(n) 8.46% (by mass) aqueous solution of nitric acid? A) 0.0433 B) 0.0830 C) 0.0208 D) 0.0257 E) The density of the solution is needed to solve the problem.

54) What is the molality of LiCl in solution that is 9.0% by mass LiCl and has a density of 1.00 g/mL? A) 2.12 B) 0.0900 C) 90.0 D) 2.33 E) 9.00

61) How much CO2 (L) is produced when 2.10 kg of sodium bicarbonate reacts with excess hydrochloric acid at 25.0 °C and 1.23 atm? A) 4.98 × 10-1 B) 4.17 × 101 C) 3.50 D) 4.98 × 102 E) 4.17 × 10-1

67) In counting the electron domains around the central atom in VSEPR theory, a ________ is not included. A) double covalent bond B) nonbonding pair of electrons C) single covalent bond D) core level electron pair E) triple covalent bond

86) A pressure of 0.500 atm is the same as a pressure of ________ of mm Hg. A) 760. B) 33.0 C) 29.9 D) 380. E) 193

90) The amount of gas that occupies 36.52 L at 68.0 °C and 672 mm Hg is ________ mol. A) 127 B) 12.7 C) 24.4 D) 1.15 E) 878

95) Of the atoms below, ________ is the most electronegative. A) Al B) B C) Ge D) C E) Si

106) The more effectively two atomic orbitals overlap, ________. A) the fewer antibonding MOs will be produced by the combination B) the more bonding MOs will be produced by the combination C) the higher will be the energy of the resulting bonding MO and the lower will be the energy of the resulting antibonding MO D) the higher will be the energies of both bonding and antibonding MOs that result E) the lower will be the energy of the resulting bonding MO and the higher will be the energy of the resulting antibonding MO

114) Heat of sublimation can be approximated by adding together ________ and ________. A) heat of freezing (solidification), heat of vaporization B) heat of fusion, heat of condensation C) heat of freezing (solidification), heat of condensation D) heat of deposition, heat of vaporization E) heat of fusion, heat of vaporization

115) What is the temperature at STP? A) 25 °C B) 298 k C) -32 °F D) 0 k E) 0 °C

118) Which of the following does not have eight valence electrons? A) Rb+ B) Ti+4 C) Xe D) Cl- E) Sr+

124) Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? Substance Molecular Mass (amu) Dipole Moment (D) Propane, CH3CH2CH3 44 0.1 . Dimethylether, CH3OCH3 46 1.3 Methylchloride, CH3Cl 50 1.9 Acetaldehyde, CH3CHO 44 2.7 Acetonitrile, CH3CN 41 3.9 . A) CH3CH2CH3 B) CH3OCH3 C) CH3Cl D) CH3CHO E) CH3CN

131) Resonance structures differ by ________. A) placement of atoms only B) number of atoms only C) number of electrons only D) number and placement of electrons E) placement of electrons only

133) What is the mole fraction of HCl in a solution that is prepared by dissolving 25.5 g of HCl in 800. g of water? The density of the solution is 1.0 g/mL. A) 32.0 B) 0.984 C) 0.0319 D) 0.874 E) 0.0155

134) What is the predominant intermolecular force in HCN? A) ionic bonding B) hydrogen bonding C) ion-dipole attraction D) London dispersion forces E) dipole-dipole attraction

143) In general, the vapor pressure of a substance increases as ________ increases. A) molecular weight B) viscosity C) temperature D) hydrogen bonding E) surface tension

15) How many hybrid orbitals are formed upon the mixing of three atomic orbitals? A) four B) six C) five D) one E) three

83) Mixing one s atomic orbital and one p atomic orbital gives rise to ________. A) three sp hybrid orbitals B) two sp hybrid orbitals C) three sp2 hybrid orbitals D) two sp2 hybrid orbitals E) two sp3 hybrid orbitals

92) Of the molecules below, the bond in ________ is the most polar. A) HI B) HF C) HBr D) HCl E) H2

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is ________ molal. A) 5.70 B) 0.569 C) 1.76 D) 63.2 E) 0.214

33) 5.25 g of zinc metal reacts with excess sulfuric acid to produce hydrogen gas. What volume (L) of hydrogen is generated at STP? A) 118 B) 0.136 C) 1.80 D) 1.97 E) 129

38) The order of MO energies in B2, C2, and N2 (σ2p > π2p), is different from the order in O2, F2, and Ne2 (σ2p < π2p). This is due to ________. A) less effective overlap of p orbitals in B2, C2, and N2 B) less effective overlap of p orbitals in O2, F2, and Ne2 C) greater 2s-2p interaction in B2, C2, and N2 D) greater 2s-2p interaction in O2, F2, and Ne2 E) the more metallic character of boron, carbon and nitrogen as compared to oxygen, fluorine, and neon

39) Of the following, ________ cannot accommodate more than an octet of electrons. A) Sb B) Ni C) Be D) Sc E) Os

45) 760 torr is equivalent to ________ mm Hg. A) 380 B) 1 C) 760 D) 121 E) 4.78 × 103

48) Based on molecular orbital theory, the bond order of the NN bond in the N2 molecule is ________. A) 0 B) 1 C) 2 D) 3 E) 1/2

50) There is/are ________ π bond(s) in the molecule below. A) 7 B) 2 C) 1 D) 0 E) 6

57) The central atom in ________ does not violate the octet rule. A) ICl4- B) XeF4 C) CF4 D) SF4 E) KrF2

58) Which two bonds are most similar in polarity? A) O-F and Cl-F . B) C-Cl and Be-Cl C) B-F and Cl-F D) I-Br and Si-Cl E) Al-Cl and I-Br

6) The density of krypton gas at 0.866 atm and 44.4 °C is ________ g/L. A) 0.359 B) 0.238 C) 2.78 D) 5.57 E) 0.0332

60) How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom? A) 2 B) 4 C) 3 D) 1 E) 5

69) 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 3.99 L (at constant pressure). A) -288 B) 288 C) 15.1 D) 546 E) 0.00

71) Of the following, only ________ has sp2 hybridization of the central atom. A) HCN B) ICl3 C) BF3 D) NF3 E) CH4

72) Which one of the following exhibits dipole-dipole attraction between molecules? A) CF4 B) SF6 C) NH3 D) O2 E) C10H22

73) The volume of 1.26 mol of gas at 69.4 kPa and 25.30 °C is ________ L. A) 0.439 B) 0.445 C) 45.1 D) 633 E) 3.82

65) A sample of Ne gas (2.5 L) at 4.5 atm and 25 °C was combined with 2.2 L of Ar gas at 6.3 atm and 25 °C at constant temperature in a 8.0 L flask. Assuming the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C, what is the total pressure (atm) in the flask? A) 5.34 B) 10.0 C) 11.4 D) 10.8 E) 3.14

66) According to valence bond theory, which orbitals overlap in the formation of the bond in Cl2? A) 2p on Cl and 2p on Cl B) 3s on Cl and 3s on Cl C) 4p on Cl and 4p on Cl D) sp on Cl and sp on Cl E) 3p on Cl and 3p on Cl

75) The bond angles marked a, b, and c in the molecule below are about ________, ________, and ________, respectively. A) 120°, 109.5°, 120° B) 109.5°, 109.5°, 90° C) 109.5°, 109.5°, 109.5° D) 90°, 180°, 90° E) 109.5°, 109.5°, 120°

76) On the phase diagram shown above, the coordinates of point B corresponds to the ________. A) triple point B) critical pressure C) critical temperature and pressure D) boiling point E) critical temperature

97) Which of the following gases would have a similar rate of effusion to CO at 350 K? A) H2 B) CO2 C) He D) NO2 E) N2

99) Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g) . In an experiment, 177 mL of wet H2 is collected over water at 27 °C and a barometric pressure of 766 torr. The vapor pressure of water at 27 °C is 26.74 torr. The partial pressure of hydrogen in this experiment is ________ atm. A) 1.01 B) 739 C) 793 D) 1.04 E) 0.972

108) A gas mixture of N2 and H2 has a total pressure of 9.40 atm and contains 11.3 mol of gas. If the partial pressure of N2 is 4.89 atm, how many moles of H2 are in the mixture? A) 5.65 B) 5.88 C) 5.42 D) 4.51 E) 11.3

111) Calculate the mole fraction of phosphoric acid (H3PO4) in a 38.5% (by mass) aqueous solution. A) 0.206 B) 0.115 C) 0.103 D) 0.0516 E) The density of the solution is needed to solve the problem.

120) The hybridization of orbitals on the central atom in a molecule is sp. The electron-domain geometry around this central atom is ________. A) octahedral B) tetrahedral C) linear D) trigonal bipyramidal E) trigonal planar

128) The volume of a sample of gas (2.49 g) was 752 mL at 1.98 atm and 62 °C. The gas is ________. A) SO2 B) SO3 C) NO2 D) NH3 E) Ne

130) For ________ forms of a molecule or ion, the observed structure is an average of the ________ forms. A) resonance, metallic B) ionic, resonance C) resonance, ionic D) resonance, covalent E) resonance, resonance

146) Which species has London dispersion forces as the only intermolecular force? A) KBr B) CH3OH C) CH3CH3 D) CH3F E) HI

149) The F-B-F bond angle in the BF3 molecule is ________. A) 90° B) 109.5° C) 120° D) 180° E) 60°

43) The molecular geometry of the right-most carbon in the molecule below is ________. A) trigonal planar B) tetrahedral C) trigonal bipyramidal D) T-shaped E) octahedral

44) A sample of hydrogen gas (3.2 L) at 3.5 atm and 25 °C was combined with 5.2 L of nitrogen gas at 7.3 atm and 25 °C at constant temperature in a 15.0 L flask. Assuming the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C, what is the total pressure (atm) in the flask? A) 3.28 B) 15.4 C) 5.85 D) 9.45 E) 10.8

46) Lattice energy is ________. A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase B) the energy given off when gaseous ions combine to form one mole of an ionic solid C) the sum of electron affinities of the components in an ionic solid D) the sum of ionization energies of the components in an ionic solid E) the energy required to produce one mole of an ionic compound from its constituent elements in their standard states

5) Which of the following has the bonds correctly arranged in order of increasing polarity? A) Be-F, Mg-F, N-F, O-F B) O-F, N-F, Be-F, Mg-F C) O-F, Be-F, Mg-F, N-F D) Mg-F, Be-F, N-F, O-F E) N-F, Be-F, Mg-F, O-F

64) The type of compound that is most likely to contain a covalent bond is ________. A) one that is composed of only nonmetals B) a solid metal C) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table D) held together by the electrostatic forces between oppositely charged ions E) There is no general rule to predict covalency in bonds.

74) Which one of the following substances is more likely to dissolve in CCl4? A) CH3CH2OH B) CBr4 C) HBr D) HCl E) NaCl

77) On the phase diagram shown above, the coordinates of point ________ correspond to the triple point. A) A B) B C) C D) D E) E

80) Which of the following has eight valence electrons? A) Kr B) Cl C)Ti4+ D) Na+ E) all of the above

82) What is the predominant intramolecular force in NaNO3? A) ionic bonding B) dipole-dipole attraction . C) hydrogen bonding D) ion-dipole attraction . E) London-dispersion forces

93) Valence bond theory addresses all of the following except ________. A) excited states of molecules B) molecular shape C) multiple bonds D) hybridization E) covalent bonding

96) Hydrogen bonding is a special case of ________. A) dipole-dipole attractions B) ion-dipole attraction C) ion-ion interactions D) London-dispersion forces E) none of the above

For the questions that follow, consider the BEST Lewis structures of the following oxyanions: (i) NO2- (ii) NO3- (iii) SO32- (iv) SO42- (v) BrO3- 94) There can be three equivalent best resonance structures of ________. A) (ii), (iii), and (v) B) (iii), (iv), and (v) C) (i) and (ii) D) (iii) and (v) E) all

53) There are ________ σ and ________ π bonds in the H2C=C=CH2 molecule. A) 2, 6 B) 4, 2 C) 6, 4 D) 2, 2 E) 6, 2

18) 34.9 grams of hydrogen gas and 17.7 grams of methane gas are combined in a reaction vessel with a total pressure at 2.92 atm. What is the partial pressure (atm) of hydrogen gas? A) 0.175 B) 2.75 C) 53.8 D) 50.5 E) 5.53

24) The Lewis structure of N2H2 shows ________. A) each nitrogen has two nonbonding electron pairs B) each nitrogen has one nonbonding electron pair C) a nitrogen-nitrogen single bond D) each hydrogen has one nonbonding electron pair E) a nitrogen-nitrogen triple bond

29) The phase diagram of a substance is shown above. The area labeled ________ indicates the liquid phase for the substance. A) w B) x C) y D) z E) y and z

32) The reaction of 50 mL of Cl2 gas with 50 mL of C2H4 gas via the equation: Cl2 (g) + C2H4 (g) → C2H4Cl2 (g) will produce a total of ________ mL of products if pressure and temperature are kept constant. A) 125 B) 50 C) 150 D) 100 E) 25

35) Which of the following Lewis structures would be an expansion to the octet rule? A) CCl4 B) SO3 C) PH3 D) PCl3 E) CO2

40) Of the molecules below, only ________ is polar. A) SiCl4 B) SeF4 C) CH4 D) CCl4

47) Based on the octet rule, phosphorus most likely forms a ________ ion. A) P5+ B) P3- C) P5- D) P+ E) P3+

68) Which of the following molecules has London Forces as its only intermolecular force? A) H2O B) CH3CH3 C) CH3CH2NH2 D) HOCH2CH2OH E) None, all of the above exhibit dispersion forces.

8) Of the following species, ________ will have bond angles of 120 °. A) NCl3 B) BCl3 C) ClF3 D) PH3 E) All of these will have bond angles of 120°.

13) A triple bond consists of ________ pairs of electrons shared between two atoms. A) 1 B) 2 C) 3 D) 4 E) 6

16) A sample of gas (1.3 mol) occupies ________ L at 22 °C and 4.0 atm. A) 0.59 B) 0.032 C) 7.9 D) 13 E) 0.079

19) Which one of the following exhibits dipole-dipole attraction between molecules? A) CF4 B) HCl C) BI3 D) CS2 E) F2

21) In order to produce sp2 hybrid orbitals, ________ s atomic orbital(s) and ________ p atomic orbital(s) must be mixed. A) two, two B) one, one C) one, two D) one, three E) two, three

27) The phase diagram of a substance is shown above. The area labeled ________ indicates the gas phase for the substance. A) w B) x C) y D) z E) y and z

28) According to the phase diagram shown above, what is the normal boiling point (°C)? A) 10 B) -3 C) 29 D) 0 E) 38

31) A gas originally at 27 °C and 1.00 atm pressure in a 3.3 L flask is cooled at constant pressure until the temperature is 11 °C. The new volume of the gas is ________ L. A) 0.27 B) 3.5 C) 3.1 D) 3.3 E) 0.24

59) A typical double bond ________. A) consists of two shared electron pairs B) consists of one σ bond and one π bond C) imparts rigidity to a molecule D) is stronger and shorter than a single bond . E) All of the above answers are correct.

100) In which of the molecules below is the carbon-carbon distance the shortest? A) H2C-C-CH2 B) H2C-CH2 C) H3C-CH2-CH3 D) H-C≡C-H . E) H3C-CH3

11) The hybrid orbitals used for bonding by the sulfur atom in the SF4 molecule are ________ orbitals. A) sp B) sp2 C) sp3 D) sp3d E) sp3d2

7) Which statement is true about liquids but not true about solids? A) They assume both the volume and the shape of their containers. B) They are highly ordered and not compressible. C) They flow and are compressible. D) They flow and are not compressible. E) They flow and are highly ordered.

84) The bond angles marked a, b, and c in the molecule below are about ________, ________, and ________, respectively. A) 109.5°, 90°, 120° B) 120°, 120°, 109.5° C) 90°, 90°, 90° D) 109.5°, 120°, 109.5° E) 120°, 120°, 90°

9) Why donʹt we draw double bonds between the Be atom and the Cl atoms in BeCl2? A) That would result in more than eight electrons around beryllium. B) That would result in the formal charges not adding up to zero. C) There arenʹt enough electrons. D) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. E) That would result in more than eight electrons around each chlorine atom.

62) In order to produce sp3 hybrid orbitals, ________ s atomic orbital(s) and ________ p atomic orbital(s) must be mixed. A) one, one B) one, two C) two, two D) two, three E) one, three

63) The central atom in ________ violates the octet rule. A) Cl2 B) SF2 C) FCN D) Br2CO E) PF5

10) A gas in a 57.1 L pressure container at 24.9 °C and 889.8 mm Hg contains ________ moles. A) 2080 B) 32.7 C) 0.0270 D) 0.366 E) 2.73

22) The highest energy occupied molecular orbital in the FF bond of the F2 molecule is ________. A) π*2s B) π2s C) σ*1p D) π2p E) π*2p

30) CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The total pressure in the container was ________ atm. A) 0.292 B) 1.60 C) 4.02 D) 6.31 E) 10.3

34) Of the following substances, ________ has the highest boiling point. A) N2 B) CH3CH2OH C) C4H10 D) Cl2 E) HOCH2CH2CH2OH

36) The angles between sp2 orbitals are ________. A) 90° B) 45° C) 109.5° D) 180° E) 120°

49) What is the density of carbon dioxide gas (g/L) at 1106.2 mm Hg and 56.3 °C? A) 0.0234 B) 13.9 C) 0.0538 D) 1800 E) 2.37

CHEM 1411-050 Chapter 8-13

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