Exam Name Bonding and IMF practice test MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) There are paired and unpaired electrons in the Lewis symbol for a phosphorus atom. A) 0, 3 B) 2, 4 C) 4, 2 D) 4, 3 E) 2, 3 1) 2) Based on the octet rule, magnesium most likely forms a ion. 2) A) Mg6- B) Mg2- C) Mg6+ D) Mg- E) Mg2+ 3) The halogens, alkali metals, and alkaline earth metals have valence electrons, respectively. A) 7, 4, and 6 B) 2, 7, and 4 C) 7, 1, and 2 D) 1, 5, and 7 E) 8, 2, and 3 4) For a given arrangement of ions, the lattice energy increases as ionic radius and as ionic charge. A) decreases, increases B) increases, decreases C) decreases, decreases D) increases, increases E) This cannot be predicted. 3) 4) 5) Elements from opposite sides of the periodic table tend to form. 5) A) ionic compounds B) compounds that are gaseous at room temperature C) homonuclear diatomic compounds D) covalent compounds that are gaseous at room temperature E) covalent compounds 6) The ability of an atom in a molecule to attract electrons is best quantified by the. 6) A) paramagnetism B) first ionization potential C) electron change-to-mass ratio D) diamagnetism E) electronegativity 7) A nonpolar bond will form between two atoms of electronegativity. 7) A) identical, equal B) identical, different C) similar, different D) different, opposite E) different, different 8) How many equivalent resonance forms can be drawn for CO3 2- - (carbon is the central atom)? 8) A) 4 B) 1 C) 0 D) 2 E) 3 1
9) Using the table of average bond energies below, the H for the reaction is kj. 9) Bond: C C C-C H-I C-I C-H D (kj/mol): 839 348 299 240 413 A) -217 B) +160 C) +63 D) -160 E) -63 10) Using the table of average bond energies below, the H for the reaction is kj. 10) H-C C-H (g) + H-I (g) H2C CHI (g) Bond: C C C=C H-I C-I C-H D (kj/mol): 839 614 299 240 413 A) -129 B) +506 C) +129 D) -931 E) -506 11) Using the table of average bond energies below, the H for the reaction is kj. 11) C O (g) + 2H2 (g) H3C-O-H (g) Bond: C-O C=O C O C-H H-H O-H D (kj/mol): 358 799 1072 413 436 463 A) -735 B) -276 C) -116 D) +276 E) +735 12) Using the table of bond dissociation energies, the H for the following gas-phase reaction is kj. 12) Bond D (kj/mol) C-C 348 C C 614 C-H 413 H-Cl 431 C-Cl 328 A) 304 B) -38 C) 38 D) -44 E) 2134 2
13) Using the table of bond dissociation energies, the H for the following reaction is kj. 13) 2HCl (g) + F2 (g) 2HF (g) + Cl2 (g) Bond D (kj/mol) H-Cl 431 F-F 155 H-F 567 Cl-Cl 242 A) -223 B) 223 C) 208 D) -359 E) 359 14) The molecular geometry of the PHCl2 molecule is. 14) A) bent B) trigonal planar C) tetrahedral D) T-shaped E) trigonal pyramidal 15) The F-B-F bond angle in the BF3 molecule is. 15) A) 120 B) 60 C) 109.5 D) 180 E) 90 16) There are and bonds in the H2C C CH2 molecule. 16) A) 6, 4 B) 4, 2 C) 2, 2 D) 2, 6 E) 6, 2 17) There is/are bond(s) in the molecule below. 17) A) 1 B) 2 C) 12 D) 13 E) 18 18) There is/are bond(s) in the molecule below. 18) A) 0 B) 1 C) 2 D) 4 E) 16 3
19) The Lewis structure of carbon monoxide is given below. The hybridizations of the carbon and oxygen atoms in carbon monoxide are and, respectively. 19) : C O : A) sp2, sp3 B) sp, sp3 C) sp2, sp2 D) sp, sp E) sp3, sp2 20) The bond angle marked a in the following molecule is about. 20) A) 90 B) 120 C) 109.5 D) 60 E) 180 21) The bond angles marked a, b, and c in the molecule below are about,, and, respectively. 21) A) 109.5, 109.5, 109.5 B) 90, 180, 90 C) 120, 109.5, 120 D) 109.5, 109.5, 90 E) 109.5, 109.5, 120 22) The molecular geometry of the left-most carbon atom in the molecule below is. 22) A) tetrahedral B) octahedral C) T-shaped D) trigonal planar E) trigonal bipyramidal 4
Consider the following species when answering the following questions: (i) PCl3 (ii) CCl4 (iii) TeCl4 (iv) XeF4 (v) SF6 23) For which of the molecules is the molecular geometry (shape) the same as the VSEPR electron domain arrangement (electron domain geometry)? A) (i) and (ii) B) (i) and (iii) C) (ii) and (v) D) (iv) and (v) E) (v) only 23) 24) Of the molecules below, only is nonpolar. 24) A) TeCl2 B) CO2 C) NH3 D) HCl E) H2O 25) Of the molecules below, only is polar. 25) A) AsH3 B) SbF5 C) I2 D) SF6 E) CH4 26) Three monosulfur fluorides are observed: SF2, SF4, and SF6. Of these, is/are polar. 26) A) SF2, SF4, and SF6 B) SF2 and SF4 only C) SF4 only D) SF6 only E) SF2 only 27) The combination of two atomic orbitals results in the formation of molecular orbitals. 27) A) 1 B) 2 C) 3 D) 4 E) 0 28) The electron-domain geometry of a carbon-centered compound is tetrahedral. The hybridization of the central carbon atom is. A) sp3d2 B) sp C) sp3d D) sp3 E) sp2 29) The hybridization of the oxygen atom labeled y in the structure below is. The C-O-H bond angle is. 28) 29) A) sp3, 109.5 B) sp2, 109.5 C) sp, 180 D) sp, 90 E) sp3d2, 90 5
30) In order to exhibit delocalized bonding, a molecule must have. 30) A) at least four atoms B) at least two bonds C) at least two resonance structures D) at least three bonds E) trigonal planar electron domain geometry 31) The bond in ethylene, H2C CH2, results from the overlap of. 31) A) sp2 hybrid orbitals B) s atomic orbitals C) sp3 hybrid orbitals D) sp hybrid orbitals E) p atomic orbitals 32) Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? 32) Molecular Dipole Substance Mass (amu) 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) CH3CN B) CH3CH2CH3 C) CH3CHO D) CH3OCH3 E) CH3Cl 33) Of the following substances, only has London dispersion forces as its only intermolecular force. A) HCl B) CH3OH C) H2S D) NH3 E) CH4 33) 34) Of the following, is an exothermic process. 34) A) freezing B) melting C) boiling D) subliming E) All of the above are exothermic. 35) The substance with the largest heat of vaporization is. 35) A) O2 B) F2 C) Br2 D) Cl2 E) I2 6
36) The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the segment corresponds to the heat capacity of the liquid of the substance. A) AB B) BC C) CD D) DE E) EF 37) The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the segment corresponds to the heat capacity of the gas. A) AB B) BC C) CD D) DE E) EF 38) 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 Hvap of this substance. A) AB B) BC C) CD D) DE E) EF 39) Which of the following is not a type of solid? 36) 37) 38) 39) ionic molecular supercritical metallic covalent-network A) metallic B) ionic C) molecular D) supercritical E) covalent-network 40) solids consist of atoms or molecules held together by dipole-dipole forces, London disperson forces, and/or hydrogen bonds. A) Metallic and covalent-network B) Molecular C) Ionic D) Covalent-network E) Metallic 40) 7
41) Crystalline solids. 41) A) have highly ordered structures B) exist only at very low temperatures C) are usually very soft D) exist only at high temperatures E) have their particles arranged randomly 42) In liquids, the attractive intermolecular forces are. 42) A) very weak compared with kinetic energies of the molecules B) strong enough to hold molecules relatively close together C) strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other D) strong enough to keep the molecules confined to vibrating about their fixed lattice points E) not strong enough to keep molecules from moving past each other 43) Which one of the following exhibits dipole-dipole attraction between molecules? 43) A) CO2 B) XeF4 C) Cl2 D) BCl3 E) AsH3 44) are particularly polarizable. 44) A) Small nonpolar molecules B) Large nonpolar molecules C) Large polar molecules D) Small polar molecules E) Large molecules, regardless of their polarity, 45) The ease with which the charge distribution in a molecule can be distorted by an external electrical field is called the. A) electronegativity B) viscosity C) hydrogen bonding D) polarizability E) volatility 45) 46) Which one of the following derivatives of ethane has the highest boiling point? 46) A) C2I6 B) C2H6 C) C2Cl6 D) C2F6 E) C2Br6 47) Elemental iodine (I2) is a solid at room temperature. What is the major attractive force that exists among different I2 molecules in the solid? A) covalent-ionic interactions B) dipole-dipole rejections C) London dispersion forces D) dipole-dipole attractions E) ionic-dipole interactions 47) 8
48) Which one of the following substances will not have hydrogen bonding as one of its intermolecular forces? A) 48) B) C) D) E) 49) What types of intermolecular forces exist between NH3 and CBr4? 49) A) dispersion forces and hydrogen bonds B) dispersion forces, hydrogen bonds, and induced dipole-induced dipole forces C) dispersion forces and dipole-induced dipole forces D) dispersion forces, hydrogen bonds, and dipole-induced dipole forces E) dispersion forces and dipole-dipole forces 50) Which statements about viscosity are true? (i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases. (iii) Viscosity increases as intermolecular forces increase. A) (i) only B) (i) and (iii) C) (ii) and (iii) D) none E) all 50) 9
51) Based on the following information, which compound has the strongest intermolecular forces? 51) Substance Hvap (kj/mol) Argon (Ar) 6.3 Benzene (C6H6) 31.0 Ethanol (C2H5OH) 39.3 Water (H2O) 40.8 Methane (CH4) 9.2 A) Water B) Ethanol C) Benzene D) Argon E) Methane 52) The phase changes B C and D E are not associated with temperature increases because the heat energy is used up to. A) break intramolecular bonds B) increase the density of the sample C) increase the velocity of molecules D) increase distances between molecules E) rearrange atoms within molecules 53) Calculate the enthalpy change associated with the conversion of 25.0 grams of ice at -4.00 C to water vapor at 110.0 C. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively. For H2O, Hfus = 6.01 kj/mol and Hvap = 40.67 kj/mol. A) 1.00 x 105 kj B) 64.8 kj C) 75.9 kj D) 1.12 x 104 kj E) 1.11 x 104 kj 52) 53) 10
54) In general, the vapor pressure of a substance increases as increases. 54) A) viscosity B) molecular weight C) temperature D) surface tension E) hydrogen bonding 55) Some things take longer to cook at high altitudes than at low altitudes because. 55) A) water boils at a higher temperature at high altitude than at low altitude B) there is a higher moisture content in the air at high altitude C) heat isn't conducted as well in low density air D) natural gas flames don't burn as hot at high altitudes E) water boils at a lower temperature at high altitude than at low altitude 11