d. natural gas flames don't burn as hot at high altitudes A) Cl C l B ) S i S i C ) C a C l D ) C r B r E ) P C l A n s : E C a t e g o r y : M e d i u m S e c t i o n : 9 . A C 60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N 2 O. C3H8 or CH3OCH3 Ans: CH3OCH3 Category:Medium Section:11.2 37. h|g CJ UVaJ h>* B*H*ph "j h|g h|g B*EHUph jn5(M A) CaCl2 B) CO2 C) CS2 D) SO2 E) OF2 Ans:A Category:Easy Section:9.2 2. A) PBr5 B) CCl4 C) BrF5 D) XeF2 E) XeF4 Ans:C Category:Medium Section:10.2 23. B R E E 4 2 E ) E M B E D E q u a t i o n . A) 0 lone pairs, tetrahedral B) 1 lone pair, distorted tetrahedron (seesaw) C) 1 lone pair, square pyramidal D) 1 lone pair, tetrahedral E) 2 lone pairs, square planar Ans:E Category:Medium Section:10.1 4. Which of the following solids would have the lowest melting point? Give the number of lone pairs around the central atom and the molecular geometry of XeF4. m n x y ) * 4 5 ? A) N2O B) CS2 C) PH3 D) CCl4 E) NO2 Ans:E Category:Medium Section:9.9 40. Large intermolecular forces in a substance are manifested by __________. e. all of the above, A volatile liquid is one that __________. In contrast, the hydrides of the lightest members of groups 1517 have boiling points that are more than 100C greater than predicted on the basis of their molar masses. e. melts rather than sublimes under ordinary conditions, Crystalline solids differ from amorphous solids in that crystalline solids have_____ Doubling the distance therefore decreases the attractive energy by 26, or 64-fold. Ans:D Category:Medium Section:10.2 20. Which one of the following is most likely to be a covalent compound? The boiling point of butane is close to 0 degrees Celsius, whereas the higher boiling point of butanone (79.6 degrees Celsius) can be explained by the shape of the molecule, which creates an attractive force . Write the Lewis structure of boron trifluoride. D) square planar. Which of the following ionic solids would have the largest lattice energy? A) NaF B) NaCl C) NaBr D) NaI Ans:A Category:Medium Section:9.3 49. Of the following, __________ has the highest boiling point. Because the boiling points of nonpolar substances increase rapidly with molecular mass, C60 should boil at a higher temperature than the other nonionic substances. They need more energy to escape to the gas phase, so the larger molecule has the higher boiling point. Arrange ethyl methyl ether (CH3OCH2CH3), 2-methylpropane [isobutane, (CH3)2CHCH3], and acetone (CH3COCH3) in order of increasing boiling points. Give the number of lone pairs around the central atom and the molecular geometry of SCl2. a. London-dispersion forces b. ion-dipole attraction c. dipole-dipole attractions d. ion-ion interactions e. none of the above, The predominant intermolecular force in (CH3)2NH is __________. Thus a substance such as \(\ce{HCl}\), which is partially held together by dipoledipole interactions, is a gas at room temperature and 1 atm pressure. B) covalent solid. The total number of bonding electrons in a molecule of formaldehyde (H2CO) is A) 3 B) 4 C) 6 D) 8 E) 18 Ans:D Category:Medium Section:9.6 29. Given the large difference in the strengths of intra- and intermolecular forces, changes between the solid, liquid, and gaseous states almost invariably occur for molecular substances without breaking covalent bonds. 1. A) ethanol, bp = 78C. The bridging hydrogen atoms are not equidistant from the two oxygen atoms they connect, however. Recall that the attractive energy between two ions is proportional to 1/r, where r is the distance between the ions. The strengths of London dispersion forces also depend significantly on molecular shape because shape determines how much of one molecule can interact with its neighboring molecules at any given time. a. Ans:B Category:Easy Section:11.2 6. h|g CJ UVaJ "j h|g h|g B*EHUph jk5(M d. Covalent-network e. Metallic and covalent-network, Crystalline solids __________. A) NF3 B) CO2 C) CF4 D) Br2 E) NO Ans:E Category:Medium Section:9.9 36. Which of the following Lewis structures is incorrect? Which of the following solids would have the highest melting point? a. have their particles arranged randomly H o w m u c h e n e r g y ( h e a t ) i s r e q u i r e d t o c o n v e r t 5 2 . 2and1 Study with Quizlet and memorize flashcards containing terms like 1) As a gaseous element condenses, the atoms become ___ and they have ___ attraction for ____ one another. )%2F11%253A_Liquids_and_Intermolecular_Forces%2F11.02%253A_Intermolecular_Forces, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). A) NF3 B) H2O C) AsCl3 D) GeH4 E) BF3 Ans:E Category:Medium Section:9.9 38. b. sublimesratherthanmeltsunderordinary conditions Heat of sublimation can be approximated by adding together __________ and __________. Explain your reasoning. 6 k J D ) 2 7 , 6 0 0 J E ) 2 5 , 0 0 0 k J A n s : A C a t e g o r y : M e d i u m S e c t i o n : 1 1 . A larger molecule is more polarizable, which is an attraction that keeps the molecules together. Write a Lewis structure for SO3 that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s). C) a dispersion force. D) dipole-induced dipole forces. As a result, it is relatively easy to temporarily deform the electron distribution to generate an instantaneous or induced dipole. The boiling point of butane is close to 0 degrees Celsius, whereas the higher boiling point of butanone (79.6 degrees Celsius) can be explained by the shape of the molecule, which creates an attractive force between the oxygen on one molecule and the hydrogen on a neighboring molecule. Instantaneous dipoleinduced dipole interactions between nonpolar molecules can produce intermolecular attractions just as they produce interatomic attractions in monatomic substances like Xe. Which one of the following compounds does not follow the octet rule? a. dipole-dipole b. ion-ion c. hydrogen bonding d. ion-dipole e. London dispersion force. In larger atoms such as Xe, however, the outer electrons are much less strongly attracted to the nucleus because of filled intervening shells. h|g h|g B*EHUph jj5(M All molecules have kinetic energy; they are vibrating. Which of the following ionic solids would have the largest lattice energy? Of the following, _____ has the highest boiling point. Indicate all the types of intermolecular forces of attraction in C2H6(g). > }  | j k l m [ y W bjbj D { { g ` | | 8 " $ f. Z ( ] ] ] %- '- '- '- '- '- '- $ ^/ 2 K- ] ] ] ] ] K- . 1and8 d. the same thing Intermolecular forces are generally much weaker than covalent bonds. D) temperature is greater than room temperature. b. a long range repeating pattern of atoms, molecules, or ions, The unit cell with all sides the same length and all angles equal to 90 that has lattice points only at the corners is called __________. This question was answered by Fritz London (19001954), a German physicist who later worked in the United States. A polar covalent bond would form in which one of the following pairs of atoms? This effect, illustrated for two H2 molecules in part (b) in Figure \(\PageIndex{3}\), tends to become more pronounced as atomic and molecular masses increase (Table \(\PageIndex{2}\)). e. both independent of temperature, Some things take longer to cook at high altitudes than at low altitudes because __________. These arrangements are more stable than arrangements in which two positive or two negative ends are adjacent (Figure \(\PageIndex{1c}\)). There are two additional types of electrostatic interaction that you are already familiar with: the ionion interactions that are responsible for ionic bonding, and the iondipole interactions that occur when ionic substances dissolve in a polar substance such as water. Which property of water allows a razor blade to float on it without sinking? The F S F bond angles in SF6 are A) 90 and 180 B) 109.5 C) 120 D) 180 E) 90 and 120 Ans:A Category:Medium Section:10.1 18. a. low vapor pressure A C60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N2O. A) 1 B) 2 C) 4 D) 6 E) 8 Ans:B Category:Medium Section:11.4 21. A) CBr4 B) CBr3F C) CBr2F2 D) CBrF3 E) CF4 Ans:E Category:Medium Section:11.2 8. (ii) Viscosity increases as molecular weight increases. @ J K \ ]  & ' 1 2 3 4 @ A , - a b v w x y "j h|g h|g B*EHUph jc5(M Bond strength rated strongest to weakest:Ionic > H-bond > Dipole > van der Waals Fewer functional groups > More functional groups (Amide>Acid>Alcohol>Ketone or Aldehyde>Amine>Ester>Alkane). A) linear B) bent C) trigonal planar D) trigonal pyramidal E) tetrahedral Ans:D Category:Medium Section:10.1 7. In nuclear fission, a nucleus of uranium-238, which contains 92 protons, can divide into two smaller spheres, each having 46 protons and a radius of 5.9010155.90 \times 10 - 155.901015 m. What is the magnitude of the repulsive electric force pushing the two spheres apart? h|g CJ UVaJ "j h|g h|g B*EHUph jm5(M very soft A molecule with a double-bonded oxygen, like butanone (C4H8O) is peaked in the middle where the oxygen is bonded to the carbon chain. Butter melts over a range of temperature, rather than with a sharp melting point. D) the temperature. 5 2 2 . B) ion-dipole forces. 5 2 1 . C) water, bp = 100C. Source: Dispersion Intermolecular Force, YouTube(opens in new window) [youtu.be]. Ans:D Category:Medium Section:11.3 15. a. can go from solid to liquid, within a small temperature range, via the application of pressure Cooking times for boiled food need to be changed to ensure the food is completely cooked. The four compounds are alkanes and nonpolar, so London dispersion forces are the only important intermolecular forces. Intermolecular forces determine bulk properties, such as the melting points of solids and the boiling points of liquids. A) Sr B) V C) Ni D) P E) I Ans:A Category:Medium Section:9.5 19. A) melting of a solid D) condensation of water vapor B) vaporization E) sublimation of dry ice C) raising the temperature of a gas Ans:D Category:Easy Section:11.8 25. B R E E 4 B ) E M B E D E q u a t i o n . Ans:A Category:Medium Section:11.8 26. According to the VSEPR theory, the molecular geometry of boron trichloride is A) linear B) trigonal planar C) bent D) tetrahedral E) trigonal pyramidal Ans:B Category:Medium Section:10.1 11. If a substance is both a hydrogen donor and a hydrogen bond acceptor, draw a structure showing the hydrogen bonding. Draw the hydrogen-bonded structures. A) Na B) As C) Ga D) Cs E) Sb Ans:B Category:Medium Section:9.5 16. A bonding molecular orbital is of lower energy (more stable) than the atomic orbitals from which it was formed. Considering CH3OH, C2H6, Xe, and (CH3)3N, which can form hydrogen bonds with themselves? Which one of the following molecules is nonpolar? %, %, %, ] Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. 0 g o f i c e a t 1 0 . e. dipole-dipole attractions, Hydrogen bonding is a special case of __________. The Lewis dot symbol for the calcium ion is A) EMBED Equation.BREE42+ B) C a C ) E M B E D E q u a t i o n . Because electrostatic interactions fall off rapidly with increasing distance between molecules, intermolecular interactions are most important for solids and liquids, where the molecules are close together. How many sigma bonds and pi bonds are contained in a ibuprofen molecule? c. high heats of fusion and vaporization CH3OH. Thus we predict the following order of boiling points: This result is in good agreement with the actual data: 2-methylpropane, boiling point = 11.7C, and the dipole moment () = 0.13 D; methyl ethyl ether, boiling point = 7.4C and = 1.17 D; acetone, boiling point = 56.1C and = 2.88 D. Arrange carbon tetrafluoride (CF4), ethyl methyl sulfide (CH3SC2H5), dimethyl sulfoxide [(CH3)2S=O], and 2-methylbutane [isopentane, (CH3)2CHCH2CH3] in order of decreasing boiling points. a. London dispersion forces b. ion-dipole forces c. ionic bonding d. dipole-dipole forces A.Hydrogen bonds involve hydrogen bonded to carbon, nitrogen, oxygen, or fluorine. Ans: Category:Medium Section:9.7 44. Calculate the amount of heat that must be absorbed by 10.0 g of ice at 20C to convert it to liquid water at 60.0C. W h i c h o n e o f t h e f o l l o w i n g i o n i c s o l i d s w o u l d h a v e t h e l a r g e s t l a t t i c e e n e r g y ? C) tetrahedral. c. are usually c. They flow and are compressible. Use the graph of vapor pressure to determine the normal boiling point of CHCl3. Dipoledipole interactions arise from the electrostatic interactions of the positive and negative ends of molecules with permanent dipole moments; their strength is proportional to the magnitude of the dipole moment and to 1/r3, where r is the distance between dipoles. B. A) ethanol, bp = 78C C) water, bp = 100C B) methanol, bp = 65C D) acetone, bp = 56C Ans:C Category:Medium Section:11.8 11. b. dipole-dipole rejections The combination of large bond dipoles and short dipoledipole distances results in very strong dipoledipole interactions called hydrogen bonds, as shown for ice in Figure \(\PageIndex{6}\). C l a s s i f y t h e C C l b o n d i n C C l 4 a s i o n i c , p o l a r c o v a l e n t , o r n o n p o l a r c o v a l e n t . The Lewis structure for CS2 is: A) EMBED Equation.BREE4 B) EMBED Equation.BREE4 C) EMBED Equation.BREE4 D) EMBED Equation.BREE4 Ans:C Category:Medium Section:9.6 30. The predicted order is thus as follows, with actual boiling points in parentheses: He (269C) < Ar (185.7C) < N2O (88.5C) < C60 (>280C) < NaCl (1465C). The number of lone electron pairs in the NO2 ion is ___. Use the graph of vapor pressure to determine the normal boiling point of O2. Larger atoms tend to be more polarizable than smaller ones, because their outer electrons are less tightly bound and are therefore more easily perturbed. If you are comparing molecules to determine which has the higher boiling point, consider the forces that are at work within the molecule. Intermolecular forces are electrostatic in nature and include van der Waals forces and hydrogen bonds. E) distorted tetrahedron (seesaw). Molecules with hydrogen atoms bonded to electronegative atoms such as O, N, and F (and to a much lesser extent, Cl and S) tend to exhibit unusually strong intermolecular interactions. Doubling the distance (r 2r) decreases the attractive energy by one-half. B) Water has an unusually high boiling point. Electrostatic interactions are strongest for an ionic compound, so we expect NaCl to have the highest boiling point. A) Se B) Sb C) K D) Ga E) Fe Ans:A Category:Medium Section:9.5 18. 5 2 3 . d. cannot be liquefied above its triplepoint A C 60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N 2 O. Arrange n-butane, propane, 2-methylpropane [isobutene, (CH3)2CHCH3], and n-pentane in order of increasing boiling points. a. monoclinic (iii) Viscosity increases as intermolecular forces increase. Potassium crystallizes in a body-centered cubic lattice. C l a s s i f y t h e C a C l b o n d i n C a C l 2 a s i o n i c , p o l a r c o v a l e n t , o r n o n p o l a r c o v a l e n t . Which one of the following molecules has a zero dipole moment? Ans:C Category:Medium Section:11.2 5. Asked for: formation of hydrogen bonds and structure. 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