c. cannot go from solid to liquid by application of pressure at any temperature The key is to know which bonds require more energy for boiling to occur. Which molecule has a Lewis structure that does not obey the octet rule? A) O B) S C) Na D) C E) N Ans:B Category:Easy Section:9.9 34. Give the number of lone pairs around the central atom and the molecular geometry of XeF2. What condition must exist for a liquid to boil? Which one of the following derivatives of ethane has the highest boiling point? A) NCl3 B) BaCl2 C) CO D) SO2 E) SF4 Ans:B Category:Easy Section:9.2 4. Of the given pair of compounds, which would have the higher boiling point? 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. The Lewis dot symbol for the a lead atom is A) EMBED Equation.BREE4 B) EMBED Equation.BREE4 C) EMBED Equation.BREE4 D) EMBED Equation.BREE4 E) EMBED Equation.BREE4 Ans: C C a t e g o r y : M e d i u m S e c t i o n : 9 . Ans:D Category:Medium Section:11.3 15. 1. Check Your Learning Ethane (CH 3 CH 3) has a melting point of 183 C and a boiling point of 89 C. On average, however, the attractive interactions dominate. Which of the following atoms does not participate in hydrogen bonding? Ans: 33 sigma bonds and 4 pi bonds (19 sigma, 4 pi) Category:Medium Section:10.5 29. Methane and its heavier congeners in group 14 form a series whose boiling points increase smoothly with increasing molar mass. Of the following, __________ has the highest boiling point. 7 k J / m o l s p e c i f i c h e a t o f s t e a m : 1 . A ) I o n i c b o n d C ) P o l a r c o v a l e n t b o n d B ) N o n p o l a r c o v a l e n t b o n d D ) C o o r d i n a t e c o v a l e n t b o n d A n s : C C a t e g o r y : M e d i u m S e c t i o n : 9 . E) Water is a polar molecule. Acetic acid and acetone are molecules based on two carbons. Identify the compounds with a hydrogen atom attached to O, N, or F. These are likely to be able to act as hydrogen bond donors. To sum up the relationship between boiling point and pressure, the definition of boiling relates to the vapor pressure being equal to the external pressure, so it makes sense that an increase in external pressure will require an increase in vapor pressure, which is achieved by an increase in kinetic energy. Ans:A Category:Medium Section:11.8 26. 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. 5 2 4 . Which of the following substances should have the highest boiling point? Of the compounds that can act as hydrogen bond donors, identify those that also contain lone pairs of electrons, which allow them to be hydrogen bond acceptors. Ans: Category:Medium Section:9.7 44. A) 1 B) 2 C) 3 D) 4 E) 5 Ans:B Category:Medium Section:9.4 26. Let's start with some basics. Small nonpolar molecules Consequently, N 2 O should have a higher boiling point. 2 1 2 . A) 0 lone pairs, linear D) 3 lone pairs, bent B) 1 lone pair, bent E) 3 lone pairs, linear C) 2 lone pairs, bent Ans:C Category:Medium Section:10.1 2. The effect of increasing the pressure is to raise the boiling point. 0 C t o s t e a m a t 1 0 0 C ? E) ionic crystal. Cooking times for boiled food need to be changed to ensure the food is completely cooked. e. hydrogen bonding, Bruce Edward Bursten, Catherine J. Murphy, H. Eugene Lemay, Matthew E. Stoltzfus, Patrick Woodward, Theodore E. Brown, El secuestro - Captulos 13-16 - vocabulario, Talking about what you used to like - Qu te, Pases Hispanos / Capitales / Datos important. 1. Consider a pair of adjacent He atoms, for example. 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. Which of the following ionic solids would have the largest lattice energy? Which statement is true about liquids but not true about solids? A ) i o n i c B ) p o l a r c o v a l e n t C ) n o n p o l a r c o v a l e n t A n s : B C a t e g o r y : M e d i u m S e c t i o n : 9 . Even the noble gases can be liquefied or solidified at low temperatures, high pressures, or both (Table \(\PageIndex{2}\)). d. covalent-ionic interactions Indicate all the types of intermolecular forces of attraction in SF6(g). London was able to show with quantum mechanics that the attractive energy between molecules due to temporary dipoleinduced dipole interactions falls off as 1/r6. a. very weak compared with kinetic energies of the molecules Although hydrogen bonds are significantly weaker than covalent bonds, with typical dissociation energies of only 1525 kJ/mol, they have a significant influence on the physical properties of a compound. A) XeF4 B) BF3 C) AsF5 D) CF4 E) NH3 Ans:D Category:Medium Section:10.1 16. 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 . CsCl crystallizes in a unit cell that contains the Cs+ ion at the center of a cube that has a Cl- at each corner. Of the given pair of compounds, which would have the higher boiling point? In contrast, each oxygen atom is bonded to two H atoms at the shorter distance and two at the longer distance, corresponding to two OH covalent bonds and two OH hydrogen bonds from adjacent water molecules, respectively. Of the species listed, xenon (Xe), ethane (C2H6), and trimethylamine [(CH3)3N] do not contain a hydrogen atom attached to O, N, or F; hence they cannot act as hydrogen bond donors. e. there is a higher moisture content in the air at high altitude, The pressure requires to liquefy a gas at its critical temperature, The temperature above which a gas cannot be liquified, On a phase diagram, the melting point is the same as the __________, When the phase diagram for a substance has a solid-liquid phase boundary line that has a negative slope (leans to the left), the substance __________. Liquids boil when the molecules have enough thermal energy to overcome the intermolecular attractive forces that hold them together, thereby forming bubbles of vapor within the liquid. As a result, it is relatively easy to temporarily deform the electron distribution to generate an instantaneous or induced dipole. T 1$ 7$ 8$ H$ $$ v01$ 7$ 8$ H$ ^`0 A C 60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N 2 O. a. water boils at a lower temperature at high altitude than at low altitude What kind of attractive forces can exist between nonpolar molecules or atoms? e. spherical cubic. Which one of the following should have the lowest boiling point? d. exist only at high temperatures e. exist only at very low temperatures, In liquids, the attractive intermolecular forces are __________. - e. strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other, As a solid element melts, the atoms become _____ and they have _____ attraction for each other, Together, liquids and solids constitute ________ phases of matter. Recall that the attractive energy between two ions is proportional to 1/r, where r is the distance between the ions. According to VSEPR theory, which one of the following molecules should have a geometry that is trigonal bipyramidal? A) NaF B) NaCl C) NaBr D) NaI Ans:A Category:Medium Section:9.3 49. . (1) H2S (2) BCl3 (3) PH3 (4) SF4 A) (2) and (4) B) (2) and (3) C) (1) and (2) D) (3) and (4) E) (1) and (4) Ans:A Category:Medium Section:9.9 37. The molecular property related to the ease with which the electron density in a neutral atom or molecule can be distorted is called A) a dipole moment. Ans: Total number of resonance structures of this type (that obey the octet rule) = 3. a. C2Br6 b. C2F6 c. C2I6 d. C2Cl6 e. C2H6, What is the predominant intermolecular force in CBr4? 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 . b. sublimesratherthanmeltsunderordinary conditions In contrast to intramolecular forces, such as the covalent bonds that hold atoms together in molecules and polyatomic ions, intermolecular forces hold molecules together in a liquid or solid. 8 0 k J / m o l . Ans: Category:Medium Section:9.9 46. Which of the following substances will display an incomplete octet in its Lewis structure? 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 . a. XeF4 b. AsH3 c. CO2 d. BCl3 e. Cl2, When NaCl dissolves in water, aqueous Na+ and Cl- ions result. Which of the elements listed below has the greatest electronegativity? Video Discussing Hydrogen Bonding Intermolecular Forces. Ans: Category:Medium 41. d. cannot be liquefied above its triplepoint The polarizability of a substance also determines how it interacts with ions and species that possess permanent dipoles. a. Ionic b. Molecular c. Metallic Ans:C Category:Medium Section:11.2 5. Which of the following solids would have the highest melting point? 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 \(\PageIndex{6}\). B) covalent solid. W X l m n o w x whVw "j! c. is highly hydrogen-bonded A) NF3 B) H2O C) AsCl3 D) GeH4 E) BF3 Ans:E Category:Medium Section:9.9 38. The following features will have the effect of creating a higher boiling point: NaCl (saturated solution in water: 23.3%w/w). Which one of the following is most likely to be a covalent compound? C.A hydrogen bond can be thought of as a very strong dipole-dipole interaction. The expansion of water when freezing also explains why automobile or boat engines must be protected by antifreeze and why unprotected pipes in houses break if they are allowed to freeze. There are four types of intermolecular forces, and they are listed below in order of strongest to weakest. Because molecules in a liquid move freely and continuously, molecules always experience both attractive and repulsive dipoledipole interactions simultaneously, as shown in Figure \(\PageIndex{2}\). This molecule has an H atom bonded to an O atom, so it will experience hydrogen bonding. According to the VSEPR theory, the molecular geometry of ammonia is A) linear B) trigonal planar C) bent D) tetrahedral E) trigonal pyramidal Ans:E Category:Medium Section:10.1 12. C 3. To describe the intermolecular forces in liquids. 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 . Which one of the following molecules is nonpolar? 8 k J D ) 4 0 . 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. Which of the following is not a type of solid? b. heat of fusion, heat of vaporization Ans:A Category:Medium Section:10.1 8. Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. D) temperature is greater than room temperature. If you are comparing molecules to determine which has the higher boiling point, consider the forces that are at work within the molecule. The effect of this is that boiling points are lower at higher altitudes. Pi bonds are covalent bonds in which the electron density is concentrated above and below a plane containing the nuclei of the bonding atoms. A C 60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N 2 O. Indicate all the types of intermolecular forces of attraction in HCl(g). e. 2and4, The predominant intermolecular force in CaBr2 is __________. Hydrogen bonds are especially strong dipoledipole interactions between molecules that have hydrogen bonded to a highly electronegative atom, such as O, N, or F. The resulting partially positively charged H atom on one molecule (the hydrogen bond donor) can interact strongly with a lone pair of electrons of a partially negatively charged O, N, or F atom on adjacent molecules (the hydrogen bond acceptor). The properties of liquids are intermediate between those of gases and solids, but are more similar to solids. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Ans:True Category:Medium Section:10.6 Chapter 11: (2 points each) 1. The ease of deformation of the electron distribution in an atom or molecule is called its polarizability. Compounds with higher molar masses and that are polar will have the highest boiling points. Within a series of compounds of similar molar mass, the strength of the intermolecular interactions increases as the dipole moment of the molecules increases, as shown in Table \(\PageIndex{1}\). Category:Medium Section:9.8 45. 11. Ans:B Category:Easy Section:11.2 6. 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. Butter is classified as a/an A) metallic crystal. h|g CJ UVaJ h>* B*H*ph "j h|g h|g B*EHUph jn5(M 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. A) CO2 B) Cl2 C) ICl D) NO E) SO2 Ans:D Category:Medium Section:9.9 33. 2and1 The CO bond dipole therefore corresponds to the molecular dipole, which should result in both a rather large dipole moment and a high boiling point. 8 2 8 . Write the Lewis structure of ammonia (nitrogen trihydride). Because of strong OH hydrogen bonding between water molecules, water has an unusually high boiling point, and ice has an open, cagelike structure that is less dense than liquid water. 0 0 k g o f i r o n a t i t s m e l t i n g p o i n t ( 1 , 8 0 9 K ) , g i v e n t h a t DH f u s = 1 3 . The ease with which the charge distribution in a molecule can be distorted by an external electrical field is called the __________. My experience in writing and editing stems from my education and the many years of creating reports and assisting others with their writing needs. Thus, London dispersion forces are responsible for the general trend toward higher boiling points with increased molecular mass and greater surface area in a homologous series of compounds, such as the alkanes (part (a) in Figure \(\PageIndex{4}\)). We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Which one of the following is most likely to be an ionic compound? A) H2O B) BF3 C) Cl2 D) SiH4 E) Ar. Northrup's Chem 112 Section TTU General Chemistry. Write the Lewis structure of boron trifluoride. Give the number of lone pairs around the central atom and the molecular geometry of SCl2. The overall order is thus as follows, with actual boiling points in parentheses: propane (42.1C) < 2-methylpropane (11.7C) < n-butane (0.5C) < n-pentane (36.1C). Arrange 2,4-dimethylheptane, Ne, CS2, Cl2, and KBr in order of decreasing boiling points. Our goal is to make science relevant and fun for everyone. C) tetrahedral. 0 4 F J Z \ ^ xfW jl5(M A) NF3 B) CO2 C) CF4 D) Br2 E) NO Ans:E Category:Medium Section:9.9 36. Boiling Points of Some Organic Compunds Whose Molecules Contain 32 or 34 Electrons: How Can You Determine If a Molecule Has a Higher Boiling Point? 5 J A n s : C C a t e g o r y : M e d i u m S e c t i o n : 1 1 . b. Ethanol has a higher boiling point because of greater London dispersion force c. Both hexane and . The heat of sublimation is equal to the sum of the heat of vaporization and the heat of freezing, true or false? A . Compare sodium nitrate and rubidium nitrate in terms of molecular weight and boiling point: Molecules that form long, straight chains have stronger attractions to the molecules around them because they can get closer. D) polar bonds, but is a nonpolar molecule. Note the last two items in the table above. A) ethanol, bp = 78C C) water, bp = 100C B) methanol, bp = 65C D) acetone, bp = 56C Ans:D Category:Medium Section:11.8 10. B) the surface area of the liquid. Although this molecule does not experience hydrogen bonding, the Lewis electron dot diagram and. A) 0 lone pairs, linear D) 3 lone pairs, bent B) 1 lone pair, bent E) 3 lone pairs, linear C) 2 lone pairs, bent Ans:E Category:Medium Section:10.1 3. a. is highly flammable The geometry of the CS2 molecule is best described as A) linear. d. not strong enough to keep molecules from moving past each other 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. h|g CJ UVaJ h>* B*OJ QJ ^J ph h>* H*h>* B*H*ph "j d. Large polar molecules Hence dipoledipole interactions, such as those in Figure \(\PageIndex{1b}\), are attractive intermolecular interactions, whereas those in Figure \(\PageIndex{1d}\) are repulsive intermolecular interactions. 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 __________. Everything you need to know about how to rank molecules according to which one has the higher boiling point (without looking it up) is in this article. B. This question was answered by Fritz London (19001954), a German physicist who later worked in the United States. h|g h|g B*EHUph jo5(M d. critical temperatures and pressures A) NH3 B) OF2 C) CH3Cl D) H2O E) BeCl2 Ans:E Category:Medium Section:10.2 19. Which of the elements listed below is most likely to exhibit an expanded octet in its compounds? D) the temperature. 5 2 3 . The molecules within the liquid are attracted to each other. Interactions between these temporary dipoles cause atoms to be attracted to one another. London dispersion forces are due to the formation of instantaneous dipole moments in polar or nonpolar molecules as a result of short-lived fluctuations of electron charge distribution, which in turn cause the temporary formation of an induced dipole in adjacent molecules; their energy falls off as 1/r6. Which response includes all the molecules below that do not follow the octet rule? The number of pi bonds in the molecule below is A) 2 B) 4 C) 6 D) 10 E) 15 Ans:B Category:Medium Section:10.5 27. a. appreciable intermolecular attractive forces a. London-dispersion forces b. ion-dipole attraction c. ionic bonding d. dipole-dipole attraction e. hydrogen-bonding, Elemental iodine (I2) is a solid at room temperature. It should therefore have a very small (but nonzero) dipole moment and a very low boiling point. A) 92 K B) 90 K C) 88 K D) 84 K E) O2 doesn't boil because it is always a gas. N2 Br2 H2 Cl2 O2. very soft Consequently, N2O should have a higher boiling point. 0 k J / m o l . Chem 1120 - Chapter 11: States of Matter: Liquids & Solids Practice Quiz 2. C12 H26 molecules are held together by __________. Which one of the following molecules has an atom with an incomplete octet? Vaporization and more. In the structure of ice, each oxygen atom is surrounded by a distorted tetrahedron of hydrogen atoms that form bridges to the oxygen atoms of adjacent water molecules. In which of the following molecules is hydrogen bonding likely to be the most significant component of the total intermolecular forces? The more pressure, the more energy is required, so the boiling point is higher at higher pressures. Electrostatic interactions are strongest for an ionic compound, so we expect NaCl to have the highest boiling point. According to the VSEPR theory, which one of the following species should be linear? B R E E 4 B ) E M B E D E q u a t i o n . A. Asked for: order of increasing boiling points. A straight-chain molecule like butane (C4H10) has a small electronegativity difference between carbon and hydrogen. Because the electron distribution is more easily perturbed in large, heavy species than in small, light species, we say that heavier substances tend to be much more polarizable than lighter ones. A) H2S B) HCN C) BF3 D) H2CO E) SO2 Ans:B Category:Medium Section:10.1 13. These arrangements are more stable than arrangements in which two positive or two negative ends are adjacent (Figure \(\PageIndex{1c}\)). . Ans:D Category:Medium Section:11.7 17. Neopentane is almost spherical, with a small surface area for intermolecular interactions, whereas n-pentane has an extended conformation that enables it to come into close contact with other n-pentane molecules. c. high heats of fusion and vaporization If the mole fractions of helium and argon are 0.25 and 0.35, respectively, how many molecules of methane are present? Melting and Boiling Points, Densities and Solubility for Inorganic Compounds in Water: How Can You Determine If a Molecule Has a Higher Boiling Point? e. They flow and are not compressible. A) 22.7 kJ B) 40.8 kJ C) 2.2 kJ D) 2,400 J E) 40.8 J Ans:D Category:Medium Section:11.8 23. 0 2 k J / m o l s p e c i f i c h e a t o f w a t e r : 4 . (i) Viscosity increases as temperature decreases. C a l c u l a t e t h e a m o u n t o f h e a t n e e d e d t o m e l t 2 . If a substance is both a hydrogen donor and a hydrogen bond acceptor, draw a structure showing the hydrogen bonding. Map: Chemistry - The Central Science (Brown et al. A) BrI B) CsI C) LiI D) NaI E) RbI Ans:A Category:Easy Section:11.2 3. A) NF3 B) CF4 C) PF5 D) AsH3 E) HCl Ans:C Category:Easy Section:9.9 35. Freezing, true which substance most likely has the highest boiling point quizlet false a molecule can be distorted by an electrical... Exhibit an expanded octet in its Lewis structure that does not obey the octet rule below a plane the! M a t 1 0 0 C Medium Section:9.9 33 Cl2, When NaCl dissolves in water aqueous. 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