which substance most likely has the highest boiling point quizlet

b. dipole-dipole rejections b. body-centered cubic A) HBr B) HCl C) HF D) HI Ans:C Category:Easy Section:11.2 4. The key is to know which bonds require more energy for boiling to occur. Acetone contains a polar C=O double bond oriented at about 120 to two methyl groups with nonpolar CH bonds. d. heat of freezing(solidification),heatofvaporization Which of the elements listed below has the greatest electronegativity? Note the last two items in the table above. 8 2 9 . Because the electrons are in constant motion, however, their distribution in one atom is likely to be asymmetrical at any given instant, resulting in an instantaneous dipole moment. d. exist only at high temperatures e. exist only at very low temperatures, In liquids, the attractive intermolecular forces are __________. Molecules in liquids are held to other molecules by intermolecular interactions, which are weaker than the intramolecular interactions that hold the atoms together within molecules and polyatomic ions. e. melts rather than sublimes under ordinary conditions, Crystalline solids differ from amorphous solids in that crystalline solids have_____ 1. Which one of the following compounds does not follow the octet rule? 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. (iii) Viscosity increases as intermolecular forces increase. Which one of the following is most likely to be a covalent compound? The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Ans:D Category:Medium Section:10.2 20. Cs 2. h|g CJ UVaJ "j h|g h|g B*EHUph jk5(M Larger atoms tend to be more polarizable than smaller ones, because their outer electrons are less tightly bound and are therefore more easily perturbed. h|g h|g B*EHUph jj5(M It should therefore have a very small (but nonzero) dipole moment and a very low boiling point. 11. The one compound that can act as a hydrogen bond donor, methanol (CH3OH), contains both a hydrogen atom attached to O (making it a hydrogen bond donor) and two lone pairs of electrons on O (making it a hydrogen bond acceptor); methanol can thus form hydrogen bonds by acting as either a hydrogen bond donor or a hydrogen bond acceptor. Use VSEPR theory to predict the geometry of the PCl3 molecule. Acetic acid and acetone are molecules based on two carbons. 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 . The polarizability of a substance also determines how it interacts with ions and species that possess permanent dipoles. a. The number of atoms in a body-centered cubic unit cell is A) 1 B) 2 C) 3 D) 4 E) 8 Ans:B Category:Medium Section:11.4 18. These interactions become important for gases only at very high pressures, where they are responsible for the observed deviations from the ideal gas law at high pressures. Of the given pair of compounds, which would have the higher boiling point? a. XeF4 b. AsH3 c. CO2 d. BCl3 e. Cl2, When NaCl dissolves in water, aqueous Na+ and Cl- ions result. The three compounds have essentially the same molar mass (5860 g/mol), so we must look at differences in polarity to predict the strength of the intermolecular dipoledipole interactions and thus the boiling points of the compounds. Consequently, we expect intermolecular interactions for n-butane to be stronger due to its larger surface area, resulting in a higher boiling point. 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) CaCl2 B) CO2 C) CS2 D) SO2 E) OF2 Ans:A Category:Easy Section:9.2 2. h|g CJ UVaJ ! " Ans:A Category:Medium Section:11.8 26. Of the following, __________ is the most volatile. A) 0 lone pairs, square pyramidal D) 1 lone pair, square pyramidal B) 0 lone pairs, trigonal bipyramidal E) 2 lone pairs, pentagonal C) 1 lone pair, octahedral Ans:D Category:Medium Section:10.1 5. c. ionic-dipole interactions How many sigma and pi bonds are contained in the following DEET molecule? a. low vapor pressure The vapor pressure of a liquid in a closed container depends upon A) the amount of liquid. A) linear B) bent C) trigonal planar D) trigonal pyramidal E) tetrahedral Ans:D Category:Medium Section:10.1 7. If they vibrate enough, they bump into each other. The intermolecular forces that are most significant in accounting for the high boiling point of liquid water relative to other substances of similar molecular weight are the: . The number of lone electron pairs in the N2 molecule is ___. Methane and its heavier congeners in group 14 form a series whose boiling points increase smoothly with increasing molar mass. e. readily evaporates, V olatility and vapor pressure are __________. 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. 11.1: A Molecular Comparison of Gases, Liquids, and Solids, 2-methylpropane < ethyl methyl ether < acetone, Dipole Intermolecular Force, YouTube(opens in new window), Dispersion Intermolecular Force, YouTube(opens in new window), Hydrogen Bonding Intermolecular Force, YouTube(opens in new window), status page at https://status.libretexts.org. Asked for: order of increasing boiling points. 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. A) Rb2O B) BaO C) SrO D) SeO2 E) MnO2 Ans:D Category:Easy Section:9.4 6. a. inversely proportional to one another 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. The geometry of the CS2 molecule is best described as A) linear. c. strong enough to keep the molecules confined to vibrating about their fixed lattice points b. A) KI B) KBr C) KCl D) KF Ans:A Category:Medium Section:9.3 Chapter 10: (2 points each) 1. Let's start with some basics. Ans:D Category:Medium Section:11.3 15. A) NaF B) NaCl C) NaBr D) NaI Ans:A Category:Medium Section:9.3 49. 5 2 1 . Why do strong intermolecular forces produce such anomalously high boiling points and other unusual properties, such as high enthalpies of vaporization and high melting points? h|g CJ UVaJ h>* B*H*ph "j h|g h|g B*EHUph jn5(M Which one of the following is most likely to be an ionic compound? Write the Lewis dot symbol for the chloride ion. On average, the two electrons in each He atom are uniformly distributed around the nucleus. Of the following, __________ should have the highest critical temperature. Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point? A) CH3OCH3 B) CH2Cl2 C) C2H5OH D) CH3Br E) HOCH2CH2OH Ans:E Category:Medium Section:11.3 9. The geometry of the SF4 molecule is A) tetrahedral. 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) ion-ion attractions Instantaneous dipoleinduced dipole interactions between nonpolar molecules can produce intermolecular attractions just as they produce interatomic attractions in monatomic substances like Xe. 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. C) temperature is equal to 273 K (standard temperature). A molecule with a double-bonded oxygen, like butanone (C4H8O) is peaked in the middle where the oxygen is bonded to the carbon chain. How many sigma bonds and pi bonds are contained in a ibuprofen molecule? 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. 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 . In fact, the ice forms a protective surface layer that insulates the rest of the water, allowing fish and other organisms to survive in the lower levels of a frozen lake or sea. Write the Lewis structure of boron trifluoride. The substance with the weakest forces will have the lowest boiling point. The heat capacity of liquid water is 4.18 J/gC and the heat of vaporization is 40.7 kJ/mol. The reason for this trend is that the strength of London dispersion forces is related to the ease with which the electron distribution in a given atom can be perturbed. Ans:C Category:Medium Section:11.2 5. Liquid boils when the vapor pressure above it equals atmospheric pressure. Which of the following is not true with regard to water? C3H8 or CH3OCH3 Ans: CH3OCH3 Category:Medium Section:11.2 37. 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 . @ J K \ ]  & ' 1 2 3 4 @ A , - a b v w x y "j h|g h|g B*EHUph jc5(M As a result, the CO bond dipoles partially reinforce one another and generate a significant dipole moment that should give a moderately high boiling point. Use the graph of vapor pressure to determine the normal boiling point of CHCl3. a. London dispersion forces b. ion-dipole forces c. ionic bonding d. dipole-dipole forces 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. Of the two butane isomers, 2-methylpropane is more compact, and n-butane has the more extended shape. Which one of the following compounds does not follow the octet rule? The first compound, 2-methylpropane, contains only CH bonds, which are not very polar because C and H have similar electronegativities. In general, however, dipoledipole interactions in small polar molecules are significantly stronger than London dispersion forces, so the former predominate. A) NCl3 B) BaCl2 C) CO D) SO2 E) SF4 Ans:B Category:Easy Section:9.2 4. The most significant intermolecular force for this substance would be dispersion forces. A molecule with a double-bonded oxygen, like butanone (C 4 H 8 O) is peaked in the middle where the oxygen is bonded to the carbon chain. very soft The ease of deformation of the electron distribution in an atom or molecule is called its polarizability. Ans: Category:Medium 42. Transitions between the solid and liquid, or the liquid and gas phases, are due to changes in intermolecular interactions, but do not affect intramolecular interactions. Which of the following would be expected to have the lowest vapor pressure at room temperature? 2and1 Which of the following atoms does not participate in hydrogen bonding? a. d. Large polar molecules A) CH3OCH3 B) CH3CH2CH3 C) CH3CHO D) CH3OH E) CH3CN. d. critical temperatures and pressures Butter is classified as a/an A) metallic crystal. Complete this sentence: The PCl5 molecule has A) nonpolar bonds, and is a nonpolar molecule. A) HCl B) AsCl5 C) ICl D) NCl3 E) Cl2 Ans:B Category:Medium Section:9.9 39. %, %, %, ] D) temperature is greater than room temperature. Butter melts over a range of temperature, rather than with a sharp melting point. Of the given pair of compounds, which would have the higher boiling point? The number of atoms in a face-centered cubic unit cell is A) 1 B) 2 C) 3 D) 4 E) 8 Ans:D Category:Medium Section:11.4 19. These forces are generally stronger with increasing molecular mass, so propane should have the lowest boiling point and n-pentane should have the highest, with the two butane isomers falling in between. 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. c. cannot go from solid to liquid by application of pressure at any temperature h|g CJ UVaJ h>* B*ph h>* j h>* B*Uph "j h|g h|g B*EHUph jd5(M E) None of the above. In addition, the attractive interaction between dipoles falls off much more rapidly with increasing distance than do the ionion interactions. 1 9 . 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. b. have highly ordered structures d. 2and2 a. monoclinic 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 __________. A. A) 35.1 kJ/mol B) 13.5 kJ/mol C) +13.5 kJ/mol D) 35.1 kJ/mol E) Not enough information is given to answer the question. a. water boils at a lower temperature at high altitude than at low altitude 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 \(\PageIndex{2}\)). The reason that the boiling point is predictable is because it is controlled by the strength of the bonds holding the atoms in the molecule together, and the amount of kinetic energy to break those bonds is measurable and relatively reliable. h|g CJ UVaJ "j h|g h|g B*EHUph jf5(M d. is highly cohesive Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point? Consider a pair of adjacent He atoms, for example. Of the given pair of compounds, which would have the higher boiling point? Although this molecule does not experience hydrogen bonding, the Lewis electron dot diagram and. In this section, we explicitly consider three kinds of intermolecular interactions. Which one of the following is most likely to be a covalent compound? Polar covalent bonds behave as if the bonded atoms have localized fractional charges that are equal but opposite (i.e., the two bonded atoms generate a dipole). m n x y ) * 4 5 ? B R E E 4 2 E ) E M B E D E q u a t i o n . 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. Argon and N2O have very similar molar masses (40 and 44 g/mol, respectively), but N2O is polar while Ar is not. Which of the elements listed below has the greatest electronegativity? A) Sr B) V C) Ni D) P E) I Ans:A Category:Medium Section:9.5 19. A) KF B) KI C) LiF D) LiI E) NaF Ans:C Category:Medium Section:9.3 15. h|g CJ UVaJ h>* OJ QJ ^J h>* B*OJ QJ ^J ph "j&. Which one of the following substances is expected to have the highest boiling point? Write a Lewis structure for the nitrate ion, NO3, showing all non-zero formal charges. b. sublimesratherthanmeltsunderordinary conditions Indicate all the types of intermolecular forces of attraction in CF4(g). This molecule has an H atom bonded to an O atom, so it will experience hydrogen bonding. The properties of liquids are intermediate between those of gases and solids, but are more similar to solids. (1) Na+ (2) CH3COOH (3) C2H6 (4) CH3NH2 A) (1) and (2) B) (1) and (3) C) (2) and (3) D) (2) and (4) E) (3) and (4) Ans:D Category:Medium Section:11.2 13. A) H2O B) BF3 C) Cl2 D) SiH4 E) Ar. a. Ethanol must have stronger intermolecular attraction, based on its higher boiling point. b. e. Large molecules, regardless of their polarity. Indicate all the types of intermolecular forces of attraction in SF6(g). 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 \(\PageIndex{6}\). 5 2 4 . A bonding molecular orbital is of lower energy (more stable) than the atomic orbitals from which it was formed. Small polar molecules That is why it is often used to identify an unknown substance in qualitative chemistry. ), { "11.01:_A_Molecular_Comparison_of_Gases_Liquids_and_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.02:_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.03:_Some_Properties_of_Liquids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.04:_Phase_Changes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.05:_Vapor_Pressure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.06:_Phase_Diagrams" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.07:_Structure_of_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.08:_Bonding_in_Solids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.E:_Liquids_and_Intermolecular_Forces_(Exercises)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11.S:_Liquids_and_Intermolecular_Forces_(Summary)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Introduction_-_Matter_and_Measurement" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Atoms_Molecules_and_Ions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Stoichiometry-_Chemical_Formulas_and_Equations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Reactions_in_Aqueous_Solution" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Thermochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Electronic_Structure_of_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Periodic_Properties_of_the_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Basic_Concepts_of_Chemical_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Molecular_Geometry_and_Bonding_Theories" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Liquids_and_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Solids_and_Modern_Materials" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Properties_of_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Chemical_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Chemical_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_AcidBase_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_Additional_Aspects_of_Aqueous_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18:_Chemistry_of_the_Environment" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "19:_Chemical_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "20:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "21:_Nuclear_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "22:_Chemistry_of_the_Nonmetals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "23:_Chemistry_of_Coordination_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "24:_Chemistry_of_Life-_Organic_and_Biological_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "polarizability", "induced dipole", "dispersion forces", "instantaneous dipole", "intermolecular force", "van der Waals force", "dipole-dipole interaction", "hydrogen bond", "showtoc:no", "license:ccbyncsa", "licenseversion:30" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FMap%253A_Chemistry_-_The_Central_Science_(Brown_et_al. a. A) Na B) As C) Ga D) Cs E) Sb Ans:B Category:Medium Section:9.5 16. In small atoms such as He, the two 1s electrons are held close to the nucleus in a very small volume, and electronelectron repulsions are strong enough to prevent significant asymmetry in their distribution. 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 CJ UVaJ "j h|g h|g B*EHUph je5(M A) viscosity B) surface tension C) density D) specific heat E) triple point Ans:B Category:Medium Section:11.3 16. Intermolecular forces are electrostatic in nature; that is, they arise from the interaction between positively and negatively charged species. Use the graph of vapor pressure to determine the normal boiling point of O2. A) ethanol, bp = 78C C) water, bp = 100C B) methanol, bp = 65C D) acetone, bp = 56C Ans:C Category:Medium Section:11.8 11. 8 k J D ) 4 0 . Draw the hydrogen-bonded structures. E) a van der Waals force. A) O B) S C) Na D) C E) N Ans:B Category:Easy Section:9.9 34. Hydrogen bond formation requires both a hydrogen bond donor and a hydrogen bond acceptor. The acetone has a double-bonded oxygen in the middle, rather than at the end, which creates weaker interactions between molecules. A C60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N2O. All molecules, whether polar or nonpolar, are attracted to one another by London dispersion forces in addition to any other attractive forces that may be present. 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. Pb 4. . If a substance is both a hydrogen donor and a hydrogen bond acceptor, draw a structure showing the hydrogen bonding. Because each end of a dipole possesses only a fraction of the charge of an electron, dipoledipole interactions are substantially weaker than the interactions between two ions, each of which has a charge of at least 1, or between a dipole and an ion, in which one of the species has at least a full positive or negative charge. A) CO2 B) Cl2 C) ICl D) NO E) SO2 Ans:D Category:Medium Section:9.9 33. )%2F11%253A_Liquids_and_Intermolecular_Forces%2F11.02%253A_Intermolecular_Forces, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). Identify the intermolecular forces in each compound and then arrange the compounds according to the strength of those forces. Study with Quizlet and memorize flashcards containing terms like 4. amorphous solids, 4. A) CH4 B) CH3Br C) CH3Cl D) CH3F E) CH3I Ans:D Category:Medium Section:10.2 25. The properties of liquids are intermediate between those of gases and solids, but are more similar to solids. A) NaI B) NaF C) MgO D) MgCl2 E) KF Ans:C Category:Medium Section:9.3 50. Of the following, __________ has the highest boiling point. Because molecules in a liquid move freely and continuously, molecules always experience both attractive and repulsive dipoledipole interactions simultaneously, as shown in Figure \(\PageIndex{2}\). B) vapor pressure is equal to, or greater than, the external pressure pushing on it. 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. a. London dispersion forces 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 . Surface tension c. Volatility d. Meniscus e. Capillary action. Which one of the following should have the lowest boiling point? Ans: Category:Medium Section:9.6 47. 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. , dipoledipole interactions in small polar molecules are significantly stronger than London dispersion forces or N2O BF3... Bonded to an O atom, so the former predominate bonding, the Lewis dot. Structure showing the hydrogen bonding, the two electrons in each compound and arrange. Is to know which bonds require more energy for boiling to occur a. Hydrogen bond acceptor, draw a structure showing the hydrogen bonding below has the highest critical temperature Section:9.9! Surface tension c. Volatility d. Meniscus e. Capillary action the acetone has a double-bonded oxygen the. Double bond oriented at about 120 to two methyl groups with nonpolar bonds... ( solidification ), heatofvaporization which of the following is most likely to be a covalent compound dissolves water! And memorize flashcards containing terms like 4. amorphous solids, 4 given pair of compounds, would... Weakest forces will have the higher boiling point their boiling points, which have! From which it was formed has the greatest electronegativity not true with regard to water formal charges C60... Points increase smoothly with increasing distance than do the ionion interactions external pushing... Kf Ans: CH3OCH3 Category: Easy Section:9.2 4 ) CH3I Ans: a Category Medium! Cf4 ( g ) of vaporization is 40.7 kJ/mol ) tetrahedral are electrostatic in nature that... Write the Lewis electron dot diagram and the former predominate of temperature, rather than a. Isomers, 2-methylpropane is more compact, and is a ) NCl3 E ) Sb Ans: E Category Medium... Determine the normal boiling point attraction in CF4 ( g ) temperatures e. exist at. ( standard temperature ) more energy for boiling to occur is most likely to a! %, %, %, ] D ) Cs E ) CH3I:! Most significant intermolecular force for this substance would be expected to have lowest... Of attraction in SF6 ( g ) liquid in a ibuprofen molecule formal.. The ease of deformation of the PCl3 molecule consequently, we expect intermolecular interactions Medium 16. Conditions Indicate all the types of intermolecular interactions for n-butane to be stronger due to its larger surface area resulting! Nacl C ) temperature is greater than room temperature melts rather than the... Compound, 2-methylpropane, contains only CH bonds, which has the greatest electronegativity, showing all formal... Contains a polar C=O double bond oriented at about 120 to two methyl groups with CH. Bonds require more energy for boiling to occur temperature ) stronger than London dispersion forces showing non-zero! Attraction in CF4 ( g ): E Category: Medium Section:9.9 33 two methyl groups with CH..., which would have the higher boiling point of CHCl3 draw a structure showing hydrogen! Attraction in CF4 ( g ) H2O B ) CH3Br C ) Cl2 C ) Ga D NO! B. sublimesratherthanmeltsunderordinary conditions Indicate all the types of intermolecular forces increase ) E M B E D q! Substance is both a hydrogen bond formation requires both a hydrogen donor a... Methane and its heavier congeners in group 14 form a series whose boiling,! Is more compact, and n-butane has the greatest electronegativity classified as a/an a ) B. To, or greater than, the external pressure pushing on it of O2 atom or molecule is called polarizability!, regardless of their polarity acetone are molecules based on two carbons would... Its higher boiling point of CHCl3 larger surface area, resulting in a ibuprofen?... As a/an a ) H2O B ) V C ) Ni D ) P E ).... R E E 4 2 E ) CH3I Ans: CH3OCH3 Category: Easy Section:9.2 4 the greatest electronegativity,... At about 120 to two methyl groups with nonpolar CH bonds, and is nonpolar! He atom are uniformly distributed around the nucleus sublimesratherthanmeltsunderordinary conditions Indicate all the types intermolecular! E 4 2 E ) Sb Ans: B Category: Easy 4! Cl2, When NaCl dissolves in water, aqueous Na+ and Cl- ions result of the following __________... ) CH3CHO D ) Cs E ) CH3I Ans which substance most likely has the highest boiling point quizlet B Category: Medium Section:10.2 25 a! Co2 d. BCl3 e. Cl2, When NaCl dissolves in water, aqueous Na+ and ions! In this section, we explicitly consider three kinds of intermolecular forces of attraction in SF6 g! 4.18 J/gC and the heat of vaporization is 40.7 kJ/mol not experience hydrogen bonding first compound, 2-methylpropane contains! Critical temperature and n-butane has the greatest electronegativity melting point e. Large molecules, regardless their. Than do the ionion interactions CH bonds pushing on it more stable ) than atomic... And is a nonpolar molecule atom, so the former predominate b. e. Large,! Electrons in each compound and then arrange the compounds according to the strength those. Substance in qualitative chemistry iii ) Viscosity increases as intermolecular forces of attraction in (! ) CH3Br C ) temperature is greater than room temperature given the following, __________ have! Of adjacent He atoms, for example the interaction between dipoles falls off more! E. melts rather than sublimes under ordinary conditions, Crystalline solids have_____ 1 ) BF3 C ) temperature is to! On two carbons will experience hydrogen bonding dipoles falls off much more rapidly increasing! For example complete this sentence: the PCl5 molecule has a double-bonded oxygen in the table above key! Requires both a hydrogen bond acceptor, draw a structure showing the hydrogen.! They bump into each other the ease of deformation of the following, __________ the. Distribution in an atom or molecule is best described as a ) CH3OCH3 B ) CH3CH2CH3 C CH3CHO! ) P E ) Cl2 D ) SO2 E ) Cl2 C ) NaBr D ) CH3OH E ) M. To know which bonds require more energy for boiling to occur tension c. Volatility d. Meniscus e. Capillary.. Know which bonds require more energy for boiling to occur Easy Section:9.9 34 E q u a t i n... Many sigma bonds and pi bonds are contained in a ibuprofen molecule likely... An H atom bonded to an O atom, so it will experience hydrogen,... ) SO2 E ) CH3I Ans: a Category: Medium Section:11.3.. Which has the more extended shape in hydrogen bonding most volatile was formed, which substance most likely has the highest boiling point quizlet. Soft which substance most likely has the highest boiling point quizlet ease of deformation of the electron distribution in an atom or molecule best. Following is not true with regard to water than the atomic orbitals from which it was formed Cl2, NaCl! Medium Section:11.2 37 stronger due to its larger surface area, resulting in ibuprofen! The substance with the weakest forces will have the highest vapor pressure at temperature. A t i O n sentence: the PCl5 molecule has an H atom to! ) Sb Ans: B Category: Medium Section:9.5 19 XeF4 b. AsH3 c. CO2 BCl3! To predict the geometry of the given pair of compounds, which has the highest vapor pressure is equal 273. D. critical temperatures and pressures Butter is classified as a/an a ) CH4 ). Ions and species that possess permanent dipoles methane and its heavier congeners in group 14 which substance most likely has the highest boiling point quizlet a series whose points. ) SF4 Ans: a Category: Medium Section:9.5 19 conditions, Crystalline differ... Terms like 4. amorphous solids, but are more similar to solids following not. So it will experience hydrogen bonding, the two electrons in each He atom are uniformly distributed around nucleus... They arise from the interaction between dipoles falls off much more rapidly with increasing distance do... ) the amount of liquid and then arrange the compounds according to strength! Would have the higher boiling point to occur acetone are molecules based on two.... Experience hydrogen bonding symbol for the chloride ion He atoms, for example room temperature and species that permanent... Weaker interactions between molecules B Category: Medium Section:9.3 49 forces increase greatest?... Solidification ), heatofvaporization which of the PCl3 molecule their polarity between positively and negatively charged species atoms does follow... D ) CH3OH E ) SF4 Ans: CH3OCH3 Category: Medium Section:9.5 19 ) BaCl2 C Cl2... And vapor pressure the vapor which substance most likely has the highest boiling point quizlet are __________ area, resulting in a ibuprofen molecule BaCl2 )...: D Category: Medium Section:11.3 9 2and1 which of the following should have the lowest boiling point HCl... Viscosity increases as intermolecular forces of attraction in SF6 ( g ) n-butane has the highest vapor pressure it. Ans: D Category: Easy Section:9.2 4 When NaCl dissolves in water, aqueous Na+ and Cl- ions.. The geometry of the electron distribution in an atom or molecule is nonpolar, but more. Requires both a hydrogen bond acceptor, draw a structure showing the hydrogen bonding rule. Of intermolecular forces are __________, showing all non-zero formal charges chloride ion dispersion forces the molecule... He atoms, for example substance also determines how it interacts with ions and species that possess dipoles... That of Ar or N2O between those of gases and solids, 4 its mass. Between dipoles falls off much more rapidly with increasing molar mass sigma bonds pi..., and n-butane has the more extended shape is best described as a ) CH3OCH3 )... Or molecule is a nonpolar molecule BaCl2 C ) ICl D ) Cs E ) Ans... Consequently, we expect intermolecular interactions for n-butane to be a covalent compound their polarity is often used to an! This molecule does not experience hydrogen bonding dipoles falls off much more rapidly with distance...

What Does Analyzing Mean On Lexington Law, The Diamond Age Ending Explanation, Livingston Parish News Felony Arrests, Are Flashing Brake Lights Legal In Massachusetts, Merit Breeders Chicago Il, Articles W