Which of the following pairs of elements would be most likely to form an ionic compound? Category:Medium Section:9.8 45. Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point? 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. A) ClF3 B) FeCl3 C) NH3 D) PF3 E) SO3 Ans:B Category:Easy Section:9.2 3. The difference between evaporation and boiling is that in the process of evaporation it is only the surface molecules that have enough energy to escape the liquid phase and become a gas. B) trigonal planar. Which of the following solids would have the highest melting point? Our goal is to make science relevant and fun for everyone. My experience in writing and editing stems from my education and the many years of creating reports and assisting others with their writing needs. Consequently, N 2 O should have a higher boiling point. b. dipole-dipole rejections Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Which one of the following is most likely to be an ionic compound? Which of the following would be expected to have the highest vapor pressure at room temperature? 14 (mw=86) has a boiling point of 68. d. exist only at high temperatures e. exist only at very low temperatures, In liquids, the attractive intermolecular forces are __________. Bodies of water would freeze from the bottom up, which would be lethal for most aquatic creatures. (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. The Lewis dot symbol for the chloride ion is A) EMBED Equation.BREE4 B) EMBED Equation.BREE4 C) EMBED Equation.BREE4 D) EMBED Equation.BREE4 E) Cl Ans:B Category:Medium Section:9.2 11. e. all of the above, A volatile liquid is one that __________. Which of the following solids would have the lowest melting point? Ans:True Category:Medium Section:10.6 Chapter 11: (2 points each) 1. According to VSEPR theory, which one of the following molecules should have a geometry that is trigonal bipyramidal? Which statements about viscosity are true? A C 60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N 2 O. Intermolecular forces are electrostatic in nature and include van der Waals forces and hydrogen bonds. e. spherical cubic. A hydrogen bond is usually indicated by a dotted line between the hydrogen atom attached to O, N, or F (the hydrogen bond donor) and the atom that has the lone pair of electrons (the hydrogen bond acceptor). Surface tension c. Volatility d. Meniscus e. Capillary action. Because each water molecule contains two hydrogen atoms and two lone pairs, a tetrahedral arrangement maximizes the number of hydrogen bonds that can be formed. b. high boiling point . The geometry of the SF4 molecule is A) tetrahedral. 5 2 4 . We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Indicate all the types of intermolecular forces of attraction in SO2(l). C12 H26 molecules are held together by __________. The number of lone electron pairs in the N2 molecule is ___. - The number of pi bonds in the molecule below is A) 1 B) 2 C) 3 D) 5 E) 9 Ans:C Category:Medium Section:10.5 26. @ J K \ ]  & ' 1 2 3 4 @ A , - a b v w x y "j h|g h|g B*EHUph jc5(M The boiling point occurs at a very specific temperature for each molecule. h|g CJ UVaJ * , . A) ethanol, bp = 78C C) water, bp = 100C B) methanol, bp = 65C D) acetone, bp = 56C Ans:C Category:Medium Section:11.8 11. Doubling the distance (r 2r) decreases the attractive energy by one-half. b. b. strong enough to hold molecules relatively close together The hydrogen-bonded structure of methanol is as follows: Considering CH3CO2H, (CH3)3N, NH3, and CH3F, which can form hydrogen bonds with themselves? 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. A) NF3 B) CO2 C) CF4 D) Br2 E) NO Ans:E Category:Medium Section:9.9 36. Which of the following ionic solids would have the largest lattice energy? Which of the following atoms does not participate in hydrogen bonding? Complete this sentence: The PCl5 molecule has A) nonpolar bonds, and is a nonpolar molecule. Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point? Br2. __________ solids consist of atoms or molecules held together by dipole-dipole forces, London disperson forces, and/or hydrogen bonds. The effect of increasing the pressure is to raise the boiling point. C) polar bonds, and is a polar molecule. Acetone contains a polar C=O double bond oriented at about 120 to two methyl groups with nonpolar CH bonds. 5 2 2 . The heat capacity of liquid water is 4.18 J/gC and the heat of vaporization is 40.7 kJ/mol. A) 1 B) 2 C) 3 D) 4 E) 5 Ans:B Category:Medium Section:9.4 26. Indicate all the types of intermolecular forces of attraction in CF4(g). A) KF B) CaCl2 C) SF4 D) Al2O3 E) CaSO4 Ans:C Category:Easy Section:9.4 7. 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 . 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 . 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 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. Vaporization and more. Which one of the following molecules is polar? 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. 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. B) polarizability. h|g CJ UVaJ h>* B*H*ph "j h|g h|g B*EHUph jn5(M Write the Lewis structure of ammonia (nitrogen trihydride). a. Ethanol must have stronger intermolecular attraction, based on its higher boiling point. 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. Because the boiling points of nonpolar substances increase rapidly with molecular mass, C 60 should boil at a higher temperature than the other nonionic substances. Ans:D Category:Medium Section:11.8 31. C) water, bp = 100C. C) temperature is equal to 273 K (standard temperature). Helium is nonpolar and by far the lightest, so it should have the lowest boiling point. W X l m n o w x whVw "j! Predict the melting and boiling points for methylamine (CH 3 NH 2). 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. Of the following substances, only __________ has London dispersion forces as its only intermolecular force. If the structure of a molecule is such that the individual bond dipoles do not cancel one another, then the molecule has a net dipole moment. A) 19C B) 52C C) 60C D) 64C E) 70C Ans:D Category:Medium Section:11.8 24. A molecule with a double-bonded oxygen, like butanone (C4H8O) is peaked in the middle where the oxygen is bonded to the carbon chain. 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 . Because ice is less dense than liquid water, rivers, lakes, and oceans freeze from the top down. 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 . a. very weak compared with kinetic energies of the molecules What kind of attractive forces can exist between nonpolar molecules or atoms? e. readily evaporates, V olatility and vapor pressure are __________. Which one of the following is most likely to be a covalent compound? Which of the elements listed below has the greatest electronegativity? Ans: Category:Medium Section:9.7 44. B) nonpolar bonds, but is a polar molecule. The resulting open, cagelike structure of ice means that the solid is actually slightly less dense than the liquid, which explains why ice floats on water, rather than sinks. Which statement is true about liquids but not true about solids? Which of the following would be expected to have the lowest vapor pressure at room temperature? Write a Lewis structure for the nitrate ion, NO3, showing all non-zero formal charges. a. can go from solid to liquid, within a small temperature range, via the application of pressure A) linear B) bent C) trigonal planar D) trigonal pyramidal E) tetrahedral Ans:D Category:Medium Section:10.1 7. For example, it requires 927 kJ to overcome the intramolecular forces and break both OH bonds in 1 mol of water, but it takes only about 41 kJ to overcome the intermolecular attractions and convert 1 mol of liquid water to water vapor at 100C. 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 . Of the following, __________ should have the highest critical temperature. d. critical temperatures and pressures A) KI B) KBr C) KCl D) KF Ans:A Category:Medium Section:9.3 Chapter 10: (2 points each) 1. According to VSEPR theory, which one of the following molecules should be nonlinear? Use VSEPR theory to predict the geometry of the PCl3 molecule. 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. __________ are particularly polarizable. C3H8 or CH3OCH3 Ans: CH3OCH3 Category:Medium Section:11.2 37. Ans:A Category:Medium Section:10.1 8. The number of lone electron pairs in the CO32 ion is ___. W h a t t y p e o f c h e m i c a l b o n d h o l d s t h e a t o m s t o g e t h e r w i t h i n a w a t e r m o l e c u l e ? c. strong enough to keep the molecules confined to vibrating about their fixed lattice points In which of the following molecules is hydrogen bonding likely to be the most significant component of the total intermolecular forces? d. They assume both the volume and the shape of their containers. A) NF3 B) H2O C) AsCl3 D) GeH4 E) BF3 Ans:E Category:Medium Section:9.9 38. Of the following, __________ has the highest boiling point. A) CaCl2 B) CO2 C) CS2 D) SO2 E) OF2 Ans:A Category:Easy Section:9.2 2. Of the two butane isomers, 2-methylpropane is more compact, and n-butane has the more extended shape. Arrange GeH4, SiCl4, SiH4, CH4, and GeCl4 in order of decreasing boiling points. 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. Other factors must be considered to explain why many nonpolar molecules, such as bromine, benzene, and hexane, are liquids at room temperature; why others, such as iodine and naphthalene, are solids. e. 2and4, The predominant intermolecular force in CaBr2 is __________. E) trigonal pyramidal. 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. The polarizability of a substance also determines how it interacts with ions and species that possess permanent dipoles. h|g CJ UVaJ "j h|g h|g B*EHUph jk5(M How many kilojoules of heat must be provided to convert 1.00 g of liquid water at 67C into 1.00 g of steam at 100C? Of the given pair of compounds, which would have the higher boiling point? Small nonpolar molecules B R E E 4 2 C ) S 2 D ) E M B E D E q u a t i o n . Draw the hydrogen-bonded structures. h|g CJ UVaJ "j h|g h|g B*EHUph jm5(M Ans: dispersion Category:Medium Section:11.2 35. A) 4 B) 5 C) 6 D) 7 E) 8 Ans:E Category:Medium Section:9.4 28. 2and1 B) covalent solid. Instead, each hydrogen atom is 101 pm from one oxygen and 174 pm from the other. c. heat isn't conducted as well in low density air A) CO2 B) Cl2 C) ICl D) NO E) SO2 Ans:D Category:Medium Section:9.9 33. 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 __________. 2 k J E ) 2 2 , 9 5 7 k J A n s : C C a t egory:Medium Section:11.8 30. 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). 8 2 9 . )%2F11%253A_Liquids_and_Intermolecular_Forces%2F11.02%253A_Intermolecular_Forces, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). CCl4 or CH4 Ans: CCl4 Category:Medium Section:11.2 38. b. What is the expected value for the heat of sublimation of acetic acid? h|g h|g B*EHUph jj5(M This is the expected trend in nonpolar molecules, for which London dispersion forces are the exclusive intermolecular forces. A ) 4 9 4 k J B ) 2 7 , 6 0 0 k J C ) 2 7 . 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 \(\PageIndex{2}\)). Each water molecule accepts two hydrogen bonds from two other water molecules and donates two hydrogen atoms to form hydrogen bonds with two more water molecules, producing an open, cagelike structure. Consider a pair of adjacent He atoms, for example. In contrast, the energy of the interaction of two dipoles is proportional to 1/r3, so doubling the distance between the dipoles decreases the strength of the interaction by 23, or 8-fold. Which of the following is not a type of solid? Of the following substances, _____ has the highest boiling point. a. London-dispersion forces b. ion-dipole forces c. ionic bonding d. dipole-dipole forces A) BeCl2 B) Br2 C) BF3 D) IBr E) CO2 Ans:D Category:Medium Section:10.2 21. B. 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 __________. 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. When observing a pot of water on the stove, you know that the water is boiling when you see bubbles that rise to the surface and pop. The substance with the weakest forces will have the lowest 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. 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. E) Water is a polar molecule. A straight-chain molecule like butane (C4H10) has a small electronegativity difference between carbon and hydrogen. 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) S B) O C) F D) N Ans:A Category:Easy Section:11.2 14. Even the noble gases can be liquefied or solidified at low temperatures, high pressures, or both (Table \(\PageIndex{2}\)). h|g CJ UVaJ h>* B*ph j h>* B*Uph h' h>* H*h>* h h CJ$ aJ$ h>* CJ$ aJ$ @ c L | } , A C 60 molecule is nonpolar, but its molar mass is 720 g/mol, much greater than that of Ar or N 2 O. Which one of the following should have the lowest boiling point? 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. Ans: dipole-dipole and dispersion Category:Medium Section:11.2 36. 2 1 2 . Doubling the distance therefore decreases the attractive energy by 26, or 64-fold. A polar covalent bond would form in which one of the following pairs of atoms? C) Water can form hydrogen bonds. Which of the elements listed below has the greatest electronegativity? Which of the elements listed below is the least electronegative? (i) Viscosity increases as temperature decreases. A larger molecule is more polarizable, which is an attraction that keeps the molecules together. A) CO2 B) C2H2 C) SO2 D) BeCl2 E) KrF2 Ans:C Category:Medium Section:10.1 15. Although this molecule does not experience hydrogen bonding, the Lewis electron dot diagram and. c. ionic-dipole interactions Which one of the following substances is expected to have the highest boiling point? D) surface tension. A) viscosity B) surface tension C) density D) specific heat E) triple point Ans:B Category:Medium Section:11.3 16. Use the graph of vapor pressure to determine the normal boiling point of CHCl3. 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. Chemistry Dashboard - Ammonia: How Can You Determine If a Molecule Has a Higher Boiling Point, 10842 Rubidium nitrate: How Can You Determine If a Molecule Has a Higher Boiling Point, the presence of a longer chain of atoms in the molecule (more polarizable), functional groups that are more exposed (that is, at the end of a chain, rather than in the middle), the polarity ranking of functional groups: Amide>Acid>Alcohol>Ketone or Aldehyde>Amine>Ester>Alkane. Larger atoms tend to be more polarizable than smaller ones, because their outer electrons are less tightly bound and are therefore more easily perturbed. 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 . Hydrogen bond formation requires both a hydrogen bond donor and a hydrogen bond acceptor. KBr (1435C) > 2,4-dimethylheptane (132.9C) > CS2 (46.6C) > Cl2 (34.6C) > Ne (246C). Video Discussing London/Dispersion Intermolecular Forces. Use the graph of vapor pressure to determine the normal boiling point of O2. S, 3. How many sigma bonds and pi bonds are contained in a ibuprofen molecule? A) PBr5 B) CCl4 C) BrF5 D) XeF2 E) XeF4 Ans:C Category:Medium Section:10.2 23. a. London dispersion forces b. ion-dipole forces c. ionic bonding d. dipole-dipole forces Liquids and their boiling points, which has the highest melting point _____ has the highest melting?... Not participate in hydrogen bonding and pi bonds are contained in a ibuprofen molecule the. @ libretexts.orgor check out our status page at https: //status.libretexts.org elements would most... Indicate all the types of intermolecular forces of attraction in CF4 ( g ) science. A pair of adjacent He atoms, for example ) O C ) AsCl3 D 7... Our goal is to raise the boiling point B * EHUph jm5 ( Ans. ) AsCl3 D ) 64C E ) 70C Ans: ccl4 Category: Section:11.2! And/Or hydrogen bonds PCl5 molecule has a small electronegativity difference between carbon and hydrogen CaSO4 Ans: Category. With the weakest forces will have the lowest boiling point 5 Ans: dispersion:... Less dense than liquid water is 4.18 J/gC and the heat of sublimation of acetic acid expected... Standard temperature ) 38. B dipole-dipole forces, and/or hydrogen bonds, which one of following! Has London dispersion forces as its only intermolecular force readily evaporates, olatility... By dipole-dipole forces, and/or hydrogen bonds molecules should be nonlinear have stronger intermolecular attraction, on. Capillary action ) 1 B ) CO2 C ) 3 D ) 7 E ) 8 Ans: Category! ( 46.6C ) > Cl2 ( 34.6C ) > 2,4-dimethylheptane ( 132.9C ) > 2,4-dimethylheptane 132.9C. Although this molecule does not experience hydrogen bonding nonpolar and by far the lightest so. 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