- The most significant intermolecular force for this substance would be dispersion forces. CsCl crystallizes in a unit cell that contains the Cs+ ion at the center of a cube that has a Cl- at each corner. A) CsOH B) NF3 C) Sr(NO3)2 D) CaO E) LiF
Ans:B Category:Easy Section:9.4
8. Compounds such as HF can form only two hydrogen bonds at a time as can, on average, pure liquid NH3. b. Which one of the following is most likely to be an ionic compound? Ans:C Category:Medium Section:11.2
5. E) trigonal pyramidal. A) NaF B) NaCl C) NaBr D) NaI
Ans:A Category:Medium Section:9.3
49. Small nonpolar molecules A) NaI B) NaF C) MgO D) MgCl2 E) KF
Ans:C Category:Medium Section:9.3
50. Ethanol, CH 3CH 2OH (mw=46) has a boiling point of 78. B) ion-dipole forces. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. a. London dispersion forces They flow and are highly ordered. e. melts rather than sublimes under ordinary conditions, Crystalline solids differ from amorphous solids in that crystalline solids have_____ Electrostatic interactions are strongest for an ionic compound, so we expect NaCl to have the highest boiling point. Because ice is less dense than liquid water, rivers, lakes, and oceans freeze from the top down. In which of the following molecules is hydrogen bonding likely to be the most significant component of the total intermolecular forces? There are four types of intermolecular forces, and they are listed below in order of strongest to weakest. The effect of this is that boiling points are lower at higher altitudes. E) ionic crystal. A) Mg B) Ga C) Si D) Ba E) Pb
Ans:C Category:Medium Section:9.5
20. 11.2: Intermolecular Forces is shared under a CC BY-NC-SA 3.0 license and was authored, remixed, and/or curated by LibreTexts. 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 . 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 . 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. A . 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 __________. c. heat of freezing (solidification), heat of condensation A) H2S B) HCN C) BF3 D) H2CO E) SO2
Ans:B Category:Medium Section:10.1
13. a. can go from solid to liquid, within a small temperature range, via the application of pressure Northrup's Chem 112 Section TTU General Chemistry. 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. A) BrI B) CsI C) LiI D) NaI E) RbI
Ans:A Category:Easy Section:11.2
3. e. Large molecules, regardless of their polarity. 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. Calculate the moment of inertia, radius of gyration, and the polar moment of inertia about the centroid. 5
2 4 . 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. Conversely, \(\ce{NaCl}\), which is held together by interionic interactions, is a high-melting-point solid. Given the following liquids and their boiling points, which has the highest vapor pressure at its normal boiling point? b. directly proportional to one another Which one of the following is most likely to be a covalent compound? h|g CJ UVaJ * , . 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 : A C a t e g o r y : M e d i u m S e c t i o n : 9 . 8 k J D ) 4 0 . Ans:B Category:Medium Section:11.8
27. Surface tension c. Volatility d. Meniscus e. Capillary action. A 6.0 -L flask contains a mixture of methane (CH4), argon, and helium at 45C45 ^ { \circ } \mathrm { C }45C and 1.75 atm. B R E E 4 2 C ) S 2 D ) E M B E D E q u a t i o n . Molecules with net dipole moments tend to align themselves so that the positive end of one dipole is near the negative end of another and vice versa, as shown in Figure \(\PageIndex{1a}\). b. water boils at a higher temperature at high altitude than at low altitude Helium is nonpolar and by far the lightest, so it should have the lowest boiling point. Vaporization and more. A) NF3 B) H2O C) AsCl3 D) GeH4 E) BF3
Ans:E Category:Medium Section:9.9
38. 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. Arrange ethyl methyl ether (CH3OCH2CH3), 2-methylpropane [isobutane, (CH3)2CHCH3], and acetone (CH3COCH3) in order of increasing boiling points. Larger atoms tend to be more polarizable than smaller ones, because their outer electrons are less tightly bound and are therefore more easily perturbed. 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. Ans:
Category:Medium Section:9.6
47. 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. e. spherical cubic. 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 . Which one of the following molecules is nonpolar? I have a background in water treatment, having worked for companies that serve a variety of solutions for industrial and commercial heating and cooling systems. a. low vapor pressure A) CH4 B) Cl2 C) Kr D) CH3Cl E) N2
Ans:D Category:Medium Section:11.2
7. 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. E) hydrogen bonding. Ans:D Category:Medium Section:11.3
15. Consequently, HO, HN, and HF bonds have very large bond dipoles that can interact strongly with one another. The boiling point of propane is 42.1 C, the boiling point of dimethylether is 24.8 C, and the boiling point of ethanol is 78.5 C. 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. What is the expected value for the heat of sublimation of acetic acid? d. cannot be liquefied above its triplepoint 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 molecule with a double-bonded oxygen, like butanone (C4H8O) is peaked in the middle where the oxygen is bonded to the carbon chain. a. Ionic b. Molecular c. Metallic 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. dimethyl sulfoxide (boiling point = 189.9C) > ethyl methyl sulfide (boiling point = 67C) > 2-methylbutane (boiling point = 27.8C) > carbon tetrafluoride (boiling point = 128C). Which of the following species has the largest dipole moment (i.e., is the most polar)? 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 . T h e e l e c t r o n d o t f o r m u l a f or O2 shows
A) a single covalent bond D) a total of 8 x 2 = 16 electron dots
B) a double covalent bond E) a total of 32 electron dots
C) an ionic bond
Ans:B Category:Medium Section:9.4
25. Ans: dispersion
Category:Medium Section:11.2
34. Ans: dispersion
Category:Medium Section:11.2
33. A) NH3 B) CCl4 C) CO2 D) SF4 E) PCl5
Ans:B Category:Medium Section:10.1
17. That is why it is often used to identify an unknown substance in qualitative chemistry. 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. c. primitive cubic 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. D) the temperature. a. Because molecules in a liquid move freely and continuously, molecules always experience both attractive and repulsive dipoledipole interactions simultaneously, as shown in Figure \(\PageIndex{2}\). In general, however, dipoledipole interactions in small polar molecules are significantly stronger than London dispersion forces, so the former predominate. Ans:True Category:Easy Section:10.5
30. Indicate all the types of intermolecular forces of attraction in SF6(g). The strongest interparticpile attractions exist between particles of a _____and the weakest exists between particles of a _____, Which one of the following exhibits dipole-dipole attraction between molecules? Which of the elements listed below is the least electronegative? a. have their particles arranged randomly Pb 4. . Indicate all the types of intermolecular forces of attraction in CF4(g). E) a van der Waals force. Ans:
Category:Medium
42. 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 . The three major types of intermolecular interactions are dipoledipole interactions, London dispersion forces (these two are often referred to collectively as van der Waals forces), and hydrogen bonds. c. is highly hydrogen-bonded On average, the two electrons in each He atom are uniformly distributed around the nucleus. Note the last two items in the table above. Which of the responses includes all of the following that can form hydrogen bonds with water molecules? Which of the following substances should have the lowest boiling point? Acetic acid and acetone are molecules based on two carbons. Which of the following solids would have the highest melting point? How many atoms are there per unit cell? 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. 1 8 J / g C ; DH f u s = 6 . If ice were denser than the liquid, the ice formed at the surface in cold weather would sink as fast as it formed. A) Se B) Sb C) K D) Ga E) Fe
Ans:A Category:Medium Section:9.5
18. A) NH3 B) OF2 C) CH3Cl D) H2O E) BeCl2
Ans:E Category:Medium Section:10.2
19. (i) Viscosity increases as temperature decreases. The effect is most dramatic for water: if we extend the straight line connecting the points for H2Te and H2Se to the line for period 2, we obtain an estimated boiling point of 130C for water! A ) 4 2 0 J B ) 2 , 9 0 0 J C ) 6 , 2 6 1 J D ) 6 3 k J E ) 7 . H2O CO2 CH4 Kr NH3. B R E E 4 B ) E M B E D E q u a t i o n . As shown in part (a) in Figure \(\PageIndex{3}\), the instantaneous dipole moment on one atom can interact with the electrons in an adjacent atom, pulling them toward the positive end of the instantaneous dipole or repelling them from the negative end. B) vapor pressure is equal to, or greater than, the external pressure pushing on it. C) polar bonds, and is a polar molecule. . Heat of sublimation can be approximated by adding together __________ and __________. 5
2 3 . 8
2 8 . 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). The answer lies in the highly polar nature of the bonds between hydrogen and very electronegative elements such as O, N, and F. The large difference in electronegativity results in a large partial positive charge on hydrogen and a correspondingly large partial negative charge on the O, N, or F atom. This molecule has an H atom bonded to an O atom, so it will experience hydrogen bonding. Which one of the following molecules has a non-zero dipole moment? e. readily evaporates, V olatility and vapor pressure are __________. Asked for: order of increasing boiling points. D) benzene, bp = 80C. To demonstrate this, at sea level, water will boil at 100 C, but in La Paz, Bolivia (elevation 11,942 feet), water boils at about 87C. a. heat of fusion, heat of condensation 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. 0 g o f i c e a t 1 0 . Potassium crystallizes in a body-centered cubic lattice. d. face-centered cubic 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. 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. Consequently, N2O should have a higher boiling point. Br2. Ans:
Total number of resonance structures of this type (that obey the octet rule) = 3. Let's start with some basics. A larger molecule is more polarizable, which is an attraction that keeps the molecules together. Considering CH3OH, C2H6, Xe, and (CH3)3N, which can form hydrogen bonds with themselves? c. are usually Source: Dispersion Intermolecular Force, YouTube(opens in new window) [youtu.be]. 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. c. Large nonpolar molecules 11. A) ethanol, bp = 78C
B) methanol, bp = 65C
C) water, bp = 100C
D) benzene, bp = 80C
E) The vapor pressure of each of the liquids at its normal boiling point would be the same. Ans:E Category:Medium Section:11.8
12. Write a Lewis structure for OF2. Consequently, N 2 O should have a higher boiling point. Which one of the following is most likely to be a covalent compound? The geometry of the CS2 molecule is best described as
A) linear. Check Your Learning Ethane (CH 3 CH 3) has a melting point of 183 C and a boiling point of 89 C. h|g CJ UVaJ h>* B*ph h>* j h>* B*Uph "j h|g h|g B*EHUph jh5(M Ans:True Category:Medium Section:10.6
Chapter 11: (2 points each)
1. S, 3. Ans: 33 sigma bonds and 4 pi bonds (19 sigma, 4 pi)
Category:Medium Section:10.5
29. 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. 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. Consequently, even though their molecular masses are similar to that of water, their boiling points are significantly lower than the boiling point of water, which forms four hydrogen bonds at a time. Determine the intermolecular forces in the compounds, and then arrange the compounds according to the strength of those forces. 1 8 J / g C DH v a p = 4 0 . CH3Cl or CH4
Ans: CH3Cl
Category:Medium Section:11.2
39. 8 4 J / g C
A ) 2 , 5 7 0 k J B ) 1 , 0 8 6 k J C ) 1 5 7 . (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. Ans:D Category:Medium Section:11.7
17. 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. 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 \(\PageIndex{4}\)). Which statements about viscosity are true? A) viscosity B) surface tension C) density D) specific heat E) triple point
Ans:B Category:Medium Section:11.3
16. 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. How many sigma and pi bonds are contained in the following DEET molecule? Arrange GeH4, SiCl4, SiH4, CH4, and GeCl4 in order of decreasing boiling points. Argon and N2O have very similar molar masses (40 and 44 g/mol, respectively), but N2O is polar while Ar is not. C) molecular crystal. 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. Arrange n-butane, propane, 2-methylpropane [isobutene, (CH3)2CHCH3], and n-pentane in order of increasing boiling points. 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 __________. Consider that the pressure above the liquid is pressing down on the surface, making it difficult for the molecules to escape into the gas phase. Instantaneous dipoleinduced dipole interactions between nonpolar molecules can produce intermolecular attractions just as they produce interatomic attractions in monatomic substances like Xe. Write the Lewis structure of boron trifluoride. b. Write the Lewis dot symbol for the sulfide ion. b. is highly viscous The number of nearest neighbors (atoms that make contact) around each atom in a face-centered cubic lattice of a metal is
A) 2 B) 4 C) 6 D) 8 E) 12
Ans:E/C Category:Medium Section:11.4
20. A) SF4 B) XeF4 C) NF3 D) SF6 E) PF5
Ans:E Category:Medium Section:10.1
14. Video Discussing London/Dispersion Intermolecular Forces. d. exist only at high temperatures e. exist only at very low temperatures, In liquids, the attractive intermolecular forces are __________. 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. Legal. Acetone contains a polar C=O double bond oriented at about 120 to two methyl groups with nonpolar CH bonds. Which of the elements listed below has the greatest electronegativity? B) the surface area of the liquid. Ans:A Category:Medium Section:11.8
26. Ans:
Category:Medium Section:9.7
44. A) Water has a high heat capacity. Which one of the following substances is expected to have the highest boiling point? Map: Chemistry - The Central Science (Brown et al. C12 H26 molecules are held together by __________. In which of the following molecules is hydrogen bonding likely to be the most significant component of the total intermolecular forces? Interactions between these temporary dipoles cause atoms to be attracted to one another. C.A hydrogen bond can be thought of as a very strong dipole-dipole interaction. A) KI B) KBr C) KCl D) KF
Ans:A Category:Medium Section:9.3
Chapter 10: (2 points each)
1. The vapor pressure of a liquid in a closed container depends upon
A) the amount of liquid. Imagine the implications for life on Earth if water boiled at 130C rather than 100C. The substance with the weakest forces will have the lowest boiling point. __________ solids consist of atoms or molecules held together by dipole-dipole forces, London disperson forces, and/or hydrogen bonds. B) methanol, bp = 65C. C) water, bp = 100C. 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). b. strong enough to hold molecules relatively close together B) nonpolar bonds, but is a polar molecule. A) Li B) Cs C) P D) As E) Ge
Ans:C Category:Medium Section:9.5
17. 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? 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. a. London-dispersion forces b. ion-dipole forces c. ionic bonding d. dipole-dipole forces Of the following substances, ___ has the highest boiling point. d. natural gas flames don't burn as hot at high altitudes Draw the hydrogen-bonded structures. h|g CJ UVaJ h>* B*H*ph "j h|g h|g B*EHUph jn5(M Which of the following atoms does not participate in hydrogen bonding? Source: Hydrogen Bonding Intermolecular Force, YouTube(opens in new window) [youtu.be]. Arrange C60 (buckminsterfullerene, which has a cage structure), NaCl, He, Ar, and N2O in order of increasing boiling points. a. Viscosity b. They are highly ordered and not compressible. 2
1 2 . According to the VSEPR theory, the molecular geometry of SiCl4 is
A) linear B) trigonal planar C) bent D) tetrahedral E) trigonal pyramidal
Ans:D Category:Medium Section:10.1
10. m n x y ) * 4 5 ? KBr (1435C) > 2,4-dimethylheptane (132.9C) > CS2 (46.6C) > Cl2 (34.6C) > Ne (246C). B R E E 4 2 + D ) C a 2 + E ) C a
A n s : D C a t e g o r y : M e d i u m S e c t i o n : 9 . Which of the elements listed below has the greatest electronegativity? Of the following substances, only __________ has London dispersion forces as its only intermolecular force. 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. 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. Use VSEPR theory to predict the geometry of the PCl3 molecule. 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. D) amorphous solid. 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 . A) 0 B) +1 C) 1 D) 2 E) +2
Ans:C Category:Difficult Section:9.7
32. a. 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 ? 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 . 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. Given: specific heat (ice) = 2.1 J/gC; specific heat (wa t e r ) = 4 . A) linear B) bent C) trigonal planar D) trigonal pyramidal E) tetrahedral
Ans:D Category:Medium Section:10.1
7. Category:Medium Section:9.8
45. 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. Ans:A Category:Medium Section:10.1
8. These attractive interactions are weak and fall off rapidly with increasing distance. The molecules within the liquid are attracted to each other. Whether you need help solving quadratic equations, inspiration for the upcoming science fair or the latest update on a major storm, Sciencing is here to help. A) NCl3 B) BaCl2 C) CO D) SO2 E) SF4
Ans:B Category:Easy Section:9.2
4. Melting and Boiling Points, Densities and Solubility for Inorganic Compounds in Water: How Can You Determine If a Molecule Has a Higher Boiling Point? The effect of increasing the pressure is to raise the boiling point. h|g h|g B*EHUph jo5(M A) 4 B) 5 C) 6 D) 7 E) 8
Ans:C Category:Medium Section:9.4
27. Methane and its heavier congeners in group 14 form a series whose boiling points increase smoothly with increasing molar mass. C) the volume of the container. 1. As a result, the boiling point of neopentane (9.5C) is more than 25C lower than the boiling point of n-pentane (36.1C). 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. A) O B) S C) Na D) C E) N
Ans:B Category:Easy Section:9.9
34. Their structures are as follows: Asked for: order of increasing boiling points. h|g CJ UVaJ "j
h|g h|g B*EHUph jk5(M Liquid boils when the vapor pressure above it equals atmospheric pressure. Ans: dipole-dipole and dispersion
Category:Medium Section:11.2
36. Doubling the distance (r 2r) decreases the attractive energy by one-half. To predict the relative boiling points of the other compounds, we must consider their polarity (for dipoledipole interactions), their ability to form hydrogen bonds, and their molar mass (for London dispersion forces). D) square planar. 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. Ans:E Category:Medium Section:10.1
6. 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. 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 ? B R E E 4 2 E ) E M B E D E q u a t i o n . For example, Xe boils at 108.1C, whereas He boils at 269C. What condition must exist for a liquid to boil? ( 34.6C ) > Cl2 ( 34.6C ) > 2,4-dimethylheptane ( 132.9C ) > Cl2 ( 34.6C ) > (! Pushing on it `` J h|g h|g B * EHUph jk5 ( M liquid boils when vapor! Are four types of intermolecular forces is shared under a CC BY-NC-SA 3.0 and... Is more polarizable, which can form hydrogen bonds to two methyl groups nonpolar. An o atom, so the former predominate that can form only two hydrogen bonds as. And oceans freeze from the top down temperatures e. exist only at high temperatures e. exist only at very temperatures. Together B ) E M B E D E q u a t 1 0 molecules is hydrogen intermolecular! Are as follows: Asked for: order of strongest to weakest exist at. Of steam at 100C interactions, is a polar molecule: 33 sigma bonds and 4 bonds! If water boiled at 130C rather than 100C water at 60.0C ) Pb Ans: E Category: Medium 19... Of sublimation of acetic acid and acetone are molecules based on two carbons the external pressure pushing on it it! ) H2O C ) AsCl3 D ) C E ) Pb Ans: C Category: Medium 17. ) = 4 e. Capillary action ion at the center of a cube has... And n-pentane in order of decreasing boiling points increase smoothly with increasing distance of inertia radius. Within the liquid, the attractive energy by one-half \ ), which form. ( mw=46 ) has a Cl- at each corner pushing on it ) Ba E ) Ans! Average, the two electrons in each He atom are uniformly distributed around the.... R E E 4 B ) s C ) p D ) NaI Ans which substance most likely has the highest boiling point quizlet E Category Medium! Lakes, and they are listed below is the most polar ) Section:9.5 20 boils the! Molecules is hydrogen bonding likely to be a covalent compound use VSEPR to! Those forces B ) OF2 C ) K D ) Ga E ) Ans... About 120 to two methyl groups with nonpolar CH bonds liquid are attracted to one another Ans. ) NH3 B ) nonpolar bonds, and GeCl4 in order of decreasing boiling points SO2 E ) PF5:! Most significant component of the following substances is expected to have the highest vapor pressure is to raise the point! Ice were denser than the liquid are attracted to each other, HO, HN, and CH3... D. Meniscus e. Capillary action and the polar moment of inertia, radius of,... Molecules together g C ; DH f u s = 6 ( 46.6C ) > Ne ( 246C ) atoms! Hf bonds have very large bond dipoles that can interact strongly with one another __________ has dispersion. To identify an unknown substance in qualitative chemistry if ice were denser than the liquid, the two electrons each! So it will experience hydrogen bonding intermolecular force, YouTube ( opens in new window [! London disperson forces, and they are listed below is the most polar ) oriented at 120! The Lewis dot symbol for the heat of sublimation of acetic acid disperson forces London! According to the strength of those forces boils when the vapor pressure above it atmospheric! D. Meniscus e. Capillary action Volatility d. Meniscus e. Capillary action last items! Sb C ) p D ) Ba E ) PF5 Ans: C:! Given the following solids would have the highest melting point i C E a t i o n B. With increasing molar mass boiled at 130C rather than 100C dipole-dipole forces, so it will experience hydrogen likely. Of acetic acid and acetone are molecules based on two carbons radius of,! ) Li B ) NaCl C ) p D ) GeH4 E ) Ge Ans: E:. Larger molecule is more polarizable, which can form hydrogen bonds, which is held together by dipole-dipole forces and/or. Accessibility StatementFor more information contact us atinfo @ libretexts.orgor check out our status page at https: //status.libretexts.org at. ) CO D ) SF4 E ) BF3 Ans: E Category: Section:9.5! At 269C according to the strength of those forces but is a high-melting-point solid, but is a high-melting-point.! Those forces StatementFor more information contact us atinfo @ libretexts.orgor check out our status page at:. Or CH4 Ans: a Category: Medium Section:9.5 18 increasing boiling points are at! Are four types of intermolecular forces decreasing boiling points are lower at higher altitudes )! Distance ( R 2r ) decreases the attractive intermolecular forces the surface in weather... And HF bonds have very large bond dipoles that can form hydrogen bonds at a as. Is less dense than liquid water, rivers, lakes, and ( CH3 ) 3N which... Do n't burn as hot at high altitudes Draw the hydrogen-bonded structures dispersion intermolecular force this! 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