e. melts rather than sublimes under ordinary conditions, Crystalline solids differ from amorphous solids in that crystalline solids have_____ Which of the following species has the largest dipole moment (i.e., is the most polar)? a. London-dispersion forces b. ion-dipole forces c. ionic bonding d. dipole-dipole forces 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. Asked for: order of increasing boiling points. Ans:B Category:Medium Section:11.8 27. c. heat isn't conducted as well in low density air This question was answered by Fritz London (19001954), a German physicist who later worked in the United States. Give the number of lone pairs around the central atom and the molecular geometry of XeF4. What is the expected value for the heat of sublimation of acetic acid? Compounds with higher molar masses and that are polar will have the highest boiling points. Which of the elements listed below is most likely to exhibit an expanded octet in its compounds? A) NH3 B) CCl4 C) CO2 D) SF4 E) PCl5 Ans:B Category:Medium Section:10.1 17. Cs 2. 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. __________ are particularly polarizable. 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. Write a Lewis structure for SO3 that expands the octet to minimize formal charge and if necessary places negative formal charges on the most electronegative atom(s). A) ethanol, bp = 78C C) water, bp = 100C B) methanol, bp = 65C D) acetone, bp = 56C Ans:C Category:Medium Section:11.8 11. 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. D) amorphous solid. Which of the following liquids would have the highest viscosity at 25C? 5 2 4 . 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 . 5 2 3 . Video Discussing Hydrogen Bonding Intermolecular Forces. b. The first compound, 2-methylpropane, contains only CH bonds, which are not very polar because C and H have similar electronegativities. E) trigonal pyramidal. Northrup's Chem 112 Section TTU General Chemistry. There are four types of intermolecular forces, and they are listed below in order of strongest to weakest. If you are comparing molecules to determine which has the higher boiling point, consider the forces that are at work within the molecule. On average, the two electrons in each He atom are uniformly distributed around the nucleus. Source: Dipole Intermolecular Force, YouTube(opens in new window) [youtu.be]. 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. 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. A) Sr B) V C) Ni D) P E) I Ans:A Category:Medium Section:9.5 19. C) dispersion forces. Category:Medium Section:9.8 45. C) water, bp = 100C. )%2F11%253A_Liquids_and_Intermolecular_Forces%2F11.02%253A_Intermolecular_Forces, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). A) CBr4 B) CBr3F C) CBr2F2 D) CBrF3 E) CF4 Ans:E Category:Medium Section:11.2 8. b. Cooking times for boiled food need to be changed to ensure the food is completely cooked. A) CaCl2 B) CO2 C) CS2 D) SO2 E) OF2 Ans:A Category:Easy Section:9.2 2. 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. a. XeF4 b. AsH3 c. CO2 d. BCl3 e. Cl2, When NaCl dissolves in water, aqueous Na+ and Cl- ions result. Ans: Category:Medium Section:9.9 46. Write a Lewis structure for OF2. In nuclear fission, a nucleus of uranium-238, which contains 92 protons, can divide into two smaller spheres, each having 46 protons and a radius of 5.9010155.90 \times 10 - 155.901015 m. What is the magnitude of the repulsive electric force pushing the two spheres apart? (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. - In larger atoms such as Xe, however, the outer electrons are much less strongly attracted to the nucleus because of filled intervening shells. Write a Lewis structure for SO3 that obeys the octet rule, showing all non-zero formal charges, and give the total number of resonance structures for SO3 that obey the octet rule. 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: . CsCl crystallizes in a unit cell that contains the Cs+ ion at the center of a cube that has a Cl- at each corner. d. They assume both the volume and the shape of their containers. 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. The geometry of the SF4 molecule is A) tetrahedral. Which of the following substances will display an incomplete octet in its Lewis structure? C) Water can form hydrogen bonds. A.Hydrogen bonds involve hydrogen bonded to carbon, nitrogen, oxygen, or fluorine. Write the Lewis dot symbol for the sulfide ion. 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 \(\PageIndex{6}\). A) KF B) CaCl2 C) SF4 D) Al2O3 E) CaSO4 Ans:C Category:Easy Section:9.4 7. How many atoms are there per unit cell? A) ClF3 B) FeCl3 C) NH3 D) PF3 E) SO3 Ans:B Category:Easy Section:9.2 3. h|g CJ UVaJ ! " 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 . 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. e. 2and4, The predominant intermolecular force in CaBr2 is __________. Note the last two items in the table above. a. appreciable intermolecular attractive forces h|g CJ UVaJ h>* B*OJ QJ ^J ph h>* H*h>* B*H*ph "j Surface tension c. Volatility d. Meniscus e. Capillary action. As a result, it is relatively easy to temporarily deform the electron distribution to generate an instantaneous or induced dipole. Of the given pair of compounds, which would have the higher boiling point? (Despite this seemingly low value, the intermolecular forces in liquid water are among the strongest such forces known!) d. the same thing 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. Intermolecular forces are electrostatic in nature and include van der Waals forces and hydrogen bonds. The attractive energy between two ions is proportional to 1/r, whereas the attractive energy between two dipoles is proportional to 1/r6. Consequently, N 2 O should have a higher boiling point. a. inversely proportional to one another B R E E 4 2 E ) E M B E D E q u a t i o n . 0 f. %, 2 Y) r 2 %, 2 %, ] ] %, ] ] ] ] ] K- K- * Z ] ] ] f. ] ] ] ] 2 ] ] ] ] ] ] ] ] ] | : Chapter 9: (2 points each) 1. 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) 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. What is the major attractive force that exists among different I2 molecules in the solid? C.A hydrogen bond can be thought of as a very strong dipole-dipole interaction. 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 force of attraction that exists between Na+ and H2O is called a(n) __________ interaction. h|g h|g B*EHUph jj5(M 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. Our goal is to make science relevant and fun for everyone. 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. The structure of liquid water is very similar, but in the liquid, the hydrogen bonds are continually broken and formed because of rapid molecular motion. In this section, we explicitly consider three kinds of intermolecular interactions. N2 Br2 H2 Cl2 O2. c. is highly hydrogen-bonded Melting and Boiling Points, Densities and Solubility for Inorganic Compounds in Water: How Can You Determine If a Molecule Has a Higher Boiling Point? Which of the following ionic solids would have the largest lattice energy? GeCl4 (87C) > SiCl4 (57.6C) > GeH4 (88.5C) > SiH4 (111.8C) > CH4 (161C). 8 k J D ) 4 0 . B R E E 4 B ) E M B E D E q u a t i o n . Acetic acid and acetone are molecules based on two carbons. The disruptive force of molecules bumping into each other allows them to overcome the attraction that they have for the molecules beside them. very soft A) NF3 B) CO2 C) CF4 D) Br2 E) NO Ans:E Category:Medium Section:9.9 36. Which one of the following molecules has an atom with an incomplete octet? Ans:D Category:Medium Section:11.8 31. 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 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. London dispersion forces b. ion-dipole forces c. ionic bonding d. dipole-dipole forces Explain your reasoning. 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 . C12 H26 molecules are held together by __________. A) NaI B) NaF C) MgO D) MgCl2 E) KF Ans:C Category:Medium Section:9.3 50. A) 1 B) 2 C) 4 D) 6 E) 8 Ans:B Category:Medium Section:11.4 21. A) 19C B) 52C C) 60C D) 64C E) 70C Ans:D Category:Medium Section:11.8 24. Vapor Pressure and Water: How Can You Determine If a Molecule Has a Higher Boiling Point? A) CsOH B) NF3 C) Sr(NO3)2 D) CaO E) LiF Ans:B Category:Easy Section:9.4 8. Imagine the implications for life on Earth if water boiled at 130C rather than 100C. The properties of liquids are intermediate between those of gases and solids, but are more similar to solids. Which of the elements listed below has the greatest electronegativity? The key is to know which bonds require more energy for boiling to occur. Study with Quizlet and memorize flashcards containing terms like 4. amorphous solids, 4. E) Water is a polar molecule. 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. Of the following, __________ has the highest boiling point. d. is highly cohesive D) Ice is more dense than liquid water. The first two are often described collectively as van der Waals forces. Which one of the following is most likely to be a covalent compound? A) 4 B) 5 C) 6 D) 7 E) 8 Ans:C Category:Medium Section:9.4 27. Indicate all the types of intermolecular forces of attraction in SO2(l). The substance with the weakest forces will have the lowest boiling point. Which property of water allows a razor blade to float on it without sinking? Argon and N2O have very similar molar masses (40 and 44 g/mol, respectively), but N2O is polar while Ar is not. Write a Lewis structure for the nitrate ion, NO3, showing all non-zero formal charges. a. is highly flammable Let's start with some basics. 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. A polar covalent bond would form in which one of the following pairs of atoms? . The number of lone electron pairs in the NO2 ion is ___. 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 \(\PageIndex{4}\)). Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of 24.3 kJ/mol. Of the following substances, ___ has the highest boiling point. 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. Which of the atoms listed below is the most electronegative? b. heat of fusion, heat of vaporization Which of the following solids would have the highest melting point? h|g CJ UVaJ "j h|g h|g B*EHUph jf5(M 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). The following features will have the effect of creating a higher boiling point: NaCl (saturated solution in water: 23.3%w/w). Use VSEPR theory to predict the geometry of the PCl3 molecule. Br2. Ans:E Category:Medium Section:11.8 12. A) H2S B) HCN C) BF3 D) H2CO E) SO2 Ans:B Category:Medium Section:10.1 13. Give the number of lone pairs around the central atom and the molecular geometry of SCl2. 1and8 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. A) HCl B) AsCl5 C) ICl D) NCl3 E) Cl2 Ans:B Category:Medium Section:9.9 39. A) 0 B) +1 C) 1 D) 2 E) +2 Ans:C Category:Difficult Section:9.7 32. B.In a hydrogen bond, the hydrogen atom on one molecule is attracted to unpaired electrons associated with nitrogen, oxygen, or fluorine on another molecule. m n x y ) * 4 5 ? B) ion-dipole forces. Which of the following ionic solids would have the largest lattice energy? h|g CJ UVaJ h>* B*ph h' h>* h>* B*OJ QJ ^J ph j h>* B*Uph "j h|g h|g B*EHUph H I ] ^ _ ` b B D F H L ` d yjXS h>* H*"j) h|g h|g B*EHUph jr5(M 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. b. high boiling point 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. 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. d. natural gas flames don't burn as hot at high altitudes A) KF B) KI C) LiF D) LiI E) NaF Ans:C Category:Medium Section:9.3 15. In contrast, the hydrides of the lightest members of groups 1517 have boiling points that are more than 100C greater than predicted on the basis of their molar masses. e. all of the above, A volatile liquid is one that __________. A) H2O B) BF3 C) Cl2 D) SiH4 E) Ar. a. low vapor pressure 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). Ans: dispersion Category:Medium Section:11.2 33. A) linear B) bent C) trigonal planar D) trigonal pyramidal E) tetrahedral Ans:D Category:Medium Section:10.1 7. Predict the melting and boiling points for methylamine (CH 3 NH 2). Consequently, N 2 O should have a higher boiling point. Mark each of the following statements as TRUE or FALSE. According to the VSEPR theory, the molecular geometry of beryllium chloride is A) linear B) trigonal planar C) bent D) tetrahedral E) trigonal pyramidal Ans:A Category:Medium Section:10.1 9. When a liquid boils, on the other hand, the molecules below the surface have enough energy to escape the liquid phase and become a gas. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. E) ionic crystal. Source: Dispersion Intermolecular Force, YouTube(opens in new window) [youtu.be]. They are highly ordered and not compressible. b. Large intermolecular forces in a substance are manifested by __________. A) Li B) Cs C) P D) As E) Ge Ans:C Category:Medium Section:9.5 17. Of the following substances, ___ has the highest boiling point. The polarizability of a substance also determines how it interacts with ions and species that possess permanent dipoles. d. heat of freezing(solidification),heatofvaporization a) ion-ion attractions E) hydrogen bonding. The heat of sublimation is equal to the sum of the heat of vaporization and the heat of freezing, true or false? Acetone are molecules based on two carbons ) NCl3 E ) 8 Ans: C Category: Medium 39., but are more similar to solids 7 E ) Cl2 Ans: B Category: Difficult Section:9.7 32 ___. Of XeF4 other allows them to overcome the attraction that exists among different I2 molecules in table... Predict the melting and boiling points for methylamine ( CH 3 NH ). Different I2 molecules in the NO2 ion is ___ highest viscosity at 25C of sublimation is equal the! Xef4 b. AsH3 c. CO2 d. BCl3 e. Cl2, When NaCl dissolves in water aqueous. Two ions is proportional to 1/r6 flashcards containing terms like 4. amorphous solids, but are more similar solids... Fun for everyone ion is ___ greatest electronegativity are at work within the molecule atoms listed below the! Last two items in the solid cscl crystallizes in a substance also determines How it with... Molecules has an atom with an incomplete octet x27 ; s Chem 112 Section TTU General.! ) SO2 E ) Ar without sinking different I2 molecules in the solid ) > (. 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