front 1 London dispersion forces are formed due to instantaneous ______________ formation. | back 1 dipole |
front 2 From these three choices, CH4 , NH3 and H2O , which one does NOT have the capacity for hydrogen bonding? | back 2 CH4 does not use hydrogen bonding because the difference in electronegativity between C and H is too small. |
front 3 Which statement explains the attraction between the water molecules? | back 3 Water is a polar molecule. The slightly negative end of the molecule attracts to the slightly positive end of other molecules. This forms a weak connection between the molecules. |
front 4 Which of the following compounds are most likely to form hydrogen bonds? | back 4 H2O |
front 5 Which of the following statements best explains why ice floats on water? | back 5 Hydrogen bonding causes water to be less dense in the solid state than in the liquid state . |
front 6 Substances that exhibit hydrogen bonding or dipole-dipole forces are generally soluble in ______________. | back 6 water |
front 7 Are melting points of molecular compounds generally higher than, lower than, or the same as those of ionic compounds? | back 7 lower than |
front 8 Which statement best explains these properties? | back 8 Ammonia is polar and experiences hydrogen bonding attractions between neighboring molecules and makes it harder to overcome the intermolecular forces needed for the phase change from liquid to gas. |
front 9 Intermolecular forces include all of the following EXCEPT: | back 9 covalent bonding |
front 10 The most important intermolecular force in CCl4 is: | back 10 london dispersion forces |
front 11 The ________ shape of water allows several water molecules to bond together, which influences its physical properties. | back 11 bent |
front 12 Select the substance with the lowest boiling point and identify the most important intermolecular force responsible for the difference in boiling point. | back 12 CH4 has the lowest boiling point because it uses London dispersion forces. |
front 13 London dispersion forces are formed due to instantaneous _____ formation. | back 13 dipole |
front 14 What is a term for attractive forces that occur between polar molecules? | back 14 dipole-dipole forces |
front 15 Generally, are London dispersion forces stronger or weaker than dipole-dipole forces? | back 15 weaker |
front 16 Movement of the ____________ creates the London dispersion forces. | back 16 electrons |
front 17 When you put sodium metal in liquid ammonia, what is the intermolecular attraction between Na+ ions and NH3 molecules? | back 17 Ion-dipole |
front 18 When KOH dissolved in ethanol, what is the intermolecular attraction between OH- ions and C2H5OH molecules? | back 18 Ion-dipole` |
front 19 Which statement about London dispersion forces is TRUE? | back 19 London Dispersion forces are temporary in nature. |
front 20 When KCl dissolved in ethanol, what is the intermolecular attraction between K+ ions and ethanol molecules? | back 20 Ion-dipole |
front 21 What are dipole-dipole forces? | back 21 intermolecular force between polar molecules |
front 22 Which noble gas below has the lowest boiling point? | back 22 Ne |
front 23 Which of the following is the weakest intermolecular force? | back 23 London dispersion force |
front 24 When KNO3 dissolved in water, what is the intermolecular attraction between NO3 - ions and H2O molecules? | back 24 Ion-dipole |
front 25 Which of the following statements best explains why ice floats on water? | back 25 Hydrogen bonding causes water to be less dense in the solid state than in the liquid state. |
front 26 Which of the following compounds is most likely to form hydrogen bonds? | back 26 H2O |
front 27 The _________ shape allows several water molecules to bond together, which influences its physical properties. | back 27 bent |
front 28 Which of the following compounds is/are most likely to form hydrogen bonds? | back 28 HF |
front 29 Complete the sentence using one of the following terms: proton, neutron or electron. When H is covalently bonded to N, O or F, the strongly electronegative atoms pull the electrons in the covalent bond close to themselves, leaving H as almost a bare ___________. | back 29 proton |
front 30 Which of the following does not have hydrogen bonds? | back 30 Hydrogen chloride |
front 31 The O-H covalent bond in a water molecule is best described as being _____. | back 31 very polar |
front 32 In addition to hydrogen bonding, what also contributes to the fact that ice is less dense than liquid water? | back 32 its bent shape |
front 33 In the case of hydrogen bonds, the hydrogen donor is strongly: | back 33 Electronegative |
front 34 True or False: Because the molecular weight of hydrogen chloride is heavier than that of water, the boiling point of hydrogen chloride is higher than that of water | back 34 False |
front 35 Properties of solids depend on: | back 35 All of the above |
front 36 Complete the sentence using one of the following terms: water, hexane or oil. Substances that exhibit hydrogen bonding or dipole-dipole forces are generally soluble in __________. | back 36 water |
front 37 Are melting points of molecular compounds generally higher or lower than those of ionic compounds? | back 37 lower |
front 38 Intermolecular forces are _____ as compared to intra-molecular forces. | back 38 Much weaker |
front 39 What type of solid is diamond? | back 39 covalent network |
front 40 Why do covalent crystals have high melting and boiling points? | back 40 The network covalent bond is very strong. |
front 41 Which of the following statements is wrong? | back 41 Covalent compounds are generally soluble in polar solvents |
front 42 Diamond is composed entirely of _____ atoms that are connected by _____ bonds. | back 42 carbon; covalent |
front 43 Intermolecular forces include all of the following EXCEPT _____ | back 43 covalent bonding |
front 44 Nonpolar solvents will most easily dissolve solids that are | back 44 nonpolar. |
front 45 This is the structure picture of fullerene (C60). The type of chemical bond that holds fullerene (C60) together is | back 45 covalent |