8.43 Identify the kinds of intermolecular forces (London dispersion, dipole−dipole, or hydrogen bonding) that are the most important in each of the following substances. (a) methane
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- Which of the following is FALSE about the water molecule? A Intermolecular forces among water molecules are the least extensive when it is in liquid form. The atoms comprising the water molecule are covalently bonded with one another. (c) The H atoms bear the partial positive charge. Its molecular geometry is not linear.arrow_forwardThe substance with the lowest known boiling point (4 K) is helium, an atomic element that has two electrons. Hydrogen isa diatomic molecule and also has two electrons, but its boiling point is significantly higher, at 20.28 K.(a) What is the dominant intermolecular force between a pair of helium atoms and a pair of H2 molecules?(b) Why do you think H2 has a higher boiling point?arrow_forwardWhich of the following set of compounds form an ionic solid, a molecular solid, and a covalent network solid, in that order? (A) Na2O, Na2O2, SiO2; (B) Na2O, MgO, Al2O3; (C) BaO, BaO2, CO2; (D) CaO, SO2, SiO2;arrow_forward
- Explain in terms of molecular forces why (i) NH3 has a higher boiling point than CH4 (ii) KCl has a higher melting point than I2arrow_forwardOctane (C8H18) is a component of fuel used in internal combustion engines. The dominant intermolecular forces in octane arearrow_forwardName the type(s) of intermolecular forces that exists between molecules (or basic units) in each of the following species and identify the following species that are capable of hydrogen-bonding among themselves. (a) BeH2, (b) CH3COOHarrow_forward
- Name the type(s) of intermolecular forces that exists between molecules (or basic units) in each of the following species and identify the following species that are capable of hydrogen-bonding among themselves. (a) C2H6, (b) HI, (c) KF, (d) BeH2, (e) CH3COOHarrow_forwardThe binary hydrogen compounds of the Group 4A elements and their boiling points are: CH4, –162ºC; SiH4, –112ºC; GeH4, –88ºC; and SnH4, –52ºC. Explain the increase in boiling points from CH4 to SnH4.arrow_forwardWhich type of intermolecular force accounts for each ofthese differences? (a) CH3OH boils at 65 °C; CH3SH boils at6 °C. (b) Xe is a liquid at atmospheric pressure and 120 K,whereas Ar is a gas under the same conditions. (c) Kr,atomic weight 84 amu, boils at 120.9 K, whereas Cl2, molecularweight about 71 amu, boils at 238 K. (d) Acetone boilsat 56 °C, whereas 2-methylpropane boils at -12 °C.arrow_forward
- 9. So far we have discussed 4 kinds of intermolecular forces: ionic, dipole-dipole, hydrogen bonding, and London forces. What kind(s) of intermolecular forces are present in the following substances: a) NH,, b) SF, c) PCI, d) LICI, e) HBr, f) CO, 3' 6' '3 (hint: čonsider AEN and molecular shape/polarity)arrow_forwardArrange the following in INCREASING strength of intermolecular force:(1) NH3 and HI; (2) H2 and CO2; and (3) HF and C10H8 O 1>2 > 3 3 > 2 > 1 2 > 3 > 1 3 >1>2 None of the above O O O Oarrow_forward9. Identify the types of intermolecular forces present in each of the following substances and select the substance in each pair that has the higher boiling point: (a) HOOH or HSSH; (b) C3H8 or CH3OCH3arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning