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Chemistry
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18 Dec 2019

All of the following statements concerning hydrogen bonding are correct EXCEPT

water is less dense in the solid phase than the liquid phase due to hydrogen bonding.
hydrogen bonding occurs in molecules with N-H, O-H, and F-H bonds.
hydrogen bonding in water results in lower than expected melting points.
the unusually high boiling points of water, ammonia, and hydrogen fluoride are the result of hydrogen bonding.
hydrogen bonding is an unusually strong dipole force.

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Related questions

Water has many unique properties due to strong hydrogen bondinginteractions. Which of the
following IS NOT a direct result of hydrogen bonding?
A. Water's relatively high boiling point
B. Water's ability to solvate a wide range of substances
C. The solid phase of water is less dense than the liquid phase ofwater
D. The low molar mass of water

* Circle the intermolecular force(s) that is/are present in each of the following species. [Hint: there may be more than one correct answer.]

Ar (hydrogen bonding, dipole-dipole forces, dispersion forces)

CH4 (hydrogen bonding, dipole-dipole forces, dispersion forces)

HBr (hydrogen bonding, dipole-dipole forces, dispersion forces)

HF (hydrogen bonding, dipole-dipole forces, dispersion forces)

CHCl3 (hydrogen bonding, dipole-dipole forces, dispersion forces)

* For the following pairs of atoms/molecules, circle the species that has the higher boiling point.

Ne or Xe

Cl2 or F2

HBr or HF

HCl or HI

H2O or H2S

* Phase changes always associate with change of enthalpy. For the following situations, name the phase

transition and indicate whether the process is exothermic or endothermic.

(a) Dry ice (solid carbon dioxide) turns to gaseous carbon dioxide.

Answer:

(b) Water vapor turns to liquid water.

Answer:

(c) Solid iron turns to liquid iron.

Answer:

(d) Iodine vapor turns to solid iodine.

Answer:

(e) Liquid helium turns to helium gas.

Answer:

* True or false

1. Intermolecular forces are stronger than ionic and covalent bonds. Answer:

2. For molecules with similar size and molar mass, those with higher polarity would have higher boiling

point. Answer:

3. Ion-dipole forces exist between ionic potassium bromide and polar water.

Answer:

4. Dispersion forces exist between argon and helium. Answer:

5. Instantaneous dipoles exist in all molecules and atoms. Answer:

6. The strength of dispersion forces depends on the molar mass but the shape of the molecules have no effect on dispersion forces. Answer:

7. Ice has a higher density than water because ice has an ordered cagelike structure. Answer:

8. Liquids with weaker intermolecular interactions have lower viscosity. Answer:

9. Viscosity decreases with increasing temperature. Answer:

10. For any molecules, the heat of vaporization is always lower than the heat of fusion because it takes more energy to make molecules to move past one another in a solid lattice. Answer:

1.

a) Which one of the following is expected to have the highest vapor pressure at room temperature? ( Ethanol bp = 78 degrees Celsius, Methanol bp =65 degrees Celsius, Diethyl ether bp = 35 degrees Celsius, Acetone bp = 56 degrees Celsius )

b) Which of the following species are NOT capable of hydrogen bonding as pure substances? ( C3H8, CH3COOH, CH3CH2OH, HCI )

c) True or False: Liquids that have strong intermolecular forces generally have higher viscosities than those that have weak intermolecular forces.

d) Graphite crystallizes as what type of crystal? ( Ionic, Covalent, Molecular, Metallic )

e) Which one of the following substances crystallizes as a molecular crystal? ( NaCI, Na, SiO2, CO2 )

f) Which one of the following statements is NOT true in regards to water? ( Water has a high heat capacity, Water has an unusually high boiling point for such a small molecule, Water can form hydrogen bonds, Ice is more dense than liquid water, Water is a polar molecule )

g) List the type(s) of intermolecular forces that exist in each of the following substances:

CH3CI

H2O

KCI

CH4

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