Question

1. Select the two compounds that are more likely to be a gas at room temperature (as opposed to a liquid).

CH₄

CH₃OH

C₂H₆

H₂O

2. The separation of charges within a polar molecule is called a(n) ________.

polar bond

strong attraction

dipole

ionic bond

dipole-dipole

3. Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C₈H₁₈) have only limited solubility in water?

dipole-dipole

ion-dipole

Both dipole-dipole and induced dipole-induced dipole

induced dipole-induced dipole

dipole-induced dipole

4. How much energy is needed to convert 64.09 grams of water at 100.°C to steam at 128.40 °C?
specific heat (steam) = 2.09 J/g°C
specific heat (water) = 4.18 J/g°C
heat of fusion = 6.02 kJ/mol
heat of vaporization = 40.6 kJ/mol

144.42 kJ

  

25.21 kJ

  

152.03 kJ

  

3.80 kJ

  

148.23 kJ

5. The charges with sodium chloride are all balanced-for every positive sodium ion there is a corresponding negative chloride ion. Since its charges are balanced, how can sodium chloride be attracted to water, and vice versa?

  

Hydrogen bonding in water allows the sodium chloride molecule to be attracted to the water molecule.

   

As a water molecule gets close to the sodium chloride it can distinguish the various ions and it is thus attracted to an individual ion by ion-dipole forces.

   

Dispersion forces come into play as the sodium chloride and water come into close proximity.

   

This is not a matter of attraction. Sodium chloride dissolves in water because water provides a medium in which the individual sodium and chloride ions can disperse.

6. Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C₈H₁₈) have only limited solubility in water?

  

dipole-dipole

   

ion-dipole

   

Both dipole-dipole and induced dipole-induced dipole

   

induced dipole-induced dipole

   

dipole-induced dipole

7. If an ionic bond is stronger than a dipole-dipole interaction, how can water dissolve an ionic compound?

  

None of these

   

The ion-dipole interactions of a bunch of water molecules gang up on the strong ionic bond and pull it into the solution.

   

The ions never overcome their interatomic attraction and therefore are not soluble.

   

The ionic bond is weakened by the ion-dipole interactions and ionic repulsion ejects the ions from the crystal.

   

The ion-dipole interaction causes the ions to heat up and vibrate free of the crystal.

8.The separation of charges within a polar molecule is called a(n) ________.

  

polar bond

   

strong attraction

   

dipole

   

ionic bond

   

dipole-dipole

9. Select the two compounds that are more likely to be a gas at room temperature (as opposed to a liquid).

  

CH₄

  

CH₃OH

  

C₂H₆

  

H₂O

10.The bonds between hydrogen and oxygen in a water molecule can be characterized as

  

intramolecular forces.

  

intermolecular forces.

  

London forces.

  

dispersion forces.

  

hydrogen bonds.

Answer 1

Please upload only one question at a time.

1. gas at very weak CH4 and C2 H6 are more likely to be room temperature because they have forces of attraction between them. Dispersion or London forces are present b/w molecules of CHy and CaH6. the 2. dipole A dipole is a separation of charges between molecule electrical charges are separated to polar molecule and make dipole due dipole - induced dipole. water is a polar molecule H2O induced dipale in C8H18 and make it a temporary dipple. This temporary dipole with palar water malecule make dipale induced dipole bonds.