Covalent Compounds and Intermolecular Forces Review

Bond Type / Bond Between / Electronegativity Difference / What happens to electrons? / Example
Ionic
Polar Covalent
Non-polar Covalent
Metallic / N/A
  1. What is electronegativity, and what general trend does it follow on the periodic table?
  1. Determine the bond formed between each of following elements. Label with charges (either full or partial) when appropriate).

  1. C-H______
  2. Li-F______
  3. N-Cl______
  4. Cs-S______
  5. O-O______
  6. P-Br______

  1. What is the difference between a polar and non-polar covalent bond?

For each of the following fill in the missing blanks.

Name Formula

  1. ______P2O5
  2. ______Si2Br6
  3. Triboron pentoxide ______
  4. ______P4S5
  5. Hexaboron monosilicide ______
  1. Draw the Lewis dot diagrams for the following:

  1. K
  2. K+
  3. Xe
  4. N
  5. N-3
  6. P
  7. S
  8. Be

  1. Typically, how many bonds does each of the following like to form?

  1. C ______
  2. H ______
  3. Cl ______
  4. P ______
  5. S ______
  6. B ______

  1. Draw the Lewis dot diagram for each of the following compounds. For covalent compounds, determine the electron group geometry, molecular geometry, draw the 3-D structure of the molecule, and indicate whether the molecule is polar or non-polar.
  1. CCl4
  1. IF3
  1. O2
  1. LiF
  1. H2O
  1. BF3
  1. PF5
  1. XeBr4
  1. CO3-2
  1. Rank the bond types in order of their length (1 being shortest) and strength (1 being weakest).

LengthStrength

  1. Single______
  2. Double ______
  3. Triple______
  1. What causes a molecule to be polar?
  1. Determine if the following molecules are polar or non-polar.

a) NH3b) CF4c) CO2d) CH3Br

______

  1. What is a dispersion force?
  1. Which hydrocarbon listed below would have the larger dispersion force? (Circle one)

C4H10 or C8H18

  1. Which hydrocarbon isomer shown below would have the greater dispersion force? (Circle one)

a.

b. Why is one dispersion force greater than the other even though the molecular weights are the same?

  1. Substance A and substance B are both non-polar , but substance A has a larger mass than B. Which substance has the higher……

a) surface tension ______b) boiling point ______

c) evaporation rate ______d) freezing point ______

  1. Rank in order of increasing melting point the following non-polar molecules. (1=lowest)

a) CH4 ____b) CH3CH3 ___c) CCl4 ___d) Br2 ___

  1. Name the three types of dipole-dipole forces and explain the polarity of the molecules involved in each.

TypePolarity of the molecules

IMF is between

a)

b)

c)

  1. Which 4 elements are involved when a hydrogen bond is present between molecules?

a)b)c)d)

  1. If a liquid has strong intermolecular forces then the ………is (either high or low).

a) surface tension ______b) boiling point ______

c) melting point ______d) evaporation rate______

  1. Describe the relationship between the viscosity of a liquid and the strength of the IMF between molecules.
  1. Complete the following table for each type of solid listed at the left.

Type StructuralIMF PresentGeneral Properties

Particles

______

Molecular Covalent

Nonpolar

______

Molecular Covalent

Polar

______

Molecular Covalent

w/ H Bonding

______

Network Covalent

______

Ionic

______

Metallic

______