Chapter 8 Review

1
Chapter 8 ReviewCovalent Bonding
2
Chapter 8 Review

• What is the correct electron configuration
  arrangement of the four valence electrons of the
  carbon atom in a methane molecule (CH4) a)
  2s22p2, or b) 2s12p3?
• Which noble gas has the same electron
  configuration as the oxygen in a water molecule?

3
Chapter 8 Review

• When placed between oppositely charged metal
  plates, the region of a water molecule attracted
  to the negative plate is the ____.
• When one atom contributes both bonding electrons
  in a single covalent bond, the bond is called
  a(n) ____.

4
Chapter 8 Review

• The shape of the methane molecule (CH4) is called
  ____. What are the bond angles?
• How is a pair of molecular orbitals formed?
• Which elements can form diatomic molecules joined
  by a single covalent bond?
• What is a typical characteristic of an ionic
  compound? Covalent?

5
Chapter 8 Review

• Experimental evidence suggests that the H-C-H
  bond angles in ethene, C2H4, are ____ degrees.
• A bond that is not symmetrical along the axis
  between two atomic nuclei is a(n) ____ bond.
• Once formed, how are coordinate covalent bonds
  different from other covalent bonds?

120
6

• Substances that show relatively strong
  attractions to an external magnetic field are
  said to be ____________?
• Oxygen is an example of a substance that is
  ____________?

7
Chapter 8 Review

• What causes hydrogen bonding?
• How many electrons can occupy a single molecular
  orbital?
• According to the VSEPR theory, molecules adjust
  their shapes to keep ____ as far apart as
  possible.
• Which of the following atoms acquires the most
  negative charge in a covalent bond with hydrogen
  a) carbon, or b) oxygen?

8
Chapter 8 Review

• How do atoms achieve noble-gas electron
  configurations in single covalent bonds?
• What is required in order to melt a network
  solid?
• Molecular orbital theory is based upon what model
  of the atom?
• Where are the electrons most probably located in
  a molecular bonding orbital?

9
Chapter 8 Review

• A molecule with a single covalent bond is a)
  CO2, or b) Cl2?
• A bond formed between a silicon atom and an
  oxygen atom is likely to be a(n) ____ bond.
• Which of the following diatomic molecules is
  joined (seemingly) by a double covalent bond a)
  O2, or b) N2?

10
Chapter 8 Review

• What causes water molecules to have a bent shape,
  according to the VSEPR theory?
• Which of these elements does not exist as a
  diatomic molecule a) Ne, or b) F?
• Which of the following elements can form diatomic
  molecules held together by triple covalent bonds
  a) fluorine, or b) nitrogen?

11
Chapter 8 Review

• Which of the following covalent bonds is the most
  polar a) H-F, or b) H-N?
• What is shown by the structural formula of a
  molecule or a polyatomic ion?
• What is thought to cause the disperson forces?

12
Chapter 8 Review

• What are the weakest attractions between
  molecules called?
• Which type of solid has the highest melting
  point a) ionic solids, or b) network solids?
• Why do atoms share electrons in covalent bonds?

13
Chapter 8 Review

• How many valid electron dot formulas having the
  same number of electron pairs for a molecule or
  ion can be written when a resonance structure
  occurs?

14
Chapter 8 Review

• Which of the forces of molecular attraction is
  the weakest a) hydrogen bonding,
  or b) dispersion forces?
• In which of the following compounds is the octet
  expanded to include 12 electrons a) PCl5, or b)
  SF6?
• Why is hydrogen bonding only possible with
  hydrogen?

15
Chapter 8 Review

• What causes dipole interactions?
• How many electrons does carbon need to gain in
  order to obtain a noble-gas electron
  configuration?
• How many covalent bonds are in a covalently
  bonded molecule containing 1 phosphorus atom and
  3 chlorine atoms?

16
Chapter 8 Review

• How many electrons does a nitrogen atom need to
  gain in order to attain a noble-gas electron
  configuration?
• What is the bond angle in a water molecule?
• How many unshared pairs of electrons are in a
  molecule of hydrogen iodide?

17
Chapter 8 Review

• How many electrons are shared in a single
  covalent bond?
• What is the total number of covalent bonds
  normally associated with a single carbon atom in
  a compound?
• How many valence electrons does an iodine atom
  have?
• How many unshared pairs of electrons does the
  nitrogen atom in ammonia possess?

18
Chapter 8 Review

• How many electrons are shared in a double
  covalent bond?
• Know the shape/bond angles of the following
  CO2, H2O, CCl4, NH3, SO3, PF5, SF6

End of Chapter 8 Review