Bonding Problem Set 2015
Please complete on separate piece of paper. If typed, molecules should be formatted in a way that matches hand
drawn diagrams. See the calendar for your class’s due date.
1. How does the octet rule explain the different types of bonding (ionic, covalent, metallic)?
2. Explain why the bond length of diatomic nitrogen is different than the bond length of diatomic fluorine.
3. Draw the Lewis structures for the following ionic compounds.
a. sodium oxide
b. barium fluoride
c. strontium phosphide
4. Label the following bonds as either ionic, non-polar covalent, or polar covalent. Draw the dipoles where
necessary. Example:
a.
b.
c.
d.
e.
H–I
Se – S
P–H
Na – F
Cl – Cl
H–F
this diagram shows that the
bond is polar covalent and that fluorine has a stronger
pull on the electrons than hydrogen.
5. Draw the Lewis structures for the following covalent compounds or polyatomic ions.
a. chlorite ion
b. silicon tetrahydride
c. phosphorus trichloride
d. sulfur hexafluoride
e. boron trihydride
6. a. The sulfite ion contains coordinate covalent bonds. Use electrons in a diagram to exemplify this
property and explain what it means.
b. Explain why the bonds in the sulfite ion are stronger than single bonds, but not quite as strong as
double bonds.
7. Draw the resonance structures for the following compounds.
a. nitrate ion
b. carbonate ion
8. For each of the following molecules or ions:
i. draw the Lewis structure with the correct geometry
ii. list the molecular geometry and bond angle
iii. list the molecular polarity
iv. list the hybridization
v. list the number of sigma and pi bonds in the molecule
vi. identify any molecule or ion with coordinate covalent bonds
a.
b.
c.
d.
e.
POCl3
NI3
NO+
PCl5
OF2
f. OCF2
g. CO