Chapter 7 WS SI
CHEM 111 Sumer 2013
SI Leader: Kristen Kelly
Key Terms:
Covalent bond
Bond length
Bond Dissociation Energy
Polar Covalent Bond
Non-polar Covalent
Ionic Bond
Valance Number
Formal Charge
Electronegativity
Lewis Dot
Lone Pair
Bonding Pair
Single Bond
Double Bond
Triple Bond
Coordinate Covalent Bond
Resonance Hybrid
Resonance Structure
MOT
VBT
Bond order
1. During the formation of a covalent bond between two atoms, the nuclei of both atoms ________ one another and the
electrons of both atoms _______ one another due to the increase in electrostatic interactions and the similarity in charge.
Yet, in this covalent bond the nuclei are _________ to the electrons.
2. In order for a covalent bond to form, the ___________________ forces must over power the ___________ forces. In order for this to
occur, both atoms must be a the _______ distance or _________ __________.
3. The amount of energy released when bonds form is referred to as the _________________________________.
4. Fill in the table by comparing both ionic solid and covalent compounds
Property
Ionic
Covalent
Melting Point
Appearance
Boiling Point
5. Define electronegativity: _______________________________________________________________________________________________________________.
6. For the following molecule identify if the bond is non-polar covalent, polar covalent, or ionic.
a.
NaCl
b.
O2
c.
HCl
d.
CBr4
7. For the following molecule identify if the bond is non-polar covalent, polar covalent, or ionic. Draw out dipole forces in
order to assess the polarity.
a.
8. The electronegative difference between the bonds in CCl3H is 0.5. Is this bond non-polar covalent, ionic, or polar covalent?
How about NaCl, which has a difference in electronegativity of 2.1?
9. Arrange a single, double, and triple bond from strongest to weakest and longest to shortest.
Chapter 7 WS SI
CHEM 111 Sumer 2013
SI Leader: Kristen Kelly
10. Fill in the following table:
Group
Element
1A
Li
2A
Be
3A
B
4A
C
5A
N
6A
O
7A
F
8A
Ne
Valance
Lewis Dot
Bond Cap.
Bond
11. There are two molecules with the formula, C2H6O. They are isomers. Draw down isomers.
12. Why do elements below the third period violate the octet rule? ____________________________________________________________________
13. Draw the electron dot structure for O2- and NH4+
14. Draw the following molecules:
a.
NH3
e.
N2H4
b.
CH2O
f.
XeF4
c.
C 2H 6
g.
PCl5
d.
C 2H 2
h.
SbCl52-
15. Draw the two Lewis Dot Structures for ClO2-. Use formal charge to assess which is the better lewis structure. For the better
lewis structure draw its resonance structure. On one of the resonance structures, indicate the hybridization of each atom.
16. Draw CN- and indicate the FC for each atom, hybridization, shape of the molecule, and bond angle.
Chapter 7 WS SI
CHEM 111 Sumer 2013
SI Leader: Kristen Kelly
17. Write the bond angle associated with the following hybirdizations:
a.
sp
d.
sp3d
b.
sp2
e.
sp3d2
c.
sp3
18. Identify the geometry and hybridization of central atoms of the following molecules (a-h) from problem #14.
a.
e.
b.
f.
c.
g.
d.
h.
19. Explain the difference between valance bond theory and molecular orbital theory. What are some assumptions that go
into the valance bond theory?
20. How does one find the bond order?