Bonding Review

Chem I | Chem II AP
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1)
Distinquish between the electron dot notation of ionic, polar covalent and nonpolar covalent compounds. Give an example of each.
Ionic
Polar Covalent
Nonpolar Covalent
Full Charges
No Lines
Partial Charges
Lines between molecules
No Charges
Lines between molecules
2)
List three characteristics of ionic compounds; list three for covalent compounds
3)
What regions of the periodic table usually combine to form ionic compounds?
covalent compounds?
4)
Distinguish between nonpolar covalent bonding and polar covalent bonding.
5)
What region of the periodic table has the elements with the highest electronegativity values?
the lowest values?
6)
If two elements have a great difference in electronegativity values, what type of bonding takes place?
Why?
7)
What is the basic idea for VSEPR theory in determining molecular shape?
8)
Determine the group that element X must be in:
a)
Given: XCl4 (Cl = chlorine)
b)
Given: X2O (O = oxygen)
c)
Given: XO (O = oxygen)
d)
Given: XCl3 (Cl = chlorine)
9)
What is the basic shape associated with:
a)
four pairs of electrons on the central atom?
b)
sp2 hybridization?
c)
bond angle of 109.5°?
d)
three pairs on the central atom?
e)
sp hybridization?
f)
120°?
g)
two pairs on the central atom?
10)
Which type of hybridization is associated with:
a)
three pairs of electrons on the central atom?
b)
Bond pairs = 2; Lone pair = 1?
c)
tetrahedrally shaped molecule?
d)
120° bond angle?
e)
linear molecule?
f)
four pairs of electrons on the central atom?
11)
Complete. Determine type of hybridization present in each molecule.
a)
BCl3
Hybridization =
ground state for B
b)
PCl3
Hybridization =
ground state for P
12)
Complete:
Compound
Type of Bonding
Electron Dot
Shape
Bond Angle
Hybridization
Dipole moment?
CsF
Ionic
crystal
none
none
none
Cl2
SiBr4
O2
H2S
BaO
GaBr3
CCl2
SrF2
BeI2
AsCl3