CHEMISTRY 11
Mr. Bellman
Ch 7/8 Bonding/Molecular Shapes/Polarity
TEST REVIEW
( 16 )
NAME____________________
Date______________Bk_____
CHAPTER 7 BONDING/POLARITY
1. Define ionic bond.
2. What kind of ions to metals and non-metals tend to form?
3. Define cation.
4. Define anion.
5. State some properties of ionic and covalent compounds.
6. Define octet rule.
7. Be able to do the Lewis or Dot structures for any group 1, 2, 13-18 element.
Give the dot structures of the following elements:
Group 1
2
13
14
15
16
17
18
H
O
F
Ne
f. O2
g. NF3
h. Br2
Be
B
C
N
8. Draw the Lewis Structures or electron dot formulas for the following molecules:
a. H2
b. CBr4
c. H2O
d. C2H2
e. HCN
9. For the above molecules, draw the molecules with lines to represent bonds.
10.
11.
12.
13.
14.
15.
16.
17.
Define covalent bond.
Define molecule.
Define molecular formula
Define structural formula
Define Lewis structures.
Define single covalent bond.
Define double covalent bond.
Define triple covalent bond.
18. Using the electronegativity chart, determine if the following bonds are polar covalent, nonpolar covalent or ionic. (You also need
to memorize the electronegativity difference chart: 0 – 0.4 = nonpolar covalent, 0.5 – 1.9 = polar covalent, 2.0 or greater = ionic )
a. H – H
b. H – Br
c. C – O
d. Li – F
e. N – O
f. P – S
b. SBr5
c. SBr6
g. Na – Cl
CHAPTER 8 BONDING/MOLECULAR SHAPES/POLARITY
19. Define VSEPR theory.
20. Write out the seven molecular shape names for chapter 8.
21. Determine the shapes of the molecules in Q 8 and 9.
22. Determine the structural formula and shapes for: a. BBr3
23.
24.
25.
26.
27.
Define hybrid orbital.
What is an ‘ sp ‘ orbital?
What molecular shape is it associated with?
2
What is an ‘ sp ‘ orbital?
What molecular shape is it associated with?
What is an ‘ sp3 ‘ orbital?
What molecular shapes is it associated with?
What are the 2 factors that influence bond length.
28.
29.
30.
31.
Define polarity.
Define dipole.
What two factors determine the polarity of a molecule ( or whether the molecule is polar or nonpolar) ?
For each of the following molecules:
a. Determine the shape of the molecule.
b. Determine the polarity of each bond in the molecule.
c. Determine if the molecule is polar or nonpolar.
d. Include delta plus ( δ + ) and delta minus ( δ - ) for polar molecules.
a. Cl2
i.
b. CO2
c. H2S
j.
d. NH3
e. CCl4
k.
f. BF3
g. SCl5
l.
h. SCl6
Answers to select questions:
7.
H
Be
B
C
N
O
F
Ne
8.
9.
18. a. H – H
b. H – Br
2.1 – 2.1 = 0
Nonpolar covalent
c. C – O
2.8 – 2.1 = 0.7
polar covalent
3.5 – 2.5=1.0
polar covalent
f. P – S
g. Na – Cl
2.5 – 2.1 = 0.4
Nonpolar covalent
3.0 – 0.9 = 2.1
ionic
d. Li – F
e. N – O
4.0 – 1.0 = 3.0
ionic
3.5 – 3.0 = 0.5
polar covalent
20. linear, bent, trigonal planar, trigonal pyramid, tetrahedral, trigonal bipyramid, octahedral
21. a. linear
b. tetrahedral
22. a. trigonal planar
24.
26.
27.
31.
c. bent
d. linear
e. linear
f. linear
b. trigonal bipyramid
g. trigonal pyramid
h. linear
c. octahedral
blending of s and one p orbital. Linear
25. Blending of s and 2 p orbitals. Trigonal planar
blending of s and three p orbitals. Tetrahedral, bent and trigonal pyramid.
size of atoms (bigger atoms will have longer bonds), number of bonds (single bonds longest, triple bonds shortest)
a. linear
b. linear
c. bent
d. trigonal pyramid
e. tetrahedral
3.0-3.0=0
Nonpolar covalent bond
Molecule is nonpolar
3.5-2.5=1.0
polar covalent bonds
nonpolar molecule
(arrows cancel)
2.5-2.1=0.4
nonpolar covalent bonds
slightly polar molecule
(arrows don’t cancel and
lone pair electrons )
3.0-2.1=0.9
polar covalent bonds
polar molecule
(arrows don’t cancel)
3.0-2.5=0.5
polar covalent bonds
nonpolar molecule
(arrows cancel)
f. trigonal planar
g. trigonal bipyramid
h. octahedral
i. tetrahedral
4.0-2.0=2.0
Ionic bonds
Nonpolar molecule
(even distribution of electrons)
3.0-2.5=0.5
polar covalent bonds
nonpolar molecule
(arrows cancel and even
distribution of electrons)
3.0-2.5=0.5
polar covalent bonds
nonpolar molecule
(all arrows cancel)
C-H 2.5-2.1=0.4 nonpolar cov. bond
C-F 4.0-2.5=1.5 polar covalent bond
polar molecule ( all arrows don’t
cancel, F pulls the electrons more)
j. trigonal planar
k. octahedral
l. linear
B-H 2.1-2.0=0.1 nonpolar cov. bonds
B-Cl 3.0-2.0=1.0 polar cov. bond
Polar molecule (uneven distribution of
electrons with Cl pulling more)
C-Cl 3.0-2.5=0.5 polar cov. bonds
C-F 4.0-2.5=1.5 polar cov bond
polar molecule ( uneven distribution of
electrons with F pulling more )
C-O 3.5-2.5=1.0 polar covalent bond
C-S 2.5-2.5=0 nonpolar covalent bond
polar molecule ( arrows don’t cancel as oxygen
pulls electrons more than S)