Chemistry – Bonding Unit Review
Please answer the following questions in preparation for your unit test. Your unit test will be on Friday, November
19th. An answer key will be posted online – please check your work!
Naming Review:
1. Determine if the compound is ionic (metal + nonmetal) or covalent (2 nonmetals).
2. If it is ionic: Determine if the metal is an s-block metal, aluminum, zinc or silver
If it is: same name as element
If it is not: same name as element PLUS roman numeral
Determine if the nonmetal is a monoatomic or diatomic
If monoatomic – root name of nonmetal PLUS –ide ending
If polyatomic – look to the polyatomic ions your memorized
3. If it is covalent: Use the prefix to represent the number of atoms for each element
Exceptions: If the first element has only one, the mono is dropped
If the element starts with a vowel, drop the a- or o- from the prefix
The first element takes the name of the element, the second element takes the root name of the
element PLUS –ide ending.
Practice:
Name the following compounds:
1. CS2 carbon disulfide
2. PBr3 phosphorus tribromide
4. FeI3 iron (III) iodide
5. Co2S3 cobalt (III) suflide
7. NaCl sodium chloride
8. K2O potassium oxide
10. NH4OH
ammonium hydroxide
11. SrN2
12. CaCO3
calcium carbonate
13. Al2(SO4)3
14. HNO3
hydrogen nitrate
15. NiO
16. Cl2O
dichlorine monoxide
3. IF5 iodine pentafluoride
6. PbO lead (II) oxide
9. MgO magnesium oxide
strontium nitride
aluminum sulfate
nickel (II) oxide
Write the formula for the following compounds:
1. nitrogen monoxide NO
2. sulfur dioxide
SO2
4. copper (I) nitride Cu3N
5. calcium fluoride
CaF2
7. zinc phosphide
Zn3P2
8. sodium chromate Na2CrO4
10. ammonium chloride NH4Cl
11. strontium hydroxide Sr(OH)2
13. dinitrogen pentoxide N2O5
14. iodine monochloride ICl
16. zinc bromide
ZnBr2
3. iron (II) chloride FeCl2
6. magnesium sulfide MgS
9. potassium bicarbonate KHCO3
12. lead (IV) oxide
PbO2
15. gold (II) chloride AgCl2
Lewis Dot Diagram Review:
1. Draw the Lewis Dot Structure for each individual atom.
2. Determine which unpaired electrons will participate in bonding.
3. Replace those electrons with lines to represent the bond
4. Double check that each atom has 8 valence electrons (2 if it is hydrogen) and that total number of valence
electrons is equal to the number of valence electrons for all of the individual atoms.
Please come to room N205 to see the answers to this section
Practice:
1. Br
5. Na+1
9. CF2Cl2
13. H2O2
2. N
6. HBr
10. C2H2
14. CH4O
3. Mg
7. BF3
11. HCOOH
15. NH3
4. Cl-1
8. CO2
12. SH2
16. CH3NH2
Shape Review:
Predict the shape using the Lewis Dot Diagram and the following chart:
# of atoms bonded to the central atom Unbonded valence electrons on the central
Shape Name
atom?
No central atom
No
Linear
2
No
Linear
3
No
Trigonal planar
4
No
Tetrahedral
3
Yes
Pyramidal
2
Yes
Bent or angular
Practice:
1. HBr linear
2. BF3 trigonal planar
3. CO2 linear
4. CF2Cl2
tetrahedral 5. C2H2 linear
6. HCOOH
trigonal planar around carbon, bent around oxygen
7. SH2 bent
8. H2O2
bent
9. CH4Otetrahedral around carbon, bent around hydrogen
1o. NH3pryramidal
11. CH3NH2 tetrahedral around carbon, pyramidal around hydrogen
12. H2Obent
Polarity Review:
Determine if the electrons are evenly distributed about the central atom.
If the electrons are evenly distributed about the central atom, compound is non-polar.
If the electrons are NOT evenly distributed about the central atom, compound is polar.
Practice:
1. HBr P
5. C2H2 NP
9. CH4O
P
2. BF3 P
6. HCOOH
10. NH3
P
P
3. CO2 NP
7. SH2 P
11. CH3NH2
P
4. CF2Cl2
8. H2O2
12. H2O
P
P
P
Types of Intermolecular Forces
What is the strongest intermolecular force present for each of the following compounds?
1.
3.
5.
7.
9.
water hydrogen bonding
ammonia (NH3)
hydrogen bonding
phosphorus trichloride
dipole-dipole
ethane (C2H6)
dispersion foces
methanol (CH3OH) dipole-dipole
2. carbon tetrachloride
dispersion forces
4. carbon dioxide
dispersion forces
6. nitrogen
dispersion forces
8. acetone (CH3COCH3) dipole-dipole
10. borane (BH3) dispersion forces
Characteristics of Ionic and Covalent Bonds
Complete the following chart using your observations from the “What bond am I?” lab.
Characteristic
Ionic Compounds
Covalent Compounds
Transfer
of
e
Sharing
of eHow does the bond form?
Metal + nonmetal
Nonmetals only
What types of elements are involved?
How do their melting points compare?
Do they conduct electricity?
Are they volatile? (Do they have an odor?)
Higher
Lower
Only when dissolved in
water
No
No
Yes
Place the following compounds in order from highest to lowest melting point:
H2O
CH4
MgO CH3Cl
Then, explain, using your knowledge of intermolecular and intramolecular forces, why you placed them in that order.
MgO
H2O
CH3Cl
CH4