Unit 4
Bonding: Ionic, Metallic and Covalent
Chemistry Assignments and Objectives
EQ: How does chemical bonding make life possible?
Lesson 1 – Learning Targets
1. Describe a chemical bond as a force that holds two atoms together.
2. Explain the difference between a cation and an anion.
3. Know the physical properties of ionic compounds: electrolytes in solution, high melting
points, high boiling points, hard, rigid and brittle.
4. Describe a crystal lattice.
5. Write formulas for ionic compounds and polyatomic ions.
6. Name ionic compounds and polyatomic ions.
7. Memorize polyatomic ions in packet.
Lesson 1 - Homework
1. What is an ionic bond and how does it form?
2. List the physical properties associated with an ionic bond.
3. Write the correct formula for the ionic compound composed of the following pairs of ions.
a. Potassium and iodide
b. Magnesium and chloride
c. Aluminum and bromide
d. Cesium and nitride
e. Barium and sulfide
f. Sodium and nitrate
g. Calcium and chlorate
h. Aluminum and carbonate
i. Potassium and chromate
j. Magnesium and carbonate
4. Name the following compounds
a. NaBr
b. CaCl2
c. KOH
d. Cu(NO3)2
e. Ag2CrO4
Lesson 2 – Learning Targets
1. Describe a metallic bond.
2. Explain the physical properties of metals in terms of metallic bonds.
3. Define an alloy as a mixture of metals.
Lesson 2 - Homework
1. What is a metallic bond?
2. What is an alloy?
3. Describe the properties of metals.
Lesson 3 – Learning Targets
1.
2.
3.
4.
Apply the octet rule to atoms that bond covalently.
Explain the formation of single, double and triple bonds.
Name molecular formulas.
List the steps used in drawing Lewis structures and be able to draw structures from
formulas
5. Write molecular formulas from their names.
6. Name binary acids and oxyacids.
Lesson 3 Homework
1. Name the following binary covalent compounds
a. CCl4
b. As2O3
c. CO
d. SO2
e. NF3
f. NH3
g. CH4
2. Write the molecular formula for each of the following compounds.
a. Disulfur trioxide
b. Iodic acid
c. Dinitrogen monoxide
d. Hydrofluoric acid
e. Phosphorus pentachloride
f. Dinitrogen trioxide
g. Hydrochloric acid
h. Chloric acid
i. Sulfuric acid
j. Sulfurous acid
3.What is the difference between a binary acid and an oxyacid?
4. Name the following acids, assuming that each compound is dissolved in water.
a. HI
b.
c.
d.
e.
HClO3
HClO2
H2SO4
H2S
Lesson 4 – Learning Targets
1.
2.
3.
4.
5.
Explain why boron only forms three covalent bonds.
Discuss the VSEPR bonding theory (Valence Shell Electron Pair Repulsion.)
Know the five basic shapes of molecules. (Bent and pyramidal are caused by lone pairs.)
Describe how electronegativity is used to determine bond type.
Compare and contrast polar and nonpolar covalent bonds AND polar and nonpolar
molecules.
6. Know the properties of covalent molecules. (Opposite of ionic compounds.)
Lesson 4 - Homework
1. Draw a Lewis Structure for each of the following.
a. NF3
b. CS2
c. BH3
2. Determine/draw the molecular geometry for the following. Determine if the compound is
polar or non-polar.
a. BF3
b. OCl2
c. CF4
d. SCl2
e. NH2Cl
f. CO2
g. CF2Cl2
h. H2O
3. Why is the CF4 molecule non polar even though it contains polar bonds?
4. Rank the following bonds according to increasing polarity.
C—H
N—H
Si—H
O—H
Cl—H
Unit 4 Review
Lewis Dot Structure Drawing Practice
For each molecule, draw the Lewis dot diagram:
1.
2.
3.
4.
CO2
O2
CH4
H2O
7. BF3
8. H2
9. NH3
10. HCl
5. SF4
6. N2
11. BeCl2
12. CF4
Ionic Compounds Practice
1. Give the electron dot diagram for the following elements.
a. Carbon
b. fluorine
c. hydrogen
d. sodium
2. Give names for the following formula units.
a. BaCl2
e. NaF
b. FeI3
f. Zn(OH)2
c. CaCO3
g. Li3PO4
d. Cu(ClO2)2
h. NiCl2
3. Give the formula units for the following names.
a. Iron(II) Sulfate
e. Aluminum Nitrate
b. Lead(III) Oxide
f. Magnesium Phosphide
c. Potassium Bicarbonate
g. Calcium Fluoride
d. Beryllium Nitrite
h. Manganese (IV) Bromide
Compound Names and Formulas
For the list on the left, name the compound. For the list on the right, give the chemical formula
that corresponds to the name.
Give Name
Write Formula
1)
NaF
13) potassium fluoride
2)
K2CO3
14) ammonium sulfate
3)
MgCl2
15) magnesium iodide
4)
Be(OH)2
16) copper (II) sulfite
5)
SrS
17) aluminum phosphate
6)
Cu2S
18) lead (II) nitrite
7)
ZnI2
19) cobalt (II) selenide
8)
Ca3(PO4)2
20) silver cyanide
9)
NH4I
21) copper (II) bicarbonate
10)
Mn(NO3)3
22) iron (II) oxide
11)
FePO4
23)
lithium cyanide
12)
CoCO3
24)
lead (IV) sulfite
Covalent Compounds Practice
1. Give names for the following molecules.
a. NCl3
b. SO2
c. HCl
d. OF2
e. CO
2. Give the formulas for the following names.
a. Phosphorous Triiodide
b. Carbon tetrachloride
c. Sulfuric Acid
d. Dinitrogen Pentaoxide
e. Carbon dioxide
Binary Compounds of Two Nonmetals (Covalent Naming)
Write the correct name for:
1) As4O10
2) BrO3
3) BN
4) N2O3
5) NI3
6) SF6
7) ClO2
8) PCl3
9) CO
10) PCl5
11) P2O5
12) S2Cl2
13) SO3
14) P4O10
Write the correct formula for:
1) chlorine monoxide
2) oxygen difluoride
3) boron monophosphide
4) dinitrogen monoxide
5) diphosphorous pentoxide
6) sulfur dioxide
7) disulfur dichloride
8) chlorine monoxide
9) dinitrogen pentasulfide
10) sulfur hexafluoride
Ionic and Covalent Naming Practice
For each of the following questions, determine whether the compound is ionic or covalent and
then name it appropriately.
1)
Na2CO3
2)
P4O10
3)
N2O5
4)
FeSO4
5)
SiO2
6)
FeCl3
7)
CoBr2
8)
B2H4
9)
CO
10)
PCl3
Naming Acids Practice
1. H2SO3
8. H3PO4
15. H2CO3
2. HClO3
9. HNO3
16. HC2H3O2
3. HCl
10. HNO2
17. HF
4. HClO
11. HClO2
18. H2Se
5. HI
12. HBr
19. H2CrO4
6. HBrO3
13. HClO4
20. H3P
7. H2SO4
14. H2S
21. H2Cr2O7