Chapter 7, 8 and 9 Study Guide
Ionic Bonding  Covalent Bonding  Chemical Names and Formulas
You do not need to glue this study guide into your notebook. However, all
answers should go in you science notebook. DO NOT answer questions directly
on any of the pages or you will not receive credit (including multiple choice
questions).
Vocabulary:







Valence Electrons
Electron Dot
Diagram
Octet Rule
Ionic Compounds
Ionic Bonds
Electrostatic
Forces
Covalent Bond







Molecule
Single/Double/
Triple Bond
Monatomic Ion
Polyatomic Ion
Electronegativity
Polar covalent
bond
Nonpolar covalent
bond





London Dispersion
Force/Van der
Waals
Dipole-dipole
Hydrogen Bond
Intermolecular
Forces
Network solids
CA State Standards:
How you should study:





Problem Sets and worksheets
o Naming Polyatomic Ions
o Lewis Dot Structures
o Electronegativity Worksheets
o Naming Compounds Worksheets
Memorize all of the Polyatomic Ions given to you (see Quizlet posted online
for flashcards)
Attached Pages of questions (many of these will appear on exam!)
Standardized Test Prep Questions (attached)
Past Exams
Study Guide Part 1
Chapter 7: Ionic Bonding
1. Write the symbol of the ion formed when:
a. A sulfur atom gains two electrons
b. A aluminum atom looses three electrons
2. Atoms of which elements tend to gain electrons? Atoms of which elements
tend to lose electrons?
3. How do cations form?
4. How do anions form?
5. How many valence electrons are in each atom?
a. Potassium
c. Carbon
b. Magnesium
d. Oxygen
6. Draw the electron dot structure for each element in Question 5.
7. How many electrons will each element gain or lose in forming an ion?
a. Calcium (Ca)
c. Fluorine (F)
b. Aluminum (Al)
d. Oxygen (O)
8. Write the correct chemical formula and name for the compounds formed
from each pair of ions.
a. Potassium and Sulfur
c. Calcium and oxygen
b. Sodium and Oxygen
d. Aluminum and Nitrogen
9. Write the formulas for each compound.
a. Barium chloride
c. Lithium oxide
b. Magnesium oxide
d. Calcium fluoride
10. Which pairs of elements are likely to form ionic compounds?
1. Cl, Br
2. K, He
3. Li, Cl
4. I, Na
11. Hypothesize as to why ionic compounds conduct electric current when they
are melted or dissolved in water?
12. Describe what is meant by ductile and malleable. (Vocab words from
previous chapter)
Study Guide Part 2
Chapter 8: Covalent Bonding
1. Draw the electron dot structures for each atom:
a. Chlorine
b. Bromine
c. Iodine
2. The following molecules have single covalent bonds. Draw an electron dot
structure for each.
a. H2O2
c. PH3
b. PCl3
d. ClF
e. H2S
3. Draw the electron dot structure of:
a. Hydroxide ion.
b. The polyatomic boron tetrafluroide anion (BF4-)
c. Sulfate (sulfur is the central atom)
d. Carbonate (carbon is the central atom)
e. The bicarbonate ion. Carbon is the central atom, and hydrogen is
attached to oxygen in this polyatomic anion.
4. Draw the electron dot structure for each molecule. Identify polar covalent
bonds by assigning slightly positive (δ+) and slightly negative (δ-) symbols to
the appropriate atoms within the molecule.
a. HOOH
c. HBr
b. BrCl
d. H2O
5. Name the intermolecular forces at work in question 4.
6. The bonds between the following pairs of the elements are covalent. Arrange
them according to polarity, listing the most polar bond first. Use the periodic
table from the electronegativity worksheet if needed.
a. H—Cl
c. H—F
e. H—H
b. H—C
d. H—O
f. S—Cl
7. What is a hydrogen bond?
8. Although the relative positions of the atoms are correct in each of these
molecule there are one or more incorrect bonds in each of the electron dot
structures. Identify the incorrect bonds. Draw the correct electron do
structures for each molecule. (::: is a triple bond, : is a lone pair of electrons)
a. H=C=C=H
c. :I:::Cl
b. :F—O—H
d. H—N:::N—H
9. Why do compounds with strong intermolecular attractive forces have higher
boiling points than compounds with weak intermolecular attractive forces?
Study Guide Part 3
Chapter 9: Chemical names and formulas
1. Write the formulas for compounds formed from these pairs of ions. Then
name them.
a. Ba2+, S2e. NH4+, SO322+
3b. Ca , N
f. Calcium ion, phosphate
+
2c. Li , O
ion
d. Cu2+, I- (Copper makes a
2+ and 1+ ion)
2. Write the formulas for these IONIC compounds:
a. Sodium iodide
h. Strontium oxide
b. Potassium sulfide
i. Lithium sulfate
c. Calcium iodide
j. Chromium (III) nitrite
d. Tin (II) chloride
k. Sodium chlorate
e. Beryllium chloride
l. Magnesium bicarbonate
f. Cesium sulfide
m. Calcium acetate
g. Sodium iodide
3. Identify any incorrect formulas. Explain your answer.
a. Mg2(SO4)3
c. Rb3As
b. BeCl3
d. NaF
4. Write the names of these molecular (covalent) compounds.
a. NCl3
e. N2H2
b. BCl3
f. N2O3
c. NI3
g. CS2
d. SO3
h. Cl2O7
5. Write the formulas for these molecular compounds.
a. Phosphorus
e. Carbon tetrabromide
pentachloride
f. Diphosphorus trioxide
b. Chlorine trifluoride
g. Boron Trichloride
c. Iodine dioxide
h. Dinitrogen tetrahydride
d. Nitrogen dioxide
6. What prefix indicates each of the following numbers of atoms in the formula
of a molecular compound?
a. 3
d. 5
b. 1
e. 4
c. 2