Name: ___________________________________ Period 1 2 3 4 5 6 7
1.
Complete the following:
 Covalent bonds exist between two or more ______- _______________.
 According to the octet rule, all elements must have ___ ___________ in their outermost energy level, with the exception of _________________ that only needs 2.
 In a covalent bond, the electrons are ________________________.
 What is the ending for all binary compounds? ____________________
2.
What are the prefixes used when naming covalent compounds?
1 _________
2 _________
3 _________
4 _________
5 _________
6 _________
7 _________
8 _________
9 _________
10 _________
On the following periodic table,
Write the number of valence electrons for each group in blue.
Write the charge (oxidation #) for each group in red.

3.
Draw the following structural formula for each compound and use your drawings to fill in the blanks on the right. a.
CH
4
Center Atom: ____________________
Shape: _________________________ b.
SiO
2
Center Atom: ____________________ c.
SO
3
Shape: _________________________
Center Atom: ____________________
Shape: _________________________ d.
H
2
O Center Atom: ______________________
Shape: ___________________________
4.
Match the chemical formula with the correct name.
S
2
Cl
SiF
6
P
4
O
10
As
2
S
5
P
3
Cl
2
S
5
I
3 triphosphorus dichloride disulfur monochloride pentasulfur triiodide silicon hexafluoride tetraphosphorus decaoxide diarsenic pentasulfide

5.
Identify the following statements as true or false.
_____ In a Lewis structure, hydrogen is always the central atom.
_____ In a Lewis structure, carbon must have 8 electrons.
_____ There are never exceptions to the octet rule.
_____ Carbon is always the central atom in a molecule of CO
2
.
_____ A silicon atom has 8 valence electrons.
_____ Oxygen wants to gain 2 electrons to become stable.
_____ An atom of Oxygen has 6 electrons and therefore has a full octet.
_____ A molecule that has a central atom with 4 single bonds has a shape of trigonal planar.
_____ A single bond contains 2 electrons.
6.
Draw the Lewis Dot Structure for the following compounds: a.
Boron Trihydride b.
Carbon tetrachloride c.
Dihydrogen monoxide
7 Which of the following are metals? Circle the metals and put a star by the metals that could have multiple charges. These "starred" metals are called ___________ _____. a. lithium b. lead c. fluorine d. calcium e. oxygen f. barium g. chromium h. gold
8 For each element use their oxidation number to determine if they will lose or gain electrons and write how many.
A
Al
B
Br
C
Sr
D
N

9 Write the formula of the compound formed by the following:
Lithium
Aluminum
Oxygen
Ex: Li
2
O
Sulfur Bromine
Potassium
Chromium (II)
Phosporous
10 Define: metallic bond ionic bond covalent bond
11 When writing a formula for an ionic compound, does the cation or anion always come first?
12 When an ionic compound forms, what will the overall charge be?
13 If magnesium and nitrogen form a compound how many Mg ions will be present: _______
How many N ions will be present: ___________

14 What is the oxidation number for each of the following?
Element Oxidation number
Al
O
I
Na
K
Ba
N
15 What must you use when you name ionic compounds that have a transition metal?
16 What must you use when writing the formula of an ionic compound that has more than one polyatomic ion? _________________Do you need these if there is only one? _____
17 A cation is a ____________ ion.
18 An anion is a ___________ ion.
19 Metals usually form (cations, anions).
20 Non-metals usually form (cations, anions).
Write the FORMULA for the following IONIC compounds:
21) potassium hydroxide __________ 27) beryllium phosphate ____________
22) copper (II) sulfide __________
23) Potassium bromide ___________
28) chromium (III) carbonate _______
29) calcium bromide ______________
24) lead (II) nitrate _______________
25) beryllium oxide _______________
26) sodium iodide ________________
30) cobalt (III) sulfite ______________
31) aluminum phosphide ___________
32) ammonium nitride ____________

Write the NAME for the following IONIC compounds:
33) MgS _______________________ 39) NH
4
OH ___________________
34) CaSO
4
______________________
35) SrCl
2
________________________
36) K
2
(CO
3
) ____________________
40) Ag
2
O_______________________
41) Mn(OH)
42) (NH
4
)
2
2
_____________________
CO
3
____________________
37) PbCl
4
_______________________
38) SnBr
2
_______________________
43) Al
2
O
3
_______________________
44) RbF _________________________
For this test I need to be able to do the following:
 Know the difference between ionic, covalent and metallic compounds
 what elements make up each compound
 how these elements are held together
 their properties and characteristics
 Know how to name both covalent and ionic compounds (with transition metals and polyatomic ions too)
 Know how to write the formulas for covalent and ionic compounds (with transition metals and polyatomic ions too)
 Know how to draw Lewis Dot Structures for Covalent Compounds (with all elements having a satisfied octet)
 Know how to determine the shape of Lewis Dot Structures for Covalent Compounds.
(linear, bent, trigonal planar, tetrahedral)