COVALENT
BONDING REVIEW
1. How many electrons are shared by a single
bond?
2. What type of elements form covalent bonds?
3. The type of covalent bonding in which two
atoms share their electrons evenly is described as _____________.
4. How many electrons are shared by a double
bond?
5. The type of covalent bonding in which two
atoms share electrons unevenly resulting in slightly positive and slightly
negative regions of the molecule is called _______________.
6. A term that describes an atom's degree of
pull for shared electrons is _______________.
7. A group of covalently bonded atoms possessing
a positive or negative charge is called a(n)
_______________.
------------------------------------------------------------------------------------------------------------------------
Choose
from these*: O2 Cl2 H2O CO2 CH4 NH3 N2
8. has a tetrahedral
shape
9. has a triple
covalent bond
10. two unshared
electron pairs on the central atom results in a polar molecule with a bent
shape
11. no unshared electron
pairs on the central atom results in a triatomic
linear molecule
12. one unshared
electron pair on the central atom results in a trigonal
pyramid shape
13. diatomic linear
molecule is nonpolar with a single bond
*
one of these choices is not used
IONIC
BONDING REVIEW
Part 1
- Complete each of the following sentences by filling in the appropriate word
or phrase from the list below.
negative
noble
gas
octet
anion
positive
electrons
ions
cation
electron configuration
1.
An ionic bond is an attraction between oppositely charged ____________________.
2.
Anions have a ____________________ charge.
3.
An atom becomes an ion by losing or gaining ____________________.
4.
The ____________________ rule states that atoms tend to gain, lose, or share
electrons in order to acquire a
full set of valence electrons.
5.
When sodium and chlorine form an ionic bond, both ions acquire the electron
configuration of a(n)
____________________.
Part 2
- If the statement is true, write "truue". If it is false,
change the underlined word or words to make it true. Write your answer on
the line.
____________________
6.
Calcium becomes a cation by gaining two
electrons.
____________________
7.
A cation has a positive charge.
____________________
8.
A sodium ion is smaller in size than a sodium atom.
____________________
9.
The Lewis dot diagram for chlorine, a group 17 element, has six dots
around it.
____________________
10.
An aluminum ion has a charge of +3 because it gains three electrons.
Part 3 -
How many electrons will the following elements gain or lose in forming an ion?
11. calcium 12.
aluminum
13. fluorine 14.
oxygen
Part 4 -
What will be the formula of the ion formed when the following elements gain or
lose valence electrons and attain noble gas configurations?
15. sulfur
16. fluorine
17. sodium
18. barium
Part 5 -
Write the electron configuration for the following ions:
19.
Ca+2 20. Al+3
21. F-1 22. O-2
23. S-2 24. Na+1
25. Ba+2 26. K+1
27. N-3
LEWIS
STRUCTURES 1
1.
SiF4 Polarity: |
2.
BF3
|
3.
NH3 Polarity: |
4.
H2O Polarity: |
5.
CHBr3 Polarity: |
6.
HI Polarity: |
7.
SO3 Polarity: |
8.
AsCl3 Polarity: |
9.
H2S Polarity: |
10.
SeH2 Polarity: |
11.
PO4-3 Polarity: |
12.
NO2-1 Polarity: |
13.
ClO3-1 Polarity: |
14.
HCN Polarity: |
15.
PI3 Polarity: |
LEWIS
STRUCTURES 2
1.
OF2 Polarity: |
2.
GeI4 Polarity: |
3.
SCl2 Polarity: |
4.
SeO2 Polarity: |
5.
SO3 Polarity: |
6.
NH4+1 Polarity: |
7.
ONCl Polarity: |
8.
CO2 Polarity: |
9.
SO4-2 Polarity: |
10.
ICl Polarity: |
11.
CH2Cl2 Polarity: |
12.
H3O+1 Polarity: |
13.
N2 Polarity: |
14.
ClO-1 Polarity: |
15.
CH2O Polarity: |
Unit 6
Review Worksheet
1. Individual atoms of elements are ( more / less ) stable than when they are
combined with
other elements.
2. What is the difference between ionic and
covalent bonding?
3. What is the cut-off number for the difference
in electronegativity to determine whether a
bond is ionic or covalent?
have 8 electrons?
18. Which type of compound has low melting points?
(D)
class, and shape of the molecule. Also tell the type(s) of IM forces that occur
within
a sample of that compound.
(F) SeS2