Name:___________________________Period:_________
Date:_____________________
Lewis Structures WS
Draw the correct Lewis structure for the following compounds. Use dots to represent
unshared electron pairs and dashes to represent bonds.
Remember the following rules:
 Group 14 will have 4 bonds
 Group 15 will have 3 bonds
 Group 16 will have 2 bonds
 Group 17 will form 1 bond
The center atom in polyatomic ions can form up to four bonds regardless of what group
it is in.
1) CF4
2) ONCl
3) F2
4) HCN
5) HNO
6) H2CO
7) PCl3
8) SPF
Chapter 6 (1) | P a g e
Name:___________________________Period:_________
Date:_____________________
9) CCl4
10) OI2
11) H2
12) SiO2
13) COF2
14) CPBr
15) SI2
16) NOH
17) SiHP
Chapter 6 (2) | P a g e
Name:___________________________Period:_________
Date:_____________________
Molecular Geometry WS
Determine the geometry of each molecule. For each molecule draw the Lewis structure
first. Once you have drawn the structure use the chart in your notes to determine the
shape of the molecule and polarity.
Possible shapes are:





linear
bent
trigonal planar
tetrahedral
1) CCl4
2) N2
Geometry:
Polar or non:
Geometry:
Polar or non:
3) PH3
4) H2O
Geometry:
Polar or non:
Geometry:
Polar or non:
5) NH3
6) ONCl
Geometry:
Polar or non:
Geometry:
Polar or non:
tetrahedral with a pyramidal base.
Chapter 6 (3) | P a g e
Name:___________________________Period:_________
Date:_____________________
7) SiO2
8) Br2
Geometry:
Polar or non:
Geometry:
Polar or non:
9) NF3
10) OCl2
Geometry:
Polar or non:
Geometry:
Polar or non:
11) CH2O
12) NH2Cl
Geometry:
Polar or non:
Geometry:
Polar or non:
13) CCl2F2
14) CPBr
Geometry:
Polar or non:
Geometry:
Polar or non:
Chapter 6 (4) | P a g e
Name:___________________________Period:_________
Date:_____________________
Ch. 6 Review WS
Multiple choice
1) An ionic bond involves the attraction between two different ions. The names of
these ions are cations and _______________ .
a. anions
c. nonmetals
b. metals
d. formula units
2) A polar covalent bond forms because the two atoms are different in their
_______.
a. density
c. electronegativity
b. state of matter
d. polarity
3) Bond form so that the two atoms are at __________________.
a. minimum energy
c. maximum distance
b. maximum energy
d. minimum distance
4) Which atom can form three covalent bonds.
a. fluorine
b. nitrogen
c. oxygen
d. neon
5) Multiple covalent bonds may form in molecules that contain carbon, nitrogen, or
_________.
a. chlorine
c. oxygen
b. hydrogen
d. helium
6) The principle that states that atoms tend to form compounds in which each atom
has eight valence electrons is called the______.
a. rule of eights
c. Avagodro principle
b. configuration rule
d. octet rule
7) An attraction between two molecules is called a(n) ______.
a. ionic bond
c. intermolecular force
b. covalent bond
d. bonding force
8) The fact that ionic compounds form crystals indicate that ______.
a. energy is lower in a crystal
c. the bond is stronger in a
b. energy is higher in a
crystal
crystal
d. none of the above
Chapter 6 (5) | P a g e
Name:___________________________Period:_________
Date:_____________________
Fill in the blank write the correct term or terms in the space provided
1) A covalent bond in which the bonded atoms have an unequal attraction for the
shared electrons is called a(n) ______________________.
2) H2, O2, N2 are all examples of ______________________.
3) Ionic bonds form between the following two types of elements, ___________and
____________________.
4) A neutral group of atoms held together by covalent bonds is called a(n)
__________________.
5) Atoms form bonds so that they will have ______ valence electrons.
6) Covalent bonds form between two _____________________.
7) A charged group of covalently bonded atoms is called a(n)
____________________.
8) A covalent bond between two atoms produced by sharing two pairs of electrons
is called a(n) _____________________.
9) The simplest collection of atoms from which the formula of an ionic compound
can be established is called a(n) _________________________.
10) Chemical bonds form so that _____________________ is at a minimum.
11) A chemical bond that results from the attraction between metal atoms and the
surrounding sea of electrons is called a(n) ________________________.
12) In metallic bonding the electrons are _____________________ between all
atoms.
13) The type of bonding that occurs between the hydrogen of one molecule and an
electronegative atom of another molecule is called
_________________________.
14) An atom that has eight valence electrons is said to have an
___________________.
15) The attraction between two polar molecules is called a
______________________ force.
16) The only attractive forces found between all atoms are
__________________________________.
Chapter 6 (6) | P a g e
Name:___________________________Period:_________
Date:_____________________
Draw the Lewis Structures and complete the table.
Number Formula
1
CH2F2
2
F2
3
HCN
4
HNO
5
PCl3
6
POF
7
OI2
8
H2
9
COF2
10
CH2Cl2
Shape
Polar or Non
Chapter 6 (7) | P a g e
Name:___________________________Period:_________
Date:_____________________
For the following molecules draw Lewis structures, and then determine the shape
and polarity of the molecules.
17) CO2
18) CH4
19) OCl2
20) N2
21) HCl
22) CI4
23) H2O
Chapter 6 (8) | P a g e
Name:___________________________Period:_________
Date:_____________________
Name or give the formulas for the following compounds as appropriate
24) Arsenic Pentabromide
_____________________
25) Sodium phosphate
_____________________
26) Iron (II) peroxide
_____________________
27) Diphosphorous Pentoxide
_____________________
28) NI3
_____________________
29) SiO2
_____________________
30) CdSO2
_____________________
31) FrCl
_____________________
Moles
32) How many moles are in 1600 cg of Ca(OH)2?
Moles: ____________
33) How many molecules are in 7.21 moles of SO2?
Molecules: _____________________
34) How many grams are in 8.1 x 1023 atoms of Sr?
Grams: ____________
Chapter 6 (9) | P a g e