Covalent Bonding Test Review
Covalent Bonds: _____________________________________________________________________________
Two types of covalent bonds: _____________________
and _____________________________.
__________________ :Unequal sharing of electrons
because one atom is more electronegative
__________________: Equal sharing of electrons
because atoms are approximately equal in
electronegativies
Covalent bonds can be single, double or triple bonded.
______________ are the strongest bonds.
Comparing Ionic, Polar Covalent and Non-Polar Covalent
Ionic
Polar Covalent
Non-Polar Covalent
_______________________
____________________
____________________
High melting point
___________ melting point
Low melting point
___________________
Solids and liquids
Liquids and gases
No dipoles
______________________
No dipoles
Dissolves in
______________
Dissolves in
________________
Dissolve in
_________________
Lewis Structures
1.
2.
3.
4.
Determine number of ___________________________________________ for each element.
Determine central atom (____________________________________________).
Write central atom and valence electron dots.
Fill in remaining elements with their valence electron dots.
Draw Lewis Structures for the following:
H20
NH3
F2
Identify the Bond Type and Solubility
Electronegativity:_______________________________
_____________________________________________
Bond Type
Bond Type
Ionic
Polar
Ionic
Non-Polar
Polar
Polar
Cmpd
Electro Diff
Soluble / Not
Soluble
Bond Type
A ______________ difference in electronegativity’s
indicates a _____________________ of electrons and
an __________________________.
Polar
Non-Polar
Non-Polar
Non-Polar
Cmpd Two
One
BaCl
H4Sn
CS2
H2O
NO2
KCl
SiF4
HN
Si4P6
H2O
Electro Diff
Bond Type
Soluble
Yes/No
Naming
Diatomic Elements: _________, __________, ________, __________, _____________, ___________, __________
Covalent Prefixes:
1
2
3
4
5
6
7


If a compound starts with a non-metal and the
compound is binary, use the prefixes and the
anion must end in –ide.
o


o

o
o
Ex/ HCl - Hydrochloric Acid
Ex/ HNO2 - Nitrite - Nitrous Acid
If the anion ends in “ate”, change the ending to
“ic” followed by acid.
Ex: O2 - Oxygen
Ex/ HNO3 - Nitrate - Nitric Acid
Practice naming these compounds:
Practice writing these compounds:
HF
Magnesium Bromide
________________________
10
If the compound is ternary (3 elements) and
starts with hydrogen (H), it is also an
_________. If the anion ends with “ite,” change
the ending to “ous” followed by acid.
Ex: NO- nitrogen monoxide
If the compound is diatomic, use the name of
the elemental symbol
9
If the compound is binary (2 elements) and
starts with hydrogen (H), it is an ________.
Binary acids start with “hydro” and end with
“ic” followed by acid.
Ex: CCl4- Carbon Tetrchloride
Do not use the ____________ prefix if the first
element of the compound contains only one
atom.
o
8
________________________
HClO2 ________________________
Triphosphorus pentachloride ________________________
I2
Hydrobromic Acid
_________________________
K3PO4 _______________________
Fluorine
________________________
NO2
Dihydrogen Dioxide
________________________
________________________
_______________________
CaF2 ________________________
Magnesium Nitrate
________________________
HCl __________________________
Silicon Tetrafluoride
_______________________
HNO3________________________
Ammonium Oxide
_______________________
O2___________________________
Iron (III) Bromide
_______________________
NaCl__________________________
Phosphorous Acid
_______________________
Fe2S3_________________________
Magnesium Hydroxide
________________________
H2___________________________
Nitrogen Monoxide
________________________
Organic
Branch of chemistry devoted to _________________________________________.
CnH2n+2
Single bond = ________________________________________________________________________________.
Hydrocarbons:________________________________________________________________________________.
CH4
C6H14
C2H6
C7H16
C3H8
C8H18
C4H10
C9H20
C5H12
C10H22
Draw the structural formula for:
Draw the condensed formula for:
Pentane:
Ethane:
Octane:
Butane:
Draw the skeletal formula for:
Hexane:
Propane:
Density
M
• Measurement of how packed or crowed the object is
• Ratio of mass to volume
• Floats in water if density is _____________________; Sinks in water if density is
_______________________
1. If a substance has a mass of 573 g and a volume of 682 mL, will it float or sink?
D
Density 
V
Mass
Volume
2. The level of water in a graduated cylinder is 65.7 mL. After a solid object with a mass of 35.0 g is
added, the level of the water rises to 92.4 mL. What is the density of the solid object?
3. The level of water in a graduated cylinder is 142.7 mL. After a solid object with a mass of 45.0 g
is added, the level of the water rises to 192.4 mL. What is the density of the solid object?
4. What is the mass of and object that has a density of 1.82 g/mL and a volume of 32.3 mL?
Review
Metal, non-metal, metalloid
P+, n0, e—: charge, location, mass
Evidence of a chemical reaction