Name:__________________________________________
Period:______________
Bonding Basics
Section A: Complete the chart using the periodic table to help you.
Element
Atomic
Symbol
# of protons
# of electrons
# of valence
electrons
Chlorine
Potassium
Magnesium
Fluorine
Aluminum
Sodium
Nitrogen
Oxygen
Hydrogen
Carbon
Argon
Lithium
Difference in electronegativity
4.0
1.7
.4
Polar-covalent
bond
0
Non-polar
covalent bond
Ionic
100%
50%
5%
0%
Percentage Ionic character
Adapted from T. Trimpe & L. Bogner 2008
http://sciencespot.net/
Electronegativity
Use the word bank to complete Section B and Section C. (Words may be used more
than once.)
metal
Non-metal
Left
Small
dipole
positive
Full/complete
Transfer
Right
Equally
negative
Ion
share
large
unequally
Section B: What is a covalent bond?
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Atoms ________________________ one or more pairs of electrons with each other to form a
covalent bond.
Each atom is left with a _______________________ outer shell.
A covalent bond forms between two _______________________.
The electronegativity difference for a covalent bond is _____________________.
If the electronegativity difference if < 0.4, atoms will share the electrons ___________________,
which results in a non-polar molecule.
In a non-polar molecule, there are no regions of _____________________ or
_________________ charge; the overall molecule is neutral.
If the electronegativity difference is between 0.4 and 2.1, atoms will share the electrons
____________________, which results in a polar molecule.
A polar molecule contains a ___________________________, which means that part of the
molecule has a positive charge and part of the molecule has a negative charge.
Section C: What is an Ionic bond?
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An atom that gains one or more electrons will have a _______________________ charge.
An atom that loses one or more electrons will have a _______________________ charge.
An atom that gains or loses one or more electrons is called an ________________.
An atom will ______________________ one or more electrons to another atom to form an ionic
bond.
Each atom is left with a ___________________________ valence shell.
An ionic bond forms between a ________________________ ion with a positive charge and a
_________________________ ion with a negative charge.
The electronegativity difference for an ionic bond is _________________________.
Metals are found on the ___________________ side of the periodic table.
Non-metals are found on the __________________________ side of the periodic table.
________________________ have a much higher electronegativity than metals.
Adapted from T. Trimpe & L. Bogner 2008
http://sciencespot.net/
Practice forming bonds between the following atoms:
1. Hydrogen + Hydrogen
3. Chlorine + Chlorine
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
2. Hydrogen + Oxygen
4. Carbon + 4 Hydrogen
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
Adapted from T. Trimpe & L. Bogner 2008

Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
http://sciencespot.net/
5. Hydrogen + Chlorine
7. Magnesium + Chlorine
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
6. Sodium + Chlorine
8. Potassium + Fluorine
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
Adapted from T. Trimpe & L. Bogner 2008

Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
http://sciencespot.net/
9. Calcium + Chlorine
11. Potassium + Chlorine
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
10. Aluminum + Chlorine (challenge)
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Electronegativity difference:
Type of bond (covalent, polar covalent, or
ionic):
Picture of bond:
Adapted from T. Trimpe & L. Bogner 2008
http://sciencespot.net/