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chemistry study guide

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Covalent Bond
Polar Covalent Bond there is a difference in electronegativity (one atoms has greater attraction for
electron than the other)
Nonpolar Covalent Bond there is NO difference in electronegativity. (electrons are shared EQUALLY
between two atoms)
Bond
# of electrons
Bond Order
Bond Strength
Bond Length
Single
2
1
Weakest
Longest
Double
4
2
Triple
6
3
Strongest
Shortest
There is a symmetrical relationship between the amounts of energy released during the formation of a covalent
bond and the amount of energy needed to break the bond. Note the flow of energy. Breaking covalent bonds
requires energy, and covalent bond formation releases energy. The amount of energy released during molecule
formation can be estimated by counting the number and types of bond in a molecule. For example, a methane
molecule has one carbon atom bound to four hydrogen atoms via four single carbon-hydrogen covalent bonds.
Carbon-hydrogen bonds release 100 kcal/mole of energy when formed, so the total energy needed to break all the
bonds in a methane molecule is 100 kcal x 4 or 400 kcal.
Bond Angle determines the geometric structure of the molecule
The unit for dipole moments is the debye (D)
Bond Length unit - picometers, pm
Bond Energy - kiloJoules per mole of bonds (kJ/mol).

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Covalent Bond Polar Covalent Bond – there is a difference in electronegativity (one atoms has greater attraction for electron than the other) Nonpolar Covalent Bond – there is NO difference in electronegativity. (electrons are shared EQUALLY between two atoms) Bond # of electrons Bond Order B ...
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