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D'Agostin: Unit #6 Notes - Bonding & Lewis Dot Structures

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John D'Agostin

on 21 March 2014

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Transcript of D'Agostin: Unit #6 Notes - Bonding & Lewis Dot Structures

Bonding & Lewis
Dot Structures

Unit #4 Notes
Single Covalent Bond
A bond in which 2 atoms share a
pair of valence electrons.
Double Covalent Bond
Triple Covalent Bond
A bond in which 2 atoms share
3 pair of valence electrons.
A bond in which 2 atoms share
2 pair of valence electrons.
Lewis Dot Structure
Describe the number of bonds found in a molecule and
the arrange of unshared pairs (lone pairs) of electrons.
1. Determine the total # of valence electrons.
2. Write the symbols of the atoms in the molecule. The central atom must be able to form more than 1 bond.
3. Draw 2 dots to represent a chemical bond.
4. No atom should have more that 8 valence electrons.
Octet Rule
Remember, covalent bonds form so
that each atom that is part of a
molecule has a complete set of
8 valence electrons.
Bond Polarity
Describes the degree to which a pair of
electrons is shared between the 2 atoms
that are part of a chemical bond
Nonpolar Covalent Bond
Polar Covalent Bond
A covalent bond that forms if the 2 atoms do NOT share a pair of valence electrons equally. This type of bond results in an unequal distribution of charge because 1 of the atoms has a greater share of the electron pair.
Ionic Bond
The bond formed between large numbers of cations (+ ions) and anions (- ions)

Remember, opposite charges attract!
A covalent chemical bond formed
if 2 atoms share a pair of valence
electrons equally. This type of bond
results in a balanced distribution
of charge.
Electronegativity
A measure of an atoms ability
to attract electrons
Lone Pair
or
Unshared Pair
An atom has a greater share of the electron pair if it has a higher electronegativity
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