Chapter 16 Notes, Part I

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Chapter 16 Notes, Part I

• Covalent Bonding Diagrams

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An Addendum to Lewis Structures

• Carbon and silicon are exceptions to the pattern
  of how to place electrons in a Lewis Dot
  Structure.
• This is because they have hybrid orbitals (where
  the s and p sublevels blend together and have
  four equal energy orbitals.)

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Covalent Bonding

• A covalent bond occurs between two non-metals
• Electrostatic bonding does not occurin other
  words, there is no give and take of electrons

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It ends up being a tug of war of electrons
Where the electrons end up somewhere in the
middle.
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Single Bonds

• A single bond occurs when one pair of electrons
  is shared by two atoms.
• This pair of bonded electrons is called a shared
  pair.

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Double and Triple Bonds

• Double bonds occur when two atoms have two shared
  pair of electrons
• Triple bonds occur when two atoms share three
  pair of electrons

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Ionic compounds bonded together dont really
exist, but molecular compounds do!
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Covalent Bonding Diagrams

• Like the ionic bonding diagrams, first draw the
  dot diagram for each element
• Now, however, the electrons are not being given
  away or taken, but shared so signify a pair
  being shared by circling both electrons.
• Every element should have eight electrons (count
  each shared pair as two).

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Covalent Bonding Diagrams

• If there is more than one of each element in the
  compound, you have to have a central atom.
• It will be the one with the most spots to bond to.

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Hydrogen

• Since hydrogen is in the first energy level, it
  will not need 8 valence electrons to be stableit
  will only need 2.

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H2
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H2O
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Cl2
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O2
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N2
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CCl4
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CO2
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HCN
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PCl3
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H2O2
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C2H4
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CSF2
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SiS2
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Covalent Bonding and Polyatomic ions

• A polyatomic ion is just a charged molecule that
  bonds covalently.
• The charge signifies how many electrons are
  given/taken away.

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OH1-
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NO21-
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CO32-
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PO33-