Ionic Bonding

1
Ionic Bonding

• Chemistry
• Mr. Carleton

2
Who Done It?

• Ionic Bonding is the bonding of a cation () with
  an anion(-).
• This commonly occurs between a metal that has
  lost one or more electrons (e-)and a non-metal
  that has gained one or more electrons (e-).

3
How Can We Tell?
4
Electronegativity Difference
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Ionic Character
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Naming

• Cations with several oxidation s get roman
  numeral notation
• Fe2, Fe3
• Cation name remains unchanged
• Na
• Monotomic anion takes on ide ending
• Cl-
• Polyatomic anion remains the same
• OH

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Naming Practice

• NaCl
• MgI2
• Ca(ClO3)2
• Aluminum chromate
• Iron (III) chloride
• Copper (II) hydroxide
• Potassium oxide

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Poison and Explosives

• Sodium go BOOM!!
• Chlorinepoison
• NaCl table salt (BIG change in properties!)

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Salt Squares?

• Crystal lattice of NaCl

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Ionic Properties

• Ionic solids are poor conductors of electricity
  and heat.
• Ionic solids generally have high melting points.
• Ionic solids are usually hard and brittle.
• Ionic solids can be melted to form liquids that
  are electrical conductors.
• Ionic solids that are water soluble, dissolve to
  form solutions that are electrical conductors.
  (Not all ionic substances are water soluble.)

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Other Ionic Compounds
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Ionic/Covalent Face-Off

• IONIC COMPOUNDS
• Strong bond with ions
• High melting/boiling points
• Solid at STP
• Hard, but brittle
• Strong intermolecular forces
• Liquid/aqueous conductor

• MOLECULAR COMPOUNDS
• Strong sharing bonds
• Lower melting/boiling points
• Gases at STP
• Moderate to weak intermolecular forces
• nonconductors