Ionic Bond

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Ionic Bonding

• Metal atoms with low ionization energies and
  non-metal atoms with high electron affinity form
  cations () and anions (-)
• Oppositely charged ions attract to a crystalline
  structure

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Lattice Energy

• Quantity of energy required for 1 mole of the
  solid ionic substance to be separated into its
  ions
• Higher more stable
• Very high in ionic substances
• This accounts for high melting temp., and hard
  and brittle nature

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Process of Ionic Bond Formation

• Always exothermic
• Compound forms because it is more stable (lower
  in energy) than its elements
• Stability comes from packing of ions together
• Lattice energy increases as the charges on ions
  increase and radii decrease

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Ionic Structures

• Can have many types of arrangements
• Arrangement depends on the charge and size of the
  ions involved

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• Which substance would have a higher lattice
  energy NaF or MgO?
• Which would have a higher lattice energy FeO or
  Fe2O3?

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Forming The Ions

• The ions are formed when electrons are
  transferred from the atom with low
  electronegativity to an atom with high
  electronegativity
• Predict the compound formed between aluminum and
  fluorine.

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Transition-Metal Ions

• Transition metals form many differently charged
  ions (some 2, some 1, some 3)
• In forming ions the transition metals lose the s
  electrons first and then as many d electrons as
  necessary to form the ion of that particular
  charge

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Write the Configuration of Each

• Co2
• Co3
• Cr3

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Sizes of Ions

• Cations are smaller than their parents
• Anions are larger than their parents
• Ions of the same charge, size increases going
  down a group
• List the following in order of decreasing size
  Mg2, Ca2, Ca

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Isoelectric Series

• Comparitive sizes of ions all possessing the same
  number of electrons
• As nuclear charge increases, the radius decreases
• O2- gt F- gt Na gt Mg2 gt Al3

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Example

• Arrange the ions S2- , Cl-, K, and Ca2 in order
  of decreasing size.