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Ch. 5.2 Notes

Ch. 5.2 Notes. Ionic Bonding and Salts. Ionic Bonds. Cations (+) lose 1 or more e- Anions (-) gain 1 or more e- Receive/give e- from/to one another Resulting + and – charges are attracted, form an ionic bond Bond creates a compound. Example…. NaCl – sodium chloride (table salt)

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Ch. 5.2 Notes

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  1. Ch. 5.2 Notes Ionic Bonding and Salts

  2. Ionic Bonds • Cations (+) lose 1 or more e- • Anions (-) gain 1 or more e- • Receive/give e- from/to one another • Resulting + and – charges are attracted, form an ionic bond • Bond creates a compound

  3. Example… • NaCl – sodium chloride (table salt) • Ionic compound • Na  Na+ + e- • Cl + e-  Cl- • The e- lost by Na is gained by Cl • Positive Na+ is attracted to negative Cl-

  4. Energy changes • Transferring electrons/forming compounds involves energy changes • Na + energy  Na+ + e- • What is this energy called? • Cl + e-  Cl- + energy • Overall formation of ionic compound (also called a salt) releases energy

  5. Energy changes • Salt formation involves endo- and exothermic steps • Overall reaction is exothermic • Amount of energy released when ionic bonds formed is called lattice energy

  6. Ionic compounds • Ratio of anions to cations always reflects a neutral charge • For every 1 Na+, there’s 1 Cl- • For every 1 Mg2+, there’s 1 O2- • For every 1 Ca2+, there are 2 Cl-

  7. Ionic compounds • Don’t consist of molecules • Form crystal lattice • Ex. NaCl – multiple ions bonded together, but still maintain the ration necessary for a neutral compound

  8. Variations in ionic crystal lattices

  9. Properties of Ionic Compounds • Strong bonds • High melting and boiling points • Rarely gaseous at room temp. • Hard • Brittle – break along a cleavage plane

  10. Properties of Ionic Compounds • Conduct electric current • (Typically) only when the ions can move around freely, aren’t locked into lattice • This happens if ionic compound is in liquid state or dissolved

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