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Ionic Compounds

Ionic Compounds. Ions. when electrons are added or removed from a neutral atom, it becomes an ion (has electric charge) Positive = less electrons than protons Negative = more electrons than protons the charge on the ion is shown to the upper right of the symbol, e.g. Al 3+ or O 2-. Ions.

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Ionic Compounds

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  1. Ionic Compounds

  2. Ions • when electrons are added or removed from a neutral atom, it becomes an ion (has electric charge) • Positive = less electrons than protons • Negative = more electrons than protons • the charge on the ion is shown to the upper right of the symbol, e.g. Al3+ or O2-

  3. Ions • when electrons are added or removed from a neutral atom, it becomes an ion (has electric charge)

  4. Ionic Compound: metal + non-metal combine. Each changes into an ion. IONS: - Metals LOSE electrons= + (e.g. Na+) - Non-metals GAIN electrons = - (e.g. Cl-) *** All atoms want a full outer shell in order to be stable!! ***

  5. Ionic Compounds Transfer Electrons

  6. Ionic Compounds + and - ions attract Connection between atoms is called a bond

  7. Ionic Compounds • Generally have these properties: • Solids at room temp (RT) • High melting point (MP) • Conduct electricity when dissolved in water e.g. NaCl, MgO, CaCl2

  8. Ionic Compounds Sodium Chloride (NaCl)

  9. Naming Compounds • Common names e.g.“Chalk” can have different meanings, e.g. drawing chalk (calcium sulphate), antacids (calcium carbonate) • “Salt”(e.g. table salt, road salt) • Use chemical formulas to clarify

  10. Naming 1. Look at the formula, e.g. CaCl2 2. Name the metal ion first = Calcium 3. Name the non-metal = Chlorine 4. Change the ending of the non-metal ion to “ide” Chlorine Chloride 5. Put them together with the metal name first: CaCl2 = CALCIUM CHLORIDE

  11. Try These: LiBr K2O Mg3N2 Be3P2 = lithium bromide = potassium oxide = magnesium nitride = beryllium phosphide

  12. Multivalent Elements • a few metals are able to form more than one stable ion so they have more than one ionic charge • E.g. tin has ionic charges of +2 and +4 • in naming these compounds, the ionic charge is placed in Roman numerals in brackets after the metal’s name

  13. Multivalent Elements • You can determine which Roman numeral to use from the subscript in the formula e.g. CrCl3 • All ion charges in a compound must add to zero (must be neutral, no net charge) • According to this rule, a Cr3+ ion has to combine with threeCl- ions to balance it out!

  14. Multivalent Elements • a "reverse criss-cross rule" may be used to figure out the metal ion charge •  example #2: Name the following compounds : 2+ 1- • (a) FeCl2 Fe Cl2 - iron (II) chloride 4+ 3- • (b) Sn3P4 Sn3 P4 - tin (IV) phosphide

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