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Ionic Bonds

Learn about ionic bonds, ions, octet rule, oxidation numbers, Lewis dot structure, naming conventions, and writing formulas for ionic compounds. Understand metals with multiple charges.

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Ionic Bonds

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  1. Ionic Bonds

  2. What is an ion? • An atom that gains or loses electrons is an ion. • A cation loses electrons and becomes a positive ion • An anion gains electrons and becomes a negative ion

  3. Octet rule • Atoms want 8 electrons. • This makes them stable and happy

  4. Some atoms will give up electrons and some will gain to get to 8.

  5. Oxidation numbers

  6. Ionic Bonds • A metal bonded to a nonmetal • Give up and take electrons • Ions held together by electrostatic force • Conduct electricity in water because they break up into their ions • High Boiling Point

  7. Ionic bonds in solution

  8. Lewis dot structure • Use only the valence electrons • Put a dot around the symbol of the element for each valence electron.

  9. The metal will give up its electrons and the nonmetal will gain electrons

  10. Naming ionic bonds • Name the first element the same name as the metal. • Name the second element and end in –ide • Example: KCl Potassium Chloride • If contain a polyatomic ion use the polyatomic ions name • Example: Al2(SO4)3 Aluminum Sulfate

  11. Writing binary ionic bonds • The charge on an ionic bond must be zero • So Na+1 and Cl-1 balance out to be zero and are written • NaCl sodium chloride • Mg +2 and S -2 balance out to be zero • MgS Magnesium sulfide

  12. When they do not balance out to zero you need more of one ion or the other. • Na+1 and S -2 • Na2S sodium sulfide • Mg +2 and Cl -1 • MgCl2 Magnesium Chloride

  13. Sometimes you need more of both. • Mg +2 P -3 • Mg3P2 Magnesium phosphide

  14. Polyatomic ions • Are covalently bonded ions that have a charge and are used in ionic bonds. • Perchlorate ClO4- • Chlorate ClO3- • Chlorite ClO2- • Hypochlorite ClO -

  15. Naming ternary ionic compounds • Ternary ionic compounds have more than 2 types of elements • Name the first element (or polyatomic ion) then name the second element (or polyatomic ion) • Example: Na2SO3 NH4CN K2SO4 Sodium sulfite Ammonium cyanide Potassium sulfate

  16. Writing formulas for ternary ionic compounds • The charge on a compound must always be zero • When there are more than one polyatomic ion it must be put into parentheses. ( )

  17. Examples • Calcium acetate: Ca +2 C2H3O2 -1 • Ca(C2H3O2)2 • Aluminum Chromate: Al+3 CrO3-1 • Al(CrO3)3 • Ammonium sulfite: NH4+1 SO3-2 (NH4)2SO3

  18. Metals with multiple charges • Many metals have more than one oxidation number • Then a roman number is used after the name of the metal • Examples • Copper (II) Oxide CuO • Copper (I) Oxide Cu2O

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