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IONIC BONDING

IONIC BONDING. What is an ion?. An ion: an atom or bonded group of atoms with a positive or negative charge Cation: A positively charged ion Anion : A negatively charged ion. Ionic Compound.

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IONIC BONDING

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  1. IONIC BONDING

  2. What is an ion? • An ion: an atom or bonded group of atoms with a positive or negative charge Cation: A positively charged ion Anion: A negatively charged ion

  3. Ionic Compound • Composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal • An ionic bond is the electrostatic force that holds oppositely charged particles together in an ionic compound.

  4. Properties of Ionic Compounds • Formed by ionic bonds • Electrons are either gained or lost • Have a regular repeating pattern called a crystal lattice • Elements are generally far apart from each other (metals with nonmetals; cations with anions) • High Melting point and Boiling Point • Conductors of electricity when mixed with water • Formation of these is exothermic • Strong bonds; stronger than covalent bonds

  5. Ionic Bonds continued: Ionic Bonding - Crystal Lattice • The strong attraction of positive ions and negative ions in an ionic compound results in a crystal lattice. • A crystal lattice is a three dimensional geometric arrangement of particles. • In a crystal lattice, each + ion is surrounded by - ions and each – ion is surrounded by + ions. Ionic crystals vary in shape due to the sizes and relative numbers of the ions bonded.

  6. Common Ion Charges C. Ionic Nomenclature +1 0 +2 +3 +4/-4 -3 -2 -1

  7. B. Lewis Structures Ionic – show transfer of e-

  8. Ionic Bond • an electron is simply transferred to another atom. By doing so, each atom is able to have a stable valence shell. It is called an ionic bond because the atoms become ions, a charged atom that has either lost an electron (positive charge) or has gained an electron (negative charge). Below is an animation of ionic bonding:

  9. C. Ionic Nomenclature Ionic Formulas Write each ion, cation first. Don’t show charges in the final formula. Overall charge must equal zero. If charges cancel, just write symbols. If not, use subscripts to balance charges.

  10. C. Ionic Nomenclature Ionic Formulas • Use parentheses to show more than one polyatomic ion. • Stock System – • Roman numerals indicate the ion’s charge • used when the ion has more than one oxidation state.

  11. C. Ionic Nomenclature • potassium chloride • magnesium nitrate • copper(II) chloride  KCl • K+ Cl- • Mg2+ NO3- Mg(NO3)2 CuCl2 • Cu2+ Cl-

  12. C. Ionic Nomenclature Ionic Names Write the names of both ions, cationfirst. Change ending of monatomic ions to -ide. Polyatomic ions have special names. Stock System - Use Romannumerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

  13. C. Ionic Nomenclature • NaBr • Na2CO3 • FeCl3 • sodium bromide • sodium carbonate • iron(III) chloride

  14. C. Ionic Nomenclature Consider the following: Does it contain a polyatomic ion? -ide, 2 elements  no -ate, -ite, 3+ elements  yes Does it contain a Roman numeral? Check the table for metals not in Groups 1 or 2.

  15. AssignmentProvide the ionic compound formula or the name • Potassium fluoride • Magnesium phosphide • Aluminum iodide • Nickel II Oxide • Lead IV Oxide • K2CO3 • Pb(NO3)2 • Ca3N2 • Zn(CN)2 • AgI

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