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IONIC BONDING

Learn about ionic bonding, including the formation of ions, properties of ionic compounds, Lewis structures, and the nomenclature of ionic compounds.

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IONIC BONDING

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  1. IONIC BONDING

  2. 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 What is an ion? + -

  3. Composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal Ionic Compound

  4. Formed by ionic bonds • Electrons are either gained or lost • Have a regular repeating pattern called a crystal lattice • Formed between metals with nonmetals; cations with anions • High Melting point and Boiling Point • Conductors of electricity Strong bonds; stronger than covalent bonds Properties of Ionic Compounds

  5. Ionic – show the transfer of electrons Lewis Structures

  6. 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:

  7. Ionic Nomenclature Ionic Formulas Write each ion,cationfirst 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.

  8. 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. Ionic Nomenclature continued…

  9. Calcium Nitrate Ca+2 NO3-1 Ca1(NO3)2 Ca(NO3)2 1(+2) + 2(-1)= 0 Cross the exponents only! not the + or - Do NOT show 1 in the final formula EXAMPLE: Polyatomic ion NO3 goes in parentheses This is your final formula! Check for the overall charge to equal zero

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

  11. Ionic Nomenclature Ionic Names Write the names of both ions, cation first. Change ending of monatomic ions to -ide. Polyatomic ionshave special names. Stock System - Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

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

  13. 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?

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

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