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Nomenclature

This guide explores the nomenclature of molecular and ionic compounds, focusing on the systematic naming conventions for covalent compounds using specific prefixes such as mono-, di-, tri-, etc. Additionally, it explains how ions are formed through the gain and loss of electrons, the distinction between anions and cations, and the general charge tendencies of metals and non-metals. The document outlines how to derive chemical formulas from names and vice versa, as well as how to name acids based on their compositions.

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Nomenclature

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  1. Nomenclature System of naming compounds

  2. Molecular Nomenclature • Naming covalentcompounds • Based on a system of prefixes

  3. One mono- six hexa- • Two di- seven hepta- • Three tri- eight octa- • Four tetra- nine nona- • Five penta- ten deca-

  4. Examples of Molecular Names • CO2 • CO • P2O5 • CCl4

  5. Ion • Formed when electrons are added or removed from an atom • Gain electrons – become negative - Anion • Lose electrons – become positive - Cation

  6. Why Form Ions • Atoms gain or lose electrons to end up with the same number of electrons as the nearest noble gas • Predict the charges expected by O Ba

  7. Ion Generalizations • Metals generally form + charges, while non-metals form – charges • Ionic compounds tend to be composed of a metal combined with a non-metal • Molecular compounds usually are two non-metals

  8. Polyatomic Ions • Atoms joined in a molecule but have a net charge • (SO4)2- • NO3 -

  9. Finding Formulas from Names • Calcium nitrate • Copper (I) carbonate

  10. Names from Formulas • AlCl3 • K(NO3) • Al2O3 • Fe3(PO4)2

  11. Acid Names • Acids all start with an H • For binary acids (H and one other element), start with prefix hydro- and end with suffix –ic

  12. Oxyacids • H, O and another element • If anion has an –ate ending, give acid an –ic ending • If anion has an –ite ending, give acid an –ous ending

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