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Nomenclature

Nomenclature. Lesson Nine. Ionic Nomenclature. Let’s review some of the features of ionic compounds Metals give up electrons to form positively charged cations Non-metals gain electrons to form negatively charged anions

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Nomenclature

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  1. Nomenclature Lesson Nine

  2. Ionic Nomenclature • Let’s review some of the features of ionic compounds • Metals give up electrons to form positively charged cations • Non-metals gain electrons to form negatively charged anions • Ionic compounds are formed from the interaction between cations and anions

  3. Ionic Nomenclature • When we name an ionic compound, we write the name of the cation comes first followed by the name of the anion, changing the name of the anion to end in –ide for monotomic anions. The names of polyatomic anions are not altered.

  4. Examples • NaCl  sodium chloride • ZnI2 zinc iodide • NaNO3 sodium nitrate • Ag2CO3 silver carbonate • (NH4)2SO4 ammonium sulfate

  5. Molecular Nomenclature • Binary Molecular Compounds • When a pair of elements form more than one type of covalent compound, Greek prefixes are used to indicate how many of each element are in a compound. The more electronegative element is written last and its ending is changed to –ide. • Least electronegative atom goes first

  6. Greek Numbers mono  1 di  2 tri  3 tetra  4 penta  5 hexa  6 hepta  7 octa  8

  7. Examples • N2O  dinitrogen monoxide • NO  nitrogen monoxide • N2O3 dinitrogen trioxide • N2O5 dinitrogen pentoxide

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