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Binary Ionic Compounds

Binary Ionic Compounds. Consist of only two elements Name the positive ion ( Cation ) Name the negative ion ( Anion ), changing the ending to – ide

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Binary Ionic Compounds

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  1. Binary Ionic Compounds • Consist of only two elements • Name the positive ion (Cation) • Name the negative ion (Anion), changing the ending to –ide • When metals that can form more than one type of ion are in a compound, use Roman Numerals in parentheses after the name of the metal to show charge. • Transition Metals Episode 603

  2. Examples: NaCl sodium chloride MgO magnesium oxide Cu2S copper (I) sulfide SnCl4 tin (IV) chloride Episode 603

  3. Ternary Ionic Compounds • Made up of three elements • Name the cation then name the polyatomic ion without changing the ending to “ide” Examples: Na2SO4 sodium sulfate FeCrO4 iron (II) chromate Hint: Iron is a transition metal and has more than one ionic charge. Episode 603

  4. Rule of Thumb • If the first element is a metal, use ionic nomenclature. • If all elements are non-metals, use the molecular namenclature. • Watch for NH4+1, cation polyatomic ion. Episode 603

  5. Naming Molecular Compounds • The elements are named in the order they appear in the formula. • Prefixes are used to denote the number of atoms each element in the molecule. An exception is that the first element named is given a prefix only if there is more than one atom of the element in the molecule. • The ‘o’ or ’a’ at the end of the prefix is dropped when the word following the prefix begins with a vowel. • The last element’s ending is changed to –ide. Episode 603

  6. Examples: ICl3 iodine trichloride As2O5 diarsenicpentoxide C4H10 butane C2H4 ethene Alkane: CnH2n+2 Alkene: CnH2n Alkyne: CnH2n-2 Episode 603

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