Chapter 7.1 Chemical Names & Formulas (p. 219-231)

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Presentation transcript:

Chapter 7.1 Chemical Names & Formulas (p )

A. 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. Use parentheses to show more than one polyatomic ion. Stock System - Roman numerals indicate the ion’s charge.

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

A. 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. No prefixes!

Common Ion Charges NA A. Ionic Nomenclature

potassium chloride magnesium nitrate copper(II) chloride K + Cl  Mg 2+ NO 3  Cu 2+ Cl   KCl  Mg(NO 3 ) 2  CuCl 2 A. Ionic Nomenclature

NaBr Na 2 CO 3 FeCl 3 sodium bromide sodium carbonate iron(III) chloride A. Ionic Nomenclature

B. Molecular Nomenclature Prefix System (binary compounds) 1.Less e - neg atom comes first. 2.Add prefixes to indicate # of atoms. Omit mono- prefix on first element. 3.Change the ending of the second element to -ide.

PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER B. Molecular Nomenclature

CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride B. Molecular Nomenclature

arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl 3 N2O5N2O5 P 4 O 10 B. Molecular Nomenclature

NOF Cl Br I H B. Molecular Nomenclature The Seven Diatomic Elements Br 2 I 2 N 2 Cl 2 H 2 O 2 F 2