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Nomenclature

Nomenclature. Chapter 2. Diatomic Molecules. These seven elements occur naturally as molecules containing two atoms. Writing Formulas. Because compounds are electrically neutral, one can determine the formula of a compound this way:

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Nomenclature

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  1. Nomenclature Chapter 2

  2. Diatomic Molecules These seven elements occur naturally as molecules containing two atoms.

  3. Writing Formulas • Because compounds are electrically neutral, one can determine the formula of a compound this way: • The charge on the cation becomes the subscript on the anion. • The charge on the anion becomes the subscript on the cation. • If these subscripts are not in the lowest whole-number ratio, divide them by the greatest common factor.

  4. Inorganic Nomenclature • Write the name of the cation. • If the anion is an element, change its ending to -ide; if the anion is a polyatomic ion, simply write the name of the polyatomic ion. • If the cation can have more than one possible charge (transition metals), write the charge as a Roman numeral in parentheses.

  5. Inorganic Nomenclature

  6. Patterns in Oxyanion Nomenclature • When there are two oxyanions involving the same element: • The one with fewer oxygens ends in -ite • NO2− : nitrite; SO32− : sulfite • The one with more oxygens ends in -ate • NO3− : nitrate; SO42− : sulfate

  7. Patterns in Oxyanion Nomenclature • The one with the second fewest oxygens ends in -ite • ClO2− : chlorite • The one with the second most oxygens ends in -ate • ClO3− : chlorate

  8. Patterns in Oxyanion Nomenclature • The one with the fewest oxygens has the prefix hypo- and ends in -ite • ClO−: hypochlorite • The one with the most oxygens has the prefix per- and ends in -ate • ClO4−: perchlorate

  9. Acid Nomenclature • If the anion in the acid ends in -ide, change the ending to -ic acid and add the prefix hydro- : • HCl: hydrochloric acid • HBr: hydrobromic acid • HI: hydroiodic acid

  10. Acid Nomenclature • If the anion in the acid ends in -ite, change the ending to -ousacid: • HClO: hypochlorous acid • HClO2: chlorous acid

  11. Acid Nomenclature • If the anion in the acid ends in -ate, change the ending to -ic acid: • HClO3: chloric acid • HClO4: perchloric acid

  12. Nomenclature of Binary Compounds • The less electronegative atom is usually listed first. • A prefix is used to denote the number of atoms of each element in the compound (mono- is not used on the first element listed, however.)

  13. Nomenclature of Binary Compounds • The ending on the more electronegative element is changed to -ide. • CO2: carbon dioxide • CCl4: carbon tetrachloride

  14. Nomenclature of Binary Compounds If the prefix ends with a or o and the name of the element begins with a vowel, the two successive vowels are often elided into one: N2O5: dinitrogen pentoxide

  15. Nomenclature for Organic Compounds • Names for compounds with all single bonds between C and H • Number of H = #C x 2 + 2

  16. Nomenclature for Organic Compounds • If contains double bond, change ending to ene • Number of H = #C x 2 • If contains triple bond, change ending to yne. • Number of H = #C x 2 - 2 • Ethene • pentyne

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