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Formulas

Formulas. 1. Ionic – metal and nonmetal, e - transferred Covalent – nonmetals, e - shared (EXTREMELY IMPORTANT) 2. It is the charge of the metal. They only appear in ionic compounds 3. An ion made of two or more atoms. Formulas. 4. Diatomic molecules – named after the element

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Formulas

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  1. Formulas 1. Ionic – metal and nonmetal, e- transferred Covalent – nonmetals, e- shared (EXTREMELY IMPORTANT) 2. It is the charge of the metal. They only appear in ionic compounds 3. An ion made of two or more atoms

  2. Formulas 4. Diatomic molecules – named after the element - Binary Molecular – uses prefixes - Oxyacids – (H and O) ate  ic and ite  ous and acid - Binary acids – (no O) hydro- and acid - Ionic compounds with only one choice of oxidation numbers – name metal, then nonmetal (-ide) - Ionic compounds with more than one choice of oxidation numbers. name metal, Roman Numeral, then nonmetal (-ide) It is also important to remember that covalent bonds can use prefixes, ionic don’t. But ionic can use roman numerals

  3. Hydrocarbons • Compounds contain C and H • Number of Carbons is given by the first part of name (1 meth-, 2 eth-, 3 prop-, 4 but-, 5 pent-, etc) • Number of Hydrogens = 2(carbon) + 2 • (Example: propane has 3 Carbons and 2(3)+2 Hydrogens, so C3H8)

  4. Formulas 5. Molecular is true formula, empirical is simplest ratio 6. Percent of each element in a compound Divide the mass of each element by molar mass of compound x 100 7. Ionic bonds are strongly bonded together making them hard solids with high boiling and melting points and are good electrolytes. Covalent are the opposite 8. Charges of one switch to subscripts of other

  5. 9. Saturated compounds only contain single bonds. Unsaturated will contain at least one double or triple bond 10. alkane – all single bonds alkene – has a double bond alkyne – has a triple bond

  6. More functional groups

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