Transcript Station 5 Answer PowerPoint

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
- 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
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)

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
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
More functional groups
Class
Alcohol
Aldehyde
Amine
Carboxylic acid
Ester
Ether
Ketone
Attached Functional
Group