Nomenclature

1
Nomenclature

• Continued
• Chapter 6 Sections 5 and 6

2
Review of Ionic Compounds

• Metal with non-metal(s)
• Cation with anions
• Charges must add up to be zero
• If the cation can have multiple charges then
  Roman Numerals must be used

3
Molecular (Covalent) Compounds

• Two or more non-metals (no charges)
• To determine the name from the formula
• Write the name of the first element.
• If there is more than one of the first element
  then a Greek prefix must be used to indicate how
  many atoms are present.
• Write the name of the second element, change the
  suffix to ide, and use Greek prefixes to show
  how many are present.

4
Greek Prefixes!

• 1 mono-
• 2 di-
• 3 tri-
• 4 tetra-
• 5 penta-

• 6 hexa-
• 7 hepta-
• 8 octa-
• 9 nona-
• 10 deca-

5
Examples!

• OF2
• SO3
• Cl2O8

oxygen difluoride
sulfur trioxide
dichlorine octoxide
6

• To determine the formula from the name
• Write the symbol for the first element and use
  the prefix to determine the subscript.
• Repeat step 1 for the second element

7
Examples!

• Carbon tetrachloride
• Diphosphorous pentoxide
• Dihydrogen monoxide

CCl4
P2O5
H2O
8
Naming Acids

• Anions connected to as many hydrogen ions (H) as
  are necessary to make the compound electrically
  neutral.
• If the anion ends with ate then the acid is
  changed to ic
• If the anion ends with ite then the acid is
  changed to ous
• If the anion ends with ide then the acid is
  hydro- -ic

9
Common Acids

• You need to know these!
• HCl hydrochloric acid
• H2SO4 sulfuric acid
• HNO3 nitric acid
• HC2H3O2 acetic acid
• H3PO4 phosphoric acid
• H2CO3 carbonic acid
• Practice on the back of the common ion sheet!