1 Figure 4.3 Examples of cycloalkane nomenclature Nomenclature.
Nomenclature Continued Chapter 6 Sections 5 and 6.
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Transcript of Nomenclature Continued Chapter 6 Sections 5 and 6.
Nomenclature
ContinuedChapter 6 Sections 5 and 6
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
Molecular (Covalent) Compounds
• Two or more non-metals (no charges)To determine the name from the formula:
1. Write the name of the first element.2. If there is more than one of the first
element then a Greek prefix must be used to indicate how many atoms are present.
3. Write the name of the second element, change the suffix to –ide, and use Greek prefixes to show how many are present.
Greek Prefixes!
1 = mono-
2 = di-
3 = tri-
4 = tetra-
5 = penta-
6 = hexa-
7 = hepta-
8 = octa-
9 = nona-
10 = deca-
Examples!
OF2 =
SO3 =
Cl2O8 =
oxygen difluoride
sulfur trioxide
dichlorine octoxide
To determine the formula from the name:
1. Write the symbol for the first element and use the prefix to determine the subscript.
2. Repeat step 1 for the second element
Examples!
Carbon tetrachloride =
Diphosphorous pentoxide =
Dihydrogen monoxide =
CCl4
P2O5
H2O
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
Common AcidsYou need to know these!
HCl = hydrochloric acidH2SO4 = sulfuric acid
HNO3 = nitric acid
HC2H3O2 = acetic acid
H3PO4 = phosphoric acid
H2CO3 = carbonic acid
Practice on the back of the common ion sheet!