Chapter 5: Nomenclature Flashcards
binary compounds
compounds composed of two elements
two broad classes of binary compounds
- compounds that contain a metal and a nonmental
- compounds containing two nonmetals
binary ionic compound
contains a positive ion (cation) and a negative ion (anion)
Type I compounds
- the metal forms only one type of cation
Note: Group 1 and 2 metals are always Type I.
Type II compounds
the metal present can form two (or more) cations that have different charges
Note: Transition metals are almost always Type II.
Rules for Naming Type I Ionic Compounds
- The cation is always named first and the anion second.
- A simple cation (obtained from a single atom) takes its name from the name of the element. (Ex: Na+ is called sodium in the names of compounds containing this ion.)
- A simple anion (obtained from a single atom) is named by taking the first part of the element name (the root) and adding -ide. (Ex: Cl- is called chloride.)
Rules for Naming Type II Ionic Compounds
- The cation is always named first and the anion second.
- Because the cation can assume more than one charge, the charge is specified by a Roman numeral in parentheses.
transition metals forming only one ion
- Ag+
- Zn2+
- Cd2+
prefixes used to indicate numbers in chemical names
- mono-
- di-
- tri-
- tetra-
- penta-
- hexa-
- hepta-
- octa-
Rules for Naming Type III Binary Compounds
Type III Binary compounds contain only nonmetals
- The first element in the formula is named first, and the full element name is used.
- The second element is named as though it were an anion.
- Prefixes are used to denote the numbers of atoms present.
- The prefix mono- is never used for naming the first element. (Ex: CO is called carbon monoxide, not monocarbon monoxide.)
3 types of binary compounds
- Type I: ionic compounds with metals that always form a cation with the same charge
- Type II: ionic compounds with metals (usually transition metals) that form cations with various charges
- Type III: compounds that contain only nonmetals
polyatomic ions
charged entities composed of several atoms bound together
oxyanions
polyatomic anions that contain an atom of a given element and different numbers of oxygen atoms
Rules for Naming Oxyanions
When there are two members in a series:
- the name of the one with the smaller number of oxygen atoms ends in -ite
- the name of the one with the larger number ends in -ate
When more than two oxyanions make up a series, use the prefixes:
- hypo- (less than)
- per- (more than
Ex:
ClO- hypochlorite
ClO2- chlorite
ClO3- chlorate
ClO4- perchlorate
acids
substances containing H+ ions (protons), which are produced by certain molecules when dissolved in water; best considered as one or more H+ ions attached to an anion
Rules for Naming Acids
- If the anion does not contain oxygen, the acid is named with the prefix hydro- and the suffix -ic attached to the root name for the element.
Ex: When gaseous HCl is dissolved in water, it forms hydrochloric acid.
- When the anion contains oxygen, the acid name is formed from the root name of the central element of the anion or the anion name, with a suffix of -ic (when the anion name ends in -ate) or -ous (when the anion name ends in -ite).
Ex: H2SO3 (acid) = SO32- (sulfite anion) = sulfurous acid
acids of the oxyanions of chlorine
HClO4 perchloric acid
HClO3 chloric acid
HClO2 chlorous acid
HClO hypochlorous acid
Acids That Do Not Contain Oxygen
HF hydrofluoric acid
HCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid
HCN hydrocyanic acid
H2S hydrosulfuric acid
Names of Some Oxygen-Containing Acids
HNO3 nitric acid
HNO2 nitrous acid
H2SO4 sulfuric acid
H2SO3 sulfurous acid
H3PO4 phosphoric acid
HC2H3O2 acetic acid
