化学专业英语之无机化合物命名
THE NOMENCLATURE OF INORGANIC COMPOUNDS
With the discovery of thousands of new inorganic compounds it has become necessary to revise the Traditional rules of nomenclature. An international committee has recommended a set of rules for naming compounds, and these are now being adopted throughout the world. Many of the older names are still used, however, and our ensuing discussion will include in many cases both the old and new, with emphasis on the latter. One of the principal changes is that proposed by Albert Stock and now known as the Stock system for the naming of compounds of metals (oxides, hydroxides, and salts) in which the metal may exhibit more than one oxidation state. In these cases the oxidation state of the metal is shown by a Roman numeral in parentheses immediately following the English name of the metal which corresponds to its oxidation number1. If the metal has only one common oxidation number, no Roman numeral is used. Another important change is in the naming of complex ions and coordination compounds. We will defer the nomenclature of the latter until these compounds are discussed.
Naming Metal Oxides. Bases, and Salts
The student should have a good start in learning nomenclature if he has learned the Valence Table 3 which gives both charges on ions and names for the more common ones2. A compound is a combination of positive and negative ions in the proper ratio to give a balanced charge and the name of the compound follows from names of the ions, for example, NaCl, is sodium chloride; Al (OH )3 is aluminum hydroxide; FeBr2 is iron ( I ) bromide or ferrous bromide; Ca (C2H3O2)2 is calcium acetate; Cr2 (SO,)3 is chromium ( I ) sulfate or chromic sulfate, and so on. Table 4 gives some additional examples of the naming of metal compounds. Of the two common systems used, the Stock system is preferred. Note that even in this system; however, the name of the negative ion will need to be obtained from Valence Table 4.
Negative ions, anions, may be monatomic or polyatomic. All monatomic anions have names ending with ide. Two polyatomic anions which also have names ending with ide are the hydroxide ion, OH- , and the cyanide ion, CN-.
Many polyatomic anions contain oxygen in addition to another element. The number of oxygen atoms in such oxyanions is denoted by the use of the sulffixes ite and ate, meaning fewer and more oxygen atoms respectively. In cases where it is necessary to denote more than two oxyanions of the same element, the prefixes hypo and per, meaning still fewer and still more oxygen atoms, respectively, may be used. A series of oxyanions is named in Table 5.
Table 3. Some Common Ions
1+
2 +
2 +
3 +
ammonium
NH4+
barium
Ba2+
magnesium
Mg2+
aluminum
Al3+
copper(1)
Cu+
calcium
replaceable
Ca2+
manganese ( I )
Mn2+
chromium ( I )
Cr3+
hydrogen
H +
chromium ( II )
Cr2+
mercury ( I )
Hg2+
iron( I )
Fe3+
potassium
K +
copper (II )
Cu2+
mercury( I )
Hg22+
silver
Ag+
iron( II )
Fe2+
tin( I )
Sn2+
sodium
Na+
lead( II)
Pb2+
strontium
zinc
Sr2+
Zn2+
3-
2-
1-
1-
arsenate
AsO43-
carbonate
CO32-
acetate
C2H3O2-
hydrogen sulfite
HSO2-
arsenite
AsO33-
chromate
CrO42-
bromide
Br-
hydride
H-
phosphate
PO43-
dichromate
Cr2O72-
chlorate
ClO3-
hydroxide
OH-
phosphite
PO33-
oxalate
O22-
chloride
Cl-
hypochlorite
ClO-
oxide
C2O42-
chlorite
ClO2
iodate
IO3-
sulfide
S2-
cyanide
CN-
nitrate
NO3-
sulfate
SO42-
fluoride
F-
iodide
I-
sulfite
SO32-
hydrogen carbonate (bicarbonate)
HCO3-
nitrate
nitrite
NO3-
NO2-
hydrogen sulfate
HSO4-
perchlorate permanganate
NO3-
MnO4-
Table 4. Names of some metal oxides .bases .and salts
FeO
iron( II )  oxide
ferrous oxide
Fe2O3
iron( III )  oxide
ferric oxide
Sn(OH)2
tin(II)  hydroxide
stannous hydroxide
Sn(OH)4
tin(IV)  hydroxide
stannic hydroxide
Hg2SO4
mercury( I )  sulfate
mercurous sulfate
HgSO4
mercury (II) sulfate
mercuric sulfate
NaClO
sodium hypochlorite
sodium hypochlorite
K2Cr2O7
potassium dichromate
potassium dichromate
Cu3(AsO4)2
copper(II)  arsenate
cupric arsenate
Cr2(C2H4O2)3
chromium(III ) acetate
chromic acetate
Naming Nonmetal oxides
The older system of naming and one still widely used employs Greek prefixes for both the number of oxygen atoms and that of the other element in the compound3. The prefixes used are (l)mono-, sometimes reduced to mon-, (2)di-, (3)tri-, (4)tetra-, (5)penta-, (6) hexa-, (7)hepata-, (8)octa-, (9)nona-and (10)deca-. Generally the letter a is omitted from the prefix (from tetra on) when naming a nonmetal oxide and often mono- is omitted from the name altogether.
The Stock system is also used with1 nonmetal oxides. Here the Roman numeral refers to the oxidation state of the element other than oxygen.
Table 5. Names of oxyanions
Fewest Oxygen Atoms
hypo — ite
Fewer Oxygen Atoms
— ite
More Oxygen Atoms
-----ate
Most Oxygen Atoms
per — ate
ClO-
hypochlorite
ClO2-
chlorite
ClO3-
chlorate
ClO4-
perchlorate
BrO-
hypobromite
BrO2-
bromite
BrO3-
bromate
BrO4-
perbromate
IO-
hypoiodite
IO2-
iodite
IO3-
iodate
IO4-
periodate
PO23-
hypophosphite
PO33-
phosphite
PO43-
phosphate
NO2-
nitrite
NO3-
nitrate
SO32-
sulfite
SO42- CO32-
sulfate
carbonate
In either system .the element other than oxygen is named first, the full name being used followed by oxide. Table 6 shows some examples.
Naming Acids
Acid names may be obtained directly from a  knowledge of Valence Table 3 by changing the name of the acid ion(negative ion)in the table as follows:

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