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<strong>Chemistry</strong> <strong>120</strong><br />
Chapter Six <strong>Notes</strong><br />
Chapter Six:<br />
Nomenclature—The Names of Chemical Compounds<br />
Types of Ions<br />
• Ions are classified according to how many atoms they contain<br />
◦ If an ion is derived from a single atom, it is called a monatomic ion.<br />
• Examples include Na + , O 2- , and Pb 4+ .<br />
◦ Ions which are derived from two or more atoms are called polyatomic ions.<br />
Polyatomic Ions<br />
• Polyatomic ions can be described as molecules which have collectively gained or lost<br />
electrons to become an ion.<br />
• Being molecules, the ions themselves are held together by covalent bonds.<br />
• From this, you would expect the atoms in a polyatomic ion to all be nonmetals.<br />
◦ Examples: NO 3 - , ClO 4 - , NH 4<br />
+<br />
• However, some polyatomic ions contain metals which are able to covalently bond.<br />
◦ Examples: Cr 2 O 7 2- , MnO 4<br />
-<br />
• All but one of the more common polyatomic ions are anions.<br />
• The ammonium ion, NH 4 + , is the only common polyatomic cation.<br />
• The common polyatomic ions must be memorized, and you must learn to recognize them in a<br />
formula on sight.<br />
1- anions<br />
OH - hydroxide<br />
-<br />
NO 3<br />
CN - cyanide<br />
-<br />
ClO 3<br />
OCN - cyanate<br />
-<br />
BrO 3<br />
SCN - thiocyanate<br />
-<br />
IO 3<br />
-<br />
MnO 4 permanganate<br />
-<br />
C 2 H 3 O 2<br />
2- anions<br />
2-<br />
CO 3 carbonate<br />
2-<br />
SO 4<br />
2-<br />
CrO 4 chromate<br />
2-<br />
Cr 2 O 7<br />
2-<br />
C 2 O 4 oxalate<br />
2-<br />
SiO 3<br />
2-<br />
S 2 O 3 thiosulfate<br />
2-<br />
O 2<br />
3- anions<br />
3-<br />
PO 4 phosphate<br />
3-<br />
BO 3<br />
nitrate<br />
chlorate<br />
bromate<br />
iodate<br />
acetate<br />
sulfate<br />
dichromate<br />
silicate<br />
peroxide<br />
borate<br />
1