nomenclature. naming compounds binary compounds - composed of two elements 1. contain a metal and a...
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Nomenclature
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Naming Compounds
Binary Compounds- composed of two elements
1. Contain a metal and a nonmetal
2. Contain two nonmetals
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Binary Ionic Compounds- cation (metal ion)- anion (nonmetal ion)
Type I - metal forms only one ion (Table 5.1 p. 125)
1. Cation first, anion second2. Cation - name the element3. Anion - change end of element
name to -ide
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Examples- NaCl Na+ Cl-
sodium chloride
- MgO Mg2+ O2-
magnesium oxide
- CaS Ca2+ S2-
calcium sulfide
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Type 2 - metal forms more than one cation (Table 5.2 p. 128)
1. Cation first, anion second2. Cation charge is specified by a
Roman numeral in parentheses
Examples- CuCl Cu?+ Cl-
copper(I) chloride
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-Fe2O3 Fe?+ O2-
0 = 2(?) - 3(2-)6 = 2(?)3 = ?
iron(III) oxide- PbCl4 Pb?+ Cl-
0 = ? + 4(-1)4 = ?
lead(IV) chloride
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Strategy for binary compounds
Decide if the cation has only one charge or can have multiple charges
a. If cation has one charge, name both ions
b. If cation can have multiple charges, use Roman numeral in parentheses to show the charge
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Type III - contains only nonmetals1. First element in formula is named
first using full element name.2. Second element is named as though
it were an anion (-ide ending).3. Prefixes are used to denote the
number of atoms present (Table 5.3 p. 132)
4. Never use mono for naming first element.
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Examples
BF3 boron trifluoride
NO nitrogen monoxide
N2O5dinitrogen pentoxide
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Polyatomic ions- ion composed of several atoms, but are bound together so they act as one unit- Table 5.4 p. 137-oxyanion - series of polyatomic ions that contain an atom of a given element and different numbers of oxygen atoms
ClO- hypochloriteClO2- chloriteClO3- chlorateClO4- perchlorate
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Examples
Na2SO4 sodium sulfate
KH2PO4 potassium dihydrogen phosphate
Mn(OH)2 manganese hydroxide
NH4ClO3 ammonium chlorate
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Naming Acids
Compounds that produce H+ ions when dissolved in water
1. If anion does NOT contain oxygen*prefix hydro-, suffix -ic acid
Examples
H2S - hydrosulfuric acidHCl - hydrochloric acid
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2. If anion contains oxygenroot name of central atom
*anion ends with ate - suffix -ic acidExample
H2SO4 - sulfate ion - sulfuric acid*anion ends with ite - suffix -ous acid
Example
HNO2 - nitrite ion - nitrous acid
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Writing formulas from names
Use names of elements to write the formula. You must check the charges of the ions (including polyatomic ions) to make sure the net charge on the compound is zero.
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Examplescalcium chloride Ca2+ Cl- ---> CaCl2dinitrogen pentoxide
N2O5
sodium carbonate Na+ CO3
2- ---> Na2CO3
nitric acidnitrate NO3- ---> HNO3
lead(IV) oxidePb4+ O2- ---> PbO2