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Ionic CompoundNomenclature
Binary Ionic Compounds Nomenclature
w/ oxidation numbers
1. The name of the cation (metal) is first. It will have its entire element name.
2. The anion (nonmetal) will have its element name with its –ide ending
For example
NaCl
Sodium chloride
Try these examples
1. ZnS
2. KCl
3. BaO
4. AlF3
5. CaO
1. Zinc Sulfide
2. Potassium Chloride
3. Barium Oxide
4. Aluminum Fluoride
5. Calcium Oxide
Oxidation Numbers
• Group 1 (IA) +1
• Group 2 (IIA) +2
• Group 13 (IIIA) +3
• Group 14 (IVA)±4
• Group 15 (VA) -3
• Group 16 (VIA)-2
• Group 17 (VIIA) -1
Criss Cross/Swap & Drop Method
1. Write the symbol and charge for each element.
2. The anion’s charge becomes the # of cations
3. The cation’s charge becomes the # of anions
4. Reduce if necessary. (if there is a common factor)
For example
Calcium chloride
Ca 2+ Cl 1-
cation anion
CaCl2
For example
Barium sulfide
Ba 2+ S 2-
cation anion
Ba2S2
Reduce.
BaS
Example
potassium chloride
K 1+ Cl 1-
cation anion
• The charge of your anion = the # of cations K1
• The charge of your cation = the # of anions Cl1• Reduce if necessary
KCl
Try these examples
1. Lithium oxide
2. Potassium sulfide
3. Sodium iodide
4. Magnesium Nitride
5. Rubidium Phosphide
Writing Formulas without Oxidation Numbers
Writing Formulas without Oxidation Numbers
• The charge of transition metals will be given in parenthesis.
Iron (III) oxide
Fe3+ O2-
• Use the criss cross method.
Fe2O3
Try these examples
1. Copper (II) iodide
2. Tin (II) chloride
3. Tin (IV) oxide
4. Chromium (VI) sulfide
Naming Binary Ionic Compounds without oxidation numbers
Naming Binary Ionic Compounds without oxidation numbers
*Use your reference sheet to determine ions of different transition metals.
1. The cation (metal) will have its entire name with its charge in parentheses.
2. The anion will have its element name with its –ide ending.
3. You will need to reverse the criss cross method to find the cations charge.
ExampleCoI2
Cobalt (?) iodide• Use the criss cross method in reverse.• Write the element symbols with their subscripts and
the charge of the anion.
CoX1 I1-
2• Set up an equation equal to zero using the charges
and number of each element. The charge of the cation is x (unknown). Then solve for x.
1(x) + (1-)(2) = 01x - 2=0X= 2+
Try these examples
1. Cu2Se
2. FeS
3. SnO2
• Copper (I) selenide• Iron (II) sulfide• Tin (IV) oxide
Tertiary Ionic CompoundNomenclature
Tertiary Ionic Compounds
• Composed of– positively charged Polyatomic ion +
nonmetal (anion)– Metal (cation) + negatively charged
polyatomic ion– Two polyatomic ions (one positive and one
negative charge)
Writing Formulas with oxidation #s
1. Write symbol and charge for each element or polyatomic ion
2. Use the crisscross method.
3. Polyatomic ions must remain in parenthesis with the amount written outside as a subscript.
i.e. 2 nitrate ions (NO3)2
Try these examples
1. Magnesium hydroxide
2. Potassium sulfate
Naming
• Must be able to recognize polyatomic ions.
1. Name the cation and (-) charge poly ion
2. Name the (+)polyatomic ion and name the anion.
3. Name both polyatomic ion.
Example
1. CaCr2O4
2. KClO3
• Calcium dichromate• Potassium chlorate
Naming Formulas without Oxidation Numbers
• Must include charge of the cation (transition metal).
• Will only include the tertiary ionic compounds with a cation (transition metal) and polyatomic ion.
1. Name the cation with its charge. May require using the criss cross method reversed.
2. Name the polyatomic ion.
Example: Sn3(PO4)2
1. The charge of your cation is the number of anions.
Or
SnX3 (PO4)3-
2
3x + (3-)(2)=03x-6=03x=6X=2+
Tin (II) phosphate
Try this One:
1. Pb(C2H3O2)2 • Lead (II) acetate
Writing Formulas Without Oxidation Numbers
1. Write elements or polyatomic ions with charges
2. Use the criss cross method
Chromium (III) nitrate
Cr 3+ NO31-
Cr(NO3)3
(3+)(1) + (1-)(3)=0
Try these examples
1. Mercury (II) hydroxide
2. Iron (III) chlorate
• Hg(OH)2
• Fe(ClO3)3