Transcript Binary Ionic Compound Nomenclature

Ionic Compound
Nomenclature
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.
2.
3.
4.
5.
ZnS
KCl
BaO
AlF3
CaO
1.
2.
3.
4.
5.
Zinc Sulfide
Potassium Chloride
Barium Oxide
Aluminum Fluoride
Calcium Oxide
Oxidation Numbers
•
•
•
•
•
•
•
Group 1 (IA)
Group 2 (IIA)
Group 13 (IIIA)
Group 14 (IVA)
Group 15 (VA)
Group 16 (VIA)
Group 17 (VIIA)
+1
+2
+3
±4
-3
-2
-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 1cation
anion
CaCl2
For example
Barium sulfide
Ba 2+ S 2cation
anion
Ba2S2
Reduce.
BaS
Example
potassium
K 1+
cation
•
•
•
chloride
Cl 1anion
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.
2.
3.
4.
5.
Lithium oxide
Potassium sulfide
Sodium iodide
Magnesium Nitride
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.
2.
3.
4.
Copper (II) iodide
Tin (II) chloride
Tin (IV) oxide
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.
Example
CoI2
•
•
•
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) = 0
1x - 2=0
X= 2+
Try these examples
1. Cu2Se
2. FeS
3. SnO2
• Copper (I) selenide
• Iron (II) sulfide
• Tin (IV) oxide
Tertiary Ionic Compound
Nomenclature
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)=0
3x-6=0
3x=6
X=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+ NO31Cr(NO3)3
(3+)(1) + (1-)(3)=0
Try these examples
1. Mercury (II)
hydroxide
2. Iron (III) chlorate
• Hg(OH)2
• Fe(ClO3)3