Ionic Compound Nomenclature. Binary Ionic Compounds Nomenclature w/ oxidation numbers 1.The name of...

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