Ionic Bonds: Naming & Writing

What we know

Metals on left of P.T., nonmetals on right

Metals want to lose electrons, become positive

Non-metals want to gain electrons, become negative

Metals: form cations

Non-metals: form anions

Ionic Bonds

Occurs between a metal and a non-metal

Metal gives up electrons, non-metal accepts electrons; electrons are transferred!

Both elements now have a complete octet!

The metal, now with a + charge is attracted to the non-metal, which has a – charge!

Forms an ionic compound!

Ionic Bonding

Rules for Naming

1. Write the name of the first element

2. Write the name of the second element with the –ide ending

Naming Practice

1. NaF

2. Li3P

3. CaBr2

4. Ba3N2

5. AlI3

1.Sodium fluoride2.Lithium phosphide3.Calcium bromide4.Barium nitride5.Aluminum iodide

Rules for Writing Formulas

1. Write the symbol for the first element

2. Determine its charge

3. Write the symbol for the second element

4. Determine its charge

5. Swap and drop the charges to give you the subscripts

1. Reduce if necessary

Swap and Drop Example

Aluminum Oxide:

Formula Practice

1. Sodium chloride

2. Magnesium iodide

3. Lithium sulfide

4. Potassium nitride

5. Gallium sulfide

1.NaCl2.MgI2

3.Li2S4.K3N5.Ga2S3

Ionic Naming with Transition Metals

Naming Compounds: Transition Metals

Note: Many transition metals can have multiple charges. (Pb and Sn included)

Iron: can have charge of +2 or +3

In order to specify what the charge is, we use roman numerals in parentheses after the cation (metal)

Ex: Iron (II) Oxide

Ex: Iron (III) Oxide

*You will need to use anion to determine the charge of cation if it is a transition metal!

Rules for Writing Formulas with Transition Metals

1. Write the symbol of the first element

2. The charge is given to you by the roman numeral that comes after the name

1. Note (Zinc and Silver don’t get roman numerals)

3. Write the symbol for the second element

4. Determine the charge

5. Swap and drop (or criss-cross) the charges and reduce if necessary

Examples: Formula Writing

1. Lead (IV) sulfide

2. Copper (I) nitride

3. Silver oxide

4. Manganese (II) phosphide

5. Lead (II) sulfide

Rules for Naming with Transition Metals

1. Write the name of the first element

2. Determine the charge of the first element and write it as a roman numeral in parenthesis

1. Use what you know about the anion (nonmetals) and reverse criss-cross/swap-drop

3. Write the name of the second element with and –ide ending

Examples: Naming

1. FeN

2. Ni2S

3. ZnCl2

4. MnO2

5. Co2S3

1.Iron (III) Nitride2.Nickel (I) sulfide3.Zinc chloride4.Manganese (IV) oxide5.Cobalt (III) sulfide

Ionic Naming with Polyatomic Ions

Ionic Bonds with Polyatomic Ions

There are some ions that are represented by groups of atoms instead of just one

Poly = many

Atomic = atoms

These ion units stick together to bond to other elementsYou cannot change their subscripts!!!

They each have their own special names associated with them

Rules for Naming with Polyatomic Ions

Follow all of the other rules for naming ionic compounds

If you see a compound with more than two capital letters, then there is a polyatomic ion presentFigure out which one it is off the list and

just write it’s name, whether it is the cation (ammonium) or the anion (everything else on the list)

Examples - Naming

1. CaCO3

2. Al(ClO2)3

3. (NH4)3PO4

4. MnSO4

5. Pb(CrO4)2

1.Calcium carbonate2.Aluminum chlorite3.Ammonium

phosphate4.Manganese (II)

sulfate5.Lead (IV) chromate

Rules for Writing Formulas with Polyatomic Ions

If you see ammonium or an ending that doesn’t have –ide, then you probably have a polyatomic ion

Use the charge to figure out what it’s symbol and charge are

Swap and drop/criss-cross the charges

IF YOU ARE PUTTING A SUBSCRIPT OTHER THAN ONE ONTO A POLYATOMIC ION, YOU MUST PUT IT IN PARENTHESIS FIRST, THEN PUT THE SUBSCRIPT

Examples – Writing Formulas

1. Sodium sulfite

2. Cobalt (III) iodate

3. Ammonium chloride

4. Copper (II) carbonate

5. Aluminum acetate

6. Magnesium hydroxide

1.Na2SO3

2.Co(IO3)3

3.NH4Cl4.CuCO3

5.Al(C2H3O2)3

6.Mg(OH)2