Naming Ionic Compounds: Ions, Polyatomic Ions, and Writing Formulas, Slides of Chemistry

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Naming Compounds

Ionic Compounds and Polyatomic Ions

Formation of Ions from Metals Metals lose_ electrons to match the number of valence electrons_ of their nearest noble gas  positive ions_ form when the #of electrons_ are less than_ the # of protons_ This value is the __# of oxidation or the charge of the ion ___ Group 1 metals  ion 1+ Group 2 metals  ion 2+

• (^) Group 13 metals  ion 3+

Some Typical Ions with Negative Charges (Anions) _Group 15____ Group 16 Group 17 ____ ____ N 3- O 2- F 1- P 3- S 2- Cl 1- As 3- Se 2- Br 1- Sb 3- Te 2- I 1-

Names of Some Common Ions

Examples of Ionic Compounds with Two Elements Formula cation anion Name NaCl Na

Cl

K 2

S

MgO CaI 2 Al 2

O

3

Polyatomic Ions

• (^) Naming compounds with Polyatomic Ions: When

the anion is a Polyatomic ion, _write the name of

the polyatomic ion after the name of the

cation__.

• (^) never change the formula_ of the polyatomic ion

or the name_

• (^) Examples:

Na

2

(SO

4

Ba(ClO

3

2

Example #

Barium Nitride

Ba has a charge of 2+, N has a charge of 3-

Swap the charges or each element and use them as

subscripts in the formula ---> _Ba2(N3)______

If the oxidation number (charge) is the same

number for both elements, they cancel out.

Example # Calcium Oxide Ca ___ and O ____ Subscripts should always be in their _____. (This is called an _____ .)