Question

I. Binary Ionic Compounds A. Metals with a single charge (Groups 1, 2 and Al) 1. To name a compound given the formula: a. 1st word: name of the cation (metal) b. 2nd word: root of the anion (nonmetal) + ide 2. To write a formula given the name: a. The cation is written first and the anion is written second. b. Since all compounds must be neutral overall, subscripts are used to indicate the number of cations and anions necessary to have the total positive charge equal the total negative charge. Cations: (Group 1A, IIA, IIIA) Na+ sodium ion Mg2+ magnesium ion Al3+ aluminum ion Monoatomic anions use root name and ide ending F1- fluoride Cl1- chloride Br1- bromide I1- iodide O2- oxide S2- sulfide N3- nitride P3- phosphide Examples : magnesium chloride Mg2+ + 2 Cl1- -> MgCl2 aluminum oxide 2 Al3+ + 3 O2- -> Al2O3

          I. Binary Ionic Compounds

A. Metals with a single charge (Groups 1, 2 and Al)

1. To name a compound given the formula:
a. 1st word: name of the cation (metal)
b. 2nd word: root of the anion (nonmetal) + ide

2. To write a formula given the name:
a. The cation is written first and the anion is written second.
b. Since all compounds must be neutral overall, subscripts are used to indicate the number of cations and anions necessary to have the total positive charge equal the total negative charge.

Cations: (Group 1A, IIA, IIIA)
Na+ sodium ion
Mg2+ magnesium ion
Al3+ aluminum ion

Monoatomic anions use root name and ide ending
F1- fluoride
Cl1- chloride
Br1- bromide
I1- iodide
O2- oxide
S2- sulfide
N3- nitride
P3- phosphide

Examples : magnesium chloride Mg2+ + 2 Cl1- -> MgCl2
aluminum oxide 2 Al3+ + 3 O2- -> Al2O3

I. Binary Ionic Compounds

A. Metals with a single charge (Groups 1, 2 and Al)

1. To name a compound given the formula:
a. 1st word: name of the cation (metal)
b. 2nd word: root of the anion (nonmetal) + ide

2. To write a formula given the name:
a. The cation is written first and the anion is written second.
b. Since all compounds must be neutral overall, subscripts are used to indicate the number of cations and anions necessary to have the total positive charge equal the total negative charge.

Cations: (Group 1A, IIA, IIIA)
Na+ sodium ion
Mg2+ magnesium ion
Al3+ aluminum ion

Monoatomic anions use root name and ide ending
F1- fluoride
Cl1- chloride
Br1- bromide
I1- iodide
O2- oxide
S2- sulfide
N3- nitride
P3- phosphide

Examples : magnesium chloride Mg2+ + 2 Cl1- -> MgCl2
aluminum oxide 2 Al3+ + 3 O2- -> Al2O3

Added by Brittany P.

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