2.1.3

Ionic Compounds

Test yourself

Empirical Formulae

You can work out the proportion of each ion in a compound. The empirical formula of an ionic compound is the simplest ratio of ions possible.

Illustrative background for Ca<sup>2+</sup> and F<sup>-</sup>Illustrative background for Ca<sup>2+</sup> and F<sup>-</sup> ?? "content

Ca2+ and F-

  • In order for the charges to balance out and for the overall formula to be neutral, there must be 2 F- ions for each Ca2+ ion.
    • The empirical formula is CaF2
Illustrative background for Na<sup>+</sup> + SO<sub>4</sub><sup>2-</sup>Illustrative background for Na<sup>+</sup> + SO<sub>4</sub><sup>2-</sup> ?? "content

Na+ + SO42-

  • In order for the charges to balance out and for the overall formula to be neutral, there must be 2 Na+ ions for each SO42- ion.
    • The empirical formula is Na2SO4.

Jump to other topics

1Atomic Structure

2Chemical Bonding

3Quantitative Chemistry

4Chemical Changes

5Energy Changes

6The Rate & Extent of Chemical Change

7Organic Chemistry

8Chemical Analysis

9Chemistry of the Atmosphere

10Using Resources

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