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22.3 – Writing formulas and Naming Compounds

This guide covers the basics of binary ionic compounds, which consist of two elements. Learn how to write chemical formulas by identifying the elements involved and their oxidation numbers. The oxidation number indicates how many electrons an atom has gained, lost, or shared for stability. For example, sodium has a charge of 1+ and an oxidation number of 1+. When naming compounds with transition elements, the oxidation number is indicated using Roman numerals. Additionally, balance the total positive and negative charges to ensure the compound is neutral, applying the criss-cross method for subscripts.

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22.3 – Writing formulas and Naming Compounds

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  1. 22.3 – Writing formulas and Naming Compounds

  2. Binary Ionic Compounds • A binary compound is a compound composed of two elements • To write a chemical formula for a binary compound, you need to know: • which elements are involved • how many electrons they lose, gain, or share in order to become stable

  3. Oxidation Number • An oxidation number tells you how many electrons an atom has gained, lost, or shared to become stable • For ionic compounds the oxidation number is the same as the charge on the ion • For example, a sodium ion has a charge of 1+ and an oxidation number of 1+.

  4. Transition Elements • When naming these compounds, the oxidation number is expressed in the name with a Roman Numeral • For example, the oxidation number of iron in iron (III) oxide is 3+.

  5. Ionic Compounds are NEUTRAL • Although the individual ions in a compound carry charges, the compound itself is neutral • A formula must have the right number of positive ions and the right number of negative ions so the charges balance

  6. Example – Calcium Fluoride • A calcium ion has a charge of 2+ and a fluoride ion has a charge of 1- • You need two fluoride ions for every calcium ion in order for the charges to cancel and the compound to be neutral • The formula = CaF2

  7. Step By Step – Writing Formulas 1. Write the symbol of the element (or polyatomic ion) with the positive oxidation number or charge 2. Write the symbol of the element (or polyatomic ion) with the negative oxidation number or charge 3. The charge (without the sign) of one ion becomes the subscript of the other ion. • Reduce the subscripts to the smallest whole numbers that retain the ratio of ions.

  8. Criss-Cross Method

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