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Chemical Formulas and Equations

Learn the basics of chemical formulas: coefficients, subscripts, and determining atoms. Explore chemical equations with reactants and products, understanding the arrow and conservation of mass law. Practice with examples like CO2 and N2O.

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Chemical Formulas and Equations

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  1. Chemical Formulas and Equations

  2. Parts of a formula • Coefficient: the number in front of the symbol, which tells you how many molecules there are. • Subscript: The number after the symbol, which tells you how many atoms there are for each element.

  3. Determining how many atoms • Multiply the coefficient by the subscript • Use a 1 for any coefficient or subscript that is missing

  4. Example 5H2 • Coefficient: • Subscript: • Element: • How many atoms?

  5. Example 5H2 • Coefficient: 5 • Subscript: 2 • Element: hydrogen • How many atoms? 5 x 2 = 10

  6. Practice • 3 CO2 • N2O • 5MgCl2 • 2 C6H12O6 Try the ones on the back of the page!

  7. Practice • 3 CO2 C = 3, O = 6 • N2O N = 2, O = 1 • 5MgCl2 Mg = 5, Cl = 10 • 2 C6H12O6 C = 12, H = 24, O = 12 Try the ones on the back of the page!

  8. Chemical equations A chemical equation is a short way to describe a chemical reaction Reactants: the starting materials in a chemical reaction (before the arrow) Products: the new substances made in a chemical reaction (after the arrow) Example: C + O2 CO2 Reactants: C (carbon) and O2 (oxygen) Products: CO2 (carbon dioxide)

  9. Chemical equations continued • What does the arrow mean? • Yields or gives you • What does the “+” mean? • “and” • Law of conservation of mass: • Atoms are not created nor destroyed • You have to have the same number of each element on both sides of the equation

  10. Let’s practice • Take out the last sheet you picked up on your way in • Let’s do the first one together

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