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Chemical Equations and Balancing in Chemistry

Learn about chemical reactions, balanced equations, coefficients, states of matter, and how to balance equations step by step. Avoid common mistakes and master the art of writing chemical equations correctly in your chemistry studies.

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Chemical Equations and Balancing in Chemistry

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  1. Chemical Reactions Chem 332 – O’Dette

  2. Chemical Equation • Reactants Products yield

  3. Symbols/States of Matter • = heated • (s) = solid • (l) = liquid • (g) = gas • (aq) = aqueous ; substance is dissolved in water

  4. Balanced Equations • A equation must have the same number of atoms on each side of the equation • Equations are balanced by using coefficients 3 O2 Coefficient Subscript

  5. Subscript vs. Coefficient

  6. Steps for Balancing Equations Example: Write the equation and states of matter for the reaction of magnesium + aqueous silver nitrate to yield aqueous magnesium nitrate + silver • Write the equation using the correct formula Mg (s) + AgNO3 (aq) Mg(NO3)2 (aq) + Ag (s)

  7. Steps for Balancing Equations • Determine if the equation is balanced **Keep polyatomics together if they are on both sides of the equation R(reactants) P(products) 1 Mg 1 Mg 1 Ag 1 Ag 1 NO3 2 NO3 Balance Balance Not Balance

  8. Steps for Balancing Equations • Balance one element/polyatomic at a time using coefficients ****Balance O and H last!!!! Mg (s) + AgNO3(aq) Mg(NO3)2 (aq) + Ag (s) 2 2

  9. Steps for Balancing Equations • Check to see if balanced R P 1 Mg 1 Mg 2 Ag 2 Ag 2 NO3 2 NO3 Balance Balance Balance

  10. Example • Write the equation and states of matter for the reaction of oxygen and aluminum to yield aluminum oxide 3 O2 + 4 Al 2Al2O3

  11. Common Mistakes • Forgetting diatomics (HOBrFINClor Big 7) • Forgetting special cases (S8 or P4) • Changing subscripts (DO NOT CHANGE SUBSCRIPTS)

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