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Chemical equation the symbolic representation of a chemical reaction (process) wherein the

Chemical equation the symbolic representation of a chemical reaction (process) wherein the reactant entities are on left side and change into product entities on right-hand side. Chemical Equation Symbols The arrow  can be read as “yields” or “produces”

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Chemical equation the symbolic representation of a chemical reaction (process) wherein the

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  1. Chemical equation the symbolic representation of a chemical reaction (process) wherein the reactant entities are on left side and change into product entities on right-hand side

  2. Chemical EquationSymbols The arrow  can be read as “yields” or “produces” The + sign reads as “and” or “plus”

  3. Chemical EquationSymbols The arrow  can be read as “yields” or “produces” Coefficients are the numbers in front of the formulas Coefficients can be changed to balance chemical equations Subscripts tell us how many atoms or molecules we have NEVER change subscripts when balancing chem. equations

  4. Br2 + Al  Al2Br6 (not balanced) Balance using coefficients Balancing Equations like solving a puzzle

  5. Balancing Equations Reactants  Products O2 + H2  H2O

  6. Balancing Equations Reactants  Products O2 + H2  H2O but this equation is not balanced why not?

  7. Conservation of Mass- Mass and/or Atoms are not Created or Destroyed during a chemical reaction. There must be the Same number of atoms on each side of the equation to balance the chemical equation. Balancing Equations

  8. Steps to Balance Chemical Equations 1. Write unbalanced equation. 2. Count # atoms on each side. 3. Add coefficients to make #s of atoms equal. Coefficient  subscript = # of atoms 4. If necessary reduce coefficients to lowest possible ratio (never change subscripts) • Update and Double check atom balance!!!

  9. Balancing Equations Step 1. Write unbalanced equation O2 + H2  H2O

  10. Balancing Equations Step 2. Count # of atoms on each side O2 + H2  H2O O = 2 0 = 1 H = 2 H = 2

  11. Balancing Equations 3. Add coefficients to make # of atoms = on each side O2 + H2  H2O O = 2 0 = 1 H = 2 H = 2

  12. Balancing Equations 3. Add coefficients to make # of atoms = on each side O2 + 2 H2  2 H2O O = 2 0 = 2 H = 4 H = 4

  13. Balancing Equations 4. If necessary find lowest ratio (never change subscripts) O2 + 2 H2  2 H2O O = 2 0 = 2 H = 4 H = 4

  14. Balancing Equations 5. Update and double check work O2 + 2 H2  2 H2O O = 2 0 = 2 H = 4 H = 4

  15. Balancing Steps 1. Write the unbalanced equation. Al + CuCl2 Cu + AlCl3

  16. Balancing Steps 1. Write the unbalanced equation. 2. Count atoms on each side. Al + CuCl2 Cu + AlCl3 1 Al 1 1 Cu 1 2 Cl 3

  17. Balancing Steps 1. Write the unbalanced equation. 2. Count atoms on each side. 3. Add coefficients to make #s equal. Coefficient  subscript = # of atoms Al + CuCl2 Cu + AlCl3 1 Al 1 1 Cu 1 2 Cl 3

  18. Balancing Steps 1. Write the unbalanced equation. 2. Count atoms on each side. 3. Add coefficients to make #s equal. Coefficient  subscript = # of atoms Al + 3 CuCl2 Cu + 2 AlCl3 1 Al 2 3 Cu 1 6 Cl 6

  19. Balancing Steps 1. Write the unbalanced equation. 2. Count atoms on each side. 3. Add coefficients to make #s equal. Coefficient  subscript = # of atoms 2 Al + 3 CuCl2 3 Cu + 2 AlCl3 2 Al 2 3 Cu 3 6 Cl 6

  20. Balancing Steps 1. Write the unbalanced equation. 2. Count atoms on each side. 3. Add coefficients to make #s equal. Coefficient  subscript = # of atoms 4. Reduce coefficients to lowest possible ratio, if necessary. 5. Double check atom balance!!!

  21. Helpful Tips • Balance one element at a time. Balance most complicated compound first! • Update ALL atom counts after adding a coefficient. • Balance (polyatomic ions) as (single units). • “1 SO4” instead of “1 S” and “4 O” • Balance most complicated compound first, balance oxygen and hydrogen last (MINOH metals, ions, non-metals, oxygen, hydrogen) • Ask yourself this question what am I forced to do to balance the equation???

  22. Examples ____ Mg + ____ O2 ____ MgO

  23. Examples 2 Mg + O2 2 MgO

  24. Examples ____ Al + ____ S  ____ Al2S3

  25. Examples 2 Al + 3 S  Al2S3 ____ C3H8 +____ O2 ____ CO2 + ____ H2O

  26. Examples 2 Al + 3 S  Al2S3 C3H8 + 5 O2 3 CO2 + 4 H2O

  27. More Examples ___ Al +____ H2SO4 ____Al2(SO4)3 +____ H2

  28. More Examples 2 Al + 3 H2SO4 Al2(SO4)3 + 3 H2

  29. Helpful Tips • Balance one element at a time. • Update ALL atom counts after adding a coefficient. • Balance (polyatomic ions) as (single units). • “1 SO4” instead of “1 S” and “4 O” • Balance most complicated compound first, balance oxygen and hydrogen last • Ask yourself this question what am I forced to do to balance the equation???

  30. Steps to Predicting Products • Determine Reaction Type • Predict Product Formulas • Verify subscripts on Product Formulas • Final Step Balance Equation

  31. Determine Reaction Type • Predict Product Formulas • Verify subscripts on Product Formulas • Final Step Balance Equation Ag + Cu(SO4) 

  32. Determine Reaction Type • Predict Product Formulas • Verify subscripts on Product Formulas • Final Step Balance Equation Ag + Cu(SO4) 

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