1. Balancing Equations

2. Law of Conservation of Matter
Matter cannot be created or destroyed.
Equations must be balanced
Have equal numbers of each type of atom on each side.

3. Subscripts vs Coefficients
Subscript multiplies the element or polyatomic ion it is attached to
Small number to the right of symbol
Coefficient multiplies the whole compound it is next to
Big number in front of a compound

4. __Na + __H2O  __NaOH + __H2
Is it balanced?
__Na + __H2O  __NaOH + __H2
Place coefficients in the blanks to balance.
Mostly just trial and error.
Never change subscripts, b/c it changes the substance.
If polyatomic ions exist on both sides of the equation keep together as a group.
Coefficients have to be at the smallest ratio. So reduce if necessary

6. ___H2 + ___O2  ___H2O

7. ___Fe2O3 + ___ H2  ___ Fe + ___ H2O

8. __Al +__HAsO3  __H2 +__Al(AsO3)3

9. ___C6H14 + ___O2 → ___CO2 + ___H2O
Sometimes you end up with and odd # on one side and an even # on the other– multiply all coefficients by 2 then balance