Balancing Chemical Reactions Part 1

Balancing Chemical ReactionsPart 1

Balancing Chemical Reactions Reactants: Zn + I2 Product: Zn I2

Chemical Equations Depict the kind of reactants and productsand their relative amounts in a reaction. 4 4 Al (s) + 3 O2(g)---> 2 Al2O3 (s) The blue numbers are called subscripts. The numbers in the front are called coefficients. The letters (s) and (g) are the physical states of compounds.

Parts of a Reaction Equation • Chemical equations show the conversion of reactants (the molecules shown on the left of the arrow) into products (the molecules shown on the right of the arrow). • A + sign separates molecules on the same side • The arrow is read as “yields” • Example 2H2 (g) + O2 (g)  2H2O (l) This reads “hydrogen gas plus oxygen gas reacts to yield dihydrogen monoxide liquid.”

Lavoisier, 1788 Chemical Equations Because of the principle of the conservation of matter, an equation must be balanced. It must have the same number of atoms of the same kind on both sides.

Symbols Used in Equations • Solid (s) • Liquid (l) • Gas (g) • Aqueous solution (aq) • Catalyst H2SO4 • Heated ()

Balancing Equations • When balancing a chemical reaction you may add coefficients in front of the compounds to balance the reaction, but you may not change the subscripts. • Changing the subscripts changes the compound. Subscripts are determined by the valence electrons (charges for ionic or sharing for covalent)

Subscripts vs. Coefficients • The subscripts tell you how many atoms of a particular element are in a compound. The coefficient tells you about the quantity, or number, of molecules of the compound.

Balancing Chemical ReactionsPart 2

Chemical Equations 4 Al(s) + 3 O2(g) ---> 2 Al2O3(s) This equation means 4 Al atoms + 3 O2 molecules ---produces---> 2 molecules of Al2O3

Ag + Cl2 AgCl Total atoms 1 2 1 1 Both sides must be equal for ALL atoms.

2 Ag + Cl2 AgCl Total atoms 1 2 1 1 2 2 Both sides must be equal for ALL atoms.

2 2 Ag + Cl2 AgCl Total atoms 1 2 1 1 2 2 2 Both sides must be equal for ALL atoms.

CH4 + O2 CO2+ H2O 1 2 1 2 4 2 1

CH4 + O2 CO2+ H2O 2 1 2 1 2 4 2 1 2 4

CH4 + O2 CO2+ H2O 2 2 1 2 1 2 4 2 1 2 4 4

Steps to Balancing Equations There are four basic steps to balancing a chemical equation. 1. Write the correct formula for the reactants and the products. DO NOT TRY TO BALANCE IT YET! You must write the correct formulas first. And most importantly, once you write them correctly DO NOT CHANGE THE FORMULAS! 2. Find the number of atoms for each element on the left side. Compare those against the number of the atoms of the same element on the right side.

Steps to Balancing Equations 3. Determine where to place coefficients in front of formulas so that the left side has the same number of atoms as the right side for EACH element in order to balance the equation. 4. Balance in the following order: Metals, Nonmetals, Oxygen & Hydrogen (whichever one is by itself…do last) 5.Check your answer to see if: • The numbers of atoms on both sides of the equation are now balanced. • The coefficients are in the lowest possible whole number ratios. (reduced)

Balancing Chemical Reactions From Words

Converting and Balancing Word Equations Sodium phosphate + iron (III) oxide  sodium oxide + iron (III) phosphate Na3PO4+ Fe2O3 Na2O + FePO4 2 3 2

Converting Word Equations into Chemical Equations #10 Strontium iodide + Lead (II) phosphate  Strontium phosphate + lead (II) iodide SrI2 + Pb3(PO4)2 Sr3(PO4)2+ PbI2 3 3

Converting and Balancing Word Equations Silver phosphate + aluminum oxide  silver oxide + aluminum phosphate Ag3PO4 + Al2O3 Ag2O + AlPO4 2 2 3

Converting Word Equations into Chemical Equations Calcium iodide + tin (II) phosphate  calcium phosphate + tin (II) iodide CaI2+ Sn3(PO4)2 Ca3(PO4)2+ SnI2 3 3

Balancing Chemical Reactions Part 1