New Stuff 2014… The Saga Continues!!!

Law of Conservation of Matter Law of Conservation of Mass Law of Conservation of Energy None of these can be created nor destroyed

Balancing a Chemical Reaction There are two parts –Reactants: What we start with –Products: What we end with They must be equal!!! THEY MUST BE EQUAL!!!

Symbols in a Reaction +Separates products and reactants →Separates reactants from products ↔,  Separates reactants from products and indicates a reversible reaction (s)Solid (l)Liquid (g)Gas (aq)Water solution

Water H 2 O H 2 + O 2 → H 2 O Reactants Products

Balance The Reaction You can NOT change a subscript!!!!! If you change a subscript, you change the chemical. You can NOT change a subscript!!!!!

Balance the Reaction Look at this reaction: H 2 + O 2 → H 2 O That gives us: 2 H + 2 O → 2 H + 1 O 2 H + 2 O ≠ 2 H + 1 O

Balance the Reaction To get the reaction to balance, we need to add a coefficient to the reaction. A coefficient changes the amount of material you put into the reaction.

Balance the Reaction When I put a coefficient in front of a chemical, I have added additional “buckets” of stuff. H 2 + O 2 → H 2 O If I place the #2 in front of H 2 O… H 2 + O 2 → 2 H 2 O

Balance the Reaction It means that I have 2 “Buckets” of water. H 2 + O 2 → 2 H 2 O 2 H + 2 O → 4 H + 2 O 2 H + 2 O ≠ 4 H + 2 O Closer… But not quite…

Balance the Reaction I need to increase the number of hydrogen molecules. If I add a coefficient to the H 2, I can balance it out. 2 H 2 + O 2 → 2 H 2 O 4 H + 2 O = 4 H + 2 O (The peasants rejoice)

Balance K Cl → K + Cl 2 2 K Cl → 2 K + Cl 2

Balance Be Cl 2 + H 2 O → Be O + H Cl Be Cl 2 + H 2 O → Be O + 2 H Cl

Balance Na Cl → Na + Cl 2 2 Na Cl → 2 Na + Cl 2

Balanced? H Cl + Na O H → H 2 O + Na Cl 2Fe 2 O 3 + 3C → 4Fe + 3C O 2

Balance Ca Cl 2 → Ca + Cl 2 Al Cl 3 → Al + Cl 2 Al 2 O 3 + H 2 → Al + H 2 O

More New Stuff!!!

Types of Reactions Synthesis Decomposition Single replacement Double replacement Combustion

Types of Reactions Synthesis A + B → A B

Types of Reactions Decomposition A B → A + B

Types of Reactions Single replacement A B + C → A C + B

Types of Reactions Double replacement A B + C D → A D + C B

Types of Reactions Combustion A + O 2 → Stuff + Heat + Light

Think about H2 O as H (O H) for most of the reactions.

Balance K Cl → K + Cl 2 H Cl + Na O H → H (O H) + Na Cl Fe 2 O 3 + C → Fe + C O 2 H 2 + O 2 → H (O H)

Balance 2 K Cl → 2 K + Cl 2 H Cl + Na O H → H (O H) + Na Cl 2 Fe 2 O C → 4 Fe + 3 C O 2 2 H 2 + O 2 → 2 H (O H)

K Cl → K + Cl 2 Decomposition H Cl + Na O H → H 2 O + Na Cl Double replacement Fe 2 O 3 + C → Fe + C O 2 Single replacement H 2 + O 2 → H (O H) Synthesis

2K Cl → 2K + Cl 2 Decomposition H Cl + Na O H → H 2 O + Na Cl Double replacement 2Fe 2 O 3 + 3C → 4Fe + 3C O 2 Single replacement 2H 2 + O 2 → 2H (O H) Synthesis

Additional New Stuff!!!

Types of Reactions Synthesis Decomposition Single replacement Double replacement Combustion

Balance and Identify K 3 N → K + N

Balance and Identify In your notes for practice: K (O H) + H Cl → K Cl + H (O H) Ca (O H) 2 + H Br → Ca Br 2 + H (O H) B 2 O 3 → B + O 2 C 6 H 12 O 6 + O 2 → C O 2 + H 2 O H (O H) + Na → Na (O H) + H 2 Al + Cl2 → Al Cl 3

Balance and Identify K (O H) + H Cl → K Cl + H (O H) Double Replacement Ca (O H) 2 + 2H Br → Ca Br 2 + 2H (O H) Double Replacement 2 B 2 O 3 → 4 B + 3 O 2 Decomposition C 6 H 12 O O 2 → 6 C O H 2 O Combustion 2 H (O H) + 2 Na → 2 Na (O H) + H 2 Single replacement 2 Al + 3 Cl 2 → 2 Al Cl 3 Synthesis

Balance and Identify Quiz: New page in notebook… Na (O H) + H I → Na I + H (O H) Li 2 S + K (O H) → Li (O H) + K 2 S Cu Cl 2 + Na → Na Cl + Cu C 6 H 12 O 6 → C + H 2 O Ag Cl + Na 2 (S O 4 ) → Ag 2 (S O 4 ) + Na Cl

Answers Na (O H) + H I → Na I + H (O H) Double Replacement Li 2 S + 2 K (O H) → 2 Li (O H) + K 2 S Double Replacement Cu Cl Na → 2 Na Cl + Cu Single Replacement C 6 H 12 O 6 → 6 C + 6 H 2 O Decomposition 2 Ag Cl + Na 2 (S O 4 ) → Ag 2 (S O 4 ) + 2 Na Cl Double Replacement