 Chemical reactions are grouped according to patterns in the chemical formulas.

 Two reactants combine to make a larger or more complex product.

An example of a synthesis reaction is: 4 Al(s) + 3 O 2 (g) 2 Al 2 O 3 (s)

 Large compounds are broken down into smaller compounds or elements.

 One element displaces another element in a compound, producing a new compound and a new element. A + BC → AC + B

 In reactions with ionic compounds and metals, the positive ion (cation) is replaced. Copper + silver nitrate → copper (II) nitrate + silver Cu(s) + 2 AgNO 3 (aq) → Cu(NO 3 ) 2 (aq) + 2 Ag

 Metals rarely occur naturally as pure elements → ….single displacements often purify metals in order to use them.

 Two elements in different compounds trade places.  Two solutions that undergo a double displacement reaction produce an insoluble compound called a precipitate.

AB + CD → AD + BC

 An example of a double displacement reaction is Pb(NO 3 ) 2 (aq) + 2 KI(aq)  PbI 2 (s) + 2 KNO 3 (aq)  Word Equation?

Pb(NO 3 ) 2 (aq) + 2 KI(aq)  PbI 2 (s) + 2 KNO 3 (aq)  Lead (II) nitrate + potassium iodide  Lead (II) Iodide + Potassium nitrate

Pb(NO 3 ) 2 (aq) + 2 KI(aq)  PbI 2 (s) + 2 KNO 3 (aq)  Precipitate?

Pb(NO 3 ) 2 (aq) + 2 KI(aq)  PbI 2 (s) + 2 KNO 3 (aq)  Precipitate  ◦ lead (II) iodide, PbI 2 ◦ appears as a bright yellow insoluble solid.

Synthesis Reaction Decomposition Reaction Single Displacement Reaction Double Displacement Reaction Precipitate

Pg. 243 # 1, 3 – 5 Course Package Pg. 22, 23

 A chemical reaction in which the fuel reacts with oxygen  Commonly known as burning  Usually results in an oxide and energy (the flame)  Oxygen is known as an oxidizer

 If there is enough oxygen, all materials are burned completely Hydrocarbon + oxygen -> carbon dioxide + water + energy C x H y (g) + O 2 (g)-> CO 2 (g) + H 2 O (g) + energy

 If there is NOT enough oxygen, all materials are NOT burned completely Hydrocarbon + oxygen -> carbon dioxide + water + carbon monoxide + carbon + energy C x H y (g) + O 2 (g)-> CO 2 (g) + H 2 O (g) + CO(g) + C (s) + energy Creates carbon monoxide and soot

 Odourless, colourless gas  Highly toxic ◦ Carbon dioxide poisoning symptoms are nausea, headache, dizziness and respiratory problems  Maintain your furnace regularly and don’t leave your car running in your garage

 Particles of Carbon

 Element + Oxygen -> Element Oxide + Energy  Hydrogen ◦ 2H 2 (g) + O 2 (g) -> 2H 2 O(g) + energy  Magnesium ◦ 2Mg(s) + O 2 -> 2MgO + energy

 If Hydrogen is exposed to a flame it reacts and produces energy in the form of a “POP”  Produces water

 In Oxygen, a flame is encouraged  If a glowing splint enters a test tube of oxygen, it relights

 Carbon dioxide smothers a flame  If a flaming splint is exposed to carbon dioxide, the flame extinguishes

 Types of Reactions ◦ Pg 243 # 2-4, 8  Combustion ◦ Pg 251 # 2,3,5,6  Read Corrosion – Pg ◦ Make point form notes