1. Movie: types of chemical reactions: http://www.youtube.com/watch?v=i-HHvx1VC_8

2. Identify, give evidence for, predict products of, and classify the following types of chemical reactions: 1. Synthesis (combination) 2. Decomposition 3. Single Replacement 4. Double Replacement 6. Combustion

3.  Synthesis  Decomposition  Single replacement  Double replacement  Combustion

4. A chemical change: any change in which a new substance is formed. Evidence of a Chemical Change:  Release of energy as heat  Release of energy as light  Change in colour  Formation of a gas  Change in odour…

5. 1.Synthesis: A + B  AB 2.Decomposition: AB  A + B 3.Single replacement: A + BC  AC + B 4.Double replacement: AB + CD  AD + CB 5.Combustion: AB + oxygen  CO 2 + H 2 O

6. –A + B  AB where A and B represent elements –The elements may form ionic compounds, like… –Sodium metal and chlorine gas combine to form sodium chloride. –2Na + Cl 2  2NaCl Sodium added to chlorine gas Synthesis reactions are also known as FORMATION reactions. Two or more reactants (usually elements) join to form a compound.

7. EXAMPLES… 1.Elements that form ionic compounds: Magnesium metal reacts with oxygen gas to form magnesium oxide. 2Mg + O 2  2MgO 2. Elements that form covalent compounds: Nitrogen gas and oxygen gas join to form dinitrogen monoxide. 2N 2 + O 2  2N 2 O

8. Decomposition reactions are the opposite of synthesis reactions. –A compounds breaks down into two or more products (often elements). –AB  A + B where A and B represent elements 1. Ionic compounds may decompose to produce elements, like the following: Table salt, sodium chloride, can be broken down into sodium metal and chlorine gas by melting salt at 800ºC and running electricity through it. 2NaCl  2Na + Cl 2

9. 2. Covalent compounds may decompose into elements, like the following: By running electricity through water, the water molecules decompose into hydrogen and oxygen gases. 2H 2 O  2H 2 + O 2

10. Single replacement reactions replace one element from a compound with another element. –A compound and an element react, and the element switches places with part of the original compound. A + BC  B + AC where A is a metal, or A + BC  C + BA where A is a non-metal

11. 1. When A is a metal: Aluminum foil in a solution of copper(II) chloride produces solid copper and aluminum chloride. 2Al + 3CuCl 2  3Cu + 2AlCl 3 2. When A is a non-metal: When fluorine is bubbled through a sodium iodide solution, iodine and sodium fluoride are produced. Fl 2 + 2NaI  I 2 + 2NaF

12. Double replacement reactions swap elements between 2 compounds that react together to form two new compounds. –Two compounds react, with elements switching places between the original compounds. AB + CD  AD + CB

13. –When potassium chromate and silver nitrate react, they form a red precipitate, silver chromate, in a solution of potassium nitrate. –K 2 CrO 4 + 2AgNO 3  Ag 2 CrO 4 + 2KNO 3 silver chromate Two solutions react to form a precipitate (solid) and another solution. Ionic solution + ionic solution  ionic solution + ionic solid. AB + CD  AD + CB

14. Combustion reactions occur when a compound or element react with oxygen to release energy and produce carbon dioxide and water. C X H Y + O 2  CO 2 + H 2 O where X and Y represent integers

15. 1. Natural gas (methane) is burned in furnaces to heat homes. »CH 4 + O 2  CO 2 + 2H 2 O + energy 2. An acetylene torch is used to weld metals together. »2C 2 H 2 + 5O 2  4CO 2 + 2H 2 O + energy 3. Carbohydrates like glucose combine with oxygen in our body to release energy. »C 6 H 12 O 6 + 6O 2  6CO 2 + 6H 2 O + energy Acetylene torch

16. http://www.youtube.com/watch?v=tE4668aarck http://www.youtube.com/watch?v=i-HHvx1VC_8