1. Movie: types of chemical reactions: http://www.youtube.com/watch?v=i-HHvx1VC_8 Day 72

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 5. Neutralization (acid/base) 6. Combustion

3.  Synthesis  Decomposition  Single displacement  Double displacement  Neutralization  Combustion

4. 1.Take 3 pieces of paper and stagger them about ¾ “-1”. 2.Flip over so that the staggered layers are at the bottom of working area. 3.Fold top layers down from top – bottom while keeping the staggered layers somewhat consistent. 4.Crease fold well, then fold over about a ½” and staple 2-3 staples across the crease to hold together. 5.Label each tab with a different reaction type. 6.On the inside: split the pages in half with a line down the center a)write a description of the reaction type on the left side b)an example of that type of reaction using elements/compounds and an example of the reaction type using the letters A, B, C and/or D on the right c)And three examples of the reaction Types of Chemical Reactions Foldable

5. 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…

6. (c) McGraw Hill Ryerson 2007 Chemical reactions result in chemical changes. –Chemical changes occur when new substances are created. –The original substance(s), called reactants, change into new substance(s) called products. See pages 202 - 203

7. (c) McGraw Hill Ryerson 2007 Chemical reactions can be written in different ways. –A word equation: Nitrogen monoxide + oxygen  nitrogen dioxide –A symbolic equation: 2 gg 2 g2NO (g) + O 2(g)  2NO 2(g) STATE OF MATTER - Letters indicate the state of each compound. (aq) = aqueous/dissolved in water (s) = solid ( ) = liquid (g) = gas COEFFICIENTS - Indicates how many of each molecule there is. -: there are 2 molecules of NO.

8. 1.Neutralization: Acid(H) + Base(OH)  salt + H(OH) 2.Combustion: AB + oxygen  CO 2 + H 2 O 3.Synthesis: A + B  AB 4.Decomposition: AB  A + B 5.Single displacement: A + BC  AC + B 6.Double displacement: AB + CD  AD + CB

9. (c) McGraw Hill Ryerson 2007 –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 See pages 258 - 259 Sodium added to chlorine gas Synthesis reactions are also known as FORMATION reactions. Two or more reactants (usually elements) join to form a compound.

11. Types: Synthesis Example C + O 2 OO C +  OO C OO C OO C O O C O O C O O C O O C O O C O O C O O C O O C O O C O O C O O C O O C General: A + B  AB

12. (c) McGraw Hill Ryerson 2007 OTHER 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 See pages 258 - 259 SYNTHESIS REACTION (iron + sulphur): http://www.youtube.com/watch?v=A5H6DVe5FAI

13. (c) McGraw Hill Ryerson 2007 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 See page 260

14. (c) McGraw Hill Ryerson 2007 See page 260

15. Types: Decomposition Example: NaCl General: AB  A + B  Cl Na Cl + Na

16. Types: Decomposition Example 2HgO  O Hg O OO + General: AB  A + B

17. (c) McGraw Hill Ryerson 2007 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 See page 260 DECOMPOSITION REACTION: http://www.youtube.com/wa tch?v=NddwtXEA_Ak

18. (c) McGraw Hill Ryerson 2007 Single displacement 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 See page 261

20. Types: Single displacement Example: Zn + CuCl 2  Zn Cl Cu + General: AB + C  AC + B Cl Zn Cu +

21. 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 SINGLE REPLACEMENT: http://www.youtube.com/watch?v=hKtynbVtMKc

22. (c) McGraw Hill Ryerson 2007 Double Displacement 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 See page 262

23. (c) McGraw Hill Ryerson 2007 See page 262

24. Types: Double displacement Example: MgO + CaS General:AB + CD  AD + CB S O  Mg Ca + O S Mg Ca +

25. (c) McGraw Hill Ryerson 2007 –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 DOUBLE REPLACEMENT: http://www.youtube.com/watch?v=opY3FLrPTa4

26. (c) McGraw Hill Ryerson 2007 Neutralization reactions occur when an acid (most compounds starting with H) and a base (most compounds ending in OH) react to form a salt and water. Neutralization reactions are a type of double replacement. Acid + base  salt + water HOH HX + MOH  MX + H 2 O where X and M are elements See page 263

27. (c) McGraw Hill Ryerson 2007 1. Sulfuric acid is used to neutralize calcium hydroxide: H 2 SO 4 + Ca(OH) 2  CaSO 4 + 2H 2 O 2. Phosphoric acid helps to neutralize the compounds that cause rust, such as iron(II) hydroxide. H 3 PO 4 + 3Fe(OH) 2  Fe 3 (PO 4 ) 2 + 6H 2 O See page 263 NEUTRALIZATION: http://www.youtube.com/watch?v=_P5hGzA6Vb0

28. (c) McGraw Hill Ryerson 2007 Combustion reactions occur when a compound or element react with oxygen to release energy and produce an oxide. –Also sometimes referred to as hydrocarbon combustion. C X H Y + O 2  CO 2 + H 2 O where X and Y represent integers See page 264 METHANOL + oxygen: http://www.youtube.com/watch?v=98JuJ-G1qXY&feature=related

29. (c) McGraw Hill Ryerson 2007 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 See page 264 Acetylene torch

30. (c) McGraw Hill Ryerson 2007 See page 265 MOVIE TO REVIEW: http://www.bcscience.com/bc10/pgs/videos_013_chemical_reactions.html