1. U NIT E XAM R EVIEW Lesson Objective: Students will have a clear expectation of how learning will be demonstrated on the unit exam.

2. 55 Multiple Choice Questions 13 Questions on Chapter 1 13 Questions on Chapter 2 15 Questions on Chapter 3 14 Questions on Chapter 2

3. “P ROJECT M ONTH ” IN J ANUARY Additional assessments requiring higher level thinking, and creativity/producing curricular content. Aren’t you lucky?!

4. R EVIEW … Class notes… do you remember why aluminum foam is used to create safer, lighter cars? What MRE’s are? How food is freeze dried? Super quick review of lab safety symbols (one question) Review the particle theory of matter (states of matter) and definitions of deposition and sublimation. Review the difference between physical and chemical properties of matter- know the definitions and be able to give examples.

5. P HYSICAL P ROPERTIES CHART ON PAGE 99 IN TEXT : Melting Point Boiling Point Hardness (Mohs’ Hardness Scale) Malleability Ductility Crystal Shape Solubility Density Conductivity

6. C HEMICAL P ROPERTIES OF M ATTER ( PAGE 102) How a substance reacts with other substances: Reaction with acids Ability to burn Reaction with water Behaviour in air Reaction to heat Evidence of a chemical change: chemical change always results in the formation of a different substance or substances. What evidence do you look for?

7. Colour Odour Formation of a gas.

8. T YPES OF P URE S UBSTANCES - MADE OF ONLY ONE TYPE OF MATTER AND HAS A UNIQUE SET OF PROPERTIES Element- cannot be broken down into simpler substances. Compounds- when two or more elements combing chemically.

9. 4 TYPES OF MIXTURES, AND BE ABLE TO DESCRIBE THEM Mechanical Mixture Solution Suspension Colloid You will be tested on the chart on page 103 in the text!

10. There are 7 questions on the timeline/history of chemistry. No problem, because you have all completed your timeline!! Review text pages 113-120.

11. 20 QUESTIONS BASED DIRECTLY ON THE PERIODIC TABLE Review class notes online… Period, group, alkali metals (group 1), alkaline- earth metals (group 2), halogens (group 17), noble gasses (group 18). Differences between ionic and molecular compounds, and rules for naming them. Definition of polyatomic ions How to balance ionic equations.

12. T ABLE, PAGE 152 Number of AtomsPrefix 1mono 2di 3tri 4tetra 5penta

13. C HEMICAL R EACTIONS Remember that chemical reactions take place when 2 or more substances combine to form new substances. The materials at the start of a reaction are called reactants. The new materials produced by the reaction are called the products.

14. C AMPFIRE E XAMPLE The burning wood undergoes a combustion reaction. The reactants, or substances being combined in the reaction, are wood and oxygen. The new materials being formed, or products, are carbon dioxide and water- they are formed while energy is released.

15. A C HEMICAL R EACTION CAN BE WRITTEN AS A W ORD E QUATION : Wood + Oxygen Carbon dioxide + water + energy released. Plus signs separate the reactants from each other and the products from each other. The arrow indicates the direction in which the reaction is most likely to occur. Reactions can occur in either direction.

16. R EMEMBER THAT SOMETIMES TESTING IN THE LAB MAY BE NEEDED TO PROVE A CHEMICAL REACTION HAS OCCURRED. For example, the formation of bubbles in a solution doesn’t always mean that a new gas is being produced in a chemical reaction… could just be evidence of boiling. Evidence of heat being released or absorbed may also indicate a physical change rather than a chemical change. Some solids, for example, release heat when they are dissolved.

17. E VIDENCE OF A CHEMICAL REACTION MAY INCLUDE ONE OR MORE OF THESE : A colour change The formation of an odour The formation of a solid or a gas The release or absorption of heat

18. E NDOTHERMIC VS E XOTHERMIC R EACTIONS Exothermic reaction: a chemical reaction that releases heat energy. E.g. When you burn an object in the presence of oxygen, or when your body metabolizes food. Endothermic reaction: a chemical reaction that absorbs heat energy. E.g. Chemical cold packs in first aid kids, or when the temperature drops just after the reaction of baking soda and vinegar. Endothermic and exothermic reactions involve the forming or breaking of chemical bonds.

19. C HEMICAL C HANGES I NVOLVING O XYGEN Among the most common types of chemical reactions. Three examples: Combustion- E.g. Fire. Combustion could be considered the first chemical reaction used by humans. Combustion occurs when oxygen reacts with a substance to form a new substance and give off energy.

20. C ORROSION Corrosion is the slow chemical change that occurs when oxygen reacts with a metal. E.g. Rusting occurs when iron reacts with oxygen to form iron oxide. Cellular respiration: is a chemical reaction that takes place in the cells of your body. Food (glucose) reacts with oxygen to produce energy, water, and carbon dioxide.

21. C ONSERVATION OF M ATTER In a chemical reaction, products are formed when the reactant(s) undergo a change. The products usually look very different than the reactants. The total mass of these products, however, is always the same as the total mass of the reactants. This law is called the conservation of matter.

22. Matter is neither created or destroyed in a chemical reaction. Experiments have been done in closed systems where no additional material is allowed to enter or to leave. The result? No exceptions to this law have ever been found in any chemical reaction.

23. O PEN S YSTEMS Sometimes the products of a chemical reaction can escape into the air… when Alka-Seltzer is dissolved in water, the products left in a beaker will not be the same as the mass in the beginning of the experiment. Carbon dioxide gas will be given off into the air- this is an example of an open system. If the carbon dioxide is “trapped” the mass would be the same. In a nuclear reaction, some of the mass is converted to energy, as Albert Einstein expressed as his famous E=mc 2

24. F ACTORS A FFECTING THE R ATE OF A C HEMICAL R EACTION : If you’ve ever coloured your hair and ended up with a burned scalp, or odd colour… Or baked a cake and ended up with batter that rose too high, or not enough… You have realized that certain factors can affect the rate of a chemical reaction: 1. The presence of a catalyst 2. The concentration of the reactants 3. The temperature of the reactants 4. The surface area of the reactants

25. C ATALYSTS Are substances that help a reaction proceed faster. They are present with the reactants, but are not consumed (used up) during a reaction. Chemical reactions involving catalysts can be found in living and non-living things. Many reactions, such as the breakdown of food, require a catalyst called an enzyme.

26. Without enzymes, may reactions would require higher temperatures… Which would be deadly to the human body. Enzymes can help get rid of poisons in the body quickly. An enzyme called catalase, which is found in many types of animal and plant cells, speeds up the breakdown of hydrogen peroxide into harmless oxygen and water.

27. C ONCENTRATION : The greater the concentration of the reactants, the faster the reaction. The increased concentration of the reactants means that there are more atoms of each reactant available to react.

28. T EMPERATURE The more heat added to the reactants, the faster the reaction. The added heat causes the atoms of each reactant to move faster.

29. S URFACE AREA Increasing the surface area of the reaction is another factor that can increase the rate of a reaction. The greater surface area of the reactants means that more area is available for reaction.