2. Chemical Reactions Chapter 7

3. A way to describe what happens in a chemical reaction. 1)Tells us what substances are involved with the reaction 2)Tells us how much of each substance is needed in a chemical reaction

4. Reactants & Products REACTANTS The substances that go into a chemical equation. Left side of the arrow PRODUCTS The substances produced or made in a chemical reaction Right side of the arrow

5. What do the numbers mean? Coefficients : the numbers placed in front of an element or compound. Tells us how many molecules or units of that substance are present. 3 NaOH Subscripts : the small numbers placed after and below an element or ion. Tells us how many atoms are present. CaCl 2

6. More chemical equations: Magnesium + oxygenmagnesium oxide Mg + O 2 MgO What is wrong with this equation?

7. Balancing Chemical Equations 1.Can only add or change coefficients NEVER subscripts. 2.Balance hydrogen atoms last. 3.Balance oxygen atoms second to last.

8. Law of Conservation of Mass Matter can neither be created nor destroyed. Developed by Antoine Lavoisier (1743-1794)

9. The Mole A special unit in chemistry used to measure the number of particles in a specific amount of mass. One mole equals exactly 6.02 x 10 23 atoms. (Avogadro’s number)

10. A mole is used the same way as:

11. Working problems with moles 1 mole of iron would have a mass of how many grams? 64 grams of sulfur is equal to how many moles? 1/2 or 0.5 moles of water has a mass of ?

12. 1. Synthesis reactions A type of chemical reaction where two or more reactants combine to form a single substance. General equation: A + B AB

13. Examples of synthesis reactions: Formation of salt from chlorine gas and solid sodium. Magnesium oxide formation. Rusting of metals

14. 2. Decomposition reactions When a complex substance breaks down into two or more simpler substances. Generic equation: AB A + B

15. Decomposition examples Electrolysis of water into hydrogen gas and oxygen gas. Production of cement. Sodium azide in safety air bags. Page 201

16. Single-Replacement reactions When an uncombined element replaces another element in compound. Generic equation: A + BCAC + B Which of the two combined elements are replaced?

17. “Like” replaces “like” Metals replace metals and non-metals replace non-metals. Examples: Zinc + copper sulfate Calcium + water Fluorine gas + potassium bromide

18. 4. Double Replacement Also known as ionic exchange reactions. Generic equation: AB + CD AD + CB Example: –Lead nitrate + potassium iodide

19. 5. Combustion reactions When a substance rapidly reacts with oxygen to produce light and/or heat. “burning” Example: Bunsen burner: methane + oxygen Sometimes these reactions are classified as synthesis reactions.

20. REDOX OXIDATION When a metal combines with oxygen. Rusting  Any process where an element loses electrons REDUCTION When an element gains electrons during a reaction.

21. Energy changes in chemical reactions 2 things that always change during a chemical reaction: 1.The properties of the reactants. 2.The amount of energy present. Energy change occurs because of breaking and formation of chemical bonds.

22. Exothermic reactions A chemical reaction that releases energy to its surroundings. Often in the form of heat. Reaction feels warm or hot. Examples: Mg + HCL

23. Endothermic reactions A chemical reaction that absorbs energy from its surroundings. Often feel cool. Examples: Ice-packs

24. Energy diagrams ExothermicEndothermic

25. Reaction rates Defined as how quickly a reaction occurs. Collision theory = The more collisions that occur at the atomic level the faster the reaction will go

26. Factors that affect rate of reaction 1)Temperature 2)Surface Area 3)Stirring 4)Concentration 5)Catalysts

27. TEMPERATURE Generally, the higher the temperature of the reactants the faster the rate of reaction.

28. SURFACE AREA The greater the surface area, the faster the rate of reaction. Example:

29. STIRRING Speeds up the molecules thus increasing the number of collisions

30. CONCENTRATION Defined as the number of particles in a given unit of volume. Example: 12 M HCl 6 M 1 M

31. CATALYSTS A substance that speeds up a reaction without being used up or directly involved in the reaction.