2. A _________ is a substance that speeds up a chemical reaction without being permanently consumed in the reaction. catalyst

3. List the naturally occurring diatomic molecules. H 2, O 2, N 2, Cl 2, Br 2, I 2, F 2

4. Using collision theory, EXPLAIN why increasing the temperature of a reaction increases the reaction rate? Increasing the temperature also increases the kinetic energy of the reacting molecules. So molecules are moving faster and will collide more often. More collisions = faster reaction rate!

5. _____________ is the speed of the disappearance of a reactant or the rate of the appearance of a product in a chemical reaction. Reaction rate

6. Equations must always be balanced because a certain law of chemistry cannot be violated. What is the name of the law that cannot be violated? Law of Conservation of Matter

7. The arrow between the reactants and products means__________. yields

8. List the four indicators that a chemical reaction occurred. Heat/light Precipitate Gas (bubbles) Color change

9. In a chemical equation, what is indicated by the  symbol? Heat is added to the reaction

10. In a chemical equation, what is indicated by the symbol? A precipitate is formed

11. What are the 4 factors that affect the reaction rate? Temperature Concentration Nature of Reactants Catalyst

12. List the reactants in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) CH 4 + 2O 2

13. Using collision theory, EXPLAIN why increasing the concentration of a reactant increases the reaction rate? More molecules are present as the concentration is increased. So more molecules present equals more collisions between reacting molecules. More collisions = faster reaction rate!

14. In a chemical equation, what is indicated by the H 2 SO 4 symbol? That H 2 SO 4 was used as a catalyst is this reaction

15. List the products in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) CO 2 + 2H 2 O

16. How many atoms of O are in 2H 2 O following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 2

17. What is does the represent in the following equation: 2H 2 + O 2 2H 2 O A reversible reaction. The reaction can go both ways- reactants yield products and product can yield reactants

18. What type of reaction would the following be classified as? AB + CD AD + CB Double displacement

19. Suppose in the following reaction that 10g of Mg was added to 14g of O 2, how many grams of MgO would be produced? 2Mg (s) + 2O 2 (g) 2MgO (s) 24 g – b/c the Law of Conservation of Matter (the amount of matter you start with is the same amount that you end with!)

20. How many atoms of C are in CO 2 following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 1

21. How many moles of CH 4 are present following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 1

22. What ions are present for H 2 0? H+ and OH-

23. How many molecules of 2O 2 are present following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 2

24. Which of the following substances would be a gas that is produced in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) CO 2

25. What type of reaction would the following be classified as? A + B AB Synthesis

26. Which type of reaction has only one REACTANT? Decomposition

27. What type of reaction would the following be classified as? A + BC AC + B Single displacement

28. Which of the following substances would be a liquid in the following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 2H 2 O

29. How many molecules of CH 4 are present following equation: CH 4 (g) + 2O 2 (g) CO 2 + 2H 2 O ( l ) 1

30. What ion is ALWAYS present in any acid? H+

31. Which type of reaction has only one PRODUCT being produced? Synthesis

32. What does (aq) represent after a substance? Aqueous – substance was dissolved in water

33. Is the following reaction correct? Explain. 2Mg (s) + 2O 2 (g) 2PbO (s) NO! – b/c the Law of Conservation of Matter (the same types of atoms must be present on both sides of the equation. Mg can’t be changed into Pb!

34. What type of reaction would the following be classified as? AB A + B Decomposition

35. Balance the following equation: potassium + water potassium hydroxide + hydrogen 2K + 2H 2 O 2KOH + H 2

36. Balance the following equation: fluorine + aluminum oxide aluminum fluoride + oxygen 6F 2 + 2Al 2 O 3 4AlF 3 + 3O 2

37. Identify the type of reaction. Finish the word equation & write the balanced equation: Aluminum + hydrochloric acid Single Displacement Aluminum chloride + hydrogen 2Al + 6HCl 2AlCl 3 + 3H 2

38. Identify the type of reaction. Finish the word equation & write the balanced equation: calcium fluoride + water Double Displacement Calcium hydroxide + hydrogen fluoride CaF 2 + 2H 2 O Ca(OH) 2 + 2HF

39. Identify the type of reaction. Finish the word equation & write the balanced equation: potassium oxide Decomposition potassium + oxygen 2K 2 O 4K + O 2

40. Identify the type of reaction. Finish the word equation & write the balanced equation: strontium + chlorine synthesis Strontium chloride Sr + Cl 2 SrCl 2 *Balanced