1. Chemical Reactions Bonding Stoichio- metry Gas LawsSolutions 100 200 300 400 500 Jeopardy Trash Ball

2. Chem Rxns : 100 Identify the type of reaction and balance: NaOH + CaBr 2  Ca(OH) 2 + NaBr Back Answer: Double Replacement (2:1:1:2)

3. Back Identify the type of reaction and balance: H 2 O  H 2 + O 2 Answer: Decomposition (2:2:1) Chem Rxns : 200

4. Back Name all the types of chemical reactions and give their examples using A, B, C, and D. Answer: Synthesis (A + B  AB) Decomposition (AB  A + B) Single Replacement (AB + C  AC + B) Double Replacement (AB + CD  AD + CB) Chem Rxns : 300

5. Back How does the law of conservation of mass relate to chemical equations? Answer: Since matter cannot be created or destroyed, chemical equations must be balanced to account for all reactants and products. Chem Rxns : 400

6. Back What is the balanced word equation for this chemical reaction: FeCl 3 + Zn  Fe + ZnCl 2 Answer: 2 moles of iron (III) chloride reacts with 3 moles of zinc to yield 2 moles of iron and 3 moles of zinc chloride. Chem Rxns : 500

7. Back Identify the type of bonding and the name of CuCl 2. Answer: Ionic Bonding, Copper (II) Chloride Bonding : 100

8. Back Describe what happens in metallic bonding. Answer: Negatively charged electrons move freely around positively charged ions of metals which bonds the atoms together. Bonding : 200

9. Back Identify the type of bonding and name of H 2 O. Answer: Covalent, dihydrogen monoxide. Bonding : 300 BONUS

10. BONUS: 200 points Describe the electron distribution in the bonding of H 2 O. Answer: Polar bond because electrons more attracted to the oxygen atom. Back

11. Which bonding is stronger: ionic or covalent? Why? Answer: covalent because electrons are shared between the two atoms so more energy would be needed to separate the atoms. Bonding : 400

12. Back Which type of bonding allows molecules to conduct electricity strongly in solid phase? in aqueous phase? Why? Answer: Solid = metallic, because sea of electrons will allow electrons to pass through Aqueous = ionic, because dissociated ions are charged and will allow electrons to pass through Bonding : 500

13. Back How many moles of oxygen are needed to react with 4 moles of hydrogen? H 2 + O 2  H 2 O Answer: 2 moles of O 2 Stoichiometry : 100

14. Back If you have 2.5 moles of potassium sulfate, how many grams of potassium sulfate do you have? Answer: 453.10 g K 2 SO 4 Stoichiometry : 200

15. Back Define limiting and excess reactants. Answer: Limiting = substance completely used up in the reaction and determines how much product can be formed Excess: substance not completely used up in the reaction Stoichiometry : 300

16. Back You want to make 70 g of aluminum sulfate. How many grams of each reactant do you need? AlBr 3 + K 2 SO 4  KBr + Al 2 (SO 4 ) 3 Answer: 109.11 g AlBr 3 and 106.96 g K 2 SO 4 Stoichiometry : 400

17. Back If you have 50 g of oxygen and 100 g C 2 H 4, how many moles of water can you make? C 2 H 4 + O 2  CO 2 + H 2 O Answer: 1.04 moles H 2 O Stoichiometry : 500

18. Back What is the relationship between pressure and volume? Describe what its graph looks like. Answer: Inverse because as pressure increases, volume will decrease. The graph is a curve line with a downward slope. Gas Laws : 100

19. Back In Zain keeps 4 moles of gas in a container with a volume of 70 L at a temperature of 500 K, what is the pressure inside the container? Answer: 2.34 atm Gas Laws : 200

20. Back List all 5 gas laws and their equations. Answer: Charles (V1/T1=V2/T2) Lussac (P1/T1=P2/T2) Boyle (P1V1=P2V2) Combined (P1V1/T1=P2V2/T2) Ideal (PV=nRT) Gas Laws : 300

21. Back Mr. Kaplan has 72 L of a gas that he holds at a pressure of 3.4 atm and a temperature of 256 K. How many moles of gas does he have? Answer: 13.25 mol Gas Laws : 400

22. A gas has the following properties: volume of 17 L, pressure of 2.3 atm, and temperature of 150 K. If Ms. Yang doubles the temperature and decreases the pressure in half, what is the new volume of the gas? Answer: 68.00 L Back Gas Laws : 500

23. Back What is the equation to find molarity? (name the variables) Answer: Molarity (M) = number of moles of solute (n) / volume of solution (V) Solutions : 100

24. Back What is the equation for dilution molarity? (name the variables) Answer: Initial Molarity (M1) * Initial Volume (V1) = Final Molarity (M2) * Final Volume (V2) Solutions : 200

25. Back If beaker A is an unsaturated solution and we add more solute to the breaker, what should we expect to see happen to the number of solid and dissolved solute particles? Answer: dissolved = increase, solid = stay zero until solution is saturated Solutions : 300

26. Answer: 25 mL of solution A Back Solution A has a molarity of 0.5 M. If you want to make 50 mL of solution B which has a molarity of 0.25 M, how many milliliters of Solution A would you need? Solutions : 400

27. Back Solution C contains 3.0 moles of CaCO 3 in 400 mL. Solution D conatins 35 grams of H 2 SO 4 in 5.0 L of solution. Which solution is more concentrated? (mm CaCO 3 = 100.09 g/mol, mm H 2 SO 4 = 98.08 g/mol) Answer: Solution C (7.5 M) > Solution D (0.07 M) Solutions : 500