1. Chemistry Review

2. Your Final! 15% of your Semester Grade 200 points 80 questions (2.5 pts each) 30% 1 st semester; 60% 2 nd semester; 10% labs All Multiple Choice You have class time ONLY for your final Bring Notes Page Calculator Pencil Snack?

3. Your Final! Work sheets from last night’s review Keys available in here (not online) Worksheets also available online Lab Final Countdown! ( _______ / _______ ) I will have them done by Monday, June 25

4. If a car is traveling at 75 km/hr, how many meters/second is it traveling? a. 21 m/sb. 0.021 m/s c. 1300 m/sd. 1.3 m/s Problem #1 A

5. Calculate the energy of a photon having a wavelength of 6.6 x 10 -5 cm. a.4.4 x 10 -38 J b.3.0x10 -19 J c.4.4x10 -36 J d.4.5x10 14 J Problem #2 B

6. Which element has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 ? a.Zn b.Ag c.Cu d.Au Problem #3 A

7. What is the name of the compound with the formula N 2 O 4 ? a. nitrous oxideb. nitrogen pentaoxide c. nitrogen oxided. dinitrogen tetraoxide Problem #4 D

8. Which of the following is the correct formula for copper(II) sulfite? a.Cu 2 SO 3 b.CuSO 3 c.CuSO 4 d.Cu 3 (SO 3 ) 2 Problem #5 B

9. In the following reaction, determine the identity of the products. AlCl 3(aq) + NaOH (aq)  a.Al(OH) 3(aq) + NaCl 3(aq) b.NaCl 3(aq) + AlOH (s) c. NaCl (s) + Al(OH) 3(aq) d.Al(OH) 3(s) + NaCl (aq) Problem #6 D

10. Calcium nitrate and sodium sulfide solutions react to form solid calcium sulfide and sodium nitrate solution. The spectator ions for the reaction above are: a) Ca 2+ and NO 3 - b) Na + and S 2- c) Ca 2+ and S 2- d) Na + and NO 3 - e) Ca 2+ and Na + Problem #7 D

11. Identify the correct coefficients ___Al(OH) 3 + ___ NaNO 3  ___ Al(NO 3 ) 3 + ___ NaOH a. 1, 3, 1, 3 b. 3, 1, 3, 1 c. 1, 1, 1, 3 d. 3, 1, 1, 1 Problem #8 A

12. A solution is made by dissolving 22.3 g of NaOH in enough water to make a 2.00 L solution. What is the molarity? a.0.279M b.0.558M c.1.11M d.0.140M Problem #9 A

13. A sample contains 40.g carbon, 6.7g hydrogen, and 53.3g oxygen. What is the empirical formula for this compound? a.C 2 H 4 O 2 b.C 40 H 7 O 54 c.C 3 H 6 O 3 d.CH 2 O Problem #10 D

14. Titrating a solution of 25.0 mL sodium hydroxide requires 42.5 mL of a 0.225M HCl solution. What is the molarity of the NaOH solution? a.0.132M b.9.56M c.0.383M d.0.225M Problem #11 C

15. Calculate the moles of oxygen gas formed when 1.20 moles of potassium chlorate, KClO 3, decomposes to produce potassium chloride, KCl, and oxygen gas in the following reaction. a.1.20 moles b.1.80 moles c.0.800 moles d.2.40 moles Problem #12 B

16. If 5.00 g of H 2 gas react with 20.0 g of O 2 gas to synthesize H 2 O, how many grams of H 2 O will be produced? a.44.6 g b.2.48 g c.22.5 g d.1.25 g Problem #13 C

17. If 20.00 g of magnesium react with excess oxygen and 28.00 g of magnesium oxide are produced, what is the percent yield? a)42.22 % b)60.31 % c) 71.43 % d) 84.44 % D Problem #14

18. For questions 15 and 16, consider the following balanced equation: 2 ZnS + 3 O 2  2 ZnO + 2 SO 2 If 3.00 moles of ZnS are combined with 4.00 moles of O 2, how many moles of ZnO can be produced? a)2.00 moles b) 2.67 moles c) 3.00 moles d) 5.67 moles B Problem #15

19. Information needed from question 15: B = 2.67 moles 2 ZnS + 3 O 2  2 ZnO + 2 SO 2 How many moles of the excess reactant will be left over after the reaction (Question 15) stops? a) 0.33 moles b) 1.00 moles c) 1.33 moles d) need more information A Problem #16

20. How much energy is needed to raise the temperature of 25.0g of H 2 O (l) from 10.0 o C to 35.0 o C? a.3.66 kJ b.2.61 kJ c.1.29 kJ d.366 J Problem #17 B

21. A sample of aluminum (0.895 J/g °C )at 75.0°C was placed in a calorimeter containing 25 grams of water at 20.0°C. The temperature stopped changing at 29.4°C. What is the mass of the sample? A.0.895g B.5.8g C.983g D.24g Problem #18 D

22. A balloon with a volume of 2.0 L at 1.0 atm pressure, is submerged underwater until the pressure is 5.0 atm. Assuming constant temperature, what will be its new volume? a.10. L b.2.0 L c.1.0 L d.0.40 L Problem #19 D

23. Nitrogen gas and hydrogen gas react to form ammonia gas (NH 3 ). If 6.0 L of hydrogen gas at STP reacts with an excess of nitrogen, how many liters of ammonia gas are produced at STP? a.6.0 L b.3.0 L c.9.0 L d.4.0 L Problem #20 D

24. Which ion is the smallest? a)Ga + b)Ge + c)Ge 2+ d)Ga C Problem #21

25. What is the shape of the BH 3 molecule? a.bent b.trigonal planar c.tetrahedral d.trigonal pyramidal Problem #22 B

26. Which of the following has the largest bond angle and what is the angle? a.PH 3 b.H 2 S c.CO 2 d.BH 3 Problem #23 c) 180˚

27. In which of the following would you expect to have hydrogen bonding? a) CH 3 OH b) CH 4 c) H 2 d) HI e) All of these Problem #24 A

28. A molecule with polar bonds can be nonpolar overall if ______. a) the bonds are ionic b) the individual dipoles cancel each other out c) the difference in eletronegativity is zero d) no halogens are involved Problem #25 B

29. A neutralization reaction between an acid and a base always produces a) salt and acidic anhydride. c) water and basic anhydride. b) salt and basic anhydride. d) salt and water. Problem #26 D

30. If 10.0 mL of 0.300 M KOH are required to neutralize 30.0 mL of gastric juice (HCl), what is the molarity of the gastric juice? A.0.900 M B.0.100 M C.0.300 M D.3.00 M Problem #27 B

31. Which of the following splits a neutron in to a proton and an emission particle? a.alpha decay b.beta decay c.fission d.fusion Problem #28 B

32. Problem #29 During an experiment to calculate specific heat, you measure the initial temperature of water in your calorimeter at 23.0 o C and the final temperature at 32.0 o C. What is the change in temperature recorded to the correct number of significant digits? a. 9 o Cb. 9.00 o Cc. 55.0 o Cd. 9.0 o C D

33. Problem #30 What type of reaction is: a.Alpha decay b.Beta decay c.Fusion d.Gamma decay A

34. Any Questions