g. is flammable h. sample size is 55 ml d. Flammability g. slicing a tomato h. the baking of a potato c. digesting your lunch

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1 Chemistry Ch. 10 & Final Exam Review Mary Stangler Center for Academic Success This review is meant to highlight basic concepts from the units covered in this course. It does not cover all concepts presented by your instructor. Refer back to your notes, unit objectives, labs, handouts, etc. to further prepare for your exam. 1. Define the following as either a chemical or physical property: Label as C or P. a. Ability to support combustion f. Inertness b. Colorless liquid c. Corrosiveness g. is flammable h. sample size is 55 ml d. Flammability i. density e. has an odor 2. Define the following as either a chemical or physical change: Label as either C or P. a. burning the morning toast b. condensation of water vapor g. slicing a tomato h. the baking of a potato c. digesting your lunch i. the explosion of nitroglycerin d. digging a hole j. the rusting of iron e. lighting a match k. winding an alarm clock f. pumping gasoline 3. Rewrite the following in scientific notation, express answers using 3 significant figures. a b Rewrite 4.63 x 10-3 in standard notation. 5. Which measurement represents the smallest quantity? a g b mg c kg d μg e ng 6. Fill in the table to describe subatomic particles: Subatomic Particle Charge Location Molecular weight Proton Neutron Electron C is the same as a. 341 K. b. 205 K. c. 285 K. d. 321 K. e. 158 K. Rev pg. 1

2 8. What is the molar mass of a substance, Mg 3 (PO 4 ) 2, formerly used in medicine as an antacid? a g b g c g d g e g 9. The electron configuration for nickel is: a. 1s22s22p63s23p64s24d8 b. 1s22s22p63s24s23d104p4 c. 1s22s22p63s23p63d10 d. 1s22s22p63s23p64s23d8 10. The element which has four valence electrons is. a. H b. S c. Si d. Na e. Mg 11. How many electrons will aluminum gain or lose when it forms an ion? a. Lose 1 b. Gain 1 c. Lose 2 d. Lose 3 e. Gain The correct name of the compound, NCl 3, is a. Nitrogen chloride b. Trinitrogen chloride c. Nickel chloride d. Nitrogen trichloride e. Nitrogen (III) chloride 13. Which element is most likely to be "X" in the diatomic molecule shown? a. Nitrogen b. Oxygen c. Fluorine d. Hydrogen e. Helium 14. Name the 7 diatomic elements. 15. Use the VESPR theory to determine the shape of PCl 3. a. Bent b. Tetrathedral c. Pyramidal d. Planar Triangular Rev pg. 2

3 16. Which of the following equations is not balanced? a. 2 Na + 2 H 2 O 2 NaOH + H 2 b. C 3 H O 2 3 CO H 2 O c. 2 H 2 + O 2 2 H 2 O d. SO 2 + O 2 SO 3 e. 2 Al + 6 HCl 2 AlCl H In the balanced reaction shown, the mole ratio of Fe2S3 to O2 is Fe2S3 + 4 O2 2 FeO + 3 SO2 a. 5 to 5 b. 1 to 4 c. 4 to 1 d. 1 to 2 e. 4 to A thimble of water contains 4.0 x 1021 molecules. The number of moles of H2O is: a. 2.4 x 1045 b. 6.6 x 10-3 c. 6.6 x d. 2.4 x e. 2.4 x How many grams of fluorine are required to produce 20.0 grams of FeF3 from the reaction shown? 2 Fe + 3F2 2 FeF3 a g b g c g d g e g 20. ΔS = ( the amount of molecular disorder in a system ) fill in the blank, circle the correct choice. a. If ΔS is positive it means disorder is increasing, LOWER/HIGHER entropy b. If ΔS is negative it means disorder is decreasing, LOWER/HIGHER entropy 21. ΔG = ( the amount of energy released or absorbed in a reaction at constant temperature and pressure) fill in the blank, circle the correct choice. a. If the ΔG is negative it means there is a release of free energy, the reaction is considered SPONTANEOUS/NONSPONTANEOUS. b. If the ΔG is positive it means the reaction absorbs free energy, the reaction is SPONTANEOUS/NONSPONTANEOUS. 22. The function of a catalyst in a reaction system is to a. Increase the yield of the product b. Decrease the amount of heat produced c. Decrease the amount of energy consumed in the reaction d. Increase the rate of reaction e. Decrease the amount of reactants consumed. Rev pg. 3

4 23. Consider the reaction: A + 2 B 2 C + D The equilibrium expression for this reaction is: a. [A] 2 [B] 2[C][D] b. [A] 2 [B] 2 2[C] 2 [D] c. 2[C][D] [A] 2 [B] d. [C] 2 [D] [A][B] 2 e. [A][B] 2 [C] 2 [D] 24. What does the size of the equilibrium constant tell you? Circle the correct choice a. If K is GREATER/LESS than 1, a forward reaction is favored or more products than reactants present. b. If K is GREATER/LESS than 1, a reverse reaction is favored or more reactants than products present. 25. States of matter: Definitions and properties of gases, liquids and solids. Fill in the blank. a. no definite shape or volume b. definite volume but takes the shape of its container c. definite shape and volume 26. What is the final concentration of a solution prepared by adding water to 50.0 ml of 1.5 M NaOH to make 1.00 L of solution? a. 7.5 M b M c M d. 30 M e. 1.5 M 27. What is the molarity of a solution prepared by dissolving 48.0 g of NaOH in enough water to make 1.50 L of solution? a M b M c M d M e M 28. What is the % (w/v) concentration of a solution containing 25.0 g of solute in 400. ml of solution? a % b % c % d % e % Rev pg. 4

5 29. How many grams of O2 are contained in a 25.0 L sample at 5.20 atm and 28.0 C? a g b. 168 g c g d g e g 30. A sample of gas has a volume of 135 ml at atm. What would be the volume if the pressure is decreased to atm while temperature is held constant? a. 101 ml b. 405 ml c. 180 ml d ml e. 135 ml 31. What will be the new volume when 128 ml of gas at 20.0 C is heated to 40.0 C while pressure remains unchanged? a ml b. 120 ml c. 256 ml d. 137 ml e. 128 ml 32. According to Brønsted-Lowry theory, acid-base reactions can be described as reactions. a. Electrolytic b. Electron transfer c. Gas phase d. Nuclear transfer e. Proton transfer 33. Which statement concerning Arrhenius acid-base theory is not correct? a. An Arrhenius acid produces hydrogen ions in water solution b. An Arrhenius base produces hydroxide inons in water solution c. A neutralization reaction produces water plus a salt d. Acid-base reactions must take place in aqueous solution e. None of the above 34. When acids and bases react the product other than water is a a. hydrogen ion. b. hydroxide ion. c. hydronium ion. d. metal. e. salt. 35. Which of the following is a diprotic acid? a. Acetic acid b. Hydrochloric acid c. Phosphoric acid d. Sulfuric acid e. Nitric acid Rev pg. 5

6 36. What is the conjugate base of water? a. H2O (l) b. H3O+ (aq) c. OH- (aq) d. H+ (aq) e. O2 - (aq) 37. What is the conjugate acid of water? a. H2O (l) b. H3O+ (aq) c. OH- (aq) d. H+ (aq) e. O2 - (aq) 38. A weak acid SLIGHTLY/COMPLETELY dissociates in water. Circle the correct choice. 39. A strong acid SLIGHTLY/COMPLETELY dissociates in water. Circle the correct choice. 40. If the [H3O+] of a water sample is M, the ph of the sample is, and the sample is. a. -4; acidic b. 4; acidic c. 4; basic d. 10; basic e. -10; basic 41. Fill in the blank. A is a combination of substances that act together to prevent a drastic change in ph; usually made up of a week acid and roughly the same concentration of its conjugate base. 42. The normality of a solution prepared by dissolving 25.0 g of Ca(OH)2 in water to make 250. ml solution is N. a b c d e How many ml of M NaOH are needed to neutralize ml of a M solution of CH3CO2H, a monoprotic acid? a ml b ml c ml d ml e ml Rev pg. 6

7 Answer Key: 1. a. C b. P c. C d. C e. P f. C g. C h. P i. P 2. a. C b. P c. C d. P e. C f. P g. P h. C i. C j. C k. P 3. a x 10 1 b x E 6. Proton - + charge, nucleus, 1 amu Neutron no charge, nucleus, 1 amu Electron - - charge, orbiting nucleus, almost no mass 7. A 8. C 9. D 10. C 11. D 12. D 13. B 14. Br, I, N, Cl, H, O, F 15. C 16. D 17. B 18. B 19. D 20. Entropy a. Higher b. Lower 21. Free energy change a. Spontaneous b. Nonspontaneous 22. D 23. D 24. a. Greater b. Less 25. a. Gas b. Liquid c. Solid 26. C 27. D 28. C 29. B 30. B 31. D 32. E 33. E 34. E 35. D 36. C 37. B 38. Slightly 39. Completely 40. B 41. Buffer 42. A 43. D Rev pg. 7