AP Chemistry 1st Semester Final Review Name:...

AP Chemistry 1st Semester Final Review Name:____________________2015-2016

A) CO2 B) C3H6

C) CH3Cl D) N2O3

E) SiO2

1. Which of the following contains only sigma (s) bonds?

A)

B)

C)

D)

2. What is the equilibrium law expression for the abovereaction?

A) [CO] and [CO2] both increaseB) [CO] and [CO2] both decreaseC) [CO] increases and [CO2] decreasesD) [CO] decreases and [CO2] increasesE) [CO] decreases and [CO2] remains constant

3. H2O(g) + CO(g) H2(g) + CO2(g)

A closed container is initially filled with H2O and CO.As the reaction proceeds towards equilibrium the

A) Activation energy is not required.B) The addition of a catalyst does not change

equilibrium concentrations.C) Changes do not occur at the microscopic level.D) Two opposing reactions occur at the same rate.E) Temperature and pressure affect the equilibrium

position equally.

4. Which of the following is characteristic of all systems atequilibrium?

A) 1.0 moles B) 2.0 molesC) 3.0 moles D) 4.0 molesE) 5.0 moles

5. H2O(g) + CO(g) H2(g) + CO2(g)

Initially 5.0 moles of H2O and 4.0 moles of CO werereacted in the system above. At equilibrium, it is foundthat 2.0 moles of H2 are present. How many moles of H2O remain in the mixture?

6. Base your answer to the following question on theequation and the choices provided. CN–(aq) + H2O(l) « HCN(aq) + OH–(aq) (A) increases (B) decreases (C) remains the same (D) increases, then decreases (E) decreases, then increases

A) A B) B C) C D) D E) E

If the pressure is increased, the [OH–]

A) 2 NO(g) « N2(g) + O2(g)B) 2 H2(g) + O2(g) « 2 H2O(g)C) 2 NH3(g) « N2(g) + 3 H2(g)D) 2 CO2(g) « 2 CO(g) + O2(g)E) 2 SO3(g) « 2 SO2(g) + O2(g)

7. When at equilibrium, which reaction shifts to the right ifpressure is increased?

1st Semester Final Review

A)

B)

C)

D)

8. N2(g) + 3 H2(g) 2 NH3(g) + 22 kcal

Which shows what happens to the concentrations of thethree gases when some NH3 is removed from the aboveequilibrium system with temperature and pressureremaining constant.

A) amount of AgCl(s) increasesB) rate of forward reaction decreasesC) concentration of Cl–(aq) increasesD) concentration of Ag(S2O3)23–(aq) decreasesE) equilibrium cannot be reestablished

9. AgCl(s) + 2 S2O32–(aq) Ag(S2O3)23–(aq) + Cl–(aq)

If more S2O32– is added to the above system atequilibrium, the

A) Adding more PbI2B) Increasing the pressureC) Decreasing the temperatureD) Increasing the temperatureE) Adding some Pb(NO3)2

10. PbI2(s) + heat Pb2+(aq) + 2I–(aq)

Which of the following changes would result in morePbI2 dissolving?

A) An increase in pressureB) An increase in temperatureC) The removal of oxygen, O2

D) The addition of water vapor, H2O(g)E) The removal of HBr(g)

11. 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)H = – 276kJ

Which change to the above system at equilibrium willincrease the concentration of Br2(g)?

A) A decrease in the total pressureB) A decrease in the concentration of H2(g)C) An increase in the volume of the reaction chamberD) A decrease in the temperature of the reaction

chamberE) A decrease in the concentration of N2(g)

12. N2(g) + 3 H2(g) 2 NH3(g) + 24 kcal

Which change will increase the above equilibriumconcentration of ammonia, NH3?

A) 0.15 B) 0.94 C) 1.5 D) 1.6 E) 9.4

13. At equilibrium, represented by the equation below, the[NO] is 2.0 M; [O2] is 3.0 M; [N2O5] is 8.0M.

4 NO(g) + 3 O2(g) 2 N2O5(g) + Heat

What is the numerical value of the equilibriumconstant, K, at this temperature?

A) 9.0 moles/liter B) 2.0 moles/literC) 3.0 moles/liter D) 4.5 moles/literE) 6.0 moles/liter

14. I2(g) 2 I(g) K = 9.0 moles/liter

At equilibrium, the concentration of I2 is 1.0 mole/liter.What is the concentration of the I at this temperature ifthe system behaves according to the above equation?


A) area I onlyB) area IV onlyC) areas II and III onlyD) areas I, II and III onlyE) areas I and IV only

15. The relative number of molecules with a given kineticenergy is plotted against kinetic energy. An uncatalyzedreaction with an activation energy, Ea, is beingconsidered. In which region of the above kinetic energydistribution graph will all collisions result in a chemicalreaction?

Base your answers to questions 16 through 21 on thediagram shown below.

A) 1 and 6 B) 2 and 3C) 3 and 4 D) 4, 5 and 6E) 3 and 6

16. A catalyst would change

A) 1 B) 2 C) 3 D) 4 E) 5

17. Which represents the heat of reaction?

A) 1 B) 2 C) 3 D) 4 E) 6

18. Which represents the activation energy for the forwardreaction?

A) 6 B) 2 C) 3 D) 4 E) 5

19. Which represents the energy of the activated complex?

A) 6 B) 2 C) 3 D) 4 E) 5

20. The products have an energy represented by number

A) reactantsB) productsC) activated complexD) endothermic reaction

21. The least stable species in this diagram is the

A) [K+] = [S2–] = 2 × [K2S]B) [K+]2 = [S2–]C) [K+] = [S2–]2D) [K+] = 2 × [S2–]E) 2 × [K+] = [S2–]

22. Potassium sulfide is completely ionized in water:K2S(s) ® 2 K+(aq) + S2–(aq) Which of the followingequations is true?

A) [Sr2+] = 0.12 M and [OH–] = 0.12 MB) [Sr2+] = 0.12 M and [OH–] = 0.24 MC) [Sr2+] = 0.090 M and [OH–] = 0.090 MD) [Sr2+] = 0.090 M and [OH–] = 0.180 ME) [Sr2+] = 0.090 M and [OH–] = 0.24 M

23. When 250. mL of 0.36 M Sr(OH)2 are added to 750.mL of water, the resulting ion concentrations are

A) C(graphite) ® C(g)B) H2O(s) ® H2O(l)C) Ne(g) ® Ne(s)D) Co(l) ® Co(s)E) Ti(l) ® Ti(s)

24. Which of the following involves the breaking ofcovalent bonds?


A) I and IV B) I and VC) III and IV D) II and VE) II and IV

25. According to the above table, which substances havemetallic bonding?

A) X–P X–Q X–S X–TB) X–Q X–P X–T X–SC) X–Q X–T X–P X–SD) X–S X–T X–P X–QE) X–Q X–P X–S X–T

26. The element X forms diatomic molecules with each ofthe elements P, Q, S, T.

Based on the table above, which lists the compounds inthe order of increasing ionic character?Lowest Highest

A) Ionic B) MetallicC) Network covalent D) Molecular covalentE) Coordinate covalent

27. A certain solid is insoluble in water, does not conductelectricity in either the solid or liquid state and melts ata temperature above 1500°C. Which type of bonding ismost likely between lattice points in its crystallinestructure?

Base your answers to questions 28 through 30 on thefollowing bonding types.

(A) Coordinate covalent bonding(B) Network covalent bonding(C) Ionic bonding(D) Metallic bonding(E) Hydrogen bonding


28. Bonding associated with nitrogen, oxygen and fluorineonly


29. Substances with this bonding type exhibit goodelectrical and thermal conductivity


30. Type of bonding exhibited by two atoms with a largeelectronegativity difference

A) SiO2 B) LiCl C) NH3 D) C2H6 E) Fe

31. Which of the following has the lowest boiling point?

Base your answers to questions 32 through 35 on thefollowing substances (all solids).

(A) RbCl(B) SiO2 (C) Ag(D) CN– (E) C3H8


32. Contains strong multiple covalent bonds


33. This substance has strong single covalent bonds, butweak intermolecular forces


34. Electrons flow in a "sea" throughout the substance


35. Held together by a lattice of positive and negative ions


Base your answers to questions 36 through 39 on thetypes of solids given below.

(A) A metallic solid(B) A molecular solid with hydrogen bonds (C) A molecular solid with non-polar molecules(D) A network solid(E) An ionic solid


36. Which describes solid benzene (C6H6)?


37. Which is described as a lattice of positive ions in a seaof mobile electrons?


38. Which best describes solid water?


39. Which describes diamond (C)?

A) 0.50 molar NaClB) 0.50 molar NaOHC) 0.50 molar Ca(OH)2

D) 0.50 molar LiOHE) 0.50 molar HBr

40. Which compound has the highest boiling point?

A) I, II, and VI onlyB) II, III, and IX onlyC) III, V, and IX onlyD) III, VII, and VIII onlyE) IV, V II, and VIII only

41. Based on the above table, which substances aremolecular?

A) Si–Si bonds are stronger than C–C bonds.B) CO2 molecules are nonpolar; SiO2 molecules are

polar.C) CO2 is a molecular solid; SiO2 is a network

covalent solid.D) The Si–O bonds in SiO2 molecules are many times

stronger than the C=O bonds in CO2 molecules.E) Si has a larger atomic radius than C.

42. CO2 is a gas at room temperature and pressure, whileSiO2 melts at about 1700°C. What accounts for thislarge difference in melting points?

A) London dispersion forcesB) Covalent bonding forcesC) Dipole forcesD) Halogen bonding forcesE) Hydrogen bonding forces

43. CF4 < CCl4 < CBr4 < CI4

According to the above trend in boiling points, whichtype of bonding force explains the trend above?

A) N2 B) O2 C) F2 D) I2 E) Hg22+

44. Which of the following substances has the strongestbonds?


A) H2 B) NaCl C) I2 D) C2H2 E) MgO

45. Which has the smallest force of attraction between itsmolecules?

A) B) C) D) E)

46. According the the above electronegativities, which of the following bonds has the most ionic character?

A)

B)

C)

D)

E)

47. A solution of Na+ ions would be best represented bywhich picture?

A) O2 B) SiO2

C) KMnO4 D) C12H22O11

E) CH4

48. Which of the following dissolves in water to form anionic solution?

A) 1000 mL B) 2000 mLC) 3000 mL D) 4000 mLE) 5000 mL

49. How many milliliters of 11.5-molar HCOOH must bediluted to obtain 23 L of 2.0-molar HCOOH?

A) 2.50 grams B) 3.00 gramsC) 6.00 grams D) 25.0 gramsE) 30.0 grams

50. The weight of HC2H3O2 (molecular weight 60.0) in20.0 milliliters of a 2.50-molar solution is

51. Base your answer to the following question on A fewdrops of the indicator bromothymol blue [HBb] isadded to water

A) KOH(aq) causes the [HBb] to increase and thesolution to turn yellow.

B) HCl(aq) causes the [H3O+] to decrease and thesolution to turn yellow.

C) HCl(aq) causes an equilibrium shift toward thereactants and the solution turns blue.

D) KOH(aq) causes an equilibrium shift toward theproducts and the solution turns yellow.

E) HCl(aq) causes the [H3O+] to increase and thesolution to turn yellow.

HBb(aq) + H2O( ) H3O+ (aq) + Bb–(aq)Yellow Blue

Which statement is correct? The addition of


A) CH3COOH, NH4+, HIO3

B) HIO3, CH3COOH,NH4+

C) HIO3,HIO3,CH3COOHD) NH4+, HIO3, CH3COOHE) NH4+, CH3COOH, HIO3

52. Based on the above table, list the acids in order of increasing acid strength.

A) Thymol blue B) Methyl violetC) Bromothymol blue D) Bromocresol greenE) None of these

53. According to the table above, which indicator will beyellow at pH 7 and blue at pH 10?

A) I only B) II onlyC) I and II only D) II and III onlyE) I, II, and III

54. CH3NH2 + H2O CH3NH3+ + OH–

Which species acts as an acid?

I. H2OII. CH3NH3+

III. CH3NH2

A) BO33– B) H2BO4–

C) H2BO3– D) H3BO3

E) HBO32–

55. The conjugate base of H2BO3– is

A) HPO42– B) H2OC) SO42– D) NH4+

E) CH3COOH

56. All of the following ions can act as Bronsted-Lowryacids in solution EXCEPT

A) SO32– B) NH4+

C) PO43– D) HSO3–

E) HCl

57. Which is amphiprotic?

A) decreased by 1 B) increased by 2C) decreased by 2 D) decreased by 4E) increased by 1

58. C2O42– + MnO2 Mn2+ + 2 CO2

As a result of the above reaction, the oxidation numberof each C atom is

A) –2 B) +1 C) +2 D) +4 E) +6

59. The oxidation number of sulfur in Na2S2O3 is

A) 1 B) 2 C) 3 D) 4 E) 5

60. If 50 mL of 0.025 M NaOH is mixed with 50 mL of 0.05 M HCl, what is the resulting pH of the mixtureclosest to?

A) and both remain the sameB) and both decreaseC) increases and decreasesD) decreases and increasesE) and both increase

61. Given the above values, Which is true abouthydronium and hydroxide ion concentrations whenwater is heated?

A) 1.83 B) 12.1 C) 3.75 D) 3.67 E) 1.88

62. The Ka of formic acid is 1.77 × 10–4. The pH of 1.20 M formic acid (aq) is

A) 2.5 × 10–5 M B) 9.5 × 10–1 MC) 6.6 × 10–1 M D) 9.7 × 10–1 ME) 4.0 × 10–10 M

63. What is the [H3O+] of a solution with a pOH of 4.60?


A) D > B > C > A B) C > D > B > AC) A > B > C > D D) B > D > C > AE) D > C > B > A

64. Solution A: [OH–] = 5.0 10–11 MSolution B: [H+] = 0.20 MSolution C: pOH = 11.30Solution D: pH = 1.20

Four monoprotic acids of the same concentration arelabeled above.

List the four solutions above in order ofDECREASING acidity.

A) 243 kJ B) 418 kJC) 661. kJ D) 904. kJE) 1320 kJ

65. 12 O2(g) + H2(g) H2O(g) + 243 kJ12 O2(g) + 2 H(g) H2O(g) + 661 kJ

Given the above two equations, how much energy isneeded to dissociate 1.00 mole of H2 according to theequation below?

H2(g) 2H(g)

A) 2 La2O3(s) ®3 O2(g) + 4 La(s)B) Cu2+(aq) + 2 Ag+ (aq) ® Cu2+ (aq) + 2 Ag(aq)C) H2(g) + 2 KOH(aq) ® H2O(l) + 2 K(s)D) 2 CO(g) + O2(g) ® 2 CO2(g)E) Pb(NO3)2(s) + 2 KI(s) ® PbI2(s) + 2 KNO3(s)

66. Which of the following reactions has the largestincrease in entropy?

A) II and IV B) II and IIIC) I and III D) I and IVE) I and II

67. According to the table above, which reactions occurspontaneously?

A) AB) BC) CD) DE) All compounds can be formed spontaneously at

298K

68. According to the table above, which compound cannot be formed spontaneously from its elements at 298 K?

A) 5.02 × 10–5 B) 34100C) 0.00003 D) 0.0782 × 10–3E) 32312 × 1052

69. Which number contains exactly 5 significant digits?

A) 7.2047 g/mL B) 7.205 g/mLC) 7.20 g/mL D) 7.2 g/mLE) 7 g/mL

70. A student calculated the mass of a small piece ofunreactive metal. This piece of metal was added to apartially filled graduated cylinder. The followingmeasurements were made by the student:Mass of metal = 13.689 gramsVolume of water before the metal was added= 7.51millilitersVolume of water after the metal was added= 9.41millilitersThe density of the metal should be reported as

Answer KeyAP 1st Semester Final Review 2015-2016

1. C2. D3. A4. D5. A6. C7. B8. D9. C10. D11. A12. D13. A14. C15. B16. D17. A18. D19. A20. C21. C22. D23. D24. A25. E26. B27. C28. E29. D30. C31. D32. D33. E34. C35. A36. C

37. A38. B39. D40. C41. A42. C43. A44. A45. A46. A47. E48. C49. D50. B51. E52. E53. C54. C55. E56. C57. D58. E59. C60. B61. E62. A63. E64. D65. B66. A67. E68. C69. E70. C

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