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CHEM 111 Mock Final Exam, Fall 2017


1. Which of the following is an example of a heterogenous mixture?

a. Hot sugar waterb. Airc. An unopened can

of sodad. Italian salad

dressing2. Which combination of

molecules would result in a homogenous mixture?

a. Propanoic Acid (C3H6O2) in Water (H2O)

b. Benzene (C6H6) in Methanol (CH3OH)

c. Hydrobromic acid (HBr) in Toluene (C7H8)

d. Sulfur tetrafluoride (SF4) in Ethanol (C2H5OH)

3. Who formulated a nuclear model that portrays electrons orbiting the nucleus like a planet orbiting the sun?

a. JJ Thomsonb. Ernest Rutherfordc. Gilbert Lewisd. Niels Bohre. James Chadwickf. Dmitri Mendeleevg. John Daltonh. Michael Faraday

4. True or False: As vapor pressure decreases, intermolecular force strength increases.

a. Trueb. Falsec. Vapor pressure is

useless.5. In the following list,

which combination(s) would create a covalently-bonded compound?I) (CO3) + SrII) Cl + BrIII) K + (OH)IV) (PO4) + (NH4)V) (MnO4) + Na

a. I onlyb. II onlyc. III onlyd. IV onlye. V onlyf. I, III, and Vg. II and IVh. I, III, IV, and V

6. Which nuclear reaction correctly depicts the beta decay of Uranium?

a. 98240U 96

236Th + 24He

b. 98240U 98

240U +e-

c. 98240U 98

240U + γd. 98

240U 98240U+ +e-


7. A magical wave has a wavelength of 0.63 mm. What is the frequency of this wave?

a. 4.8 * 1011 Hzb. 1.9 * 105 Hzc. 3.0 * 108 Hzd. 2.1 * 10-12 Hz

8. According to the ________ Principle, the position and velocity of a particle cannot be known at the exact same instant in time.

a. Bohrian Momentumb. Lewis Cyclec. Heisenberg

Uncertaintyd. Schrodinger

Compromise9. In order to pass

chemistry lab, 500. mL of C6H6 (MW = 78 g/mol)(ρ = 0.879 g/mL) must be formed by the following reaction:C6H6Br + NaOH C6H6 + NaBr + OH-

How many grams of NaOH (MW = 40 g/mol) must be added to achieve the desired yield?

a. 256 gb. 975 gc. 225 gd. 291 g

10. Who is accredited with discovering the proton and nucleus in the early twentieth century?


11. How many of the following ions are isoelectronic with Argon?S3-, Br-, Na+, P3+, Al3+

a. Zerob. Onec. Twod. Threee. Fourf. Five

12. How many of the following molecules are polar?H2, CHFBr, BI3, SCl2, SiH4, CH3CH2OCH2CH3

a. Zerob. Onec. Twod. Threee. Fourf. Fiveg. Six


13. The central atom in a strange compound is surrounded by three lone pairs and two single bonds. What is its molecular geometry?

a. Bentb. Linearc. Tetrahedrald. Trigonal

Bipyramidale. Octahedralf. Square Pyramidalg. Trigonal

Pyramidal14. Which ranking of

electromagnetic waves is correct based on increasing frequency?

a. X Ray > Gamma Ray > Visible Light > Infrared

b. Visible Light > Infrared > Microwave > Ultraviolet

c. Radio Wave > Microwave > Ultraviolet > Gamma Ray

d. Gamma Ray > Visible Light > Infrared > Radio Wave

15. True or False: Toluene (C7H8) is miscible with benzene (C6H6).

a. Trueb. Falsec. “Miscible” is not

a real word.

16. Which set of quantum numbers corresponds to the electron with the most energy?

a. n = 2, L = 1, mL = 0, ms = -1/2

b. n = 7, L = 0, mL = 0, ms = -1/2

c. n = 4, L = 3, mL = -3, ms = -1/2

d. n = 5, L = 2, mL = 2, ms = +1/2

17. What is the hybridization at the starred carbon and oxygen in this molecule?

a. C = spO = sp

b. C = spO = sp2

c. C = spO = sp3

d. C = sp2

O = spe. C = sp2

O = sp2

f. C = sp2

O = sp3

g. C = sp3

O = sph. C = sp3

O = sp2

i. C = sp3

O = sp3


18. A certain molecule has ten single bonds, three double bonds, and four triple bonds. How many sigma (σ) and pi (π) bonds are in this molecule?

a. 17 σ, 0 πb. 0 σ, 17 πc. 11 σ, 17 πd. 17 σ, 11 πe. 10 σ, 7 πf. 7 σ, 10 πg. 21 σ, 4 πh. 4 σ, 21 π

19. Which molecule listed below will have the highest viscosity?

a. H2Ob. C2H2

c. SO2

d. HCle. HI

20. True or False: A pi (π) bond is formed from hybridized orbitals.

a. Trueb. Falsec. Pi bonds should

be eaten.21. What is the most

correct electron configuration for Zr2+?

a. 1s22s22p63s23p64s2

3d104p64d2

b. 1s22s22p63s23p64s2

3d104p65s2

c. 1s22s22p63s23p64s2

3d104p65s14d1

d. 1s22s22p63s23p64s2

3d104p65s24d2

22. What is the most correct chemical reaction for the following situation? Liquid toluene (C7H8) is treated with bromine gas and carbon tetrachloride to form a gaseous mixture of benzyl bromide (C7H7Br), chlorine, and dibromo-dichloro methane (CBr2Cl2).

a. C7H8 + Br2 + CCl4

C7H8Br + Cl2 + CCl2Br2

b. C7H8(L) + Br2(g) + CCl4(g) C7H8Br(g) + Cl2(g) + CCl2Br2(g)

c. 2C7H8(L) + 2Br(g) + CCl4(g) 2C7H8Br(g) + 2Cl(g) + CCl2Br2(g)

d. 2C7H8(L) + Br2(g) + CCl4(g) 2C7H8Br(g) + Cl2(g) + CCl2Br2(g)

23. Reactions that are ________ show energy as a reactant in chemical equations.

a. Single Displacement

b. Isotropicc. Endothermicd. Combustione. Additionf. Exothermic


24. Who discovered the first subatomic particle using the Cathode Ray Experiment?


25. Rank the following in terms of atomic size:Se, I, Rb, Fr, C, V, F

a. Fr > Rb > C > V > I > Se > F

b. Fr > C > I > Se > Rb > V > F

c. Fr > Rb > V > I > Se > C > F

d. Fr > I > Rb > V > C > Se > F

26. A Bohr Model electron moves from n = 2 to n = 7. How much energy was added or released to cause this transition?

a. -5.01 * 10-19 Jb. 5.01 * 10-19 Jc. -7.79 * 10-19 Jd. 7.79 * 10-19 J

27. For the Angular Quantum Number, L = 0 corresponds to a(n) ______ orbital, and L = 2 represents a(n) ______ orbital.

a. s, fb. d, pc. p, sd. s, d

28. This principle states that low-energy orbitals are filled before high-energy orbitals.

a. Aufbau Principleb. Hund’s Rulec. Pauli Exclusion

Principled. Heisenberg

Uncertainty Principle

e. Photoelectric Effect

29. ___GeF4 + ____Na2O ___GeO2 + ___NaFIn the above reaction, how many grams of Na2O is required to produce 25 g GeO2?

a. 30. gb. 84 gc. 7.4 gd. 21 g

30. The empirical formula for Catechol is C3H3O. If the molecular weight of this compound is 110.1 g/mol, what is the molecular formula?

a. C12H12O4

b. C9H9O3

c. C6H6O2

d. C3H3O


31. Red light has a wavelength of 700 nm, lime-colored light is 560 nm, cyan light is 490 nm, and violet is 410 nm. Which colored light possesses the most energy?

a. Cyanb. Limec. Redd. Violet

32. What two subgroups constitute pure substances?

a. Elements and mixtures

b. Suspensions and compounds

c. Compounds and elements

d. Mixtures and suspensions

e. Matter and elements

33. ________ refers to a solid changing to a gas in one step, and _______ refers to a liquid that changes into a gas.

a. Vaporization, Melting

b. Deposition, Vaporization

c. Freezing, Condensation

d. Sublimation, Vaporization

e. Deposition, Sublimation

f. Condensation, Freezing

34. Which of the following pairs of compounds would combine to form a solution?

a. CH2BrI and H2Ob. C2H5OH and CF4

c. C6H6 and HCNd. H2O and C4H10

35. What is the overall charge on the following molecule?

a. -2b. -1c. 0d. +1e. +2

36. What is the proper name for Au(ClO4)3

a. Gold Chlorotetraoxide

b. Gold (III) Perchlorate

c. Gold (III) Chlorate

d. Gold (III) Chlorite

e. Gold (III) Hypochlorite

f. Gold (I) Perchlorate

g. Gold (I) Chlorateh. Gold (I) Chloritei. Gold (I)

Hypochlorite


37. The ________ and _______ are found in the nucleus, while the ________ are found in orbitals surrounding the nucleus.

a. Neutrons, Electrons, Protons

b. Protons, Electrons, Neutrons

c. Protons, Neutrons, Electrons

d. Electrons, Neutrons, Protons

e. Electrons, Protons, Neutrons

38. Which of the following molecules would have the highest boiling point?

a. GaI3

b. KIc. CuTed. CaBr2

e. AgF39. The electronegativity

difference between two atoms is 0.80. Is this molecule nonpolar, polar, or ionic?

a. Ionicb. Nonpolarc. Polard. It doesn’t

matter.

40. Which of the following is nonpolar?

a. Chlorine monoiodide

b. Hexanec. C2H5COOHd. Rubidium Fluoride

41. Who published a theory on the existence and basic properties of atoms in the beginning of the 19th century?


42. How many atoms of oxygen are in 33 g C6H5NO2?

a. 33 * 1023 atoms b. 3.2 * 1023 atomsc. 4.9 * 1027 atomsd. 8.8 * 10-25 atoms

43. 2041Ca, 20

45Ca, and 2037Ca

are all __________ of the element calcium.

a. Ionsb. Isotopesc. Reactionsd. Metalloids

44. Which of the following elements is the most electronegative?

a. Osb. Asc. Nad. Cle. Bf. Ig. Fr


45. How many of the following molecules demonstrate ionic character?HF, GaI3, NH4F, O2, CH3OH, BaS, Al(PO4)

a. Zerob. Onec. Twod. Threee. Fourf. Fiveg. Sixh. Seven

46. Which of the following is the smallest atom?Rb+, Sr+, Br-, Ba, As3-,

a. Br-

b. Bac. Rb+

d. As3-

e. Sr+

47. Which set of quantum numbers corresponds to the last electron added to Gold?

a. n = 6, L = 2, mL = 1, ms = -1/2

b. n = 5, L = 1, mL = -1, ms = -1/2

c. n = 6, L = 3, mL = 2, ms = +1/2

d. n = 5, L = 3, mL = 1, ms = -1/2

e. n = 6, L = 2, mL = -1, ms = +1/2

f. n = 5, L = 2, mL = 1, ms = -1/2

g. n = 6, L = 2, mL = -1, ms = -1/2

h. n = 5, L = 3, mL = -2, ms = +1/2

48. How many micromoles of molybdenum(VI) chloride are produced in the following reaction if 11 L of molten MgCl2 (ρ = 2.32 kg/L) is added?____Mo(SiO3)3 + ___MgCl2(l) ____Mg(SiO3) + ____MoCl6

a. 8.94 * 107 μmolb. 8.51 * 109 μmolc. 1.68 * 107 μmold. 7.22 * 101 μmole. 7.66 * 10-2 μmol

49. 24.112 mg of glucose is to be added to 6.20 mg of water. What is the total mass of the solution (in mg) to the correct number of sig figs?

a. 24.17 mgb. 24.2 mgc. 644.11 mgd. 644 mge. 30.3 mgf. 30.31 mgg. 86.11 mgh. 86 mg

50. Which of the following elements would have properties most like Phosphorus?

a. Fb. Lic. Cd. Ne. Sf. Al


51. Who first created a basic version of the periodic table in the mid-late 19th century?


52. 130Te has _______ protons, _______ neutrons, and ________ electrons.

a. 52, 130, 52b. 130, 52, 52c. 52, 52, 130d. 52, 78, 52e. 78, 52, 52f. 52, 52, 78g. 26, 78, 26h. 78, 26, 26i. 26, 26, 78

53. How much energy per photon is contained in a wave whose wavelength is 104 nm?

a. 2.07 * 10-32 Jb. 1.91 * 10-18 Jc. 2.30 * 10-49 Jd. 31.2 J

54. Ionization energy increases as you move ______ and ______ across the periodic table.

a. Left and Upb. Right and Upc. Left and Downd. Right and Down

55. What is the molecular geometry of Iodine Tetrafluoride? (Hint: free radicals count as an electron domain (“port”))

a. Tetrahedralb. Square Pyramidalc. Square Planard. Octahedrale. Linear

56. For n = 5, what are the possible values for the angular quantum number, L?

a. 0,1,2,b. 0,1,2,3c. 0,1,2,3,4d. 0,1,2,3,4,5e. 0f. 1g. 2h. 3i. 4j. 5

57. True or False: Hund’s Rule states that you pair electrons before filling other orbitals at the exact same energy level.

a. Trueb. False


58. Which of the following are diatomic atoms?I) CarbonII) NitrogenIII) HeliumIV) BoronV) HydrogenVI) SulfurVII) LithiumVIII) Iodine

a. I onlyb. II onlyc. III onlyd. IV onlye. V onlyf. VI onlyg. VII onlyh. VIII onlyi. More than one is

correct59. What is the most

proper name of PbSO4?a. Probium Sulfur

Tetraoxideb. Probium Sulfitec. Probium Sulfated. Lead (II) Sulfur

Tetraoxidee. Lead (II) Sulfitef. Lead (II) Sulfateg. Lead (I) Sulfur

Tetraoxideh. Lead (I) Sulfitei. Lead (I) Sulfate

60.

How many of the following are resonance structures for the compound above?I)

II)

III)

IV)

a. Noneb. Onec. Twod. Threee. Four


61. How many of the following are strong electrolytes?NaBr, CH3COOH, C6H5F, NH4Cl, HNO3, H2CO3

a. Zerob. Onec. Twod. Threee. Fourf. Fiveg. Six

62. Which of the following is not a strong acid?

a. HBrb. H3PO4

c. H2SO4

d. HClO4

e. HFf. There are two

correct answers.g. Three are three

correct answers.h. None of the

above.63. How would you prepare

a 4.2 M solution of MgO (MW = 40.3 g/mol)?

a. 170 g MgOb. 9.6 g MgOc. 81 g MgOd. 430 g MgO

64. How many of the following are soluble in water?AgNO3, Ba(OH)2, HgCH3COO, HClO3, Li3(PO4)

a. Oneb. Twoc. Threed. Foure. Five

65. As temperature _________, liquid solubility decreases, and as pressure _________ gas solubility increases.

a. Increases, Increases

b. Increases, Decreases

c. Decreases, Increases

d. Decreases, Decreases

66. Which of the following is a strong base?

a. NH4+

b. Ag(OH)c. Sr(OH)2

d. C5H10Ne. Mg(OH)2

67. What is the molarity of a 23.15 g sample of NH4CH3COO that is dissolved in water to give 800. mL of solution?

a. 28.9 Mb. 0.240 Mc. 0.375 Md. 2.66 M

68. Barium hydroxide is added to water to form a 1 L solution. How many moles of hydroxide ions are in the solution if 42 g Ba(OH)2 was added?

a. 21 mol OH-

b. 0.25 mol OH-

c. 0.49 mol OH-

d. 2.47 mol OH-


e. 4.9 mol OH-

69. What do the following reactions represent?I)2CuNO3(aq) + K2CO3(aq) 2KNO3(aq) + Cu2(CO3)(s)

II)NH4+(l) + CH3COO-

(l) NH3(l) + CH3COOH(l) II)HI(aq) + Rb(OH)(aq) RbI(aq) + H2O(l)

a. I) PrecipitationII/III) Acid-Base

b. I) RedoxII/III) Precipitation

c. I) PrecipitationII) CombustionIII) Acid-Base

d. I/II) RedoxIII) Acid-Base

70. How many of the following would you expect to see dissolve in ethanol (C2H5OH)?I) Iron (III)

NitrateII) Cesium FluorideIII) Molybdenum (VI)

AcetateIV) Calcium ChlorateV) Strontium

HydroxideVI) Lithium Sulfide

a. Oneb. Twoc. Threed. Foure. Fivef. Six

71. PdI2(aq) + 2HgNO3(aq) Pd(NO3)2(aq) + 2HgI(s)

In the reaction above, who is(are) the spectator ion(s)?

a. Pb2+

b. I-

c. Hg+

d. NO3+

e. Pb2+ and I-

f. Pd2+ and NO3-

g. Hg+ and NO3-

h. I- and Hg2+

72. How do you prepare a 21% by volume solution of aqueous hydroiodic acid?

a. 79 mL HI per 100 mL

b. 79 L HI per 100 mL

c. 21 mL HI per 100 mL

d. 21 L HI per 100 mL

e. 12 mL HI per 100 mL

f. 12 L HI per 100 mL

73. 3250 cm3 of a 3.40 M potassium hydroxide solution is to be diluted to 1.10 M. What will be the final volume (in liters) of the solution?

a. 1.15 Lb. 10.1 Lc. 1.05 Ld. 6.05 L


74. A(n) ____________ _____ is a proton donor in solution.

a. Brønsted–Lowry Acid

b. Arrhenius Basec. Arrhenius Acidd. Brønsted–Lowry

Base75. What is the oxidation

state of carbon in CO3

2-?a. -2b. +2c. –4d. +4e. -6f. +6

76. 2 MgF2(s) + O2(g) 2MgO(s)

+ F2(g)

What is the reducing agent in the above reaction?

a. Mg2+

b. F-

c. O22-

d. F2

77. How many moles of sulfate ions are in solution after 1.42 mol H2SO4 is added to 1000 mL of water?

a. 1.42 mol SO42-

b. 136 mol SO42-

c. 2.84 mol SO42-

d. 25.6 mol SO42-

78. True or False: As temperature increases, the solubility of solids decreases.

a. Trueb. False

79. The concentration of an acetic acid solution is 5.20 M. How many moles of CH3COOH are present in 1200 mL of the solution?

a. 4.3 mol CH3COOHb. 6.24 mol CH3COOHc. 0.0043 mol

CH3COOHd. 6240 mol CH3COOH

80. ZrO2 + 4FeF ZrF4 + 2Fe2OWhat is the limiting reactant in the above reaction if 7 mol ZrO2

and 16 mol FeF are added?

a. ZrF4

b. ZrO2

c. FeFd. Fe2O

81. How do you prepare a 43% by mass NaOH aqueous solution?

a. For every L of solution, add 43 g NaOH.

b. Combine 43 g NaOH with every kg of solution.

c. Take the percentage, multiply it by the molecular weight of NaOH, and then divide by the solution mass.

d. Add 43 g NaOH per 100 g of solution.


82. A(n) __________ _____ produces hydronium ions when added to water.

a. Brønsted–Lowry Base

b. Arrhenius Acidc. Brønsted–Lowry

Acidd. Arrhenius Base

83. What is the elemental percent composition of calcium in Ca3(PO4)2?

a. 14%b. 41%c. 20%d. 62%e. 39%

84. 2 C6H7Br + Sr(OH)2 2C6H6 + SrBr2 + 2H2O Using the above reaction, what is the maximum amount of benzene (C6H6) that is produced when 42.1 g C6H7Br (MW = 159 g/mol) and 49.5 g Sr(OH)2

(MW = 121 g/mol) are added?

a. 6690 mol C6H6

b. 0.265 mol C6H6

c. 5990 mol C6H6

d. 0.818 mol C6H6

e. 0.133 mol C6H6

f. 0.409 mol C6H6

g. 142 mol C6H6

85. How many of the following are strong electrolytes?HF, Sr(OH)2, PbSO4, HNO3, HNO2, AgBr


86. __CaCO3 3CaO + __CO2

In the above reaction, 10.3 kg of CaCO3 (MW = 100.09 g/mol) is used to produce calcium oxide and carbon dioxide. If the actual yield of CaO (MW = 56.08 g/mol) is 4.32 kg, what is the percent yield?

a. 63%b. 75%c. 52%d. 83%e. 31%

87. Oxidation can be described in three ways: the gain of ______, loss of ______, or the _______ of electrons.

a. Hydrogen, Oxygen, Gain

b. Hydrogen, Oxygen, Loss

c. Oxygen, Hydrogen, Gain

d. Oxygen, Hydrogen, Loss


88. What is the molarity of a nitrobenzene (C6H5NO2) solution if there are 6.2 moles in 720 mL of liquid?

a. 0.0086 Mb. 120 Mc. 0.12 Md. 8.6 M

89. Reduction is the _______ of electrons, and a(n) _______ in the oxidation number.

a. Gain, Decreaseb. Gain, Increasec. Loss, Decreased. Loss, Increase

90. How many of the following are strong bases?Be(OH)2, NO2

-, NaOH, HClO, Ba(OH)2, OH-


91. IF + CH4 HF + CH3IIn the above reaction, carbon was ______ because its oxidation number _______.

a. Reduced, Increased

b. Reduced, Decreased

c. Oxidized, Increased

d. Oxidized, Decreased

92. An unknown compound consists of 36% carbon, 54% beryllium, and 9% hydrogen by mass. What is the empirical formula for this unknown compound?

a. CBeHb. C2Be4H2

c. C3Be2Hd. C2Be3He. CBe2H3

f. C3BeH2

93. What is the oxidation number of manganese in RbMnO4?

a. +8b. +7c. +6d. +5e. +4f. 0g. -4h. -5i. -6j. -7k. -8

94. BeSO4 + Sr(NO3)2 Be(NO3)2 + SrSO4

In the above reaction, is a precipitate formed?

a. Yesb. Noc. It’s impossible

to tell.


95. If 5.000 mol Ba2TiO4 (MW = 386.5 g/mol) is combined in sulfuric acid, how many grams of barium sulfate (MW = 233.4 g/mol) is produced?___Ba2TiO4 + ___H2SO4 ___H4TiO4 + ___BaSO4

a. 1167 g BaSO4

b. 1933 g BaSO4

c. 3865 g BaSO4

d. 2334 g BaSO4

e. 6.039 g BaSO4

96. The following reaction depicts the combustion of heptane:___C7H16 + ___O2 + 5N2 __CO2 + __H2O + __N2

If 5.3 kg of C7H16 and 17.9 kg O2 are added, which species is in excess?

a. Heptaneb. Oxygenc. Nitrogend. Cannot be

determined.97. Carbon tetrachloride

is magically transformed into carbon dioxide. In the process, was carbon oxidized or reduced?

a. Reducedb. Oxidizedc. Neither

98. A diluted solution of calcium hydroxide has a total volume of 1.8 L and concentration of 0.244 M. If 560 mL is the initial volume, what is the concentration of the stock solution?

a. 0.078 Mb. 0.78 Mc. 4.1 Md. 0.00078 M

99. _________ refers to a solution that has dissolved the maximum amount of solute without changing the system conditions.

a. Concentratedb. Saturatedc. Titratedd. Stock

100. True or False: An insoluble ionic compound is a weak electrolyte.

a. Trueb. False

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