Экзаменационные тесты по органической химии



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С.Ж. АСФЕНДИЯРОВ АТЫНДАҒЫ

ҚАЗАҚ ҰЛТТЫҚ МЕДИЦИНА УНИВЕРСИТЕТІ






KAZAKH NATIONAL MEDICAL

UNIVERSITY BY S.D.ASPHENDIYAROV



Department of Chemistry

TESTS FOR FORINERS







" Confirmed "

Vice-rector for educational work

________________K.A.Tulebaeb



EXAMINATION TESTS

on the Chemistry

for foreigners

on 2014-2015 academic year


 
1. Which of the following is an example of a physical change?

  1. Ice forming after water is placed in a freezer.

  2. A certain liquid is added to a solid, and bubbles of gas form.

  3. Adding baking powder to vinegar.

  4. A bicycle rusting in the rain.

2. Which of the following changes is a chemical change?



  1. Water is boiled.

  2. Wood is burned.

  3. Aluminum foil is crumpled.

  4. Glass is shattered.

3. This is the formula for vinegar CH3CO2H. What are all of the elements found in the formula for vinegar?



  1. Hydrogen and Oxygen

  2. Carbon, Hydrogen, and Oxygen

  3. Carbon and Oxygen

  4. Chrome, Cobalt, and Hydrogen

4. Name the three states of matter



  1. protons, neutrons, and electrons

  2. metals, non-metals, and metalloids

  3. solid, liquid, and gas

  4. freezing, melting, and evaporation

5. A substance consisting of two elements chemically combined is known as



  1. mixture

  2. solution

  3. element

  4. compound

6. A positive charge particle found in the nucleus is called



  1. neutron

  2. proton

  3. electron

  4. atom

7. A change from liquid to solid is called



  1. melting

  2. boiling

  3. freezing

  4. condensation

8. A change from liquid to gas is known as



  1. condensation

  2. melting

  3. sublimation

  4. evaporation

9. A change from gas to liquid is called



  1. sublimation

  2. evaporation

  3. freezing

  4. condensation

10. A mixture of sand and iron particles can be separated by



  1. distillation

  2. magnetism

  3. decantation

  4. filtration

11. Water is an example of



  1. compound

  2. element

  3. atom

  4. mixture

12. One molecule of water is composed of



  1. two atoms of oxygen and one atom of hydrogen

  2. one atom of oxygen and two atoms of hydrogen

  3. two atoms of oxygen and two atoms of hydrogen

  4. one atom of oxygen and one atoms of hydrogen

13. The symbol of magnesium is



  1. Mn

  2. M

  3. Mo

  4. Mg

14. The symbol of copper is



  1. Co

  2. Cu

  3. C

  4. Cp

15. What is the name of the element with symbol Sr



  1. sodium

  2. silicon

  3. scandium

  4. strontium

16. An example of alkali metal is



    1. K

    2. Ca

    3. P

    4. Cl

    5. Au

17. An example of a noble gas is



    1. N

    2. Na

    3. Ne

    4. No

18. An example of a hallogen is



    1. Ca

    2. Co

    3. Br

    4. S

19. How many valence electron are present in an oxygen atom



    1. 4

    2. 5

    3. 6

    4. 7

    5. 8

20. Which of the following pair belong in the same group



    1. Na and Ca

    2. Si and Al

    3. C, Ge

    4. S, Cl

21. To get the atomic mass, we sum up the numbers of



    1. protons and electrons

    2. electrons and neutrons

    3. protons and neutrons

    4. atomic number and number of protons

22. Which of the following elements will most likely not participate in bonding



    1. Si

    2. Sr

    3. Xe

    4. K

23. An atom contains 11 protons, 11 electrons, and 12 neutrons. What is the mass number



    1. 11

    2. 12

    3. 23

    4. 25

24. Which of the following is an example of a chemical change?



  1. Sodium and chlorine combining to form NaCl.

  2. CO2 in the form of dry ice evaporating into CO2 gas.

  3. Glass that is shattered by a baseball.

  4. The condensation of steam into liquid water.

25. Which statement relating to compounds is incorrect.



  1. Different compounds can contain the same type of elements.

  2. Two different compounds cannot have the exact same type of elements.

  3. Compounds are formed from the combination of different elements.

  4. Elements combine in compounds in whole number ratios.

26. Which of the following represents a compound with four different types of atoms?



  1. H2O

  2. NO2

  3. Ca(C2H3O2)2

  4. Fe(NO3)2

27. Which method would best be used to recover sugar from a solution of sugar and water?



  1. boiling the solution to remove the water.

  2. filtering the solution with filter paper

  3. adding additional sugar to the solution to cause the sugar to precipitate

  4. adding alcohol to the solution

28. 50 grams of acetic acid C2H4O2 are dissolved in 200 g of water. Calculate the weight % of the acetic acid in the solution.



  1. 20%

  2. 0.069%

  3. 25%,

  4. 20%

29. Place the following in the correct order of increasing acidity.



  1. HCl< HF< HI< HBr

  2. HCl< HBr< HI< HF

  3. HI< HBr< HCl< HF

  4. HF< HCl< HBr< HI

30. 100 g of ethanol C2H6O is dissolved in 100 g of water. The final solution has a volume of 0.2 L. What is the density of the resulting solution?



  1. 0.5 g/mL

  2. 1 g/mL

  3. 46 g/mL

  4. 40 g/mL

31. Which particle in the atom has a neutral charge.



  1. proton

  2. neutron

  3. electron

  4. nucleus

32. Atoms become ions by losing or gaining which particle?



  1. neutron

  2. ion

  3. electron

  4. proton

33. If a neutral atom has 10 protons and 10 electrons, what charge will the resulting ion have if the atom loses 3 electrons?



  1. postive

  2. negative

  3. neutral

  4. cannot be determine without the number of neutrons

34. Which term describes a negatively charged ion?



  1. positron

  2. anion

  3. ionic

  4. cation

35. The addition of 2 electrons to a neutral atom results in an ion of charge:



  1. atoms don’t lose electrons

  2. a charge of -2

  3. a charge of +2

  4. can only be determine by knowing the number of protons in the nucleus

36. Which statement is not true for an ion of sulfur with a charge of -2 (S-2)



  1. The number of protons decreased by 2 to form this ion.

  2. There are two more electons than protons in this ion.

  3. The number of electrons increased by 2 to form this ion.

  4. The number of neutrons did not change when this ion was formed.

37. Which of the following elements occurs as a diatomic element.



  1. Argon

  2. Krypton

  3. Fluorine

  4. Carbon

38. What is the charge of an ion that has 6 protons, 9 neutrons, and 7 electrons?



  1. +1

  2. -1

  3. +2

  4. -2

39. What is the correct maximum number of electrons contained in the s-orbital.



  1. 2

  2. 6

  3. 10

  4. 14

40. Which of the following electon configurations is correct for the potassium atom?



  1. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d1

  2. 1s2, 2s2, 2p6, 3s2, 3p6, 3d11

  3. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2

  4. 1s2, 2s2, 2p6, 3s2, 3p6, 4s1

41. Which of the following electon configurations is correct for the chlorine atom ?



  1. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6

  2. 1s2, 2s2, 2p6, 3s2, 3p5

  3. 1s2, 2s2, 2p6

  4. 1s2, 2s2, 2p6, 3s2, 3p6

42. Which electron configuration correctly represents a nonmetal element on the periodic chart?



  1. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p5

  2. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d9

  3. 1s2, 2s2, 2p6, 3s2, 3p6, 4s1

  4. 1s2, 2s2, 2p6, 3s2, 3d6

43. Which electron configuration most likely represents an element in the last column of the periodic chart?



  1. 1s2, 2s2, 2p6, 3s2, 3p6

  2. 1s2, 2s2, 2p6, 3s2, 3p6, 4s1

  3. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10

  4. 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p3

44. Which of the following elements has the most electrons in the outer p-orbital?



  1. oxygen

  2. Fluorine

  3. Sodium

  4. Magnesium

45. Which element does not occur as a diatomic molecule?



  1. helium

  2. fluorine

  3. nitrogen

  4. bromine

46. Choose the correct formula for the compound: Magnesium Bromide



  1. MgBr

  2. MgBr2

  3. Mg2Br

  4. Mg2Br2

47. Choose the correct formula for the compound: Magnesium Sulfide



  1. Mg2S2

  2. Mg2S

  3. MgS2

  4. MgS

48. Choose the correct formula for the compound: Lithium Sulfide



  1. Li2S2

  2. LiS

  3. Li2S

  4. LiS2

49. Choose the correct formula for the compound: Aluminum Sulfide



  1. AlS2

  2. Al3S2

  3. Al2S3

  4. AlS

50. Choose the correct formula for the compound: Barium Hydroxide



  1. BaH2

  2. BaOH

  3. BaOH2

  4. Ba(OH)2

51. Choose the correct formula for the compound: Ammonium Carbonate



  1. NH4CO3

  2. (NH4)2CO3

  3. NH4(CO3)2

  4. NH3CO3

52. Choose the correct formula for the compound: Barium Phosphate



  1. Ba3(PO4)2

  2. BaPO4

  3. Ba3PO4

  4. Ba2(PO4)3

53. Choose the correct formula for the compound: Sulphuric acid



  1. H2SO3

  2. H3SO3

  3. H3SO4

  4. H2SO4

54. Choose the correct formula for the compound: Copper (II) Bromide



  1. Cu2Br2

  2. CuBr2

  3. CuBr

  4. Cu2Br

55. Choose the correct formula for the compound: Chromium (III) Iodide



  1. Cr3I

  2. CrI

  3. CrI3

  4. Cr3I3

56. Choose the correct formula for the compound: Lead (II) Sulfide



  1. PbS

  2. Pb2S

  3. Pb2S2

  4. PbS2

57. Choose the correct formula for the compound: Mercury (I) Sulfide



  1. HgS

  2. Hg2S2

  3. HgS2

  4. Hg2S

58. Choose the correct formula for the compound: Sulfur Trioxide



  1. SO3

  2. SO

  3. S2O

  4. SO2

59. Choose the correct formula for the compound: Silicon Dioxide



  1. Si2O2

  2. SiO2

  3. Si2O

  4. SiO

60. Choose the correct name for the compound: BaI2



  1. Barium Iodate

  2. Barium Diiodide

  3. Barium (II) Iodide

  4. Barium Iodide

61. Choose the correct name for the compound: AlCl3



  1. Aluminum (III) Chloride

  2. Aluminum Chloride

  3. Aluminum Trichloride

  4. Aluminum Tetrachloride

62. Choose the correct name for the compound: CaS



  1. Calcium sulfide

  2. Calcium Monosulfide

  3. Calcium (II) sulfide

  4. Calcium (I) sulfide

63. Choose the correct name for the compound: K2SO3



  1. Potassium Sulfide

  2. diPotassium Sulfite

  3. Potassium (II) Sulfite

  4. Potassium Sulfite

64. Choose the correct name for the compound: (NH4)3PO4



  1. Aluminum Phosphate

  2. Ammonium Phosphate

  3. Nitrogen TriHydrate Phosphate

  4. Triammonium Phosphate

65. Choose the correct name for the compound: NH4Br



  1. Nitrous Tetrahydrogen

  2. Ammonium Bromide

  3. MonobromideAmmonium Bromide

  4. Nitrogen Hydrogen Bromine

66. Choose the correct name for the compound: Al2(CO3)3



  1. Aluminum Tricarbonate

  2. Aluminum Carbonate

  3. Aluminum Carbide

  4. Ammonium Tricarbide

67. Choose the correct name for the compound: Fe(NO3)2



  1. Iron (II) Nitrite

  2. Iron (II) Nitrate

  3. Iron Nitrite

  4. Iron Dinitrite

68. Choose the correct name for the acid: H2SO4



  1. Hydro Sulfuric Acid

  2. Sulfuric Acid

  3. Sulfurous Acid

  4. Hydro Sulfurous Acid

69. The type of reaction illustrated by the equation below would best be described as:

2Al(OH)3 → Al2O3 + 3H2O


  1. double replacement

  2. decomposition

  3. combination

  4. combustion

70. The type of reaction illustrated by the equation below would best be described as:

2C2H6 + 5 O2 → 2CO2 + 6H2O


  1. double replacement

  2. decomposition

  3. combination

  4. combustion

71. For the indicated reaction, choose the products that are most likely to be formed.

K2CO3


  1. K2C + O2

  2. KO + CO2

  3. KO2 + CO2

  4. K2O + CO2

72. For the indicated reaction, choose the products that are most likely to be formed.

Ag + S →


  1. AgS

  2. SAg

  3. Ag2S

  4. S2Ag

73. For the indicated reaction, choose the products that are most likely to be formed.

Fe + Cl2 (assume Fe .. Fe+2) →


  1. FeCl2

  2. FeCl + Cl

  3. FeCl3

  4. FeCl

74. For the indicated reaction, choose the products that are most likely to be formed.

Al + Pb(NO3)2


  1. Al(NO3)3 + Pb

  2. Al(NO3)2 + Pb

  3. AlPb + NO3

  4. PbAl + NO3-

75. For the indicated reaction, choose the products that are most likely to be formed.

K + H2O →


  1. K2O + H2

  2. KOH + H2

  3. KO + H2

  4. K2O + H2O

76. For the indicated reaction, choose the products that are most likely to be formed.

K2CrO4 + Pb(NO3)2


  1. KPb + NO3CrO4

  2. K2Pb + NO3CrO4

  3. KNO3 + PbCrO4

  4. K2(NO3)2 + PbCrO4

77. For the indicated reaction, choose the products that are most likely to be formed.

F2 + BaCl2


  1. BaF + Cl

  2. BaF2 + Cl2

  3. Ba + FCl

  4. Ba + ClF

78. For the indicated reaction, choose the products that are most likely to be formed.

Na + H2O →


  1. NaH + O2

  2. NaH2 + O2

  3. Na2O + H2

  4. NaOH + H2

79. For the indicated reaction, choose the products that are most likely to be formed.

C2H6 + O2


  1. CH2O

  2. CO2 + H2O

  3. C6H12O6

  4. C6H6 + H2O

80. The molar mass of 1 mole of carbon is:



  1. 6.0 g

  2. 12.0 g

  3. 18.0 g

  4. 24.0 g

81. The molar mass of one mole of nitrogen gas is:



  1. 7.0 g

  2. 14.0 g

  3. 21.0 g

  4. 28.0 g

82. The molar mass of HCl is:



  1. 36.46 g

  2. 18.00 g

  3. 72.90 g

  4. 35.45 g

83. The molar mass of H3PO4 is:



  1. 8.00 g

  2. 47.98 g

  3. 82.00 g

  4. 98.00 g

84. Equation: Zn + 2HCl → ZnCl2 + H2

From the indicated equation, if 5.0 moles of zinc are used with excess HCl, how many moles of the product ZnCl2 would be formed.


  1. 1.0

  2. 2.5

  3. 5.0

  4. 10.0

85. Equation: Zn + 2HCl → ZnCl2 + H2

From the indicated equation, if 5.0 moles of HCl are used with excess Zn, how many moles of the product ZnCl2 would be formed.


  1. 1.0

  2. 2.5

  3. 5.0

  4. 10.0

86. Equation: Zn + 2HCl → ZnCl2 + H2

From the indicated equation, if 5.0 moles of HCl are used with 5.0 moles of Zn, how many moles of the product ZnCl2 would be formed.


  1. 1.0

  2. 2.5

  3. 5.0

  4. 10.0

87. Equation: Zn + 2HCl → ZnCl2 + H2

From the indicated equation, if 5.0 moles of HCl are used with 2.0 moles of Zn, how many moles of the product ZnCl2 would be formed.


  1. 1.0

  2. 2.0

  3. 2.5

  4. 5.0

88. When a catalyst is added to a system at equilibrium, a decrease occurs in the



  1. activation energy

  2. heat of reaction

  3. potential energy of the reactants

  4. potential energy of the products

89. In a chemical reaction, a catalyst changes the



  1. potential energy of the products

  2. potential energy of the reactants

  3. heat of reaction

  4. activation energy

90. Which is a property of a reaction that has reached equilibrium?



  1. The amount of products is greater than the amount of reactants.

  2. The amount of products is equal to the amount of reactants.

  3. The rate of the forward reaction is greater than the rate of the reverse reaction.

  4. The rate of the forward reaction is equal to than the rate of the reverse reaction.

91. Which procedure will increases the solubility of KCl in water?



  1. stirring the solute and solvent mixture

  2. increasing the surface area of the solute

  3. raising the temperature of the solvent

  4. increasing the pressure on the surface of the solvent

92. Given the reaction at equilibrium: 2CO(g) + O2(g) <-> 2CO2(g) When the reaction is subjected to stress, a change will occur in the concentration of



  1. reactants, only

  2. products, only

  3. both reactants and products

  4. neither reactants nor products

93. In which reaction will the point of equilibrium shift to the left when the pressure on the system is increased?



  1. C(s) + O2(g) ↔ CO2(g)

  2. CaCO3(s) ↔ CaO(s) + CO2(g)

  3. 2Mg(s) + O2(g) ↔ 2MgO(s)

  4. 2H2(g) + O2(g) ↔ 2H2O(g)

94. Given the reaction at equilibrium: 2 SO2(g) + O2(g) ↔ 2 SO3(g) + heat

Which change will shift the equilibrium to the right?


  1. adding a catalyst

  2. adding more O2(g)

  3. decreasing the pressure

  4. increasing the temperature

95. Given the unbalanced equation: Al + O2 = Al2O3. When this equation is completely balanced using the smallest whole numbers, what is the sum of the coefficients?



  1. 9

  2. 7

  3. 5

  4. 4

96. Which is the correct formula for nitrogen (I) oxide?



  1. NO

  2. N2O

  3. NO2

  4. N2O3

97. What is the total number of atoms represented in the formula CuSO4 . 5H2O?



  1. 8

  2. 13

  3. 21

  4. 27

98. What is the total number of atoms contained in 2.00 moles of nickel?



  1. 58.9

  2. 118

  3. 6.02 x 1023

  4. 1.2 x 1024

99. What is the percent by mass of oxygen in magnesium oxide, MgO?



  1. 20%

  2. 40%

  3. 50%

  4. 60%

100. Which solution is the most concentrated?



  1. 1 mole of solute dissolved in 1 liter of solution?

  2. 2 moles of solute dissolved in 3 liters of solution?

  3. 6 moles of solute dissolved in 4 liters of solution?

  4. 4 moles of solute dissolved in 8 liters of solution?

101. What is the total number of moles of hydrogen gas contained in 9.03 x 1023



  1. 1.5 moles

  2. 2.00 moles

  3. 6.02 moles

  4. 9.03 moles

102. What is the total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0 M solution of H2SO4?



  1. 2.5

  2. 5.0

  3. 10

  4. 20

103. What is the mass in grams of 3.0 x 1023 molecules of CO2?



  1. 22 g

  2. 44 g

  3. 66 g

  4. 88 g

104. At STP, 32.0 liters of O2 contain the same number of molecules as



  1. 22.4 L Ar

  2. 28.0 L of N2

  3. 32. 0 L of H2

  4. 44.8 L of He

105. What is the molarity of a KF (aq) solution containing 116 grams of KF in 1.00 liter of solution?



  1. 1.00 M

  2. 2.00 M

  3. 3.00 M

  4. 4.00 M

106. Given the reaction CH4 + 2O2 → CO2 + 2H2O,

What amount of oxygen is needed to completely react with 1 mole of CH4?


  1. 2 moles

  2. 2 atoms

  3. 2 grams

  4. 2 molecules

107. What is the total number of moles of hydrogen atoms contained in one mole of (NH4)2C2O2?



  1. 6

  2. 2

  3. 8

  4. 8

  5. 4

108. Given the balanced equation: Mg(s) + 2HCL(aq) → MgCl2(aq) + H2(g)

At STP, what is the total number of liters of hydrogen gas produced when 3.00 moles of hydrochloric acid solution is completely consumed?


  1. 11.2 L

  2. 22.4 L

  3. 33.6 L

  4. 44.8 L

109. What is the oxidation number of chlorine in HClO4?



  1. +1

  2. +5

  3. +3

  4. +7

110. Which compound is a salt?



  1. Na3PO4

  2. H3PO4

  3. CH3COOH

  4. Ca(OH)2

111. Which compound will conduct an electric current when dissolved in water?



  1. NaOH

  2. C2H5OH

  3. C6H12O6

  4. C12H22O11

112. Which statement best describes compounds containing ionic bonds?



  1. These compounds generally contain two non-metals.

  2. These compounds generally contain a metal and a non-metal.

  3. These compounds generally contain two metals.

  4. These compounds generally contain two semi-metals.

113. The molecule F2 is best described by which statement?



  1. This is a slightly polar covalent molecule.

  2. This is a very polar covalent molecule.

  3. This is a very polar ionic molecule.

  4. This is a non-polar covalent molecule.

114. The molecule H2O is best described as:



  1. Ionic molecule

  2. Nonpolar covalent molecule

  3. Polar covalent molecule

  4. Nonpolar Ionic molecule

115. What is the expected shape of the molecule CH4?



  1. triangular

  2. angular

  3. triganol pyramidal

  4. tetrahedral

116. The molar volume of any gases at STP is defined as:



  1. 100.0 liters

  2. 22.4 mL

  3. 22.4 liters

  4. 1.00 liters

117. Which type of reaction is occurring when a metal undergoes corrosion?



  1. oxidation-reduction

  2. neutralization

  3. polymerization

  4. saponification

118. What is the oxidation number of carbon in NaHCO3?



  1. +6

  2. +2

  3. -4

  4. +4

119. Which formula represents a salt?



  1. KOH

  2. KCl

  3. CH3OH

  4. CH3COOH

120. Which element is present in all organic compounds?



  1. carbon

  2. nitrogen

  3. oxygen

  4. phosphorous

121. Which compounds are isomers?



  1. 1-propanol and 2-propanol

  2. methanoic acid and ethanoic acid

  3. methanol and methanal

  4. ethane and ethanol

122. Which statement explains why the element carbon forms so many compounds?



  1. Carbon atoms combine readily with oxygen.

  2. Carbon atoms have very high electronegativity.

  3. Carbon readily forms ionic bonds with other carbon atoms.

  4. Carbon readily forms covalent bonds with other carbon atoms.

123. Which polymers occur naturally?



  1. starch and nylon

  2. starch and cellulose

  3. protein and nylon

  4. protein and plastic

124. What products are obtained with CH4(g) burns completely in an excess of oxygen?



  1. CO and H2O

  2. CO and C

  3. CO2 and H2O

  4. CO2 and CO

125. Which formula represents butane?



  1. CH3CH3

  2. CH3CH2CH3

  3. CH3CH2CH2CH3

  4. CH3CH2CH2CH2CH3

126. A hydrocarbon molecule is considered to be saturated if the molecule contains



  1. Single covalent bonds, only

  2. A double covalent bond, only

  3. A triple covalent bond

  4. Single and double covalent bonds

127. What is the name of the compound that has the molecular formula C6H6?



  1. butane

  2. butene

  3. benzene

  4. butyne

128. In which pair of hydrocarbons does each compound contain only one double bond per molecule?



  1. C2H2 and C2H6

  2. C2H2 and C3H6

  3. C4H8 and C2H4

  4. C6H6 andC7H8

129. The reaction CH2CH2 + H2 → CH3CH3 is an example of



  1. substitution

  2. addition

  3. esterification

  4. fermentation

130. Which compound is a saturated hydrocarbon?



  1. ethane

  2. ethene

  3. ethyne

  4. ethanol

131. What type of reaction is CH3CH3 + Cl2 → CH3CH2Cl + HCl?



  1. an addition reaction

  2. a substitution reaction

  3. a saponification reaction

  4. an esterification reaction

132. What is the maximum number of covalent bonds than an atom of carbon can form?



  1. 1

  2. 2

  3. 3

  4. 4

133. Which class of organic compounds can be represented as R-OH?



  1. acids

  2. alcohols

  3. esters

  4. ethers

134. Which molecule contains a total of three carbon atoms?



  1. 2-methylpropane

  2. 2-methylbutane

  3. propane

  4. butane

135. What substance is made up of monomers joined together in long chains?



  1. ketone

  2. protein

  3. ester

  4. acid

136. Which compound is an organic acid?



  1. CH3OH

  2. CH3OCH3

  3. CH3COOH

  4. CH3COOCH3

137. Which organic compound is classified as a primary alcohol?



  1. Ethylene glycol

  2. Ethanol

  3. Glycerol

  4. 2-butanol

138. For ethyne: C2H2

What is the total number of electrons shared between the carbon atoms?


  1. 6

  2. 2

  3. 3

  4. 4

139. Which set contains one natural polymer and one synthetic polymer?



  1. Cellulose and Starch

  2. Polyethylene and Nylon

  3. Protein and Starch

  4. Protein and Nylon

140. Aldehydes can be synthesized by the oxidation of



  1. Primary alcohols

  2. Secondary alcohols

  3. Organic acids

  4. Inorganic acids

141. Given the reaction: C2H2 + 2H2 → C2H6

This reaction represents:


  1. Substitution

  2. Addition

  3. Esterification

  4. Saponification

142. Which pair of names refers to the same compound?



  1. Ethyne and Acetylene

  2. Ethyne and Ethene

  3. Ethane and Acetylene

  4. Ethane and Ethene

143. A condensation polymerization reaction is best described as the



  1. Joining of monomers by the removal of oxygen

  2. Joining of monomers by the removal of water

  3. Oxidation of a hydrocarbon by oxygen

  4. Oxidation of a hydrocarbon by water

144. Which formula represents a ketone?



  1. CH3COOH

  2. C2H5OH

  3. CH3COCH3

  4. CH3COOCH3

145. The bond between hydrogen and oxygen in a water molecule is classified as



  1. Ionic and Nonpolar

  2. Ionic and Polar

  3. Covalent and Nonpolar

  4. Covalent and Polar

146. What is the total number of hydrogen atoms required to form 1 molecule of C3H5(OH)3?



  1. 1

  2. 5

  3. 3

  4. 8

147. A compound that can act as an acid or a base is referred to as



    1. A neutral substance

    2. An amphoteric substance

    3. A monomer

    4. An isomer

148. Which compound is an electrolyte?



    1. CH3OH

    2. CH3COOH

    3. C3H5(OH)3

    4. C12H22O11

149. Which organic compound is classified as an acid?



    1. CH3CH2COOH

    2. CH3CH2OH

    3. C12H22O11

    4. C6H12O6

150. During fractional distillation, hydrocarbons are separated according to their



    1. Boiling points

    2. Melting points

    3. Triple points

    4. Saturation points

Discussed and confirmed at a meeting of the Department of Chemistry,

16.06.14 Protocol № 11

Head. Department of Сhemistry,

professor N.U.Aliev

Developers:

Nechepurenko E.V.

(in.tel.7219)





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