Pharmaceutical Faculty
Department of General Chemistry
1 Course
Module 1. GENERAL CHEMISTRY
1. Oxides are:
A. BaCO3. CaCl2, MgCl2, Na3PO4, Ca3(PO4)2
B. MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
C. CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn(OH)2
D. KOH, C, Cl2, CuO, HSO4, NaH
E. HCl, HBr, H2S, HNO3, H3PO4
ANSWER: B
2. Bases are:
A. BaCO3. CaCl2, MgCl2, Na3PO4, Ca3(PO4)2
B. MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
C. CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn(OH)2
D. KOH, C, Cl2, CuO, HSO4, NaH
E. HCl, HBr, H2S, HNO3, H3PO4
ANSWER: C
3.
Choose the simple compound:
A. СО2
B. H2O
C. О2
D. CO
E. HNО3
ANSWER: C
4. Formula of molecule is:
A. O2
B. O-2
C. 2O
D. 3O
E. ОНANSWER: A
5.
Bases are:
A. Compound which molecules consist of one-type atoms
B. Complex substances that consist from two elements, one of which is oxygen
C. Complex substances in which atoms of metals bonded with one or several hydroxyls groups
D. Complex substances that consist from hydrogen atoms
E. Complex substances which consist from atoms of metal and acid residuals
ANSWER: C
6.
Oxides are:
A. Compound which molecules consist of one-type atoms
B. Complex substances that consist from two elements, one of which is oxygen
C. Complex substances, in which atoms of metals bonded with one or several hydroxyls groups
D. Complex substances that consist from hydrogen atoms
E. Complex substances, which consist from atoms of metal and acid residuals
ANSWER: B
7.
Acids are:
A. Compound which molecules consist of one-type atoms
B. Complex substances that consist from two elements, one of which oxygen
C. Complex substances in which atoms of metals bonded with one or several hydroxyls groups
D. Complex substances that consist from hydrogen atoms
E. Complex substances which consist from atoms of metal and acid residuals
ANSWER: E
8.
Choose oxygen-containing acids:
A. H2SO4
B. HI
C. HCl
D. HBr
E. H2S
ANSWER: A
9.
Relative atomic mass of Oxygen is:
A. 16
B. 18
C. 12
D. 15
E. 8
ANSWER: A
10. Avogadro’s number is:
A. 3.01 ·1020 mol–1
B. 6.02 ·1022 mol–1
C. 3.01 ·1023 mol–1.
D. 6.02 ·1025 mol–1
E. 6.02 ·1023 mol–1
ANSWER: E
11. What concept can to consider is correct?
A. The atom of Oxygen
B. The molecule of Oxygen
C. The molecule of Hydrogen
D. The atom of ozone
E. The atom of Mor's salt
ANSWER: A
12. The molar mass of sulfuric acid H2SO4 is:
A. 65 g/mol
B. 98 g/mol
C. 106 g/mol
D. 80 g/mol
E. 98 g
ANSWER: B
13. How many groups are in periodical table?
A. 5
B. 4
C. 9
D. 8
E. 6
ANSWER: D
14. What equivalent weight has potassium hydroxide NaOH?
A. 78 g/eq
B. 28 g/eq
C. 56 g/eq
D. 9 g/eq
E. 65 g/eq
ANSWER: C
15. What element has the most nonmetallic properties?
A. Ag
B. F
C. P
D. Na
E. S
ANSWER: B
16. What element has the most metallic properties?
A. Cl
B. Fr
C. F
D. Al
E. O
ANSWER: B
17. How many periods are in periodical table?
A. 3
B. 4
C. 7
D. 8
E. 6
ANSWER: C
18. The atomic mass of the element is determined as:
A. Sum mass of protons which are in nucleus
B. Sum mass of all electrons which are in main electronic levels
C. Sum mass of all protons and neutrons which are in nucleus
D. Sum mass of neutrons which are in nucleus
E. Sum mass of all electrons which are in atom
ANSWER: C
19. What type of chemical bond is between the water molecules?
A. Ionic
B. Hydrogen
C. Polar covalent
D. Non-polar covalent
E. Metallic
ANSWER: B
20. Two or more atoms which have the same atomic number but the difference atomic mass are:
A. Spin
B. Isotopes
C. Isotones
D. Isochors
E. Protons
ANSWER: B
21. Choose the electronic configuration (formula) of Hydrogen:
A. 1s1
B. 1s2
C. 1s12s1
D. 1s22s1
E. 1s3
ANSWER: A
22. To select a formula of the crystallohydrate:
A. H2O
B. HCl + H2O
C. NaOH + H2O
D. KCl + H2O
E. CuSO4*5H2O
ANSWER: E
23. To select the row of substances that forms a liquid solution:
A. Sulfuric acid and water
B. Copper and nitrogen
C. Hydrogen and helium
D. Sand and water
E. Oxygen and carbon monoxide
ANSWER: A
24. To choose the correct record the dimension of the molar concentration:
A. mol/l
B. kg/ mol
C. mol /kg
D. g/ml
E. % or fraction from 1
ANSWER: A
25. Solution is:
A. Heterogeneous system which consists of two components
B. Homogeneous system which consists of two or more components and their products
C. Heterogeneous system which consists of two or more components and their products
D. Heterogeneous system in which it is impossible to distinguish component parts
E. Homogeneous system which consists of one component
ANSWER: B
26. How many grams of a solute do contain in 100 g 15 % solution of glucose?
A. 25 g
B. 15 g
C. 100 g
D. 85 g
E. 20 g
ANSWER: B
27. To select a formula of the crystallohydrate:
A. Li2O + H2O
B. MgSO4*7H2O
C. H2O
D. KOH
E. KCl + H2O
ANSWER: B
28. As an antiseptic in a medicine uses (as an external) an aqueous solution of potassium
permanganate with a mass fraction KMnO4 0.2%. What mass of salt does need to prepare of such
solution by the mass 100g?
A. 2 g
B. 0.02 g
C. 0.2 g
D. 0.1 g
E. 2 g
ANSWER: C
29. What is the color of phenolphthalein in an acid solution?
A. Yellow
B. Colourless
C. Red
D. Violet
E. Orange
ANSWER: B
30. What is the process according to this reaction of H2(g)+ Cl2(g) + h  2HCl(g) + Q:
A. Exothermic
B. Endothermic
C. Adiabatic
D. Extensive
E. Intensive
ANSWER: A
31. How can you classify thermodynamics systems according to their phases?
A. Solid, liquid, gaseous
B. Homogeneous and heterogeneous
C. Isolated, opened, closed
D. Equilibrium and unequilibrium
E. Combustion, synthesis, decomposition
ANSWER: B
32. Record of reaction of N2(g)+ O2(g.)= 2NO(g.) – 180,8 kJ/mol means that:
A. For formation 1 mol of NO is taken of 100,0 kJ heat
B. For formation 1 mol NO is released 180,8 kJ heat
C. For formation1 mol N2 and 1 mol O2 is released 180,8 кJ heat
D. For formation 1 mol N2 and 1 mol O2 is released 90,4 kJ heat
E. For formation 2 mol NO is released 180,8 kJ heat
ANSWER: E
33. Enthalpy is measured in:
A. kJ/mol
B. kJ
C. kkal
D. kJ/mol*K
E. kkal/K
ANSWER: A
34. What substance has a standard enthalpy of formation of zero?
A. О2
B. СО2
C. Н2O
D. С6Н12О6
E. NO
ANSWER: A
35. All the vital biochemical processes in living organisms take place with the biochemical
catalysts, which are called:
A. Enzymes
B. Elements
C. Rudiments
D. Albuminaties
E. Carbohydrates
ANSWER: A
36. Record of reaction of C(graphite) + O2(g) = CO2(g), ∆H° = -393 kJ/mol means that:
A. For formation 1 mol of CO2 is taken of 393 kJ heat
B. For formation 2 mol of CO2 is taken of 393 kJ heat
C. For formation 1 mol of CO is taken of 393 kJ heat
D. For formation 1 mol of CO2 is taken of 196.5 kJ heat
E. For formation 1 mol of CO2 is taken of 98.25 kJ heat
ANSWER: A
37. Record of reaction 2H2+ O2  2H2O + 571 kJ/mol means that:
A. For formation 0,5 mol of water is selected 285,5 kJ heat
B. For formation 2 mol of water is taken in 571 kJ heat
C. For formation 0,5 mol of water is selected 145,75 kJ heat
D. For formation 0,5 mol of water is taken in 285,5 kJ heat
E. For formation 1 mol of water is selected 285,5 kJ heat
ANSWER: B
38. Thermodynamics state when V = const is named:
A. Isochoric
B. Isothermal
C. Adiabatic
D. Isobaric
E. There is not right answer
ANSWER: A
39. Thermodynamics state when p = const is named:
A. Isochoric
B. Isothermal
C. Adiabatic
D. Isobaric
E. There is not right answer
ANSWER: D
40. Thermodynamics state when T = const is named:
A. Isochoric
B. Isothermal
C. Adiabatic
D. Isobaric
E. There is not right answer
ANSWER: B
41. What are parameters cann’t characterize solution?
A. Density, mass fraction
B. Temperature, pressure and concentration
C. Volume
D. Mass
E. Dissociation constant
ANSWER: E
42. Isothermic process is:
A. А process is carried out in such а manner that the temperature remains constant throughout
the process
B. A process is carried out in such а manner that no heat can flow from the system to the
surroundings or conversely i.e. the system is completely insulated from the surroundings
C. А process during which the volume of the system is kept constant
D. А process during which the pressure of the system is kept constant
E. А process which is carried out infinitesimally slowly so that all changes occurring in the
direct process can be exactly reversed
ANSWER: A
43. Isobaric process is:
A. А process is carried out in such а manner that the temperature remains constant throughout
the process
B. A process is carried out in such а manner that no heat can flow from the system to the
surroundings or conversely i.e. the system is completely insulated from the surroundings
C. А process during which the volume of the system is kept constant
D. А process during which the pressure of the system is kept constant
E. А process which is carried out infinitesimally slowly so that all changes occurring in the
direct process can be exactly reversed
ANSWER: D
44. The catalysis in which rate of reaction increase is named:
A. Heterogeneous catalysis
B. Catalysis
C. Positive catalysis
D. Negative catalysis
E. Autocatalysis
ANSWER: C
45. The processes in which both catalyst and reagents are in different phase are called:
A. Heterogeneous catalysis
B. Homogeneous catalysis
C. Positive catalysis
D. Negative catalysis
E. Autocatalysis
ANSWER: A
46. Isotonic solutions are the solutions having the same:
A. Surface tension
B. Vapour pressure
C. Osmotic pressure
D. Viscosity
E. Mass
ANSWER: C
47. Cations are:
A. Positively charged ions
B. Negatively charged ions
C. Neutral particles
D. Cathode
E. Anode
ANSWER: A
48. What ion has the name of the hydronium ion?
A. Н3О+
B. ОНC. Н2О
D. Н+
E. О2ANSWER: A
49. What is the degree of dissociation of an electrolyte, if for every 100 of his molecules, 68
collapsed on ions?
A. 68 %
B. 32 %
C. 100 %
D. 86 %
E. 30 %
ANSWER: A
50. The number of the degrees of dissociation of phosphoric acid H3PO4 is:
A. 1
B. 2
C. 5
D. 4
E. 3
ANSWER: E
51. The interaction between NaOH and H2SO4 describes the following short ionic-molecular
equation:
A. CH3COO- + H+ CH3COOH
B. H+ + OH-  H2O
C. NaOH + H+ Na2SO4 + H2O
D. 2NaOH + H2SO4  Na2SO4 + 2H2O
E. 2Na+ + 2H+ 2NaH
ANSWER: B
52. The interaction between sodium carbonate and nitric acid is a reaction between the
substances…:
A. Na2C + H2SO3
B. Na2CO3 + H2SO4
C. Na2CO3 + HNO3
D. Na2C + HNO2
E. Na2C + HNO2 + CO2
ANSWER: C
53. Anions are:
A. Positively charged ions
B. Negatively charged ions
C. Natural particles
D. Anode
E. Cathode
ANSWER: B
54. What ion has the name of carbonate ion?
A. СО32
B. С2О42
C. НСО3
D. СН3СОО
E. НС2О4 –
ANSWER: A
55. To choose the formula of an ampholyte:
A. Аl(OH)3
B. NaCl
C. К2SO4
D. НСl
E. NaOH
ANSWER: A
56. What electrolyte is a strong electrolyte?
A. HNO3
B. H2SiO3
C. N2O5
D. Na
E. H2S
ANSWER: A
57. What substance is forming the Mn2 + ions after process dissociation?
A. KMnO4
B. Na2MnO4
C. MnCl2
D. MnO2
E. К2MnO4
ANSWER: C
58. рН = 6.5. What is the medium of a solution:
A. Strong alkaline
B. Neutral
C. Weakly acidic
D. Weakly alkaline
E. Strong acid
ANSWER: C
59. What is рН of a base solution?
A. рН – 7
B. рН < 7
C. рН = 7
D. рН >7
E. рН = 4
ANSWER: D
60. Ampholytes (amphoteric substances) in aqueous solution:
A. Dissociate only at the high concentrations
B. Dissociate only in the presence of acids
C. Do not dissociate on ions, and decay without the formation of ions
D. Dissociate as a base and as acid
E. Dissociate only in the presence of bases
ANSWER: D
61. What value of water product?
A. Кw = 10-7
B. Кw = 107
C. Кw = 10
D. Кw = 10-14
E. Кw = 10-10
ANSWER: D
62. pH of a neutral solution is:
A. pH = 2
B. pH = 10
C. pH = 7
D. pH = 4
E. pH = 12
ANSWER: C
63. What electrolyte is forming the chloride-ions after process dissociation?
A. KClO3
B. Ca(ClO)2
C. FeCl3
D. NaClO
E. NaClO4
ANSWER: C
64. What particle is an anion?
A. Fe3+
B. Mn2+
C. SO42–
D. K+
E. S
ANSWER: C
65. Which solution doesn’t change the pH at the adding to it a little quantity of a base or acid?
A. Acidic
B. Basic
C. Buffer
D. Neutral
E. Saturated
ANSWER: C
66. Physiological solution is a solution that contains the salts and other constituents in
concentrations similar to physiological media with 0.98 % percent by weight of:
A. NaCl
B. CO2
C. KNO3
D. Hg2Cl2
E. None of the above
ANSWER: A
67. Where is Sulfur only reducing agent?
A. SO2
B. H2S
C. SO3
D. H2SO3
E. SO3
ANSWER: B
68. Determine the oxidation state of Mn in this compound KMnO4:
A. +3
B. +2
C. +5
D. +6
E. +7
ANSWER: E
69. What is central ion in complex compound [Cu(NH3)4]CrO4?
A. Ammine
B. Copper
C. Chromium
D. Oxygen
E. Hydrogen
ANSWER: B
70. What is the name of the process which is characterized by the giving of the electrons?
A. Oxidation
B. Reduction
C. Electrolysis
D. Electroosmosis
E. Electrophoresis
ANSWER: A
71. The substance that contains the element which taking electrons is named:
A. Oxidizing agent
B. Reduction agent
C. Acceptor
D. Donor
E. Electrolyte
ANSWER: A
72. Determine the oxidation number of chlorine in this compound HClO.
A. -1
B. +2
C. +7
D. -2
E. +1
ANSWER: E
73. What compound cannot dissolve in water at standard state?
A. Acetic acid
B. Ethanol
C. Sodium chloride
D. Oil
E. Sugar
ANSWER: D
74. Hypertonic solution is:
A. Solution that has a lower osmotic pressure than in blood plasma
B. Solution that has the same osmotic pressure as blood plasma
C. Solution that has the greater osmotic pressure then blood plasma
D. Solution in which the concentration of solute is greater than in a saturated solution
E. Solution in which the concentration of solute is less than in a saturated solution
ANSWER: C
75. Hypotonic solution is:
A. Solution that has a lower osmotic pressure than in blood plasma
B. Solution that has the same osmotic pressure as blood plasma
C. Solution that has the greater osmotic pressure then blood plasma
D. Solution in which the concentration of solute is greater than in a saturated solution
E. Solution in which the concentration of solute is less than in a saturated solution
ANSWER: A
76. What formula is used for calculate pH of solution?
A. КW = [Н+][ОН-]
B. рН = - lg[Н+]
C. рН = - lg[ОН-]
D. рН = lg[Н+] lg[ОН-]
E. рН = - lg[Н+] lg[ОН-]
ANSWER: B
77. The oxidation-reduction reactions are reaction in which:
A. Molecules are dissociated into ions
B. Acid-basic interaction
C. Change of oxidation number of elements
D. Hydrolyzed of salt
E. Dissociate of acids
ANSWER: C
78. What micro element is in erythrocytes?
A. Sodium
B. Vanadium
C. Fluorine
D. Bromine
E. Iron
ANSWER: E
79. What element is in bones?
A. Sodium
B. Vanadium
C. Fluorine
D. Calcium
E. Iron
ANSWER: D
80. What oxidation number of Sodium which present in human body (NaCl)?
A. +3
B. 0
C. +1
D. +4
E. +2
ANSWER: C
81. What oxidation number of Potassium in KCl?
A. +3
B. +1
C. 0
D. +4
E. +2
ANSWER: B
82. What oxidation number of Chlorine in KCl?
A. +3
B. +1
C. 0
D. -1
E. +5
ANSWER: D
83. The species formed by linking of а number of ions or molecules by co-ordinate bonds to the
central metal atom (or ion) carries positive or negative charge, it is called:
A. Acid
B. Base
C. Complex ion
D. Oxide
E. Alloy
ANSWER: C
84. What mass fraction of sugar in a solution does contain 10 g sugar in 20 g of a solution?
A. 20 %
B. 30 %
C. 10 %
D. 50 %
E. 60 %
ANSWER: D
85. What mass fraction of salt in a solution does contain 20 g salt in 100 g of a solution?
A. 20 %
B. 30 %
C. 10 %
D. 50 %
E. 60 %
ANSWER: A
86. Neutral ligands are all except:
A. NН3
B. Н2О
C. CO
D. ClE. CS
ANSWER: D
87. Negative ligand is:
A. NН3
B. ClC. Н2О
D. CO
E. CS
ANSWER: B
88. Neutral ligand is:
A. NO3B. Н2О
C. CO3D. ClO2+
E. NO+
ANSWER: B
89. Positive ligand is:
A. NO3B. Н2О
C. CO3D. ClO2+
E. NO
ANSWER: D
90. Choose the substance solubility which is increase with increasing pressure:
A. Sodium sulfate
B. Ethanol
C. Nitrogen
D. Acetic acid
E. Calcium hydroxide
ANSWER: C
91. Solid solution is:
A. Mixture of N2 and О2
B. Mixture of clay and water
C. Solution of sand and oil
D. Solution of copper sulfate
E. Alloy of nickel and copper
ANSWER: E
92. Hemolysis is phenomenon when cells are placed in а sodium chlorate solution with:
A. 0,9 %
B. 2,9 %
C. 0,5 %
D. 1,5 %
E. 2,5 %
ANSWER: C
93. The matters which increase activity of catalyst named:
A. Promoter (activator)
B. Inhibitors
C. Hormones
D. Indicators
E. Enzyme
ANSWER: A
94. The matters which inactive of catalyst named:
A. Promoters
B. Inhibitors
C. Hormone
D. Indicator
E. Enzyme
ANSWER: B
95. Catalyst influence for:
A. Change of chemical equilibrium
B. Increase temperature
C. Increase pressure
D. Rate of reaction
E. Increase volume
ANSWER: D
96. The catalysis in which rate of reaction decrease is named:
A. Heterogeneous catalysis
B. Homogeneous catalysis
C. Positive catalysis
D. Negative catalysis
E. Autocatalysis
ANSWER: D
97. The processes in which both catalyst and reagents are in same phase are called:
A. Heterogeneous catalysis
B. Homogeneous catalysis
C. Positive catalysis
D. Negative catalysis
E. Autocatalysis
ANSWER: B
98. Determine the oxidation state of Sulphur in this compound H2SO4:
A. +3
B. +2
C. +5
D. +6
E. +7
ANSWER: D
99. Determine the oxidation state of Carbon in this compound K2CO3:
A. +3
B. +4
C. +5
D. +6
E. +7
ANSWER: B
100. Acids are:
A. BaCO3, CaCl2, MgCl2, Na3PO4, Ca3(PO4)2
B. MgO, Al2O3, Cr2O3, SO3, P2O5, CrO3
C. CuOH, NaOH, Ba(OH)2, Fe(OH)3, Zn (OH)2
D. KOH, C, Cl2, CuO, HSO4, NaH
E. HCl, HBr, H2S, HNO3, H3PO4
ANSWER: E