Chemistry pt1

1. The electrooic configuration of Cu2+ ion is: 3d7 4s2. 3d8 4s1. 3d9 4s0. 3d10 4s1.

2. Which element has the largest atomic radius: Br. K. Mg. Na.

3. Which is the correct order for the listed atoms with increase of the atomic radius?. Li, Be, B, Na. Li, Na, B, Be. Na, Li, Be, B. B, Be, Li, Na.

4. Which of the following pairs of elements and valence electrons is incorrect?. Al - 3. Br - 7. S - 5. Sr - 2.

5. Which one of the formulas for ionie compounds below is incorrect?. Sr Cl2. Cs2 S. Al Cl3. Al3 P2.

6. A n-bond is the result of: overlap of two s-orbitals. overlap of an s- and a p-orbital. overlap of two p-orbitals. overlap of an s- and a d-orbital.

7. A triple bond contains _ s-bond(s) and _ p- bond(s): 0, 3. 3, 0. 2, 1. 1, 2.

8. Consider the species 72 Zn, 75 As and 74 Ge. These species have: the same number of electrons. the same number of protons. the same number of neutrons. the same number of protons and neutrons.

9. Which element has the largest atomic radius?. Li. Na. Rb. F.

10. Which of the following is NOT true for the Group 1A elements?. Most of them are soft, silvery corrosive metals. Their atomic radii increases with increasing molecular weight. They are named the alkaline earth metals. They are excellent conductors of heat and electricity.

11. Which of the following properties of the alkaline earth metals decreases with increasing the atomic weight?. ionie radii. ionization energy. atomic radii. atomic number.

12. Which of the following is NOT true for the halogens?. they are nonmetals. the electronic configuration of their outermost electrons is ns2 np6. their compounds with metals are generally ionie in nature. elemental halogens exist as diatomic molecules.

13. What is the ground electronic state of Mn2+: 1s2 2s2 2p6 3s2 3p6 3d5 4s2. 1s2 2s2 2p6 3s2 3p6 3d3 4s2. 1s2 2s2 2p6 3s2 3p6 3d5. 1s2 2s2 2p6 3s2 3p6 4s2 4p3.

14. Which of the following ions has the smallest ionie radius?. K+. Ca2+. Cl -. Br-.

15. The capability of alcohols to form intermolecular hydrogen bonds leads to: decreased boiling point. poor solubility in water. decreased vapor pressure. increased solubility in non polar solvents.

16. Which of the following elements has the lowest ionization energy?. Be. C. Cs. Li.

17. Which is the correct order of halogen ions with decrease of reductive properties?. F-, Cl-, Br-, I-. I-, Br-, Cl-, F-. F-, l-, Br-, Cl-. Cl-, l-, Br-, F-.

18. Space direction is NOT characteristic for: s- atom orbitals (AO). p-AO. sp-AO. d-AO.

19. Which of the following has the largest a tomie radius?. F. I. Br. Cl.

20. The nucleus of a hydrogen atom consists of: only 1 proton. 1 proton and 2 neutrons. only 1 neutron. only 1 electron.

21. The mass number of an atom is equal to: the number of protons. the number of protons and electrons. the number of nucleons. the number of neutrons.

22. What is the type of the chemical bond between an alkaline and a halogen element?. ionie. covalent polar. covalent nonpolar. donor-acceptor.

23. The element X has an atomic number of 8 and a mass number of 17. The atoms of this element contain: 9 protons. 9 electrons. 9 neutrons. 9 protons and 9 electrons.

24. Which of the following elements exists as a monoatomic gas under standard conditions?. nitrogen. bromine. ozone. neon.

25. The atoms of an element contain an equal number of: protons and neutrons. neutrons and different number of protons. protons. neutrons.

26. Hydrogen may NOT be obtained by: interaction of zinc and hydrochloric acid;. interaction of sodium and water;. interaction of copper and nitric acid;. electrolysis of water;.

27. Which of the listed simple substances can participate in a chemical reaction only as an oxidant?. nitrogen;. sodium;. iron;. fluorine.

28. After interaction of ferric hydroxide (Fe(OH)3) and H2 SO4 are obtained: iron (III) sulphate and water;. iron (III) sulphite and water;. iron (III) sulphide and water;. iron (III) sulphide and hydrogen;.

29. The industrial process of production of sulfuric acid includes the following stages: production of hydrogen sulphide, oxidation of H2S with ozone, dissolving the obtained product in water;. production of S02, catalytic oxidation to S03 and interaction of S03 with water;. displacement of H2S04 from its salts with nitric acid and distillation;. preparation of a mixture of sulfur chlorides and oxidation of the resulting compounds with ozone;.

30. An aqueous solution of sodium carbonate is reacting with solutions of the following substances: HCl, KNO3, Na2 SiO3, NaOH;. Ca(OH)2 , Cu Cl2, NH4 OH, K2 SO4 ;. H2 SO4, Ca Cl2, CH3 COOH, Cu Cl2;. Ba(OH)2 , KCl, NaHCO3 , Na2 S;.

31. For amphoteric hydroxides the following interactions are characteristic: with acids and bases;. only with acids;. only with bases;. with alkenes;.

32. Which of the presented reactions is NOT oxidative-reductive?. interaction of iron with hydrochloric acid;. buming of methane in the presence of oxygen;. interaction of nitrogen with hydrogen;. interaction of calcium hydroxide with sulphuric acid;.

33. Which of the made allegations is true?. in the atom the number of electrons is always equal to the number of neutrons;. the helium atom contains 4 protons;. the outermost electron shell of magnesium has 2 electrons;. the protons circle around a nucleus consisting of electrons and neutrons;.

34. Mark the wrong statement: calcium reacts with water with release of hydrogen, reacts with chlorine, sulfur and oxygen;. magnesium bums in presence of oxygen, but does not internet with sulphuric hydrochloric acid;. sodium easily interacts with most of the non metals, but does interact with methane;. a strong oxide layer on the aluminum surface prevents it from further oxidation;.

35. Mark the list of substances which includes only acid oxides: P2 O5, SO2, Li2 O, CuO, Cl2 O7;. CO2, SO3, SiO2, NO2, SO2;. HgO, CaO, FeO, CuO, MgO;. ZnO, Al2 O3, BaO, Cr2 O3, Ag2 O.

36. A chemical element is: a substance consisting of the same type of atoms;. the smallest particle of a substance possessing its chemical properties;. electro neutral particle, consisting of nucleus and electronic shell;. a set of atoms with the same charge of the nucleus.

37. Mark the line which includes only salts, whose water solutions are basic: sodium carbonate, potassium sulphite, potassium phosphate;. iron (III)nitrate, potassium hydrogen carbonate, copper sulphate ;. iron (III)chloride, sodium sulphide, barium acetate;. copper nitrate, iron (IlI)bromide, magnesium sulphate.

38. Chlorine CANNOT be obtained: from hydrochloric acid and potassium permanganate;. through electrolysis of water solution of calcium chloride;. by interaction of hydrogen chloride with potassium chlorate;. by interaction of sodium chloride with concentrated sulphuric acid;.

39. The degree of dissociation of a weak base: depends on the nature of the base;. depends on the temperature and the pressure but does not depend on the concentration of the solution;. is determined entirely from the solvent type;. depends on the temperature, the concentration and the solvent type;.

40. Oxidation of iron (U) sulfate with an acidic aqueous solution of potassium dichromate yields: Cr2 (S04)3, Fe2(S04 )3, K2SO4. Cr SO4, Fe2(SO4)3, K2 SO4. K3 [Cr(OH)6] and Fe2(SO4)3. Cr O2, Fe2(SO4}3 and K2SO4.

41. To draw the equilibrium in reaction H 2(g) + l2(g) = 2Hl (g) + Q in the direction of hydrogen iodide formation one must: increase the pressure:. use a catalyst;. decrease the temperature;. increase the temperature;.

42. lncreasing the pressure in an equilibrium system containing gas molecules leads to the with drawal of the chemicaI equilibrium in the direction of the reaction: flowing with beat absorption:. flowing with heat release;. flowing with decrease in the gas molecules number;. flowing with incrcase in the gas molecules number.

43. At two fold increase of the pressure, the rates of the straight and the reverse reaction of the systcm A(g) + 2B(g) = AB2 (g) are changed accordingly: straight - increased 8 times, reverse - slowed down 2 times;. straight - increased 8 times, reverse - increased 4 times;. straight - increased 16 times, reverse - increased 8 times;. straight - increased 8 times. reverse - increased 2 times.

44. If the pressure for the reaction A(s) + B(g) = AB(s) is increased 4 times, then the rate of the reaction: will not change;. will increase 8 times;. will increase 4 times:. will increase 16 times;.

45. Which group of substances are NOT electrolytes: H2, H2 SiO3;. MgSO4, HCI;. KOH, HBr;. NaOH, HCI;.

46. The largest number of sodium ions are formed by dissociation of 1 mole: sodium carbonate;. sodium nitrate;. sodium sulphate;. sodium phosphate;.

47. Which of the listed substances are electrolytes (A-aluminium oxide, B-sodium chloride, C-barium hydroxide, D-glucose, E-iron, F-hydrochloric acid. A, B, E;. B, C, F;. C, D, F;. A, C, F;.

48. 10 moles of benzene contain: 10 benzene molecules;. 22.4 benzene molecules;. 6.02x1024 benzene molecules;. 6.02x 1023 benzene molecules;.

49. Which of the listed reactions are ion exchanging? 1) Cr Cl3 + 3Na OH --> Cr(OH3)+ 3NaCI 2) 2Na HCO3 --> Na2 CO3 + CO2 + H2O 3) 2Al + Fe2O3 -->2Fe + A]iO3 4) 2Fe Cl2 + Cl2 --> 2Fe Cl3 5) AgNO3 + KI --> Agl + KNO3. 2,3,4;. 1,5;. 1,3,4;. 2,4;.

50. Between which of the suggestcd atoms (O, S, Na, K, Ca) a covalent potar bond is formed: O and S;. O and K, S and Na;. Ca and S;. all;.

51. ln oxidative-reductive processes the reducer: increases its oxidation number. decreases its oxidation number. loses 1 electron and decreases its oxidation number. gains 1 electron and decreases its oxidation number.

52. In oxidative-reductive processes the oxidizing agent: increases its oxidation number. decreases its oxidation number. loses 1 electron and decreases its oxidation number. gains 1 electron and decreases its oxidation number.

53 . Oxidative-reductive processes could be: intermolecular. intramolecular. disproportionation. all answers are correct.

54. The oxidation number for hydrogen in NaH is: +1. +2. 0. -1.

55. Of the compounds below, in which one does chlorine have the highest oxidation number?. HCl. K CI O3. HCl O2. KCI O4.

56. In the reaction Al+ Fe3+ -Al3+ -->Al3+ + Fe, the oxidizing agent is: Al. Fe. Al3+. Fe3+.

57. In the chemical reaction 2Cr + 3Ni2+ --> 2Cr3+ + 3Ni, which species is reduced?. Cr. Ni2+. Cr3+. Ni.

58. A solution of CuSO4 could be stored in bottles from. Fe. Al. Ni. Ag.

59. When Fe2+ is oxidized to Fe3+, the Fe2+ ion: loses 1 electron. loses 1 proton. gains 1 electron. gains 1 proton.

60. When nonspontaneous redox reactions occur by use of a direct electric current, the process is called: neutralization. eterification. electrolysis. hydrolysis.

61. The degree of ionization depends on the: nature of the solvent and nature of the solute. concentration of the solution. temperature of the solution. all of the above.

62. The method that CANNOT be used for removing permanent hardness of water is: adding sodium carbonate. distillation. adding caustic soda. boiling.

63. The hydroxonium ion is represented as: H2O-. H3 O+. HOH+. H-.

64. In electrolysis of CuCl2, the substance liberated on the anode is: copper. chlorine. hydrogen. copper dichloride.

65. Ionie compounds will conduct an electric current when they are: solidified. melted. frozen. dehydrated.

66. The chemical elements presented are arranged in order of decrease in their reactivity, according to the activity series of metals. Ca, Na, Mg, Zn, Fe, H, Cu, Hg, Ag, Au Which is the best reducing agent, which is oxidized the easiest?. Ca. Au. H. Fe.

67. The cathode in an electrochemical cell is the electrode that is: the electrode where oxidation takes place. always positive. always neutral. the electrode where reduction takes place.

68. During electrolysis of an aqueous solution of NaCl on the cathode is produced: sodium. chlorine. hydrogen. oxygen.

69. Which of the presented factors does NOT affect the reaction rate?. nature of the reactarius. concentration. temperature. time.

70. With addition of a catalyst to a system at equilibrium: the point of equilibrium is shifted to the right. the point of equilibrium is shifted to the left. the forward and reverse reactions rates are increased unequally. the forward and reverse reactions rates are increased equally.

71. A catalyst is added to a system at equilibrium. The concentration of the reactants will: decrease. increase. remain the same. approach zero.

73. The chemical reaction 2Cl2 + H20 <=> O2+ 4HCI is in chemical equilibrium. The rate of the forward reaction is: equal to zero. equal to the rate of the reverse reaction. lower than the rate of the reverse reaction. higher than the rate of the reverse reaction.

74. Hydrogen peroxide is easily decomposed to water and oxygen according to the reaction 2H2 O2 --> 2H 2O + O2. Its stability is increased in the presence of H3 PO4: H3PO4 is positive catalyst and the catalysis is heterogeneous. H3PO4 is positive catalyst and thc catalysis is homogeneous. H3PO4 negative catalyst and the catalysis is heterogeneous. H3PO4 negative catalyst and: the catalysis is homogeneous.

75. For the process CaO(s) + CO2(g) <=> CaCO3(s) the rate of the straight reaction is: v = K.[CaO].[CO2].[CaCO3]. v = K.[CaO].[CO2]. v = K.[CaO]. v= K.[CO2].

76. How many times the rate of the reaction 2NO + O2 --> 2N02 will increase if the concentration of all substances is increased two times?. 16 times. 8 times. 6 times. 4 times.

77. With decreasing of the temperature the rate of chemical reaction: always increases. always decreases. increases or decreases depending on the thermal effect. increases or decreases depending on the activation energy.

78. How many times the rate of the straight reaction in the gas system 2SO2 + O2 <=> 2SO3 will increase if the pressure is increased three times?. 3 times. 6 times. 9 times. 27 times.

79. The reaction rate of a multistage reaction is determined by: the rate of the tirst stage. the rate of the last stage. the rate of the fastest stage. the rate of the slowest stage.

80. The rate constant does NOT depend on the: concentration of the substances. temperature. presence of a catalyst. nature of the substances.

81. The chemical elements of Group IB have: 1 electron in their outermost electronic shell,. 18 electron in their outermost electronic shell,. 2 electron in their outermost electronic shell,. all answers are correct,.

82. CuO: is reduced by hydrogen to Cu,. is oxidized by hydrogen to Cu,. is reduced by hydrogen to oxygen,. does not react with hydrogen.

83. The soluble salts of Group IB elements: may oxidize the metals before them in the Reactivity Series of Metals,. may oxidize the metals behind them in the Reactivity Series of Metals,. since they are soluble they react with all metals,. all answers are correct,.

84. A qualitative.reaction for Cu2+ is: interaction with halogens,. interaction with concentrated nitric acid,. interaction with concentrated sulphuric acid,. obtaining a tetra ammoniurn complex ion.

85. The chemical element Zn is a: group IA element,. group lB element,. group IlB element,. group IlA element,.

86. ZnO is: amphoteric,. acidic,. basic,. neutral,.

87. ZnO may be obtained from: thermal decomposition of Zn(OH)2. thermal decomposition of Zn(NO3 )2,. thermal decomposition of ZnCO3 ,. all answers are correct,.

88. The atomic nucleus is: the positively charged part of the atom,. the negatively charged part of the atom,. neutral,. all answers are correct,.

89. The mass of the proton is approximately equal to: the mass of one hydrogen atom,. the mass of two hydrogen atoms,. the mass of three hydrogen atoms,. the mass of four hydrogen atoms,.

90. The neutron: is not a charged subatomic particle,. is a charged subatomic particle,. is indicated by the symbol m,. is indicated by the symbol N.

91. Z is: the mass number,. the atomic number,. the number of neutrons,. the element Zinc,.

92. The isotopes: occupy one and the same location in the periodic table of elements,. occupy adjacent locations in the periodic table of elements,. are other atoms,. have different atomic numbers.

93. The electron is a subatomic particle which: is not charged,. is positively charged,. is negatively charged,. is not a particle.

94. The principal quantum number: is marked with n and adopts integer values. is associated with the energy of the electron. is related to the size of the electronic cloud. all answers are correct.

95. The azimuthal quantum number: considers the differences in the shape of the electronic clouds. increases with the energy of the individual states. is marked with I and adopts integer values. all answers are correct.

96. The magnetic quantum number: adopts values of 21 for each 1. is related to the energy of the electron. does not take into account the shape and orientation of electron clouds in space. is marked with m.

97. The shape of the wave function /the orbitali is defined by: the quantum numbers n and m. the quantum numbers 1 and m. the quantum numbers n, 1, n. the quantum number 1.

98. Finding the permitted states of electrons: is done with the help of Hund's rule. is done with the help of Pauli's principle. is done with the help of the principal quantum number. all answers are wrong.

100. Which statement for an equiiibrium system is true: the rates of the straight and the reverse reactions are equal. the concentrations of the reactants are equal to the concentrations of the products. the concentrations of the reactants and the products are changed by addition of a catalyst. the concentrations or the reactants and the producls does not change with change in the temperature.

72. The average rate of the homogenous process A+B --> AB could be expressed as: A. B. C. D.

99. What is the equilibrium constant expression, Kc, for the reaction: A. B. C. D.