General, Organic, and Biochemistry Hybrid Edition by 2nd Edition by James Armstrong-Test Bank

 

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Sample Test

Chapter_03_Chemical_Bonds     True / False

 

1. The element Co (cobalt) satisfies the octet rule.   a. True   b. False   ANSWER:   False

 

2. Based on the number of valence electrons, sulfur (S) would normally form 1 bonds.   a. True   b. False   ANSWER:   False

 

3. In the following compound, phosphorus (P) would be at the center of the molecule. PBrClF   a. True   b. False   ANSWER:   True

 

4. A possible bonding pattern for an element in Group 5A would be to form one single bond and one double bond.   a. True   b. False   ANSWER:   True

 

5. Based on electronegativity values, in the bond shown below, nitrogen will have the negative charge. H—N   a. True   b. False   ANSWER:   True

 

6. The formula that corresponds to the IUPAC name dichlorine monoxide is Cl2O.   a. True   b. False   ANSWER:   True

 

7. Metals gain electrons to become ions in ionic compounds.   a. True   b. False   ANSWER:   False

 

8. The compound represented below contains two single covalent bonds.   a. True   b. False   ANSWER:   False

 

9. The compound represented below has the formula Na2S.   a. True   b. False   ANSWER:   True

 

10. The name for the compound formed between Co3+ and O2- is cobalt(II) oxide.   a. True   b. False   ANSWER:   False

 

11. Phosphorus must gain three electrons to obey the octet rule.   a. True   b. False   ANSWER:   True

 

12. The Lewis structure for Cl2O could be written as:   a. True   b. False   ANSWER:   True

 

13. Potassium tends to form a cation (K+).   a. True   b. False   ANSWER:   True

 

14. Chloride ion (Cl–) is an anion because it has lost an electron.   a. True   b. False   ANSWER:   False

 

15. Sodium loses an electron in forming an ion which gives the ion a +1 charge.   a. True   b. False   ANSWER:   True

 

16. Strontium forms an anion by losing two electrons.   a. True   b. False   ANSWER:   False

 

17. Aluminum and oxygen form a compound with the formula Al2O3. Oxygen and gallium (Ga) could from a compound with a formula unit containing two oxygen atoms and three gallium atoms.   a. True   b. False   ANSWER:   False

 

18. Sodium combines with oxygen to form Na2O. The expected formula between lithium and tellurium would be Li2Te.   a. True   b. False   ANSWER:   True

 

19. Examine the following image showing a “subatomic” level diagram of two atoms forming a bond. The type of bond formed is a single covalent bond.   a. True   b. False   ANSWER:   False

 

20. Using normal bonding requirements for atoms, the following correctly shows the bonding in a compound with the formula C2H3N.   a. True   b. False   ANSWER:   False

 

21. Neither O or F can from triple bonds.   a. True   b. False   ANSWER:   True

 

22. The following is a statement of the octet rule. Representative elements normally form compounds in which each atom has eight electrons in its outermost shell.   a. True   b. False   ANSWER:   True

 

23. Calcium carbonate is used as a phosphate binder to treat someone with too much phosphate, known as hyperphosphatemia, as can be seen in renal/kidney failure. The formula for this compound is CaCO3.   a. True   b. False   ANSWER:   True

 

24. 18.01 g of water (H2O) and 36.46 g of HCl contain the same number of molecules.   a. True   b. False   ANSWER:   True

 

Multiple Choice

 

25. How many bonds does a carbon atom typically form?   a. 2   b. 4   c. 6   d. 8   ANSWER:   b

 

26. An element with the following Lewis structure would most likely form how many covalent bonds?   a. 1 b. 2   c. 3 d. 4   ANSWER:   d

 

27. Which of the following is a correct electron dot formula for ICl?   a. b.   c. d.   e. f.   ANSWER:   a

 

28. How many electrons are associated with a double bond?   a. 1   b. 2   c. 4   d. 6   ANSWER:   c

 

29. High electronegativities are associated with which type of elements?   a. metals   b. metalloids   c. noble gases   d. nonmetals   ANSWER:   d

 

30. Which of the following statements is generally true about electronegativity?   a. Electronegativity decreases as we move left to right and decreases as we move top to bottom.   b. Electronegativity decreases as we move left to right and increases as we move top to bottom.   c. Electronegativity increases as we move left to right and decreases as we move top to bottom.   d. Electronegativity increases as we move left to right and increases as we move top to bottom.   ANSWER:   c

 

31. In which of the following cases is a polar covalent bond formed?   a. when an electron is transferred from one atom to another   b. when the electrons of a bond are shared equally by the two atoms   c. when the electrons of a bond are shared unequally by the two atoms   d. when a metallic element forms a bond with a non-metallic element   ANSWER:   c

 

32. When we name a molecular binary compound which of the following is true?   a. The element that has more atoms in the molecule is named first.   b. The elements are named in alphabetical order.   c. The less electronegative element is named first.   d. The more electronegative element is named first.   ANSWER:   c

 

33. What is the correct IUPAC name for a compound with the formula N2O3?   a. nitrogen oxide   b. nitrogen trioxide   c. nitrogen ozide   d. dinitrogen trioxide   ANSWER:   d

 

34. Which of the following is an acceptable way to represent dinitrogen monoxide?   a. N2O   b. nitric oxide   c. NO2   d. both a and b   ANSWER:   a

 

35. In order to satisfy the octet rule, an atom with the following electron arrangement can shell 1: 2 electrons shell 2: 8 electrons shell 3: 5 electrons   a. gain three electrons.   b. gain two electrons.   c. gain one electron.   d. lose three electrons.   ANSWER:   a

 

36. An ionic bond is associated with which of the following?   a. interactions between nuclei   b. equal sharing of electrons   c. unequal sharing of electrons   d. the transfer of electrons   ANSWER:   d

 

37. Which of the following occurs when an ionic bond is formed?   a. Electrons are transferred from the more electronegative element to the less electronegative element.   b. Electrons are transferred from the less electronegative element to the more electronegative element.   c. Electrons are shared equally.   d. Electrons are shared unequally.   ANSWER:   b

 

38. When an ionic compound forms between aluminum (Al) and nitrogen (N) atoms,   a. nitrogen donates electrons to aluminum.   b. nitrogen attains a positive charge and aluminum a negative charge.   c. aluminum donates electrons to nitrogen.   d. both a and b   ANSWER:   c

 

39. Using most common charges, the ionic compound that forms between calcium (Ca) and sulfur (S) has the formula   a. Ca2S   b. CaS   c. CaS2   d. Ca2S3   ANSWER:   b

 

40. Which of the following occurs when a sulfur atom is converted to S2–?   a. The sulfur atom gains two electrons and loses two protons.   b. The sulfur atom gains two electrons.   c. The sulfur atom loses two electrons and two protons.   d. The sulfur atom loses two electrons.   ANSWER:   b

 

41. Which of the following elements could form more than one compound with bromine (Br)?   a. Fe   b. Cs   c. Li   d. Al   ANSWER:   a

 

42. The anion in an ionic compound whose name ends in “-ide” is   a. always a monoatomic ion.   b. always a polyatomic ion.   c. either a monoatomic or polyatomic ion.   d. positively charged.   ANSWER:   c

 

43. The tin compound used to strengthen teeth has the formula SnF2. Which of the following is the correct IUPAC name for this compound?   a. tin difluoride   b. monotin difluoride   c. tin fluoride   d. tin(II) fluoride   ANSWER:   d

 

44. Which of the following metals would not use a Roman numeral as part of its name in a compound?   a. Cr   b. Mn   c. Co   d. Ca   ANSWER:   d

 

45. The correct name for K2SO4 is   a. potassium sulfate.   b. potassium sulfide.   c. potassium sulfite.   d. potassium tetrasulfoxygen.   ANSWER:   a

 

46. What is the correct name for BaI2?   a. barium iodine   b. barium iodide   c. barium diiodide   d. monobarium diiodide   ANSWER:   b

 

47. What is the formula for a compound named calcium nitride?   a. CaN   b. Ca3N2   c. Ca2N3   d. Ca3N   ANSWER:   b

 

48. The correct formula of an ionic compound containing Fe2+ and ClO is   a. FeClO4   b. Fe2(ClO4)3   c. Fe(ClO4)2   d. Fe3(ClO4)2   ANSWER:   c

 

49. Which of the following has the highest electronegativity?   a. O   b. N   c. Si   d. P   ANSWER:   a

 

50. Which of the following pairs of elements is most likely to form a covalent bond?   a. Fe and H   b. Cs and Br   c. Cl and O   d. Zn and S   ANSWER:   c

 

51. Which is most likely true for an atom with one valence electron?   a. It will gain one electron.   b. It will gain two electrons.   c. It will lose one electron.   d. It will lose two electrons.   ANSWER:   c

 

52. What is the name of the species formed when a bromine atom gains an electron?   a. bromate   b. bromide ion   c. bromine   d. bromine ion   ANSWER:   b

 

53. What type of particles can atoms gain or lose when they become ions?   a. protons   b. neutrons   c. electrons   d. It depends on the atom involved.   ANSWER:   c

 

54. An ion of phosphorus has a –3 charge. Which of the following is true?   a. It is a cation.   b. It contains more protons than electrons.   c. It contains 18 electrons.   d. It contains 12 protons.   ANSWER:   c

 

55. How many bonding electron pairs are represented in the following Lewis structure?   a. 2   b. 4   c. 8   d. 12   ANSWER:   a

 

56. The following represents the formation of bond between atoms A and X. Based on this diagram which element is more electronegative?   a. A   b. X   c. A and X have the same electronegativity.   ANSWER:   b

 

57. Consider the molecule shown below. ClCFBrI Which element in this molecule is the central atom?   a. Cl   b. C   c. F   d. Br   e. I   ANSWER:   b

 

58. What is the correct IUPAC name for the following compound? SBr2   a. sulfur dibromide   b. sulfur(II) bromide   c. monosulfur dibromide   d. sulfur bromide   ANSWER:   a

 

59. What is the formula for the compound named as tetraphosphorus decoxide? Assume “deca” represents 10.   a. P4O10   b. P2O5   c. P10O4   d. PO4   ANSWER:   a

 

60. What is the mass of 1.00 mol of sulfur trioxide?   a. 48.06 g   b. 80.06 g   c. 32.06 g   d. 112.18 g   ANSWER:   b

 

61. How many moles of oxygen are in 1.00 mol of carbon monoxide?   a. 1 mol   b. 2 mol   c. 4 mol   d. 3 mol   ANSWER:   a

 

Completion

 

Phosgene is a compound used as a building block of some pharmaceuticals. It contains two chlorine atoms, one oxygen atom, and one carbon atom. Complete the following statement using the appropriate chemical symbol for the elements.

 

62. The central atom in phosgene is_____________________. ANSWER:   C carbon

 

63. In the Lewis structure for phosgene, there is a double bond between_____________________and ____________________. ANSWER:   C, O O, C carbon, oxygen oxygen, carbon

 

64. In the Lewis structure for phosgene, two electrons are shared between the___________________ atom and the ____________________atom. ANSWER:   C, Cl Cl, C carbon, chlorine chlorine, carbon

 

65. Based on electronegativity values, the _________________________atom in phosgene would have a positive charge. ANSWER:   C carbon

 

66. In the Lewis structure for phosgene, the _____________________atom has four nonbonding electrons. ANSWER:   O oxygen

 

The following is the Lewis structure for the compound commonly known as acetylene   Fill in the blanks with the appropriate integer including zero if necessary (0, 1, 2, 3, etc.).

 

67. There are____________________single bonds in acetlyene. ANSWER:   2 two

 

68. Acetylene contains_____________________nonbonding electrons. ANSWER:   0 zero

 

69. __________________atoms in acetylene obey the octet rule. ANSWER:   2 two

 

Aluminum (Al) and sulfur (S) combine to form an ionic compound. Fill in the blank with the symbol for the appropriate element.

 

70. In the formation of this compound _____________________gains electrons and __________________loses electrons. ANSWER:   S, Al sulfur, aluminum S, aluminum sulfur, Al

 

71. The formula for the ionic compound formed contains two_______________________ions and three ______________________ions. ANSWER:   Al, S aluminum, sulfur aluminum, sulfide Al, sulfur Al, sulfide aluminum, S

 

72. In the formation of this ionic compound, the _____________________atom attains a –2 charge. ANSWER:   S sulfur

 

73. Enter an integer number (1, 2, 3, …) in the blank. How many electrons are in shell 2 of a N3– ion? ____________________electrons ANSWER:   8 eight

 

74. N3– and O2– have the same number of _____________________. ANSWER:   electrons valence electrons

 

75. Which atom will be positively charged (if any) in the following bond? Enter the symbol for the element or none as appropriate in the blank. P-P ________ ANSWER:   none

 

76. Which Group 5A element has the strongest attraction for electrons? Enter the chemical symbol in the blank. ________ ANSWER:   N

 

77. Which Period 3 element has the weakest attaction for electrons? Enter the chemical symbol in the blank. ________ ANSWER:   Na

 

Subjective Short Answer

 

78. Redraw the following Lewis structure using lines to represent bonding electron pairs. ANSWER:   H—O—Cl

 

79. Draw the Lewis structure for the following using lines to represent bonding electron pairs. SiF4 ANSWER:

 

80. Draw the Lewis structure for the following using lines to represent bonding electron pairs. CS2 ANSWER:

 

81. Draw the Lewis structure for the following using lines to represent bonding electron pairs. H2O2 ANSWER:

 

82. Write the formula that corresponds to the name given below. phosphorous trichloride ANSWER:   PCl

 

83. Write the name that corresponds to the formula given below. NF3 ANSWER:   nitrogen trifluoride

 

Chapter_05_Solution_Concentration   1. A normal saline solution is a 0.90% (w/v) aqueous solution of NaCl. This is the same as:   a. True   b. False   ANSWER:   False

 

2. The %(v/v) of a solution can be defined as:   a. True   b. False   ANSWER:   False

 

3. Solution contains 55 mg of magnesium in 2.5 L of solution. The concentration of this solution is 2.2 mg/dL.   a. True   b. False   ANSWER:   True

 

4. The concentration of cholesterol in plasma was determined to be 215 mg/dL. The mass of cholesterol in 59.1 mL of this plasma is 127 mg.   a. True   b. False   ANSWER:   True

 

5. The total molarity of an intravenous solution is given on the label as 151 mEq/L. The osmolarity of this solution is also 151 mEq/L.   a. True   b. False   ANSWER:   True

 

6. Dialysis and osmosis are used for the same purposes.   a. True   b. False   ANSWER:   False

 

7. The osmotic pressure of a 0.10 M NaCl solution will be the same as that of a 0.10 M urea solution.   a. True   b. False   ANSWER:   False

 

8. Putting a celery stick in distilled water results in the uptake of water by the celery.   a. True   b. False   ANSWER:   True

 

9. The conversion factor for converting from moles of HPO42–- to equivalents is:   a. True   b. False   ANSWER:   True

 

10. For a 2.00 M solution, the conversion factor for determining the number of moles of solute in a given volume of solution is:   a. True   b. False   ANSWER:   True

 

11. There is a 9 M aqueous HCl solution in the stock room, but a 5 M solution is required for an experiment. Doubling the volume of the 9 M sample with water will produce the 5 M solution.   a. True   b. False   ANSWER:   True

 

12. The following equation can be used when C represents either a M or % (w/v) concentration.   a. True   b. False   ANSWER:   True

 

13. When you have your blood drawn, the most common method of expressing the plasma level of sodium and potassium is as mEq/L.   a. True   b. False   ANSWER:   True

 

14. In cases of cerebral endema, a hypertonic solution is administered. The goal of giving the patient the hypertonic solution would be to pull fluid from the cells through the process of osmosis.   a. True   b. False   ANSWER:   True

 

15. If you have 9 g of NaCl in 1 L of water, this solution is 0.9% NaCl and is called normal saline or NS.   a. True   b. False   ANSWER:   True

 

16. Consider the following graph. The solute is probably a gas.   a. True   b. False   ANSWER:   True

 

17. Solution concentration is an intensive property.   a. True   b. False   ANSWER:   True