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CHM 101- Exam 3 Practice Questions

by: SunDevil_21

CHM 101- Exam 3 Practice Questions CHM 101

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Practice questions for Exam 3 for CHM 101 with Richard Bauer at Arizona State University
CHM 101
Richard Bauer
Study Guide
Science, Chemistry
50 ?




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This 7 page Study Guide was uploaded by SunDevil_21 on Tuesday May 10, 2016. The Study Guide belongs to CHM 101 at Arizona State University taught by Richard Bauer in Fall 2014. Since its upload, it has received 26 views. For similar materials see CHM 101 in Chemistry at Arizona State University.

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Date Created: 05/10/16
Chapter 6 44. When 75.0 g of hot water was added to 150.0 g of water at 22.0 ºC, the final temperature was 35.0ºC.  How much  heat was gained by the cold water?  (The specific heat of water is 4.184 J/g∙ºC.)   A. 54.4 J D. 8160 J B. 4080 J E. 94,140 J C. 6900 J  45. Suppose 6.0 mol of hydrogen is placed in a vessel containing 4.0 mol of nitrogen and allowed to react according to  the equation: 3H 2g)  +  N2(g)    2NH (3) What will be present in the vessel after the reaction is complete? A.  4.0 mol NH  o3ly B.  4.0 mol NH  a3d unreacted nitrogen C.  6.0 mol NH  a3d unreacted hydrogen D.  8.0 mol NH  a3d unreacted hydrogen E.  8.0 mol NH  a3d unreacted nitrogen 46.Hydrogen gas reacts with oxygen gas to produce water.  The image below shows a mixture of molecules  before the reaction occurs.  What is present when the reaction is complete?  (The larger molecules represent  oxygen.)   A. three water molecules and one hydrogen molecule B. three water molecules and seven hydrogen molecules C. six water molecules and one hydrogen molecule D. six water molecules and one oxygen molecule E. seven water molecules and one oxygen molecule 47. Magnesium metal reacts with oxygen gas to form magnesium oxide.  How many moles of magnesium oxide are  expected from the complete reaction of 0.0376 mol of O ?  (2int: Write a balanced equation for the reaction.) A. 0.0376 mol MgO D. 1.20 mol MgO B. 0.0188 mol MgO E. 1.52 mol MgO C. 0.0752 mol MgO 48. Sodium metal reacts with liquid bromine to form sodium bromide.  How many grams of bromine are required to react with 75.0 g of sodium?  2Na(s)  +  Br (l2    2NaBr(s) A. 3.26 g Br 2 D. 521 g Br 2 B. 150 g Br 2 E. 1040 g Br 2 C. 261 g Br 2 ­1­ Copyright 2013 by Richard C. Bauer 49. When 20.0 g of sodium is placed in 100.0 g of bromine a reaction occurs that is described in the previous question.   How many moles of sodium react? A. 0.313 mol Na D. 1.25 mol Na  B. 0.626 mol Na E. 1.73 mol Na  C. 0.870 mol Na  50. Sodium metal reacts with liquid bromine to form sodium bromide.  How many grams of bromine are required to react with 75.0 g of sodium?  2Na(s)  +  Br2(l)    2NaBr(s) A. 3.26 g Br 2 D. 521 g Br 2 B. 150 g Br 2 E. 1040 g Br 2 C. 261 g Br 2 51. How many joules of heat energy are required to heat 375 g of iron from 25.0ºC to 200.0ºC?  (The specific heat of iron is 0.449 J/g∙ºC) A. 4.77 J D. 29,500 J B. 4150 J E. 33,700 J  C. 4210 J  Chapter 7 52. Which of the following types of electromagnetic radiation has the lowest frequency? A. Red light D. violet light  B. green light E. ultraviolet radiation C. blue light  53. Upon electrification, hydrogen produces the following line spectrum in the visible region of the electromagnetic  spectrum.  The light emitted for each line corresponds to transitions from the third (n=3), fourth (n=4), fifth (n=5), or  sixth (n=6) energy level down to the second (n=2).  Which color of light corresponds to the transition of an electron  from the n=6 to the n=2 energy level? Color Wavelength (λ), nm Indigo 410.1 Blue 434 Blue­green 486 Red 656.3 A. indigo B. blue C. blue­green D. red E. all these colors are observed 54. Light with a wavelength of 650.0 nm appears as red light to the human eye?  What is the energy of this light in  joules?  A. –13 –31 1.291 × 10 D. 4.307 × 10 B. 3.056 × 10 –19 E. 4.612 × 10 14 C. –28 3.056 × 10 55. How many valence electrons does an atom of phosphorus have? A. 0 D. 8 B. 3 E. 15 C. 5 56. Which of the following elements requires the most energy to remove an electron from a neutral atom? A. Li B. Na C. K D. Rb  E. Cs 57. Which of the following represents the electron configuration of cobalt? A.  [Ar]3s 3p 9 D. [Ar]4s 3d   7 B.  2 9 2 9 [Ar]3s 3d E. [Ar]4s 4p C.  [Ar]3d 7 58. How many orbitals are in a d subshell? A. 1 B. 3 C. 5 D. 6  E. 10 59. Which of the following orbital diagrams represents the correct ground state electron configuration for the oxide ion? A.              1s        2s                      2p B.              1s        2s                      2p C.   1s        2s                      2p D.   1s        2s                      2p E.   1s        2s                      2p 60. An element was found to have two electrons in its valence s subshell and five electrons in its valence p subshell.  To  which group on the periodic table does this element belong? A. IIA (2) D. VA (15) B. IIIB (3) E. VIIA (17) C. VIIB (7) 61. Which of the following species has the electron configuration 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p ? A. Se D. Xe B. Mo E. Po C. Te 62. Which of the following best represents a p orbital?  D A B C D 63. Which of the following species has the most electrons? 3– + 2+ A. P B. Ar C. K D. Ca   E. All have the same number of electrons 64. Which species has its valence electrons closest to the nucleus? A. N B. P C. As D. Sb  E. All have the same distance to the valence electrons Chapter 8 65. Which of the following compounds is expected to have the lowest boiling point? A. KNO 3 D. Mg(NO ) 3 2 B. CsF  E. H 2 C. NaCl ­has covalent bonds (nm+nm) 66. Which of the following statements best describes a covalent bond in a compound? A. It is composed of only nonmetals. B. It is composed of a solid elemental metal. C. The compound is composed a metal and a nonmetal. D. It is held together by oppositely charged ions. E. There is no general rule to predict covalent bonds. 67. Which of the following species requires more than one electron dot symbol to describe the distribution of electrons?  A. H 2 D. CH 4 B. CO 2– E. Br 3 2 C. H 2 68. When the electron dot symbol is complete for formaldehyde, CH2O, how many bonding electrons are present?  (The  connectivity of the atoms is shown below.)  O C H       H A. 2 D. 6 B. 3 E. 8 C. 4 ­count valence electrons for each 69. What is the electron pair geometry and the molecular shape, respectively, for 3H ? A. tetrahedral, trigonal planar  B. tetrahedral, trigonal pyramidal  C. tetrahedral, bent D. trigonal planar, trigonal planar E. trigonal pyramidal, trigonal pyramidal 70. Which of the following compounds is not an exception to the octet rule?  (In each case the first element in the  formula is central to all the other atoms.) A. PCl 5 D. SF 6 B. NO  2 E. NO C. CF 4 71. Which of the following elements is least electronegative?  A. fluorine D. cesium  B. carbon E. lithium C. boron 72. In which of the following compounds is the bonding polar covalent? A. CsF B. CO C. F D. NaCl  E. O 2 2 2 73. Which of the following molecules is composed of polar bonds but has a zero dipole moment (i.e. is nonpolar)?  A. Cl 2 B. SO 2 C. CO   2 D. NF 3 E. PCl 3 74. In the complete electron dot structure for 3F , which statement is not true?  A. The F—N—F angle is about 109.5º. B. Nitrogen has six bonding and zero non­bonding electrons. C. There are 26 valence electrons. D. All atoms have satisfied valence shells. E. The molecule has tetrahedral electron pair geometry and trigonal pyramidal molecular shape. 75. In which of the following are partial negative and positive charges correctly placed? δ– δ+ δ– δ+ A. F—F D. N—O B. δ+F—F δ– E. δ+N—O δ– δ– δ+ C. S—F 76. The electron pair geometry and molecular shape in SO 2 respectively, are  A. tetrahedral, bent B. tetrahedral, trigonal planar C. tetrahedral, tetrahedral D. trigonal planar, trigonal planar E. trigonal planar, bent ­draw lewis structure Sample Exam Answers Question Answer 33 C 67 B 34 B 68 E 1 C 35 E 69 B 2 B 36 C 70 C 3 B 37 C 71 D 4 E 38 A 72 B 5 A 39 C 73 C 6 E 40 A 74 B 7 E 41 E 75 E 8 C 42 A 76 E 9 B 43 D 77 C 10 D 44 D 78 D 11 A 45 B 79 B 12 E 46 C 80 E 13 A 47 C 81 C 14 B 48 C 82 D 15 A 49 C 83 C 16 B 50 C 84 A 17 E 51 D 85 A 18 C 52 A 86 A 19 D 53 A 87 C 20 D 54 B 88 C 21 C 55 C 89 D 22 D 56 A 90 B 23 A 57 D 91 B 24 B 58 C 92 D 25 D 59 E 93 D 26 B 60 E 94 D 27 E 61 D 95 A 28 E 62 D 96 E 29 B 63 E 97 A 30 E 64 A 98 B 31 B 65 E 99 C 32 A 66 A 100 C ­7­ Copyright 2013 by Richard C. Bauer


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