CHM 2041 Spring 2020 Final Exam reviewDisclaimer

This is my own personal review; this should not be the only resource used to study. You should also study using notes, PowerPoint, homework, etc. I have not seen the exam, so I cannot say for certain what is going to be on the exam. In addition, answers to the review WILL NOT be posted on the WordPress site. Answers to the review will be given during SI sessions and Study Union.

Chapter 7

Important Equations/ relationships

1. the deBroglie wavelengths of a moving electron are given. Which wavelength would correspond to the greatest speed of the moving electron?

a. 8.25 X 10 9 mb. 1.35 X 10 -13 mc. 8.25 X 1012 m d. 1.21 X 10 -6 me. 1.21 X 10 -10 m

2. choose the electron that is on average the farthest from the nucleus a. an electron in a 2p orbitalb. an electron in a 4p orbitalc. an electron in a 5f orbitald. an electron in a 2d orbitale. an electron in a 1s orbital

3. which of the following resembles most closely the uncertainty principle a. matter and energy are really the same thingb. it is impossible to know anything about the energy of a particle c. there can only be one uncertain digit in a reported number d. it is impossible to know the exact position and momentum of an electron e. it is impossible to know how many electrons there are in an atom

4. what lists the correct order of wavelengths with increasing frequency?a. Gamma, X-rays, Infrared, Ultraviolet, Visible, Micro, Radiob. Gamma, X-rays, Ultraviolet, Infrared, Visible, Micro, Radioc. Radio, Micro, Ultraviolet, Visible, Infrared, X-ray, Gammad. Radio, Micro, Infrared, Visible, Ultraviolet, X-rays, Gamma

5. Calculate the wavelength of light emitted when an electron in the hydrogen atom makes a transition from an orbital with n=5 to an orbital with n=3

a. 1.28 X 10-6 mb. 2.28 X 10-6 mc. 6.04 X 10-7 md. 1.55 X 10-19 me. 2.28 X 10-5 m

6. the lowest energy state of an atom is the most stable one, and is called the a. excited levelb. ground statec. Bohr orbitd. Ionization energye. Absorption spectrum

7. What is the photoelectric effect a. The total reflection of light by metals giving them their typical lusterb. The ejection of electrons by a metal when struck with light of sufficient energy c. The production of current by silicon solar cells when exposed to sunlight d. The darkening of photographic film when exposed to an electric field e. The emission of light by the hydrogen atom

8. Of the following transitions in the Bohr hydrogen atom, which is responsible for the emission of highest amount of energy

a. N=1 n=6b. N=5 n=2 c. N=6 n=1d. N=3 n=6e. N=1 n=4

9. Which set of three quantum numbers cannot occur together to specify an orbital a. N=2 l=1 ml=-1b. N=3 l=2 ml=0c. N=4 l=3 ml=0d. N=3 l=3 ml=-2e. N=5 l=3 ml=+3

10. Which of the following orbitals represents possible combinations of the quantum numbers n and l

a. 2db. 3fc. 1dd. 1pe. 5p

11. what are all the possible values of ml if l has a value of 2a. -2,0,+2b. -3,-2,-1,0c. 0,+1,+2d. -1,0,+1e. -2,-1,0,+1,+2

12. which orbital is represented by n=4 , l=1 , ml=+1a. 2sb. 4pc. 3dd. 1se. 3f

13. determine the energy of 1 mol of photons of light which has a wavelength of 500 nm a. 434 Jb. 3.98 X 10 -19 kJc. 2.72 X 10 -16 kJd. 239 kJe. 187 kJ

Ch 8

Important Equations/relationships

14. if the ground state electron configuration of an element is [Ar]3d104s24p3, what is the typical charge on the monatomic ion of the element

a. +2b. +1c. -1d. -2e. -3

15. which group in the periodic table contains elements with the valence electron configuration of ns2np1

a. 1Ab. 2Ac. 3A (group 13)d. 4A (group 14)e. 8A (group 18)

16. which of the following correctly represents the second ionization of calcium a. Ca (g) Ca+ (g) + eb. Ca+ (g) Ca2+ (g) + ec. Ca- (g) + e Ca2- (g)d. Ca+ (g) + e Ca2+ (g) e. Ca+ (g) + e Ca (g)

17. What is the ground state electron configuration of gallium, Gaa. 1s22s23s23p64s23d104p1

b. 1s22s22p63s23p64s24d104p1

c. 1s22s22p63s23p64s23d104p1

d. 1s22s22p63s23p64s23d104d1

e. [Ar]4s23d11

18. in which pair is the first member larger than the second a. Li+ and Lib. Li+ and Na+c. Be and Mgd. Li+ and Be2+e. Cl and Cl-

19. Which electron configuration belongs to the atom with the highest (or most negative) electron affinity EA

a. 1s22s22p63s1

b. 1s22s22p63s2

c. 1s22s22p63s23p1

d. 1s22s22p63s23p4

e. 1s22s22p63s23p5

20. name an element in the fourth row of the periodic table with four 4p electrons a. Crb. Sic. Krd. See. Zn

21. Complete the following: screening of the nuclear charge by core electrons in atom is a. Less efficient than that by valence electrons b. More efficient than that by valence electrons c. Essentially identical to that by valence electrons d. Responsible for a general decreases in atomic radius going down a group e. Both essentially identical to that by valence electrons and responsible for a general

decrease in atomic radius going down a group

22. Which of the following correctly represents the electron affinity of elemental phosphorus a. P (g) P+ (g) + eb. P (g) + e P- (g) c. P4 (g) + e P(g)d. P4 (g) + 4e 4P- (g) e. P+ (g) + e P (g)

23. Consider the following successive ionization energes in kJ/mol for element Xi. IE1 = 590

ii. IE2 = 1120iii. IE3 = 4911

What is the most likely formula for a stable ion of X

a. X2+ b. X3+

c. X+

d. X-

e. X2-

24. arrange the following atoms according to decreasing effective nuclear charge experienced by their valence electrons S, Al, Si, Mg

a. S > Al > Si > Mg b. Mg > Al > Si > Sc. Al > S > Si> Mg d. S > Si > Al > Mge. Si > Al > Mg > S

25. How many unpaired electrons are in a ground state germanium atom Gea. 0 b. 1c. 2d. 3e. 4

26. which of the following illustrates the correct order for atomic radius for these elements in the third row of the periodic table

a. Mg > Na > P > Si > Arb. Ar > Si> P > Na > Mg c. Si > P > Ar > Na > Mg d. Na > Mg > Si > P > Ar e. Ar > P > Si > Mg > Na

27. Which of the following ions have the same electron configuration : Sn4+ , Pb4+ , Sr2+ , Br-

a. Sn and Pb b. Pb and Src. Sr and Brd. Pb and Br e. Sn , Sr, and Br

28. Which of the following statements are true?a. The number of valence electrons in a transition metal can be more than 8.b. Due to the Aufbau principle electrons will fill each orbital before pairing upc. When a cation forms it is typically larger than the original elementd. Transition metals loose their ns electrons before the (n-1)d electrons e. As the atomic mass of an element increases across a row so does its radius

Ch 9

Important Equations/relationships

29. in which compound below is it inappropriate to use a line or dash to represent a shared electron pair in a bond

a. KCl b. HClc. Br2

d. BrFe. I2

30. Which compound is likely to have an incomplete octeta. NH3 b. SO3

c. N2Od. BH3

e. None of the above

31. Which of the following molecules or ions are likely to be free radicalsa. N2O and OCl-

b. N2O and NOc. NO and OCl-

d. NO and ClO2

e. OCl- and ClO2

32. Which of the following is false regarding electronegativitya. A non-polar bond is formed between an electronegativity difference of 0.4b. An ionic bond forms when the electronegativity difference is 2.1c. F is the most electronegative elementd. A polar molecule can have nonpolar bonds.e. Electronegativity is the tendency of an atom to attract electrons to itself when bonded

to another atom

33. Which of the following is false regarding formal charge?a. The best lewis structure has a formal charge of zero on all atomsb. A negative FC will go on the least electronegative atomc. FC = valence electrons- lone pair electrons- # of bondsd. The best lewis structure has the lowest formal charge on each atome. The overall formal charge is represented by the charge of the molecule

34. Given the electronegativities below, which single bond has the lowest degree of polarity i. Element: H C N O

ii. Electronegativity 2.1 2.5 3.0 3.5 a. C-Hb. N-Hc. O-Hd. O-Ce. O-N

35. predict the formula for magnesium phosphide? What is the total number of electrons transferred

a. Mg2P3 ; 3 electrons are transferred from Mg to Pb. Mg3P2 ; 6 electrons are transferred from Mg to P c. Mn3P ; 3 electrons are transferred from P to Mn d. MgP3 ; 6 electrons are transferred from Mg to P e. MgP2 ; 4 electrons are transferred from P to Mg

36. Which of the following is the best Lewis structure for the compound which has the molecular formula

a. 1 and 2 b. 2c. 3d. 2 and 3e. 1,2 and 3

37. which of the following species will have a Lewis structure most like that of the hydronium ion , H3O+

a. NO3-

b. NH3

c. SO3

d. CO32-

e. H2CO

38. Consider the reaction : CH4 + Cl2 CH3Cl + HClCalculate the overall enthalpy change for the reaction (Hrxn) using the bond energy data given

C-H 414 kJ O=O 498 kJ H-Cl 431 kJ C-O 360 kJC-Cl 339 kJ C=O 799 kJCl-Cl 243 kJ H-O 464 kJ

a. -92 kJb. + 92 kJc. -113 kJ d. 273 kJ e. 301 kJ

39. the type of compound that is most likely to contain a covalent bond is which of the following a. one that is composed of a metal from the far left of the periodic table and a nonmetal

from the far right of the periodic table b. a solid metalc. a substance held together by the electrostatic forces between oppositely charged ions d. one that is composed of two nonmetals e. there is no general rule to predict covalency in bonds

40. Select the compound with the shortest and strongest carbon-carbon bond respectively a. H2C=CH2

b. C2H6

c. H-C≅C-CH3

d. H2C=C=CH2

e. H3C-CH2-CH3

41. What is the formal charge on the nitrogen in the nitrate ion NO3-

a. -1b. 0c. +1d. +2

42. which of the following compounds is expected to have the strongest ionic bond a. MgOb. KBrc. NaId. SrOe. CaS

43. The diagram below is the Born-Haber cycle for the formation of crystalline potassium fluoride KF

Which energy change (by number) corresponds to the lattice energy of KF

a. 5b. 2c. 4d. 1e. 6

44. which of the following best represents the Lewis structure for ozone O3

a. 1b. 2c. 5d. 4e. 3

45. which molecule below has the largest dipole moment a. HBrb. HIc. HFd. HCle. H2

CH 10

Important equations/relationships

46. What is the value of the smallest bond angle in XeBr4

a. 109.5b. 120c. 90d. 180e. 45

47. determine the expected molecular geometry of CBr4

a. linearb. trigonal planerc. tetrahedrald. trigonal pyramidale. see saw

48. what is the expected molecular geometry of IBr4+

a. see sawb. trigonal planarc. octahedrald. tetrahedrale. trigonal bipyramidal

49. what is the expected electronic geometry of H2Sa. linearb. trigonal planerc. tetrahedrald. v-shaped or bente. t-shaped

50. of the following which molecule has the largest bond anglea. SO3

b. SF2

c. HCNd. H2Se. PF3

51. Select the molecule which has one lone pair on the central atoma. NH2

-

b. H2Oc. CH4

d. H3O+

e. BeCl2

52. Which molecule below is nonpolar a. SF4

b. OF2

c. PH3

d. CBrCl3

e. XeCl4

53. What is the hybridization of the oxygen atom labeled x in the structure below

a. Spb. Sp2c. Sp3d. Sp3de. Sp3d2

54. Which molecule below is polara. SF4

b. GaH3

c. SiH4

d. CBr4

e. XeF4

55. If PBr3Cl2 is a nonpolar molecule, determine the Cl-P-Br bond anglea. 120b. 180c. 90d. 109e. 55

56. what type of hybridization is exhibited by the central atom in CH2Oa. sp2b. spc. sp3d. sp3de. sp3d2

57. in general what bond types make up a triple bond a. three sigma bonds b. two sigma bonds and a pi bondc. a sigma bond and two pi bonds d. two sigma bonds and two overlapping sp hybrid orbitals e. three pi bonds

58. which of the following shows these molecules in order from most polar to least polar a. CH4 > CF2Cl2 > CCl4 CCl2H2

b. CH4 > CF2H2 > CF2Cl2 > CCl4 > CCl2H2

c. CF2Cl2 > CF2H2 > CCl2H2 > CH4 = CCl4

d. CF2H2 > CCl2H2 >CF2Cl2 > CH4 = CCl4

e. CF2Cl2 > CF2H2 > CCl4 > CCl2H2 > CH4

59. consider the following Lewis structure select which statement is false

a. there are 10 sigma and 2 pi bonds b. the C-2 atom is sp2 hybridized with bond angles of about 120 c. the oxygen atom is sp3 hybridized d. this molecule contains 28 valence electrons e. there are some H-C-H bond angles of about 109 in the molecule

Ch 5

Important equations/relationships

60. which of the following statements is falsea. gases are highly compressibleb. distances between molecules of gases are very large compared to bond distances within

molecules c. non-reacting gas mixtures are homogeneous d. gases expand spontaneously to fill the container they are placed ine. gases have densities higher than solids

61. If the pressure exerted by ozone, O3 in the stratosphere is 3.0 X 103- atm and the temperature is 255 K, how many ozone molecules are in one liter

a. 6.0 X 10 18

b. 6.1 X 1022

c. 8.6 X 1019

d. 1.4 X 1018

e. 2.7 X 10 20

62. Aluminum reacts with Chlorine gas to form aluminum chloride. What minimum volume of chlorine gas (at 298 K and 255 mm Hg) is required to completely react with 7.85 g of aluminum.

2 Al (s) + 3 Cl2 (g) -> 2 AlCl3

a. 31.37 Lb. 24.0 Lc. 0.0474 Ld. 16.0 L

63. iron reacts with HCl to produce iron(II)chloride and hydrogen gas. The hydrogen gas from the reaction of 4.4 g of iron with excess acid is collected in a 1.0 L flask at 25°C. What is the H2 pressure in atm

i. Fe (s) + 2HCl (aq) FeCl2 (aq) + H2 (g)a. 1.9b. 8.2c. 0.95d. 0.33e. 5.6

64. At STP what volume of N2 will react completely with 22.2L H2 to produce NH3

i. N2(g) + 3H2 (g) 2NH3 (g)a. 7.4 Lb. 14.8 Lc. 22.2 Ld. 44.4 Le. 66.6 L

65. which of the following are postulates of the kinetic molecular theory of gasesi. the distance between gas molecules is large in comparison to their size

ii. gas molecules are in constant random motioniii. the kinetic energy of gas particles is proportional to the kelvin temperature

a. 1b. 2c. 1,2,3d. 3e. 1,2

66. place the following gases in order of increasing average velocity at 400K : Ne, Ar, SO2, N2

a. Ar <Ne<N2<SO2

b. Ne<Ar<N2<SO2

c. N2< SO2 < Ne< Ard. Ne< Ar = SO2 < N2

e. SO2 < Ar< N2 < Ne

67. What is the molar volume of a gas at STP in liters a. 1.00b. 14.7c. 22.4d. 0.08206e. 62.36

68. which gas sample has the greatest volume at STPa. 5 g Arb. 5g Rnc. 5g Ned. 5g Kre. 5g Xe

69. for a fixed amount of gas, what happens to its pressure, if the temperature is doubled and the volume is doubled

a. the pressure will be halvedb. the pressure will decrease to one-quarter of its initial value c. the pressure will be increased by a factor of 4d. the pressure will be doublede. there will be no change in the pressure

70. rank the following in order of decreasing rate of effusion i. F2 SF6 CO Kr

a. Kr> CO> SF6 > F2

b. F2 > Kr > CO > SF6

c. CO > F2 > Kr > SF6

d. CO > F2 > SF6 > Kre. SF6 > Kr > F2 > CO

71. a cylinder with a moveable piston contains 0.87 mol of a gas and a volume of 334 ml. what is the volume after 0.22 mol of the same gas is added to the cylinder

a. 420 mlb. 310 mlc. 22.0 Ld. 850 mLe. 640 mL

72. a gaseous mixture of O2 and N2 contains 39.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 505 mmHg

a. 171 mmHgb. 60 mHgc. 870 mmHgd. 304 mmHge. 700 mmHg

73. of the following gases which one has the greatest density at 1.0 atm and 23°Ca. CH4

b. Nec. COd. N2

e. NO

74. an ideal gas differs from a real gas in that the particles of an ideal gasa. have very large molecular volume b. do not exert molecular forces c. have a molecular weight of zerod. generally have no kinetic energy e. do not exert any pressure

75. Which gas sample has the greatest volume at STP?a. 10.0 g Arb. 10.0 g Krc. 10.0 g Xe

d. None of the above (they all have the same volume)