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Midterm 1 Essay

Chemistry 110 Midterm 1 October 11, 2005 1. What are the possible values for the orbital angular momentum quantum number l given the following values for the other three quantum numbers: n = 4, l = ? , ml = 0, ms = +1/2 A. B. C. D. E. 0 1, 2, 3, or 4 3 0, 1, 2, or 3 none of these answers 2. If the wavelength of an electron is equal to the radius of the n=2 orbit in He+, what must the velocity of the electron be? A. B. C. D. E. 6. 88 x 106 m/s 1. 38 x 107 m/s 3. 44 x 106 m/s 5. 47 x 105 m/s The velocity cannot have an exact value 3. The element seaborgium (Sg) has Z=106. What would you predict the electron configuration to of Sg2+ to be?

A. B. C. D. E. The same configuration as rutherfordium (Rh) Z=104 [Rn] 6d4 [Rn] 5f14 6d4 [Rn] 5f14 6d2 7s2 [Rn] 5f12 6d4 7s2 4. Praseodymium (Pr Z=59) is one of the lanthanide (rare earth) elements. Which of the following statements is a TRUE statement about the orbital into which the last electron was filled for the element Pr? A. B. C. D. E. The number of radial nodes is greater than the number of angular nodes The orbital is a 5f orbital The orbital contains valence electrons The orbital is one member of a set of seven degenerate orbitals none of the other four statements is true 5.

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Davisson and Germer (as well as G. P. Thompson) conducted a famous and important experiment. Which of the following statements is TRUE concerning their experiment? A. B. C. D. E. They observed diffraction patterns from photons confirming that light had wave properties They observed diffraction patterns of electrons confirming that matter had wave properties Their experiment contradicted DeBroglie’s equation They observed standing wave patterns from electrons confirming the existence of orbitals None of the other four statements is true Page 1, v1 Chemistry 110 Midterm 1 October 11, 2005 6.

A two-photon absorption transition is observed using a laser that emits light having a wavelength of 500 nm? Which of the following statements is/are TRUE about this electronic transition? A. B. C. D. E. The single photon transition would be caused by UV light with a wavelength of 1000 nm The single photon transition would be caused by IR light with a wavelength of 1000 nm The single photon transition would be caused by UV light with a wavelength of 250 nm The single photon transition would be caused by IR light with a wavelength of 250 nm None of the other four statements is true . Which of the following statements is/are TRUE ? A. The wavefunction, ? , is a solution to the Schrodinger equation B. The square of the wavefunction, ? 2, is the total probability of finding the electron in a spherical shell at distance r from the nucleus C. Orbitals with the same n cannot overlap in space D. For the same orbital type (i. e. same l quantum number), orbitals with the higher n value will have a more negative energy E. two of the other four statements are true 8. Which is not a valid set of quantum numbers for an electron?

A. B. C. D. E. n = 6, l = 2, ml = 0, ms = 1/2 n = 3, l = 2, ml = -2, ms = 1/2 n = 7, l = 0, ml = 0, ms = 1/2 n = 17, l = 16, ml = 16, ms = -1/2 n = 4, l = -2, ml = 2, ms = -1/2 9. Which statement(s) is (are) FALSE in comparing the electronic transition from ni = 5 to nf =2 in H with that of electronic transition from ni = 2 to nf =5 in Be3+ A. The photon involved in the H transition lies in the visible spectrum while that involved in the Be3+ transition lies in the UV region of the spectrum. B.

A photon of the same frequency is involved in both transitions, but is emitted the H electronic transition and absorbed in the Be3+ electronic transition. C. The wavelength of the photon emitted by H is 16 times the wavelength of the photon absorbed by Be3+ D. The transition in H is a Balmer emission series line E. two of the other four statements are FALSE Page 2, v1 Chemistry 110 Midterm 1 October 11, 2005 10. Assume that we conduct a Stern Gerlach type experiment by passing a beam of cobalt (Co) atoms and zinc (Zn) atoms simultaneously through an external magnetic field.

What would be the expected pattern on the detector? A. B. C. D. E. Two spots: one deflected up, one deflected down Two spots: one undeflected, one deflected up Four spots: two deflected up, two deflected down Three spots: one undeflected, one deflected up, one deflected down Three spots: two deflected up, one deflected down 11. The workfunction for Na is 2. 70 eV, for Mg is 3. 66 eV, and for Cs is 2. 14 eV. Assume we shine light with a wavelength of 400 nm on the surface of each of these metals. Which of the following statements is/are TRUE about the observed results? (Note 1 eV = 1. 609 x 10-19 J) A.

B. C. D. E. Electrons are not ejected from Mg, but would be if the intensity of the light were increased Electrons are ejected from both Cs and Na and they would have a greater velocity from Cs No electrons are ejected from Na, Mg, or Cs but would be if the light frequency were increased Electrons are ejected from Mg and they have a velocity of 4. 4 x 105 m/s Two of the other four statements are true 12. Assume that the uncertainty in determining the position of an electron is equal to its DeBroglie wavelength. What would be the uncertainty in the momentum for an electron traveling with a velocity of 1. 0 x 107 m/s? A. B. C. D. E. > 9. 109 x 10-24 kg m/s > 7. 27 x 10-11 kg m/s > 1. 38 x 1024 kg m/s > h/(4*pi) > 7. 25 x 10-25 kg m/s 13. Which of these species has the greatest number of unpaired electrons? A. B. C. D. E. Mn (Z=25) P (Z=15) Rb (Z=37) Mo (Z=42) Cu (Z=29) 14. Arrange the following species in order of decreasing radius: Br- , Y3+, Rb+, Se2- , Kr? A. B. C. D. E. Se2- , Br- , Kr, Rb+, Y3+ Y3+, Rb+, Kr, Br- , Se2Kr, Se2- , Br- , Rb+, Y3+ Kr, Y3+, Rb+, Br- , Se2Rb+, Y3+, Kr, Se2- , Br- Page 3, v1 Chemistry 110 Midterm 1 October 11, 2005 15.

Arrange the following species in order of increasing radius Se, Pb, Sn, Ge, As? A. B. C. D. E. As, Ge, Sn, Pb, Se Se, Pb, As, Sn, Ge As, Se, Ge, Sn, Pb Se, As, Ge, Sn, Pb Pb, Sn, Ge, As, Se 16. What would be a valid set of quantum numbers for the last electron filled in the electronic configuration for osmium (Os Z=76)? A. B. C. D. E. n = 6, l = 0, ml = 0, ms = 1/2 n = 5, l = 3, ml = -3, ms = 1/2 n = 6, l = 1, ml = 0, ms = 1/2 n = 6, l = 2, ml = 0, ms = 1/2 n = 5, l= 2, ml = -2, ms = 1/2 17. Which of the following species is the most paramagnetic? A. B. C. D. E.

Fe3+ Ga+ Os N Cr 18. Assume that at an elevated temperature, the ground state for Be3+ is n=5. What would be the ionization energy for this species in this case? (1eV = 1. 609 x 10-19 J) A. B. C. D. E. 8. 667 eV 216. 7 eV 138. 7 eV 2. 167 eV None of the other four answers 19. What would be the velocity of an electron ejected from sodium if light of 350 nm is directed at a surface of the metal (the workfunction for sodium is 2. 70 eV and 1eV = 1. 609 x 10-19 J) A. B. C. D. E. 382 km/s 5. 41 x 105 km/s 17,010 km/s 541 km/s None of the other four answers Page 4, v1

Chemistry 110 Midterm 1 October 11, 2005 20. What would be the ground state electron configuration for Ge3+? A. B. C. D. E. [Ar] 3d10 4s2 4p2 [Ar] 3d9 4s2 [Ar] 3d10 4s1 [Ar] 3d7 4s2 4p2 [Ar] 3d10 4p1 21. If an electron was in an orbital with 1 radial node and 3 angular nodes, what type of orbital is the electron occupying? A. B. C. D. E. 4d 5p 5f 4f None of the other four answers 22. One of the Lyman series emission lines for hydrogen (H) is observed at 102. 5 nm. This transition involves an electron dropping down to the ground state level from a higher energy level.

What is the ninitial value for the higher energy orbit (i. e. what is ni)? A. B. C. D. E. 1 2 3 4 None of the other four answers 23. Arrange the following species in order of increasing ionization energy: Al, In, Ga, Si, S? A. B. C. D. E. In, Ga Si, S, Al Si, S, Al, Ga, In In, Al, Ga, Si, S In, Ga, Al, Si, S S, Si, Al, Ga, In 24. Which of the following represents the orbit with the largest radius? A. B. C. D. E. n=2 orbit for Be3+ n=1 orbit for H n=3 orbit for Li2+ n=4 orbit for He+ n=3 orbit for H Page 5, v1 Chemistry 110 Midterm 1 October 11, 2005 25.

The term “ultraviolet catastrophe” referred to what aspect in the scientific developments that led to the new quantum theory? A. B. C. D. E. The energy density went to infinity at short wavelengths in the classical theory for blackbody radiation That the intensity of ultraviolet light had no effect in producing photoelectric emission That the Balmer series emission lines for H were only observed in the visible region That the light exhibited wave particle duality None of these other four answers 26. What is the energy of light that has a wavelength of 1 micrometer (1µm)? A. B. C. D. E. 1. 986×104 kJ/mol 1. 96 x 105 kJ/mol 1. 986 x 10-19 kJ/mol 119. 6 kJ/mol None of these other four answers 27. [Xe]f145d10 6s1 is the ground state electronic configuration of which species? A. B. C. D. E. Hg Pb2+ Au Pt Tl+ 28. How many valence electrons are found in tellurium (Te Z=52)? A. B. C. D. E. 1 2 4 6 16 29. What would be a permitted value for the principle quantum number if we knew that the magnetic quantum number (ml) was 7? A. B. C. D. E. 5 6 7 15 none of these other four answers Page 6, v1 Chemistry 110 Midterm 1 October 11, 2005 30. Which of the following statements is/are TRUE about the species Sn2+? A. B. C. D. E.

It is a paramagnetic species It has a completely filled f orbital set It would be expected to have a larger radius than Sn It has 48 protons in the nucleus none of these other four answers is true Page 7, v1 Answer Key for Test “Chem110MT1F05. tst”, 10/12/2005 No. in No. on Q-Bank Test 7 120 1 7 121 2 7 122 3 7 123 4 7 124 5 7 125 6 7 126 7 7 127 8 7 128 9 7 129 10 7 130 11 7 131 12 7 132 13 7 133 14 7 134 15 7 135 16 7 136 17 7 137 18 7 138 19 7 139 20 7 140 21 7 141 22 7 142 23 7 143 24 7 144 25 7 145 26 7 146 27 7 147 28 7 148 29 7 149 30 Correct Answer D A C D B C A E B D B E D A D E E A D C C C D E A D C D D E

Page 1, v1 Chemistry 110 Midterm 1 October 11, 2005 1. [Xe]f145d10 6s1 is the ground state electronic configuration of which species? A. B. C. D. E. Hg Pt Pb2+ Au Tl+ 2. Which of the following species is the most paramagnetic? A. B. C. D. E. Os Fe3+ N Ga+ Cr 3. Arrange the following species in order of increasing radius Se, Pb, Sn, Ge, As? A. B. C. D. E. Se, Pb, As, Sn, Ge As, Ge, Sn, Pb, Se Se, As, Ge, Sn, Pb As, Se, Ge, Sn, Pb Pb, Sn, Ge, As, Se 4. Assume that we conduct a Stern Gerlach type experiment by passing a beam of cobalt (Co) atoms and zinc (Zn) atoms simultaneously through an external magnetic field.

What would be the expected pattern on the detector? A. B. C. D. E. Two spots: one deflected up, one deflected down Four spots: two deflected up, two deflected down Three spots: one undeflected, one deflected up, one deflected down Three spots: two deflected up, one deflected down Two spots: one undeflected, one deflected up 5. What would be the velocity of an electron ejected from sodium if light of 350 nm is directed at a surface of the metal (the workfunction for sodium is 2. 70 eV and 1eV = 1. 609 x 10-19 J) A. B. C. D. E. 17,010 km/s 5. 41 x 105 km/s 541 km/s None of the other four answers 382 km/s Page 1, v2

Chemistry 110 Midterm 1 October 11, 2005 6. The term “ultraviolet catastrophe” referred to what aspect in the scientific developments that led to the new quantum theory? A. B. C. D. E. The energy density went to infinity at short wavelengths in the classical theory for blackbody radiation None of these other four answers That the light exhibited wave particle duality That the Balmer series emission lines for H were only observed in the visible region That the intensity of ultraviolet light had no effect in producing photoelectric emission 7. How many valence electrons are found in tellurium (Te Z=52)? A. B.

C. D. E. 16 6 2 1 4 8. Praseodymium (Pr Z=59) is one of the lanthanide (rare earth) elements. Which of the following statements is a TRUE statement about the orbital into which the last electron was filled for the element Pr? A. B. C. D. E. The orbital is a 5f orbital none of the other four statements is true The number of radial nodes is greater than the number of angular nodes The orbital is one member of a set of seven degenerate orbitals The orbital contains valence electrons 9. If the wavelength of an electron is equal to the radius of the n=2 orbit in He+, what must the velocity of the electron be?

A. B. C. D. E. 5. 47 x 105 m/s 1. 38 x 107 m/s The velocity cannot have an exact value 3. 44 x 106 m/s 6. 88 x 106 m/s 10. What are the possible values for the orbital angular momentum quantum number l given the following values for the other three quantum numbers: n = 4, l = ? , ml = 0, ms = +1/2 A. B. C. D. E. 1, 2, 3, or 4 none of these answers 3 0 0, 1, 2, or 3 Page 2, v2 Chemistry 110 Midterm 1 October 11, 2005 11. The element seaborgium (Sg) has Z=106. What would you predict the electron configuration to of Sg2+ to be? A. B. C. D. E. Rn] 6d4 [Rn] 5f12 6d4 7s2 The same configuration as rutherfordium (Rh) Z=104 [Rn] 5f14 6d4 [Rn] 5f14 6d2 7s2 12. Which of the following statements is/are TRUE about the species Sn2+? A. B. C. D. E. It would be expected to have a larger radius than Sn none of these other four answers is true It is a paramagnetic species It has 48 protons in the nucleus It has a completely filled f orbital set 13. Which statement(s) is (are) FALSE in comparing the electronic transition from ni = 5 to nf =2 in H with that of electronic transition from ni = 2 to nf =5 in Be3+ A.

A photon of the same frequency is involved in both transitions, but is emitted the H electronic transition and absorbed in the Be3+ electronic transition. B. two of the other four statements are FALSE C. The photon involved in the H transition lies in the visible spectrum while that involved in the Be3+ transition lies in the UV region of the spectrum. D. The transition in H is a Balmer emission series line E. The wavelength of the photon emitted by H is 16 times the wavelength of the photon absorbed by Be3+ 14.

Assume that the uncertainty in determining the position of an electron is equal to its DeBroglie wavelength. What would be the uncertainty in the momentum for an electron traveling with a velocity of 1. 00 x 107 m/s? A. B. C. D. E. > 9. 109 x 10-24 kg m/s > h/(4*pi) > 1. 38 x 1024 kg m/s > 7. 25 x 10-25 kg m/s > 7. 27 x 10-11 kg m/s 15. A two-photon absorption transition is observed using a laser that emits light having a wavelength of 500 nm? Which of the following statements is/are TRUE about this electronic transition? A. B. C. D. E. The single hoton transition would be caused by UV light with a wavelength of 250 nm The single photon transition would be caused by UV light with a wavelength of 1000 nm The single photon transition would be caused by IR light with a wavelength of 1000 nm None of the other four statements is true The single photon transition would be caused by IR light with a wavelength of 250 nm Page 3, v2 Chemistry 110 Midterm 1 October 11, 2005 16.

What would be a valid set of quantum numbers for the last electron filled in the electronic configuration for osmium (Os Z=76)? A. B. C. D. E. = 6, l = 2, ml = 0, ms = 1/2 n = 6, l = 0, ml = 0, ms = 1/2 n = 5, l= 2, ml = -2, ms = 1/2 n = 6, l = 1, ml = 0, ms = 1/2 n = 5, l = 3, ml = -3, ms = 1/2 17. One of the Lyman series emission lines for hydrogen (H) is observed at 102. 5 nm. This transition involves an electron dropping down to the ground state level from a higher energy level. What is the ninitial value for the higher energy orbit (i. e. what is ni)? A. B. C. D. E. None of the other four answers 4 3 1 2 18. What is the energy of light that has a wavelength of 1 micrometer (1µm)? A. B. C. D. E. 1. 196 x 105 kJ/mol None of these other four answers 1. 86 x 10-19 kJ/mol 119. 6 kJ/mol 1. 986×104 kJ/mol 19. Which is not a valid set of quantum numbers for an electron? A. B. C. D. E. n = 3, l = 2, ml = -2, ms = 1/2 n = 7, l = 0, ml = 0, ms = 1/2 n = 17, l = 16, ml = 16, ms = -1/2 n = 6, l = 2, ml = 0, ms = 1/2 n = 4, l = -2, ml = 2, ms = -1/2 20. What would be a permitted value for the principle quantum number if we knew that the magnetic quantum number (ml) was 7? A. B. C. D. E. 6 7 5 none of these other four answers 15 Page 4, v2 Chemistry 110 Midterm 1 October 11, 2005 21. Arrange the following species in order of decreasing radius: Br- , Y3+, Rb+, Se2- , Kr?

A. B. C. D. E. Se2- , Br- , Kr, Rb+, Y3+ Rb+, Y3+, Kr, Se2- , BrY3+, Rb+, Kr, Br- , Se2Kr, Y3+, Rb+, Br- , Se2Kr, Se2- , Br- , Rb+, Y3+ 22. Assume that at an elevated temperature, the ground state for Be3+ is n=5. What would be the ionization energy for this species in this case? (1eV = 1. 609 x 10-19 J) A. B. C. D. E. 8. 667 eV None of the other four answers 138. 7 eV 2. 167 eV 216. 7 eV 23. If an electron was in an orbital with 1 radial node and 3 angular nodes, what type of orbital is the electron occupying? A. B. C. D. E. 5f None of the other four answers 5p 4d 4f 24. Davisson and Germer (as well as G.

P. Thompson) conducted a famous and important experiment. Which of the following statements is TRUE concerning their experiment? A. B. C. D. E. They observed standing wave patterns from electrons confirming the existence of orbitals None of the other four statements is true They observed diffraction patterns from photons confirming that light had wave properties They observed diffraction patterns of electrons confirming that matter had wave properties Their experiment contradicted DeBroglie’s equation 25. Which of the following represents the orbit with the largest radius? A. B. C. D.

E. n=3 orbit for H n=3 orbit for Li2+ n=2 orbit for Be3+ n=1 orbit for H n=4 orbit for He+ Page 5, v2 Chemistry 110 Midterm 1 October 11, 2005 26. The workfunction for Na is 2. 70 eV, for Mg is 3. 66 eV, and for Cs is 2. 14 eV. Assume we shine light with a wavelength of 400 nm on the surface of each of these metals. Which of the following statements is/are TRUE about the observed results? (Note 1 eV = 1. 609 x 10-19 J) A. B. C. D. E. No electrons are ejected from Na, Mg, or Cs but would be if the light frequency were increased Electrons are ejected from Mg and they have a velocity of 4. x 105 m/s Two of the other four statements are true Electrons are ejected from both Cs and Na and they would have a greater velocity from Cs Electrons are not ejected from Mg, but would be if the intensity of the light were increased 27. Arrange the following species in order of increasing ionization energy: Al, In, Ga, Si, S? A. B. C. D. E. In, Al, Ga, Si, S In, Ga, Al, Si, S S, Si, Al, Ga, In Si, S, Al, Ga, In In, Ga Si, S, Al

28. Which of these species has the greatest number of unpaired electrons? A. B. C. D. E. P (Z=15) Mo (Z=42) Mn (Z=25) Rb (Z=37) Cu (Z=29) 9. What would be the ground state electron configuration for Ge3+? A. B. C. D. E. [Ar] 3d10 4s2 4p2 [Ar] 3d9 4s2 [Ar] 3d10 4p1 [Ar] 3d10 4s1 [Ar] 3d7 4s2 4p2 30. Which of the following statements is/are TRUE ? A. The square of the wavefunction, ? 2, is the total probability of finding the electron in a spherical shell at distance r from the nucleus B. The wavefunction, ? , is a solution to the Schrodinger equation C. Orbitals with the same n cannot overlap in space D. two of the other four statements are true E. For the same orbital type (i. e. ame l quantum number), orbitals with the higher n value will have a more negative energy Page 6, v2 Answer Key for Test “Chem110MT1F05. tst”, 10/12/2005 No. in No. on Q-Bank Test 7 146 1 7 136 2 7 134 3 7 129 4 7 138 5 7 144 6 7 147 7 7 123 8 7 121 9 7 120 10 7 122 11 7 149 12 7 128 13 7 131 14 7 125 15 7 135 16 7 141 17 7 145 18 7 127 19 7 148 20 7 133 21 7 137 22 7 140 23 7 124 24 7 143 25 7 130 26 7 142 27 7 132 28 7 139 29 7 126 30 Correct Answer D E C C C A B D E E D B A D A C C D E E A A A D A D B B D B Page 1, v2 Chemistry 110 Midterm 1 October 11, 2005 1.

Assume that we conduct a Stern Gerlach type experiment by passing a beam of cobalt (Co) atoms and zinc (Zn) atoms simultaneously through an external magnetic field. What would be the expected pattern on the detector? A. B. C. D. E. Two spots: one deflected up, one deflected down Four spots: two deflected up, two deflected down Three spots: one undeflected, one deflected up, one deflected down Two spots: one undeflected, one deflected up Three spots: two deflected up, one deflected down 2. Arrange the following species in order of decreasing radius: Br- , Y3+, Rb+, Se2- , Kr? A. B. C. D.

E. Kr, Se2- , Br- , Rb+, Y3+ Y3+, Rb+, Kr, Br- , Se2Se2- , Br- , Kr, Rb+, Y3+ Rb+, Y3+, Kr, Se2- , BrKr, Y3+, Rb+, Br- , Se2- 3. Praseodymium (Pr Z=59) is one of the lanthanide (rare earth) elements. Which of the following statements is a TRUE statement about the orbital into which the last electron was filled for the element Pr? A. B. C. D. E. The number of radial nodes is greater than the number of angular nodes none of the other four statements is true The orbital contains valence electrons The orbital is one member of a set of seven degenerate orbitals The orbital is a 5f orbital . What would be a valid set of quantum numbers for the last electron filled in the electronic configuration for osmium (Os Z=76)? A. B. C. D. E. n = 6, l = 1, ml = 0, ms = 1/2 n = 5, l = 3, ml = -3, ms = 1/2 n = 5, l= 2, ml = -2, ms = 1/2 n = 6, l = 2, ml = 0, ms = 1/2 n = 6, l = 0, ml = 0, ms = 1/2 5. Which of the following represents the orbit with the largest radius? A. B. C. D. E. n=4 orbit for He+ n=1 orbit for H n=2 orbit for Be3+ n=3 orbit for Li2+ n=3 orbit for H Page 1, v3 Chemistry 110 Midterm 1 October 11, 2005 6. Xe]f145d10 6s1 is the ground state electronic configuration of which species? A. B. C. D. E. Pb2+ Hg Pt Au Tl+ 7. The element seaborgium (Sg) has Z=106. What would you predict the electron configuration to of Sg2+ to be? A. B. C. D. E. [Rn] 5f12 6d4 7s2 [Rn] 5f14 6d4 [Rn] 5f14 6d2 7s2 [Rn] 6d4 The same configuration as rutherfordium (Rh) Z=104 8. What would be the ground state electron configuration for Ge3+? A. B. C. D. E. [Ar] 3d9 4s2 [Ar] 3d10 4s2 4p2 [Ar] 3d10 4p1 [Ar] 3d7 4s2 4p2 [Ar] 3d10 4s1 9. Which of the following species is the most paramagnetic? A. B. C. D. E. Cr Ga+ N Fe3+ Os 10.

If the wavelength of an electron is equal to the radius of the n=2 orbit in He+, what must the velocity of the electron be? A. B. C. D. E. 1. 38 x 107 m/s 6. 88 x 106 m/s 3. 44 x 106 m/s 5. 47 x 105 m/s The velocity cannot have an exact value Page 2, v3 Chemistry 110 Midterm 1 October 11, 2005 11. What is the energy of light that has a wavelength of 1 micrometer (1µm)? A. B. C. D. E. 1. 986×104 kJ/mol 119. 6 kJ/mol 1. 196 x 105 kJ/mol None of these other four answers 1. 986 x 10-19 kJ/mol 12. The term “ultraviolet catastrophe” referred to what aspect in the scientific developments that led to the new quantum theory?

A. B. C. D. E. That the light exhibited wave particle duality The energy density went to infinity at short wavelengths in the classical theory for blackbody radiation That the intensity of ultraviolet light had no effect in producing photoelectric emission None of these other four answers That the Balmer series emission lines for H were only observed in the visible region 13. A two-photon absorption transition is observed using a laser that emits light having a wavelength of 500 nm? Which of the following statements is/are TRUE about this electronic transition? A. B.

C. D. E. The single photon transition would be caused by IR light with a wavelength of 250 nm None of the other four statements is true The single photon transition would be caused by IR light with a wavelength of 1000 nm The single photon transition would be caused by UV light with a wavelength of 250 nm The single photon transition would be caused by UV light with a wavelength of 1000 nm 14. Davisson and Germer (as well as G. P. Thompson) conducted a famous and important experiment. Which of the following statements is TRUE concerning their experiment? A. B. C. D. E.

None of the other four statements is true They observed diffraction patterns from photons confirming that light had wave properties They observed standing wave patterns from electrons confirming the existence of orbitals Their experiment contradicted DeBroglie’s equation They observed diffraction patterns of electrons confirming that matter had wave properties 15. If an electron was in an orbital with 1 radial node and 3 angular nodes, what type of orbital is the electron occupying? A. B. C. D. E. None of the other four answers 5p 4f 5f 4d Page 3, v3 Chemistry 110 Midterm 1 October 11, 2005 16.

What would be a permitted value for the principle quantum number if we knew that the magnetic quantum number (ml) was 7? A. B. C. D. E. 5 6 7 none of these other four answers 15 17. Which of these species has the greatest number of unpaired electrons? A. B. C. D. E. Mo (Z=42) P (Z=15) Cu (Z=29) Mn (Z=25) Rb (Z=37) 18. Which statement(s) is (are) FALSE in comparing the electronic transition from ni = 5 to nf =2 in H with that of electronic transition from ni = 2 to nf =5 in Be3+ A. A photon of the same frequency is involved in both transitions, but is emitted the H electronic transition and absorbed in the Be3+ electronic transition.

B. The wavelength of the photon emitted by H is 16 times the wavelength of the photon absorbed by Be3+ C. The photon involved in the H transition lies in the visible spectrum while that involved in the Be3+ transition lies in the UV region of the spectrum. D. two of the other four statements are FALSE E. The transition in H is a Balmer emission series line 19. Arrange the following species in order of increasing radius Se, Pb, Sn, Ge, As? A. B. C. D. E. As, Se, Ge, Sn, Pb Se, Pb, As, Sn, Ge Pb, Sn, Ge, As, Se Se, As, Ge, Sn, Pb As, Ge, Sn, Pb, Se 20. One of the Lyman series emission lines for hydrogen (H) is observed at 102. nm. This transition involves an electron dropping down to the ground state level from a higher energy level. What is the ninitial value for the higher energy orbit (i. e. what is ni)? A. B. C. D. E. 4 3 1 2 None of the other four answers Page 4, v3 Chemistry 110 Midterm 1 October 11, 2005 21. Arrange the following species in order of increasing ionization energy: Al, In, Ga, Si, S? A. B. C. D. E. In, Al, Ga, Si, S S, Si, Al, Ga, In Si, S, Al, Ga, In In, Ga Si, S, Al In, Ga, Al, Si, S 22. How many valence electrons are found in tellurium (Te Z=52)? A. B. C. D. E. 2 6 1 4 16 3. Which is not a valid set of quantum numbers for an electron? A. B. C. D. E. n = 7, l = 0, ml = 0, ms = 1/2 n = 6, l = 2, ml = 0, ms = 1/2 n = 4, l = -2, ml = 2, ms = -1/2 n = 3, l = 2, ml = -2, ms = 1/2 n = 17, l = 16, ml = 16, ms = -1/2 24. Assume that the uncertainty in determining the position of an electron is equal to its DeBroglie wavelength. What would be the uncertainty in the momentum for an electron traveling with a velocity of 1. 00 x 107 m/s? A. B. C. D. E. > h/(4*pi) > 7. 27 x 10-11 kg m/s > 1. 38 x 1024 kg m/s > 7. 25 x 10-25 kg m/s > 9. 09 x 10-24 kg m/s 25. What are the possible values for the orbital angular momentum quantum number l given the following values for the other three quantum numbers: n = 4, l = ? , ml = 0, ms = +1/2 A. B. C. D. E. 0, 1, 2, or 3 0 1, 2, 3, or 4 3 none of these answers Page 5, v3 Chemistry 110 Midterm 1 October 11, 2005 26. Which of the following statements is/are TRUE ? A. The square of the wavefunction, ? 2, is the total probability of finding the electron in a spherical shell at distance r from the nucleus B. The wavefunction, ? , is a solution to the Schrodinger equation C. wo of the other four statements are true D. Orbitals with the same n cannot overlap in space E. For the same orbital type (i. e. same l quantum number), orbitals with the higher n value will have a more negative energy 27. Which of the following statements is/are TRUE about the species Sn2+? A. B. C. D. E. It has 48 protons in the nucleus It is a paramagnetic species It would be expected to have a larger radius than Sn none of these other four answers is true It has a completely filled f orbital set 28. The workfunction for Na is 2. 70 eV, for Mg is 3. 66 eV, and for Cs is 2. 14 eV.

Assume we shine light with a wavelength of 400 nm on the surface of each of these metals. Which of the following statements is/are TRUE about the observed results? (Note 1 eV = 1. 609 x 10-19 J) A. B. C. D. E. Electrons are ejected from Mg and they have a velocity of 4. 4 x 105 m/s Electrons are ejected from both Cs and Na and they would have a greater velocity from Cs No electrons are ejected from Na, Mg, or Cs but would be if the light frequency were increased Electrons are not ejected from Mg, but would be if the intensity of the light were increased Two of the other four statements are true 9. Assume that at an elevated temperature, the ground state for Be3+ is n=5. What would be the ionization energy for this species in this case? (1eV = 1. 609 x 10-19 J) A. B. C. D. E. 216. 7 eV None of the other four answers 138. 7 eV 8. 667 eV 2. 167 eV 30. What would be the velocity of an electron ejected from sodium if light of 350 nm is directed at a surface of the metal (the workfunction for sodium is 2. 70 eV and 1eV = 1. 609 x 10-19 J) A. B. C. D. E. None of the other four answers 541 km/s 382 km/s 5. 41 x 105 km/s 17,010 km/s Page 6, v3

Answer Key for Test “Chem110MT1F05. tst”, 10/12/2005 No. in No. on Q-Bank Test 7 129 1 7 133 2 7 123 3 7 135 4 7 143 5 7 146 6 7 122 7 7 139 8 7 136 9 7 121 10 7 145 11 7 144 12 7 125 13 7 124 14 7 140 15 7 148 16 7 132 17 7 128 18 7 134 19 7 141 20 7 142 21 7 147 22 7 127 23 7 131 24 7 120 25 7 126 26 7 149 27 7 130 28 7 137 29 7 138 30 Correct Answer C C D C E D B E A B B B D E D E A A D B E B C D A B D B D B Page 1, v3 Chemistry 110 Midterm 1 October 11, 2005 1. What is the energy of light that has a wavelength of 1 micrometer (1µm)?

A. B. C. D. E. None of these other four answers 1. 196 x 105 kJ/mol 119. 6 kJ/mol 1. 986 x 10-19 kJ/mol 1. 986×104 kJ/mol 2. Arrange the following species in order of decreasing radius: Br- , Y3+, Rb+, Se2- , Kr? A. B. C. D. E. Rb+, Y3+, Kr, Se2- , BrKr, Y3+, Rb+, Br- , Se2Kr, Se2- , Br- , Rb+, Y3+ Se2- , Br- , Kr, Rb+, Y3+ Y3+, Rb+, Kr, Br- , Se2- 3. The term “ultraviolet catastrophe” referred to what aspect in the scientific developments that led to the new quantum theory? A. B. C. D. E.

That the Balmer series emission lines for H were only observed in the visible region The energy density went to infinity at short wavelengths in the classical theory for blackbody radiation That the intensity of ultraviolet light had no effect in producing photoelectric emission None of these other four answers That the light exhibited wave particle duality 4. A two-photon absorption transition is observed using a laser that emits light having a wavelength of 500 nm? Which of the following statements is/are TRUE about this electronic transition? A. B. C. D. E.

The single photon transition would be caused by UV light with a wavelength of 1000 nm The single photon transition would be caused by IR light with a wavelength of 1000 nm The single photon transition would be caused by UV light with a wavelength of 250 nm The single photon transition would be caused by IR light with a wavelength of 250 nm None of the other fo

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