Chapter 6 Electronic Structure and the Periodic Table

Transcription

1 Chapter 6 Electronic Structure and the Periodic Table MULTIPLE CHOICE 1. The Navy uses electromagnetic radiation of extremely long wavelengths to communicate with submerged submarines. The Navy's ELF (Extremely Low Frequency) systems emit 76 s -1 radiation from facilities located in Wisconsin and Michigan. What is the wavelength of this radiation (in meters)? a m b m c m d m e m 2. The lowest frequency available on a radio's AM dial is 570 khz. What is the wavelength of this light? a m b m c m d m e m 3. A microwave oven emits radiation at a frequency of Hz. What is the wavelength of this light? a m b m c m d m e m 4. Many hand held laser pointers emit 650 nm light. What is the frequency of this light? a Hz b Hz c Hz d Hz e Hz 5. Green laser pointers emit radiation at 532 nm. What is the frequency of this radiation? a Hz b Hz c Hz d Hz e Hz 1

2 6. Place the following regions of the electromagnetic spectrum in order from longest to shortest wavelength. a. radio > microwave > visible > ultraviolet > gamma ray b. gamma ray > microwave > radio > visible > ultraviolet c. ultraviolet > visible > microwave > radio > gamma ray d. microwave > radio > ultraviolet > visible > gamma ray e. visible > gamma ray > radio > ultraviolet > microwave 7. Place the following regions of the electromagnetic spectrum in order from highest to lowest energy. a. infrared > gamma rays > x-rays > visible > radio b. gamma rays > x-rays > visible > infrared > radio c. x-rays > gamma rays > infrared > visible > radio d. radio > x-rays > gamma rays > visible > infrared e. visible > infrared > radio > x-rays > gamma rays 8. All of the following statements are false EXCEPT a. the wavelength of light is directly proportional to its frequency. b. the frequency of light is inversely proportional to its energy. c. the energy of a photon of light is inversely proportional to its wavelength. d. the frequency of light is directly proportional to the speed of light (in a vacuum). e. the wavelength of light is directly proportional to the speed of light (in a vacuum). 9. Some digital cordless phones operate at 2.4 GHz (1 GHz = 10 9 Hz). What is the energy, in joules, of a single 2.4 GHz photon? a J b J c J d J e J 10. A helium-neon (or HeNe) laser emits light at nm. What is the energy of a single photon from this laser? a J b J c J d J e J 11. When Cs-137 decays, it emits gamma radiation. The energy of one photon is J. What is the wavelength of this radiation? a m b m c m d m e m 2

3 12. The energy required to break one mole of hydrogen bonds in H 2 (g) is 436 kj. What is the longest wavelength of light that is capable of breaking this bond? a nm b. 103 nm c. 192 nm d. 208 nm e. 274 nm 13. According to the Bohr model for the hydrogen atom, the energy necessary to excite an electron from n = 5 to n = 6 is the energy necessary to excite an electron from n = 3 to n = 4. a. greater than b. equal to c. less than d. either equal to or greater than e. either less than or equal to 14. Calculate the wavelength of the line in the Lyman series that results from the transition n = 3 to n = 1. The Rydberg constant equals J. a nm b nm c nm d nm e nm 15. Calculate the energy of a photon in the Balmer series that results from the transition n = 5 to n = 2. What is the region of the electromagnetic spectrum? The Rydberg constant equals J. a J; visible b J; x-ray c J; visible d J; radio e J; ultraviolet 16. A line in the Pfund series (n lo = 5) occurs at m. What is n hi for this transition? The Rydberg constant equals J. a. 6 b. 7 c. 8 d. 9 e. 10 3

4 17. Which of the following electronic transitions would emit the lowest energy photon? a. n = 1 to n = 2 b. n = 2 to n = 1 c. n = 3 to n = 2 d. n = 5 to n = 2 e. n = 5 to n = The Schrödinger wave equation a. proves electrons have positive and negative spins. b. calculates the precise position and momentum of an electron at any given time. c. is used to compute the wavelength of small particles. d. can be solved to find the probability of finding an electron in a region of space. e. proves that photons are particles. 19. The Pauli exclusion principle states that a. no two electrons from a given atom can have the same spin. b. no two electrons from a given atom can have the same four quantum numbers. c. two electrons can occupy an orbital if they have the same spin. d. two electrons can occupy an orbital if they have opposite spins. e. two electrons can occupy an orbital if they have opposite charges. 20. Which of the following sets of quantum numbers refers to a 3p orbital? a. n = 3, = 0, m = 0, m s = + 1/2 b. n = 3, = 1, m = -1, m s = + 1/2 c. n = 3, = 2, m = 1, m s = + 1/2 d. n = 3, = 3, m = -2, m s = + 1/2 e. n = 3, = 3, m = 3, m s = + 1/2 21. Which of the following sets of quantum numbers refers to a 2s orbital? a. n = 1, = 2, m = 2, m s = + 1/2 b. n = 1, = 2, m = 1, m s = + 1/2 c. n = 2, = 2, m = 0, m s = + 1/2 d. n = 2, = 1, m = -1, m s = + 1/2 e. n = 2, = 0, m = 0, m s = + 1/2 22. All of the following sets of quantum numbers are allowed EXCEPT a. n = 1, = 0, m = 1, m s = - 1/2. b. n = 2, = 1, m = 0, m s = + 1/2. c. n = 3, = 1, m = -1, m s = - 1/2. d. n = 4, = 3, m = -1, m s = - 1/2. e. n = 6, = 3, m = -3, m s = + 1/2. 4

5 23. How many orbitals have the following quantum numbers: n = 4, = 1? a. 0 b. 1 c. 3 d. 4 e How many orbitals have the following quantum numbers: n = 6, = 2, m = -2? a. 0 b. 1 c. 3 d. 5 e What is the total capacity of electrons in n = 3? a. 5 b. 10 c. 18 d. 32 e What is the total capacity of electrons in n = 5, = 3? a. 2 b. 6 c. 10 d. 14 e Which of the following sets of quantum numbers refers to a 4f orbital? a. n = 4, = 1, m = 0, m s = + 1/2 b. n = 4, = 2, m = -1, m s = - 1/2 c. n = 4, = 3, m = -2, m s = - 1/2 d. n = 4, = 4, m = 0, m s = + 1/2 e. n = 4, = 4, m = -4, m s = + 1/2 28. What type of orbital is designated by n = 5, = 2, m = +1? a. 5d b. 2f c. 5p d. 2s e. 5p 5

6 29. Which quantum number designates the shape of an atomic orbital? a. n b. c. m d. m s e. m s and m 30. What is the ground state electron configuration of 25 Mn? a. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 4s 1 b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 2 c. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 7 d. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 e. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4d What is the ground state electron configuration of 24 Cr? a. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 4 b. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 c. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 4 4s 2 d. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 1 e. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s What is the ground state electron configuration of 94 Pu? a. [Xe]5f 6 6s 2 b. [Xe]6f 6 7s 2 c. [Rn]6f 6 7s 2 d. [Rn]5f 6 7s 2 e. [Rn]5f 6 6d 10 7s What is the electron configuration of S 2-? a. 1s 2 2s 2 2p 6 b. 1s 2 2s 2 2p 6 3s 2 c. 1s 2 2s 2 2p 6 3s 2 3p 4 d. 1s 2 2s 2 2p 6 3s 2 3p 6 e. 1s 2 2s 2 2p 6 3s 2 3p 6 4s What is the electron configuration of Cu +? a. [Ar]3d 8 b. [Ar]3d 9 c. [Ar]3d 10 d. [Ar]3d 8 4s 2 e. [Ar]3d 9 4s 1 6

7 35. What is the electron configuration of Ga +? a. [Ar]3d 10 4s 2 b. [Ar]3d 10 4p 2 c. [Ar]3d 8 4s 2 4p 2 d. [Ar]3d 10 4s 2 4d 4 e. [Ar]3d 10 4s 2 4p Hund's rule predicts that a. the most stable electronic structure of an atom has electron spins paired. b. no two electrons will share the same orbital. c. electrons in an orbital have equal but opposite charges. d. electrons must have opposite spins to share an orbital. e. when several orbitals of equal energy are available, as in a given subshell, electrons enter singly with parallel spins. 37. What is the symbol of the atom or ion with the following orbital diagram? 1s 2s 2p ( ) ( ) ( )( )( ) a. 5B b. 7N c. 8O d. 16S e. 9F 38. What is the symbol of the atom or ion with the following orbital diagram? 1s 2s 2p 3s 3p 3d 4s ( ) ( ) ( )( )( ) ( ) ( )( )( ) ( )( )( )( )( ) ( ) a. 26Fe b. 26Fe 2+ c. 27Co + d. 28Ni e. 28Ni What is the symbol of an ion with the following orbital diagram? 3d 4s [Ar] ( )( )( )( )( ) ( ) a. 21Sc 3+ b. 22Ti 2+ c. 22Ti 4+ d. 24Cr 2+ e. 24Cr 3+ 7

8 40. What is the correct orbital diagram for phosphorus? 1s 2s 2p 3s 3p a. ( ) ( ) ( )( )( ) b. ( ) ( ) ( )( )( ) c. ( ) ( ) ( )( )( ) ( ) ( )( )( ) d. ( ) ( ) ( )( )( ) ( ) ( )( )( ) e. ( ) ( ) ( )( )( ) ( ) ( )( )( ) 41. What is the correct orbital diagram for Ca 2+? 1s 2s 2p 3s 3p 4s a. ( ) ( ) ( )( )( ) b. ( ) ( ) ( )( )( ) ( ) ( )( )( ) c. ( ) ( ) ( )( )( ) ( ) ( )( )( ) d. ( ) ( ) ( )( )( ) ( ) ( )( )( ) ( ) e. ( ) ( ) ( )( )( ) ( ) ( )( )( ) ( ) 42. What is the correct orbital diagram for Fe 2+? 3d 4s a. [Ar] ( )( )( )( )( ) ( ) b. [Ar] ( )( )( )( )( ) ( ) c. [Ar] ( )( )( )( )( ) ( ) d. [Ar] ( )( )( )( )( ) ( ) e. [Ar] ( )( )( )( )( ) ( ) 43. What is the correct orbital diagram for O 2-? 1s 2s 2p a. ( ) ( ) ( )( )( ) b. ( ) ( ) ( )( )( ) c. ( ) ( ) ( )( )( ) d. ( ) ( ) ( )( )( ) e. ( ) ( ) ( )( )( ) 8

9 44. Elements and compounds with unpaired electrons are attracted to a magnetic field. These materials are called paramagnetic. Which of the following elements or ions are paramagnetic in the ground state? a. Cl - b. Fe 2+ c. Ne d. Ca 2+ e. Sc In general, ionization energies a. increase down a group and increase across a period. b. increase down a group and decrease across a period. c. decrease down a group and increase across a period. d. decrease down a group and decrease across a period. e. increase with atomic mass and increase with atomic radii. 46. In general, atomic radii a. increase down a group and decrease across a period. b. increase down a group and increase across a period. c. decrease down a group and decrease across a period. d. are proportional to atomic mass. e. decrease down a group and increase across a period. 47. Place the following atoms in order of increasing size: Al, Cl, Mg, O, and P. a. Cl < O < P < Al < Mg b. Cl < P < Al < Mg < O c. O < Cl < P < Al < Mg d. O < Mg < Al < P < Cl e. none of the above 48. Place the following atoms in order of increasing size: Ba, Ca, Mg, Na, and Rb. a. Na < Mg < Ca < Rb < Ba b. Mg < Na < Ca < Rb < Ba c. Na < Rb < Mg < Ca < Ba d. Ba < Rb < Ca < Mg < Na e. Ba < Rb < Ca < Na < Mg 49. Place the following ions in order of increasing radius: Al 3+, F -, Mg 2+, and N 3-. a. F - < Mg 2+ < N 3- < Al 3+ b. F - < N 3- < Al 3+ < Mg 2+ c. F - < N 3- < Mg 2+ < Al 3+ d. N 3- < F - < Mg 2+ < Al 3+ e. Al 3+ < Mg 2+ < F - < N 3-9

10 50. Place the following atoms or ions in order of increasing radius: O, O 2-, S 2-, and Se 2-. a. O 2- < O < S 2- < Se 2- b. Se 2- < S 2- < O 2- < O c. O 2- < O < Se 2- < S 2- d. Se 2- < S 2- < O < O 2- e. O < O 2- < S 2- < Se Which of the following chemical expressions refers to the first ionization energy of calcium? a. Ca(s) Ca + (s) + e - b. Ca(g) + e - Ca + (g) c. Ca(s) + e - Ca + (s) d. Ca(g) Ca + (g) + e - e. Ca(g) Ca 2+ (g) + e Which of the following atoms would have the largest second ionization energy? a. Na b. Ca c. Mg d. Ba e. Sr 53. Place the following atoms in order of increasing ionization energy: C, N, and Si. a. C < N < Si b. C < Si < N c. Si < C < N d. Si < N < C e. N < C < Si 54. Electronegativity increases a. moving down a group in the periodic table. b. moving from left to right across the periodic table. c. with increasing atomic mass. d. when electrons are paired. e. with increasing atomic radii. 10