Homework answers / question archive / Chapter 7: Electron Structure of the Atom 1) Rank the following types of electromagnetic radiation from shortest wavelength to longest wavelength:  visible, ultraviolet, microwave, infrared, x-ray

Chapter 7: Electron Structure of the Atom 1) Rank the following types of electromagnetic radiation from shortest wavelength to longest wavelength:  visible, ultraviolet, microwave, infrared, x-ray

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Chapter 7: Electron Structure of the Atom

1) Rank the following types of electromagnetic radiation from shortest wavelength to longest wavelength:  visible, ultraviolet, microwave, infrared, x-ray.

            A)      x-ray < visible < ultraviolet < infrared < microwave

            B)      x-ray < ultraviolet < visible < microwave < infrared

            C)      x-ray < ultraviolet < visible < infrared < microwave

            D)      infrared < microwave < ultraviolet < visible < x-ray

            E)      microwave < infrared < visible < ultraviolet < x-ray

 

        2.  Rank the following types of electromagnetic radiation from lowest frequency to highest frequency:  visible, ultraviolet, microwave, infrared, x-ray.

            A)      x-ray < visible < ultraviolet < infrared < microwave

            B)      x-ray < ultraviolet < visible < microwave < infrared

            C)      x-ray < ultraviolet < visible < infrared < microwave

            D)      infrared < microwave < ultraviolet < visible < x-ray

            E)      microwave < infrared < visible < ultraviolet < x-ray

 

        3.  Rank the following types of electromagnetic radiation from lowest energy to highest energy:  visible, ultraviolet, microwave, infrared, x-ray.

            A)      x-ray < visible < ultraviolet < infrared < microwave

            B)      x-ray < ultraviolet < visible < microwave < infrared

            C)      x-ray < ultraviolet < visible < infrared < microwave

            D)      infrared < microwave < ultraviolet < visible < x-ray

            E)      microwave < infrared < visible < ultraviolet < x-ray

 

        4.  List the following colors of visible light from lowest frequency to highest frequency:  green, blue, yellow, red, violet.

            A)      red < yellow < green < blue < violet     D)      violet < blue < green < yellow < red

            B)      violet < yellow < green < blue < red     E)      yellow < red < green < violet < blue

            C)      blue < violet < green < red < yellow              

 

        5.  List the following colors of visible light from shortest wavelength to longest wavelength:  green, blue, yellow, red, violet.

            A)      red < yellow < green < blue < violet     D)      violet < blue < green < yellow < red

            B)      violet < yellow < green < blue < red     E)      yellow < red < green < violet < blue

            C)      blue < violet < green < red < yellow              

        6.  List the following colors of visible light from lowest energy to highest energy:  green, blue, yellow, red, violet.

            A)      red < yellow < green < blue < violet     D)      violet < blue < green < yellow < red

            B)      violet < yellow < green < blue < red     E)      yellow < red < green < violet < blue

            C)      blue < violet < green < red < yellow              

 

        7.  Which of the following statements regarding electromagnetic radiation is incorrect?

            A)      The distance between two corresponding points on a wave is its wavelength.

            B)      Each type of electromagnetic radiation has its own characteristic range of wavelengths and frequencies.

            C)      The visible portion of the electromagnetic spectrum has the lowest energy of any of the types of electromagnetic radiation.

            D)      The energy of electromagnetic radiation is directly proportional to its frequency.

            E)      The wavelength of electromagnetic radiation is inversely proportional to its frequency.

 

        8.  A laser used in DVD players has a wavelength of 405 nm.  What is the frequency of this light in hertz (s^–1)?

            A)      7.41 ´ 10⁵ s^–1                                         D)      1.35 ´ 10^–13 s^–1

            B)      7.41 ´ 10¹⁴ s^–1                                        E)      1.22 ´ 10² s^–1

            C)      1.35 ´ 10^-6 s^–1                                                 

        9.  The wavelength of the yellow light given off by a sodium vapor street lamp is 589 nm. 

            What is the frequency of this light in hertz (s^–1)?

            A)      5.09 ´ 10⁵ s^–1                                         D)      1.96 ´ 10^–13 s^–1

            B)      5.09 ´ 10¹⁴ s^–1                                        E)      1.77 ´ 10² s^–1

            C)      1.96 ´ 10^–6 s^–1                                                

 

      10.  The wavelength of the blue light given off by a mercury vapor street lamp is 436 nm.  What is the frequency of this light in hertz (s^–1)?

            A)      6.88 ´ 10⁵ s^–1                                         D)      1.45 ´ 10^–13 s^–1

            B)      6.88 ´ 10¹⁴ s^–1                                        E)      1.31 ´ 10² s^–1

            C)      1.45 ´ 10^–6 s^–1                                                

 

      11.  What is the energy of a photon of yellow light whose wavelength is 589 nm?

            A)      3.37 ´ 10^–19 J                                         D)      5.09 ´ 10⁵ J

            B)      3.37 ´ 10^–10 J                                         E)      3.38 ´ 10^–28 J

            C)      1.77 ´ 10² J                                                    

 

      12.  A laser used in DVD players has a wavelength of 405 nm.  What is the energy of this light in joules?

            A)      4.91 ´ 10^–28 J                                         D)      8.05 ´ 10^–23 J

            B)      4.91 ´ 10^–19 J                                         E)      2.98 ´ 10^–48 J

            C)      8.05 ´ 10^–32 J                                                  

      13.  The wavelength of the blue light given off by a mercury vapor street lamp is 436 nm.

            What is the energy of this light in joules?

            A)      4.56 ´ 10^–28 J                                         D)      8.67 ´ 10^–23 J

            B)      4.56 ´ 10^–19 J                                         E)      9.63 ´ 10^–40 J

            C)      8.67 ´ 10^–32 J                                                  

 

      14.  A laser emits light with a frequency of 4.69 ´ 10¹⁴ s^–1.  Calculate the wavelength of this light.

            A)      640 nm                                                  D)      1.41 ´ 10²⁵ m

            B)      6.40 ´ 10^–9 m                                         E)      1.41 ´ 10¹⁴ nm

            C)      1.56 ´ 10⁶ m                                                   

 

      15.  If the energy of a photon of light is 3.37 ´ 10^–19 J, what is the frequency of the light?

            A)      1.12 ´ 10^–27 s^–1                                      D)      6.70 ´ 10^–44 s^–1

            B)      8.90 ´ 10²⁶ s^–1                                        E)      1.01 ´ 10^–10 s^–1

            C)      5.09 ´ 10¹⁴ s^–1                                                

 

      16.  Which of the following statements regarding spectra is incorrect?

            A)      Sunlight produces a continuous spectrum.

            B)      A heated ionic compound produces a line spectrum.

            C)      Several elements can produce the same line spectrum.

            D)      If you know the wavelength of a line in a spectrum, the energy of the light associated with that line can be calculated.

            E)      If you know the wavelength of a line in a spectrum, the frequency of the light associated with that line can be calculated.

 

      17.  Which of the following statements regarding the Bohr model of the hydrogen atom is incorrect?

            A)      Bohr's model shows the electron circling the nucleus in fixed orbits.

            B)      In Bohr's model, electrons could exist between orbits.

            C)      In Bohr's model, when an electron absorbs energy, it can move to a higher-energy orbit.

            D)      In Bohr's model, when an electron emits energy, it can move to a lower-energy orbit.

            E)      In Bohr's model, n = 1 is the lowest energy orbit.

      18.  Which of the following statements regarding the Bohr model of the hydrogen atom is incorrect?

            A)      In Bohr's model, when 1 electron moves directly from the n = 5 to the n = 3 orbit, two photons are emitted.

            B)      In Bohr's model, when 1 electron moves from the n = 5 to the n = 4 orbit and then from the n = 4 to the n = 3 orbit, two photons are emitted.

            C)      In Bohr's model, the transition of an electron from the n = 4 to the n = 3 orbit would result in the emission of a lower energy photon than a transition from the n = 3 to the n = 2 orbit.

            D)      In Bohr's model, the transition of an electron from the n = 4 to the n = 3 orbit would result in the emission of a longer wavelength photon than a transition from the n = 3 to the n = 2 orbit.

            E)      In Bohr's model, the four colored lines in the hydrogen spectrum result from transitions of electrons from higher energy levels down to the n = 2 orbit.

 

      19.  Rank the following electron transitions in a hydrogen atom from lowest energy to highest energy:  n = 5 to n = 2, n = 4 to n = 2, n = 6 to n = 2, n = 3 to n = 2

            A)      n = 6 to n = 2 < n = 5 to n = 2 < n = 4 to n = 2 < n = 3 to n = 2

            B)      n = 3 to n = 2 < n = 4 to n = 2 < n = 5 to n = 2 < n = 6 to n = 2

            C)      n = 5 to n = 2 < n = 4 to n = 2 < n = 6 to n = 2 < n = 3 to n = 2

            D)      n = 5 to n = 2 < n = 6 to n = 2 < n = 4 to n = 2 < n = 3 to n = 2

            E)      n = 6 to n = 2 < n = 4 to n = 2 < n = 5 to n = 2 < n = 3 to n = 2

 

      20.  Rank the following electron transitions in a hydrogen atom from shortest wavelength  to longest wavelength:  n = 5 to n = 2, n = 4 to n = 2, n = 6 to n = 2, n = 3 to n = 2

            A)      n = 6 to n = 2 < n = 5 to n = 2 < n = 4 to n = 2 < n = 3 to n = 2

            B)      n = 3 to n = 2 < n = 4 to n = 2 < n = 5 to n = 2 < n = 6 to n = 2

            C)      n = 5 to n = 2 < n = 4 to n = 2 < n = 6 to n = 2 < n = 3 to n = 2

            D)      n = 5 to n = 2 < n = 6 to n = 2 < n = 4 to n = 2 < n = 3 to n = 2

            E)      n = 6 to n = 2 < n = 4 to n = 2 < n = 5 to n = 2 < n = 3 to n = 2

 

      21.  The red line observed in the line spectrum for hydrogen has a wavelength of 656 nm.  What is the frequency of this light in hertz (s^–1)?

            A)      4.57 ´ 10⁵ s^–1                                         D)      2.18 ´ 10^–13 s^–1

            B)      4.57 ´ 10¹⁴ s^–1                                        E)      1.97 ´ 10² s^–1

            C)      2.18 ´ 10^-6 s^–1                                                 

 

      22.  The green line observed in the line spectrum for hydrogen has a wavelength of 486 nm.  What is the frequency of this light in hertz (s^–1)?

            A)      1.46 ´ 10² s^–1                                         D)      1.62 ´ 10^–6 s^–1

            B)      6.17 ´ 10⁵ s^–1                                         E)      1.62 ´ 10^-13 s^–1

            C)      6.17 ´ 10¹⁴ s^–1                                                

 

      23.  The red line observed in the line spectrum for hydrogen has a wavelength of 656 nm.  What is the energy of a photon of this light?

            A)      3.03 ´ 10^–28 J                                         D)      3.30 ´ 10¹⁸ J

            B)      3.03 ´ 10^–19 J                                         E)      1.30 ´ 10^–22 J

            C)      3.30 ´ 10²⁷ J                                                   

      24.  The green line observed in the line spectrum for hydrogen has a wavelength of 486 nm.  What is the energy of a photon of this light?

            A)      9.66 ´ 10^–23 J                                         D)      2.44 ´ 10¹⁸ J

            B)      4.09 ´ 10^–28 J                                         E)      2.44 ´ 10²⁷ J

            C)      4.09 ´ 10^–19 J                                                  

 

      25.  Upon electrification, hydrogen produces a characteristic line spectrum consisting of four lines in the visible region of the electromagnetic spectrum.  The light emitted in different regions of the visible spectrum 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 transition corresponds to the red line in the hydrogen spectrum?

            A)      n = 2 ® n = 3                                        D)      n = 4 ® n = 2

            B)      n = 2 ® n = 6                                        E)      n = 6 ® n = 2

            C)      n = 3 ® n = 2                                                 

 

      26.  Upon electrification, hydrogen produces a characteristic line spectrum consisting of four lines in the visible region of the electromagnetic spectrum.  The light emitted in different regions of the visible spectrum 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 transition corresponds to the violet line in the hydrogen spectrum?

            A)      n = 2 ® n = 3                                        D)      n = 4 ® n = 2

            B)      n = 2 ® n = 6                                        E)      n = 6 ® n = 2

            C)      n = 3 ® n = 2                                                 

 

      27.  Upon electrification, hydrogen produces the following line spectrum in the visible region of the electromagnetic spectrum.  If the light emitted 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 transition corresponds to the emission of light with lowest frequency?

           

Color	Wavelength (l), nm
Violet	410
Indigo	434
Blue-green	486
Red	656

 

            A)      n = 2 ® n = 3                                        D)      n = 4 ® n = 2

            B)      n = 2 ® n = 6                                        E)      n = 6 ® n = 2

            C)      n = 3 ® n = 2                                                 

 

      28.  Upon electrification, hydrogen produces the following line spectrum in the visible region of the electromagnetic spectrum.  If the light emitted 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 transition corresponds to the emission of light with highest frequency?

           

Color	Wavelength (l), nm
Violet	410
Indigo	434
Blue-green	486
Red	656

 

            A)      n = 2 ® n = 3                                        D)      n = 4 ® n = 2

            B)      n = 2 ® n = 6                                        E)      n = 6 ® n = 2

            C)      n = 3 ® n = 2                                                 

 

      29.  Upon electrification, hydrogen produces the following line spectrum in the visible region of the electromagnetic spectrum.  If the light emitted 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 transition corresponds to the emission of light with highest energy?

           

Color	Wavelength (l), nm
Violet	410
Indigo	434
Blue-green	486
Red	656

 

            A)      n = 2 ® n = 3                                        D)      n = 4 ® n = 2

            B)      n = 2 ® n = 6                                        E)      n = 6 ® n = 2

            C)      n = 3 ® n = 2                                                 

 

      30.  Which of the following statements regarding orbitals is correct?

            A)      There is no difference between the orbitals of the modern model of the atom and the orbits of the Bohr model of the atom.

            B)      A 1s orbital can be represented as a two-dimensional circle centered around the nucleus of an atom.

            C)      A 2p orbital is smaller than a 3p orbital.

            D)      The p orbitals always come in sets of four.

            E)      The d orbitals always have three lobes.

 

      31.  Which of the following statements regarding orbitals is correct?

            A)      A picture of an n = 1 Bohr orbit would look the same as a picture of a 1s orbital.

            B)      The d orbitals always come in sets of four.

            C)      The s orbitals always have two lobes.

            D)      An orbital can hold four electrons.

            E)      A 2p orbital is lower in energy than a 3p orbital.

 

      32.  Which of the following statements regarding orbital diagrams is correct?

            A)      The 2p sublevel has two orbitals.

            B)      The 4p sublevel has four orbitals.

            C)      Four electrons can be placed in each orbital.

            D)      All of the electrons in a given orbital must have the same spin.

            E)      Electrons will fill a given sublevel in a way that gives the maximum number of unpaired electrons.

 

      33.  When completing the orbital diagram for the element silicon, which of the following statements is correct?

            A)      There are five electrons in the third energy level.

            B)      The 2p sublevel is not full.

            C)      There are no electrons in the 3d sublevel.

            D)      There are no electrons in the 3s sublevel.

            E)      There are no unpaired electrons in the 3p sublevel.

 

      34.  When completing the orbital diagram for the element phosphorus, which of the following statements is correct?

            A)      There are five electrons in the third energy level.

            B)      The 2p sublevel is not full.

            C)      There are electrons in the 3d sublevel.

            D)      There are no electrons in the 3s sublevel.

            E)      There is one unpaired electron in the 3p sublevel.

 

      35.  When completing the orbital diagram for the element argon, which of the following statements is correct?

            A)      There are six electrons in the third energy level.

            B)      The 3p sublevel is not full.

            C)      There are electrons in the 3d sublevel.

            D)      There are no electrons in the 4s sublevel.

            E)      There is one unpaired electron in the 3p sublevel.

 

      36.  How many unpaired electrons are in the orbital diagram for carbon?

            A)  0    B)  2    C)  4    D)  6    E)  8

 

      37.  How many unpaired electrons are in the orbital diagram for phosphorus?

            A)  0    B)  1    C)  2    D)  3    E)  6

 

      38.  How many unpaired electrons are in the orbital diagram for sulfur?

            A)  0    B)  1    C)  2    D)  3    E)  4

 

      39.  Which of the images represents a p orbital?

           

 

            A)  A    B)  B    C)  C    D)  D    E)  none of the above

 

      40.  Which of the images represents an s orbital?

           

 

            A)  A    B)  B    C)  C    D)  D    E)  none of the above

 

      41.  Which of the following is the correct orbital diagram for phosphorus?

            A)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­   ­   ­_

                      1s    2s        2p        3s        3p

            B)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­¯  ­   __

                      1s    2s        2p        3s        3p

            C)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­¯  ­¯  ­¯

                      1s    2s        2p        3s        3p

            D)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­   ­   __

                      1s    2s        2p        3s        3p

            E)      ­¯  ­¯  ­¯ ­¯ ­¯  ­_  ­¯  ­   ­_

                      1s    2s        2p        3s        3p

 

      42.  Which of the following is the correct orbital diagram for silicon?

            A)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­   ­   ­_

                      1s    2s        2p        3s        3p

            B)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­¯      __

                      1s    2s        2p        3s        3p

            C)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­¯  ­¯  ­¯

                      1s    2s        2p        3s        3p

            D)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­   ­   __

                      1s    2s        2p        3s        3p

            E)      ­¯  ­¯  ­¯ ­¯ ­¯  ­_  ­   ­   ­_

                      1s    2s        2p        3s        3p

 

      43.  Which of the following is the correct orbital diagram for sulfur?

            A)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­¯  ­¯  __

                      1s    2s        2p        3s        3p

            B)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­   ­   __

                      1s    2s        2p        3s        3p

            C)      ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­¯  ­_  ­_

                      1s    2s        2p        3s        3p

            D)      ­¯  ­¯  ­¯ ­¯ ­¯  ­_  ­¯  ­¯   ­¯

                      1s    2s        2p        3s        3p

 

      44.  Which of the following is the correct ground state electron configuration for chlorine?

            A)      1s²2s²2p⁵                                                D)      1s²2s²2p⁶3s²3p⁶

            B)      1s²2s²2p⁶3s²4p⁵                                      E)      1s²2s²2p⁶3s²4p⁶

            C)      1s²2s²2p⁶3s²3p⁵                                              

 

      45.  Which of the following is the correct ground state electron configuration for a magnesium atom?

            A)      1s²2s²2p⁸                                                D)      1s²2s²2p⁶3s²3p²

            B)      1s²2s²2p⁶3s²                                           E)      1s²2s²2p⁶3s¹

            C)      1s²2s¹⁰                                                            

 

      46.  Which of the following is the correct ground state electron configuration for a phosphorus atom?

            A)      1s²2s²2p³                                                D)      1s²2s²2p⁶3s⁵

            B)      1s²2s²2p⁶3s²4p³                                      E)      1s²2s⁸3s⁵

            C)      1s²2s²2p⁶3s²3p³                                              

      47.  Which of the following is the correct ground state electron configuration for a sulfur atom?

            A)      1s²2s²2p⁴                                                D)      1s²2s²2p⁶3s⁶

            B)      1s²2s²2p⁶3s²4p⁴                                      E)      1s²2s⁸3s⁶

            C)      1s²2s²2p⁶3s²3p⁴                                              

 

      48.  Which of the following is the correct ground state electron configuration for a sodium atom?

            A)      1s²2s²2p⁷                                                D)      1s²2s²2p⁶3p¹

            B)      1s²2s²2p⁶3s²3p¹                                      E)      1s²2s²2p⁶

            C)      1s²2s²2p⁶3s¹                                                    

      49.  Which of the following is the correct ground state electron configuration for a silicon atom?

            A)      1s²2s²2p⁶3s⁴                                           D)      1s²2s²2p⁶3p⁴

            B)      1s²2s²2p⁶3s²3p²                                      E)      1s²2s²2p⁶3s²3p⁶

            C)      1s²2s²2p⁶3s²3p⁴                                              

 

      50.  The following orbital diagram corresponds to the element___________.

                   ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­¯  ­¯  ­_

                   1s    2s        2p        3s        3p

            A)  Br    B)  Cl    C)  P    D)  S    E)  Si

 

      51.  The following orbital diagram corresponds to the element___________.

                   ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­_ ­_ ­_

                   1s    2s        2p        3s        3p

            A)  Al    B)  Si    C)  P    D)  S    E)  Cl

 

      52.  The following orbital diagram corresponds to the element___________.

                   ­¯  ­¯  ­¯ ­¯ ­¯  ­¯  ­¯ ­_ ­_

                   1s    2s        2p        3s        3p

            A)  P    B)  Si    C)  S    D)  Se    E)  Cl

 

      53.  Elements that have five electrons in the highest-energy p sublevel in their ground state are called:

            A)      alkali metals.                                          D)      noble gases.

            B)      alkaline earth metals.                             E)      transition metals.

            C)      halogens.                                                        

 

      54.  Elements that have only one electron in the highest-energy s sublevel in their ground state are called:

            A)      alkali metals.                                          D)      noble gases.

            B)      alkaline earth metals.                             E)      transition metals.

            C)      halogens.                                                        

 

      55.  Elements that have six electrons in the highest-energy p sublevel in their ground state are called:

            A)      alkali metals.                                          D)      noble gases.

            B)      alkaline earth metals.                             E)      transition metals.

            C)      halogens.                                                        

      56.  Elements that have a partially filled d sublevel in their ground state are called:

            A)      alkali metals.                                          D)      noble gases.

            B)      alkaline earth metals.                             E)      transition metals.

            C)      halogens.                                                        

 

      57.  Elements that have a partially filled f sublevel in their ground state are called:

            A)      lanthanides or actinides.                        D)      noble gases.

            B)      alkaline earth metals.                             E)      transition metals.

            C)      halogens.                                                        

 

      58.  The element that has the abbreviated ground state electron configuration [Ne]3s²3p² is:

            A)  Al    B)  P    C)  Si    D)  Cl    E)  Ar

 

      59.  The element that has the abbreviated ground state electron configuration [Ne]3s²3p⁵ is:

            A)  S    B)  Ar    C)  Cl    D)  P    E)  Br

 

      60.  The element that has the abbreviated ground state electron configuration [Ar]4s²3d⁸ is:

            A)  Co    B)  Ni    C)  Kr    D)  Cu    E)  Ca

 

      61.  The element that has the abbreviated ground state electron configuration [Ar]4s²3d⁶ is:

            A)  Fe    B)  Co    C)  Se    D)  Mn

 

      62.  The element that has the abbreviated ground state electron configuration [Ar]4s²3d⁵ is:

            A)  Mn    B)  Cr    C)  V    D)  Fe    E)  no element—this configuration is incorrect.

 

      63.  What is the abbreviated ground state electron configuration for Sc?

            A)  [Ar]4s³    B)  [Ar]4s²4p¹    C)  [Ar]4s²4d¹    D)  [Ar]4s²3d¹    E)  [Ar]3d³

 

      64.  What is the abbreviated ground state electron configuration for Co?

            A)  [Ar]4s⁹    B)  [Ar]3d⁹    C)  [Ar]4s²4p⁷    D)  [Ar]4s²4p⁶4d¹    E)  [Ar]4s²3d⁷

 

      65.  The element that has two completely filled p sublevels, and four electrons in its other p sublevel is:

            A)  S    B)  O    C)  Se    D)  Si    E)  Ge

 

      66.  The element that has three completely filled s sublevels, one electron in its other s sublevel, and no d electrons is:

            A)  Na    B)  K    C)  Ca    D)  Mg    E)  C

      67.  The element that has four completely filled s sublevels, and three d electrons is:

            A)  V    B)  Cr    C)  Nb    D)  Ti    E)  Sc

      68.  Which of the following statements regarding valence electrons is incorrect?

            A)      The valence electrons are the electrons in the last-filled principal energy level.

            B)      For main-group elements, the number of valence electrons is equal to the number of electrons in the highest-energy s and p sublevels.

            C)      Except for helium, the Roman numeral group number corresponds to the number of valence electrons for the main-group elements.

            D)      The period number of an element equals the energy level of the valence electrons.

            E)      Elements in the p-block in the fourth period and below include their d electrons as part of their valence electron count.

 

      69.  Which of the following statements regarding valence electrons is incorrect?

            A)      Main-group elements in the same group have the same number of valence electrons.

            B)      The group numbers of the main-group elements are the sum of the number of s and p valence electrons.

            C)      The elements in the s-block can have up to two valence electrons.

            D)      An element in Group IVA will have six valence electrons.

            E)      The electron configuration for nitrogen is 1s²2s²2p³, so it has five valence electrons.

 

      70.  The valence level and the number of valence electrons, respectively, for calcium

             are:

            A)  4 and 2    B)  2 and 4    C)  4 and 4    D)  3 and 2    E)  2 and 2

 

      71.  The valence level and the number of valence electrons, respectively, for arsenic are:

            A)  3 and 3    B)  3 and 5    C)  4 and 3    D)  4 and 5    E)  4 and 2

 

      72.  The valence level and the number of valence electrons, respectively, for bromine are:

            A)  3 and 5    B)  3 and 7    C)  4 and 5    D)  4 and 7    E)  5 and 5

 

      73.  The valence level and the number of valence electrons, respectively, for phosphorus are:

            A)  2 and 3    B)  2 and 5    C)  3 and 3    D)  3 and 5    E)  3 and 6

 

      74.  The valence level and the number of valence electrons, respectively, for chlorine are:

            A)  2 and 5    B)  2 and 7    C)  3 and 5    D)  3 and 7    E)  3 and 6

      75.  What is the ground state electron configuration for the oxide ion?

            A)  1s²2s²2p²    B)  1s²2s²2p⁴    C)  1s²2s²2p⁶    D)  1s²2p⁶    E)  1s²2p⁸

 

      76.  What is the ground state electron configuration for the calcium ion, Ca²⁺?

            A)      1s²2s²2p⁶3s²3p⁶                                      D)      1s²2s²2p⁶3s²3p⁶4s²3d²

            B)      1s²2s²2p⁶3s²3p⁶3d²                                E)      1s²2s²2p⁶3s²3p⁶3d⁴

            C)      1s²2s²2p⁶3s²3p⁶4s²                                          

 

      77.  Some elements have electron configurations that deviate from normal electron filling rules.  Which element has the ground-state electron configuration [Kr]4d¹⁰?

            A)  Ni    B)  Pd    C)  Cd    D)  Zn    E)  Xe

 

      78.  Some elements have electron configurations that deviate from normal electron filling rules.  Which element has the ground-state electron configuration [Ar]4s¹3d¹⁰?

            A)  Ni    B)  Ag    C)  Cd    D)  Sn    E)  Cu

 

      79.  The electron configuration 1s²2s²2p⁶ applies to all of the following species except:

            A)  Ne    B)  F^-    C)  O^2-    D)  Na⁺    E)  Ca²⁺

 

      80.  The electron configuration 1s²2s²2p⁶3s²3p⁶ applies to all of the following species except:

            A)  Cl^-    B)  Ar    C)  Ca²⁺    D)  Na⁺    E)  K⁺

 

      81.  The electron configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶applies to all of the following species except:

            A)  Br^-    B)  Kr    C)  Sr²⁺    D)  Rb⁺    E)  K⁺

      82.  The abbreviated electron configuration [Kr] applies to all of the following species except:

            A)  Br^-    B)  As^3-    C)  Se^2-    D)  Sr²⁺    E)  Rb^-

      83.  The abbreviated electron configuration [Ne] applies to all of the following species except:

            A)  Cl^-    B)  N^3-    C)  O^2-    D)  Mg²⁺    E)  F?

 

      84.  The abbreviated electron configuration [Ar] applies to all of the following species except:

            A)  Cl^-    B)  P^3-    C)  O^2-    D)  Ca²⁺    E)  K⁺

 

      85.  Rank the following elements in order of increasing ionization energy:  P, F, Cs, Mg

            A)      Cs < Mg < F < P                                   D)      P < Mg < F < Cs

            B)      Cs < F < Mg < P                                   E)      Cs < Mg < P < F

            C)      F < P < Mg < Cs                                            

 

      86.  Rank the following elements in order of increasing ionization energy:  Al, Ba, O, C

            A)      Al < Ba < O < C                                   D)      O < C < Al < Ba

            B)      Ba < Al < O < C                                   E)      C < O < Al < Ba

            C)      Ba < Al < C < O                                            

 

      87.  Rank the following elements in order of increasing ionization energy:  Ge, Rb, S, Ne

            A)      Ge < Rb < Ne < S                                 D)      Rb < Ge < S < Ne

            B)      Rb < S < Ne < Ge                                 E)      Rb < Ge < Ne < S

            C)      S < Ne < Ge < Rb                                          

 

      88.  Rank the following elements in order of increasing ionization energy:  Sr, He, Si, F

            A)      Sr < Si < He < F                                    D)      Si < F <He < Sr

            B)      F < Si <He < Sr                                     E)      He < F < Sr < Si

            C)      Sr < Si <F < He                                              

 

      89.  Rank the following elements in order of increasing atomic size:  Sr, He, Si, F

            A)      F < He < Sr < Si                                    D)      Sr < Si < F < He

            B)      F < Sr < Si < He                                    E)      Si < Sr < F < He

            C)      He < F < Si < Sr                                             

 

      90.  Rank the following elements in order of increasing atomic size:  Ge, Rb, Ne, S

            A)      Ge < Rb < Ne < S                                 D)      Ne < S < Ge < Rb

            B)      Rb < S < Ne < Ge                                 E)      Rb <Ge < Ne < S

            C)      S < Ne < Ge < Rb                                          

 

      91.  Rank the following elements in order of increasing atomic size:  P, F, Cs, Mg

            A)      Cs < Mg < F < P                                   D)      P < Mg < F < Cs

            B)      Cs < F < Mg < P                                   E)      Cs < Mg < P < F

            C)      F < P < Mg < Cs                                            

      92.  Rank the following elements in order of increasing atomic size:  Al, Ba, O, C

            A)      Al < Ba < O < C                                   D)      O < C < Al < Ba

            B)      Ba < Al < O < C                                   E)      C < O < Al < Ba

            C)      Ba < Al < C < O                                            

 

      93.  Select the pair that has the larger atom or ion listed first.

            A)  Al³⁺, Al    B)  O, O^2-    C)  K⁺, Ca²⁺    D)  N, N^3-    E)  O^2-, Cl^-

      94.  Select the pair that has the larger atom or ion listed first.

            A)  Ca²⁺, Ca    B)  Cl, Cl^-    C)  Rb⁺, Sr²⁺    D)  Br^-, Se^2-    E)  Br, Br^-

      95.  Select the pair that has the larger atom or ion listed first.

            A)  P, P^3-    B)  Na⁺, Na    C)  S, S^2-    D)  Br^-, Kr    E)  Mg²⁺, Mg

 

      96.  Select the pair that has the larger atom or ion listed first.

            A)  S, S^2-    B)  Cl, Cl^-    C)  F^-, Ne    D)  P, P^3-    E)  Br^-, Se^2-

 

      97.  Which ion is expected to be the largest?

            A)  O^2–    B)  Mg²⁺    C)  Na⁺    D)  F^–    E)  All these ions have the same size.

 

      98.  Which ion is expected to be the largest?

             A)  Ca²⁺    B)  S^2–    C)  K⁺    D)  Cl^–    E)  All these ions have the same size.

 

      99.  The formula of the compound that would be formed when calcium and fluorine react is:

            A)  CaF    B)  Ca₂F    C)  CaF₂    D)  F₂Ca    E)  FCa

 

    100.  The formula of the compound that would be formed when magnesium and fluorine react is:

            A)  MgF    B)  Mg₂F    C)  MgF₂    D)  F₂Mg    E)  FMg

 

    101.  Wavelength is inversely proportional to frequency.

 

    102.  Wavelength is inversely proportional to energy.

 

    103.  Frequency is directly proportional to wavelength.

 

    104.  The type of radiation with wavelengths just slightly longer than red light is infrared.

 

    105.  The type of radiation with wavelengths just slightly shorter than violet is superviolet.

 

    106.  The color of visible light with the lowest energy is red.

 

    107.  The color of visible light with the longest wavelength is violet.

 

    108.  The color of visible light with the highest frequency is red.

 

    109.  Colored light from a heated ionic compound produces a continuous spectrum.

 

    110.  Since neon and argon are both noble gases, they produce the same spectrum.

 

    111.  In the Bohr model of the hydrogen atom, an electron can exist between orbits.

 

    112.  In the Bohr model of the hydrogen atom, when an electron absorbs energy, it moves into a higher energy orbit.

 

    113.  When an electron moves directly from the n = 3 to the n = 1 orbit, it emits two photons.

 

    114.  There are three orbitals in the 2p sublevel.

 

    115.  The maximum number of electrons in the 2nd principal energy level is 8.

 

    116.  The maximum number of electrons in the 3rd principal energy level is 28.

 

    117.  There is one unpaired electron in a phosphorus atom.

    118.  The alkaline earth elements have one valence electron.

 

    119.  Sodium has a higher ionization energy than cesium because its valence electron is closer to the nucleus.

 

    120.  A fluorine atom is larger than a carbon atom because it has more protons and more electrons.

 

    121.  The green light in the hydrogen spectrum has a wavelength of 434.1 nm.  What is the photon energy of this light?

 

    122.  Write the electron configuration and orbital diagram for the element chlorine.

    123.  Write the electron configuration and orbital diagram for the element phosphorus.

 

    124.  Explain what is wrong with the given electron configuration for bromine, and correct it:  1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p⁶

 

    125.  Explain what is wrong with the given electron configuration for selenium and correct it:  1s²2s²2p⁶3s²3p⁶4s²4d¹⁰4p²

 

    126.  Identify [Ne]3s²3p²   by its abbreviated electron configuration.

    127.  Identify [Ar]4s²3d⁸   by its abbreviated electron configuration.

 

    128.  Identify [Kr]5s²4d¹⁰5p³   by its abbreviated electron configuration.

 

    129.  Identify [Ne]3s²3p⁴    by its abbreviated electron configuration.

 

    130.  Identify [Ar]4s²3d⁶   by its abbreviated electron configuration.

 

    131.  Identify [Kr]5s²4d¹⁰5p¹ abbreviated electron configuration.

 

    132.  Explain why the number of valence electrons for a main-group element is equal to its Roman numeral group number.

 

    133.  Use electron configurations to explain why more energy is required to remove one electron from a fluorine atom than from a chlorine atom.

 

    134.  Use electron configurations to explain why more energy is required to remove one electron from a sodium atom than from a potassium atom.