End of Chapter Problems

Test your skills on the following problems. 

Emission vs. Absorption

Example: Which of the following transitions (in a hydrogen atom) represent emission of the smallest or shortest wavelength?

a. n = 4 to n = 2

b. n = 3 to n= 4

c. n = 1 to n = 2

d. n = 7 to n = 5

e. n = 2 to n = 5

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Example: Which of the following transitions represent absorption of a photon with the highest frequency?

a. n = 3 to n = 1

b. n = 2 to n = 4

c. n = 1 to n =2

d. n = 6 to n = 3

e. n = 1 to n = 3

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Quantum Numbers

Example: Provide the n, l and ml value for each of the given orbitals.

a) 7s      n =                               b) 5d     n =

              l  =                                             l =

             ml =                                            ml =

 

c) 2p     n =                                d) 4f      n =

             l  =                                             l  =

             ml =                                           ml =

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Example: Which statement about the four quantum numbers is false?

a. n = principal quantum number,            n = 1 to ∞

b. l = azimuthal quantum number,           l = 0,1,2, . . ., (n+1)

c. mL = magnetic quantum number, mL = (-l), . . .,0,. . ., (+l)

d. ms = spin quantum number,    ms = + 1/2  or − 1/2

e. The first three quantum numbers deal with the atomic orbitals except for the ms quantum number, which deals with the electrons in the atomic orbitals.

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Example: Each of the following sets of quantum numbers gives information on a specific orbital. Find the error in each.

a. n = 4, l = 0 , ml = 1, ms = – 1/2

b. n = 5, l = 2 , ml = - 1, ms = 1

c. n = 7, l = 7, ml = - 5, ms = – 1/2

d. n = 0, l = 5, ml = - 3, ms = 1/2

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Example: How many electrons can have the following quantum sets?

a) n = 4, mL = -1 

b) n = 5, mL = 0 , mS = – 1/2

c) n = 9, l = 4, mS = – 1/2

d) n = 2, mS = 1/2

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Example: For n = 2, what are the possible sublevels?

a) 0

b) 0, 1

c) 0, 1, 2

d) 0, 1,2, 3

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Quantum Numbers & Atomic Shape

Example: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 2, l = 1, ml = 0

b) n = 3, l = 2, ml = –1

c) n = 4, l = 0, ml = +1

d) n = 1, l = 1, ml = 0

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Example: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 3, l = 2, ml = 0, ms = – 1/2

b) n = 3, l = 1, ml = – 3, ms = 1

c) n = 4, l = 0, ml = 0, ms = – 1/2

d) n = 4, l = 2, ml = – 3, ms = 1/2

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Example: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 3, l = 3, ml = 0, ms = 1/2

b) n = 1, l = 3, ml = – 3, ms = 1

c) n = 7, l = 3, ml = – 4, ms = – 1/2

d) n = 6, l = 3, ml = – 3, ms = – 1/2

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Paramagnetism vs. Diamagnetism

Example: Give the electron configuration for the following element and its ion. For the ion, state if it is paramagnetic or diamagnetic:

a. Ag

      Ag+

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Example: Give the electron configuration for the following element and its ion. For the ion, state if it is paramagnetic or diamagnetic:

a. Cl

     Cl+

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Electron Configurations

Example: Which of the following represents an “excited” state?

a) Cl: 1s22s22p63s23p5

b) Be: 1s22s2

c) Na: 1s22s22p63p1

d) N: 1s22s22p3

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Example: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Br (33rd electron)      n = ,        l = ,        ml = ,        ms =

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Example: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Ca (19th electron)         n = ,        l = ,          ml = ,             ms =

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Example: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Cu (27th electron)        n = ,         l = ,        ml = ,            ms =

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Example: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Mo3+ (38th electron)       n = ,         l = ,       ml = ,         ms =

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Example: For a multi-electron atom, arrange the electron subshells of the following listing in order of increasing energy:

6s, 4f, 2p, 5d.

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