Test your skills on the following problems.

Example #1: Which of the following transitions (in a hydrogen atom) represent __ emission__ of the

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

Example #2: Which of the following transitions represent __ absorption__ of a photon with the

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

Example #3: Provide the n, l and ml value for each of the given orbitals.

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

l = ? l = ?

m_{l} = ? m_{l} = ?

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

l = ? l = ?

m_{l} = ? m_{l} = ?

Example #4: Which statement about the four quantum numbers is false?

a) n = principal quantum number, n = 1 to infinity

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.

Example #5: 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

Example #6: How many electrons can have the following quantum sets?

a) n = 4, m_{L} = -1

b) n = 5, m_{L} = 0 , m_{S} = – 1/2

c) n = 9, l = 4, m_{S} = – 1/2

d) n = 2, m_{S} = 1/2

Example #7: For n = 2, what are the possible sublevels?

a) 0

b) 0, 1

c) 0, 1, 2

d) 0, 1,2, 3

Example #8: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 2, l = 1, m_{l }= 0

b) n = 3, l = 2, m_{l} = –1

c) n = 4, l = 0, m_{l} = +1

d) n = 1, l = 1, m_{l} = 0

Example #9: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 3, l = 2, m_{l} = 0, m_{s} = – 1/2

b) n = 3, l = 1, m_{l} = – 3, m_{s} = 1

c) n = 4, l = 0, m_{l} = 0, m_{s} = – 1/2

d) n = 4, l = 2, m_{l} = – 3, m_{s} = 1/2

Example #10: 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

Example #11: Give the electron configuration for the following element and its ion. For the ion, state if it is paramagnetic or diamagnetic:

Ag and Ag^{+}

Example #12: Give the electron configuration for the following element and its ion. For the ion, state if it is paramagnetic or diamagnetic:

Cl and Cl^{+}

Example #13: Which of the following represents an “excited” state?

a) Cl: 1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}

b) Be: 1s^{2}2s^{2}

c) Na: 1s^{2}2s^{2}2p^{6}3p^{1}

d) N: 1s^{2}2s^{2}2p^{3}

Example #14: Give the set of four quantum numbers that represent the indicated electron in the following element:

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

Example #15: Give the set of four quantum numbers that represent the indicated electron in the following element:

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

Example #16: Give the set of four quantum numbers that represent the indicated electron in the following element:

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

Example #17: Give the set of four quantum numbers that represent the indicated electron in the following element:

a. Mo^{3+} (38th electron) n = , l = , m_{l} = , m_{s} =

Example #18: For a multi-electron atom, arrange the electron subshells of the following listing in order of increasing energy:

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