1) Which of the following statements is correct for an electron that has the quantum numbers n = 4 and ml = -2? A

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1) Which of the following statements is correct for an electron that has the quantum numbers n = 4 and ml = -2?

A. the electron may be in a p orbital
B. the electron may be in a d orbital
C. the electron is in the second principal shell
D. the electron must have a spin quantum number ms = + ½

2) The set of quantum numbers, n = 4, l = 3, ml = 2

A. describes an electron in a 3p orbital
B. is not allowed
C. describes an electron in a 4d orbital
D. describes one of seven orbitals of a similar type

3) Which of the following statements is correct for an electron that has the quantum numbers n = 5 and ml = -4?

A. the electron may be in a f orbital
B. the electron must have a spin quantum number ms = -1/2

C. the electron may be in a p orbital
D. none of the above

4)Identify the subshell in which electrons with the quantum numbers n = 3, l = 2 may be found.
A. 3d
B. 4f
C. 4d
D. 3p

5)What type of orbital is occupied by an electron with the quantum numbers n = 4, l = 1. How many orbitals of this type are found in a multi-electron atom?

6) Identify the subshell in which electrons with the quantum numbers n = 6, l = 1 may be found.
A. 6p
B. 3d
C. 6f
D. 5p

7. Consider the sulfur atom. For how many electrons does this atom have n = 2 and l = 1?

8. Consider the argon atom. For how many electrons does this atom have ml = 1 and ms = + 1/2?

9. Consider the chlorine atom. For how many electrons does this atom have n = 3 and l = 0?

10. Identify the subshell in which electrons with the quantum number n = 5, l = 4 are found.

11. Give the corresponding atomic orbital designations for electrons with the following quantum numbers.

n
l
ml
ms

1)
3
2
0
-1/2

2)
5
3
-1
-1/2

3)
4
1
+1
-1/2

A. 3p,5d,3s
B. 2d,5f,4p
C. 2d,5d,4p
D. 3d,5f,4p
Give the corresponding atomic orbital designations for electrons with the following quantum numbers;

n
l
ml
ms

1)
2
1
0
-1/2

2)
5
3
-1
-1/2

3)
3
2
+1
-1/2

A. 2p,5f,3p
B. 2s,5d,3p
C. 2p,5d,3p
D. 2p,5f,3d

13. Which of the following sets of quantum numbers is not allowed?
A. n = 3, l = 1, ml = -1, ms = + ½

B. n = 2, l = l, ml = 0, ms = + ½

C. n = 3, l = 0, ml = 0, ms = + ½

D. n = 2, l = 2, ml = -1, ms = - ½

14. Which of the following sets of quantum numbers is not allowed?
A. n = 3, l = 1, ml = -1

B. n = 2, l = 0, ml = 0

C. n = 3, l = 2, ml = -3

D. n = 2, l = l, ml = 0

15. Which of the following sets of quantum numbers are not allowed for an electron in an atom?

n
l
ml
ms

1)
2
1
0
+1/2

2)
2
3
+1
-1/2

3)
3
2
-2
-1/2

4)
2
2
0
+1/2

5)
2
1
0
+1/2

A. 1, 3, 5
B. 2, 4
C. 2, 4, 5
D. 3, 4

16. Elements of a group in the periodic table _____________
A. have similar chemical properties.
B. are isotopes.
C. are also called a period.
D. have consecutive atomic numbers

17. A horizontal row in the periodic table containing a sequence of elements is a ____________
A. period
B. group
C. family
D. subgroup

18. What would be the atomic number of an element that might have one electron in the 6f subshell?
A. 109
B. 12
C. 127
D. 118

19. Which of the following electron configurations is correct for cobalt, (atomic number 27)?
A. [Ar]5s24d7

B. [Ar]4s23d7

C. [Ar]4s24d9

D. [Kr]4s23d7

20. Which of the following electron configurations is correct for sulfur, (atomic number 16)?
A. 1s22s22p63s43p2

B. 1s22s22p63p23p4

C. 1s22s22p63s23p2

D. 1s22s22p63s43p4

21. Which of the following electron configurations is correct for iron, (atomic number 26)?
A. [Kr]4s14d7

B. [Kr]4s13d6

C. [Ar]4s23d6

D. [Kr]4s23d6

22. Consider the chlorine atom. For how many electrons does this atom have n = 3 and l = 0?

23. Consider the argon atom. For how many electrons does this atom have ml = 1?
A. 0
B. 1
C. 2
D. 4

24. Which of the following elements has the smallest electron affinity?
A. F(9)
B. B(5)
C. N(7)
D. C(6)

25. Which of the following elements has the largest electron affinity?
A. N(7)
B. Na(11)
C. O(8)
D. F(9)