1. Give the values of the quantum numbers associated with the orbitals in the 2s subshell.
n ________________
l _______________________
ml (There may be more blanks than answers. Fill the anwer boxes from left to right and fill any remaining boxes with NA.)
______ ,_______ ,________ ,_______ ,___________ , ________ , ____________

2. What is the total number of orbitals associated with the principal quantum number n = 4?

3. Write the four quantum numbers for an electron in a 5p orbital. (Place the n value in the 1st box, the l value in the 2nd box, the ml value in the 3rd box, and the ms value in the 4th box per set. Put sets with positive ms values on the left. Enter your answers from least to greatest vertically, using fractions instead of decimals, and be sure to include the sign.)
ms = +
ms = -
ms = -

4. Calculate the total number of electrons that can be present in the principal level for which n = 5.

5. Write the ground-state electron configuration for calcium (Ca).

6. A d subshell has how many orbitals?

7. Any single orbital may contain a maximum of how many electrons?

8. Give the values of the quantum numbers associated with the following orbitals.
(a) 2p
ml = 1, 0, or −1 ml = only 1    ml = only 0
(b) 3s
ml = 0 ml = −1    ml = 1
(c) 5d
ml = 2, 1, 0, −1, or −2 ml = only 2    ml = only −2

9. Calculate the total number of electrons that can occupy the following orbitals.
(a) one s orbital
one, two,    three, or six
(b) three p orbitals
three, six,    nine, or twelve
(c) five d orbitals
five, nine,    ten, or fifteen
(d) seven f orbitals
six, seven,    twelve or fourteen

10. Determine the maximum number of electrons that can be found in each of the following subshells.
3s__________
5s______________
4s______________
5d______________
5p_________________

11. For each of the following pairs of hydrogen orbitals, indicate which is higher in energy.
(a) 1s, 2s
1s, 2s, or Both are equal.
(b) 2p, 3p
2p, 3p, or    Both are equal.
(c) 3dxy, 3dyz
3dxy, 3dyz or    Both are equal.
(d) 3s, 3d
3s, 3d, or Both are equal.
(e) 4f, 5s
4f ,5s, or Both are equal

12.
Which element has the following electron configuration 1s22s22p63s2?
Mg
Na
Al
Ne

13. Which element has the following electron configuration [Kr]5s24d105p3?
Sn
Bi
Pb
Sb

14. The element having atomic number (Z) = 35 and atomic mass number = 80, has how many valence electrons?
6
4
5
7

15. The third principal energy level (n = 3) can have which of the subshells?
s
s, p and d
s, p, d and f
s and p

16. A p subshell has how many orbitals?
2
5
4
3

17. In the following listing, select the set of quantum numbers that is NOT possible.
N l m1 mS
A. 3 0 1 -1/2
B. 4 3 -2 +1/2
C. 3 0 0 +1/2
D. 2 1 1 -1/2

D
C
A
B

18. To calculate the maximum number of electrons that can occupy an energy level as a function of the principal quantum number (n) use
2n2.
2n.
n + 1.
n2.

19. For n = 4 and l = 2, the notation for the subshell is
4d
4p
4s
4f

20. Subshell designations are based on the
principal quantum number (n).
magnetic quantum number (ml).
spin quantum number (ms).
angular momentum quantum number (l).

21. To determine the energy of an electron in the hydrogen atom, we would consider the
principal quantum number (n).
principal and angular momentum quantum numbers (n + l).
angular momentum quantum number (l).
principal and magnetic quantum numbers (n + ml).

22. Based on its electronic configuration an atom of manganese would have ____ unpaired electrons and would be expected to be__________.
0, diamagnetic
5, paramagnetic
3, paramagnetic
2, diamagnetic

23. Transition metal atoms or ions have partly filled
p subshells.
f subshells.
s subshells.
d subshells.

24. Rare earth or Lanthanide elements usually have partly filled
d subshells.
s subshells.
f subshells.
p subshells.

25. Within the periodic table, there are some elements whose ground state electronic configurations cannot be accurately predicted using the Aufbau principle; three notable exceptions are Cr, Mo and W. Select the correct ground state electronic configuration for Mo.
[Ar]4s24d4
[Kr]5s14d5
[Kr]5s24d6
[Kr]5s24d4

1. Give the values of the quantum numbers associated with the orbit...