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Blast from the Past III – Quantum Numbers and Electron Configuration Practice!
1. When an electron in a hydrogen atom moves from a higher to a lower energy state, the energy difference is
emitted as a quantum of ________.
2. Define the four quantum numbers (n, l, ml, ms) explain what information is given by each..
3. Orbitals of the same energy are said to be ________________.
4. The space occupied by one pair of electrons is called a(n) __________.
5. What is the formula for calculating the maximum number of electrons that can occupy any energy level in an
atom?
6. Complete the following table:
Energy level Number of sublevels Number of orbitals Maximum number of electrons
1
2
3
4
7. What is paramagnetic and diamagnetic?
8. Complete the following table
Sublevel Number of orbitals Maximum number of electrons
s
p
d
f
9. Write electron configurations, orbital diagrams, and lewis dot diagrams for the following atoms:
a. carbon
b. gold c. iron
d. lead
e. sodium
Write true if the statement is correct, or write in the blank a correction that will make the statement correct.
10. If two electrons occupy the same orbital, they must have opposite spins.
11. The principal quantum number describes the size of the orbital in an atom.
12. The shape of a d orbital is a clover-leaf.
13. Four quantum numbers are required to describe completely an electron in an atom.
14. A degenerate set of p orbitals is able to hold a maximum of eight electrons
Assign quantum numbers to the following elements:
15. O
16. Ca
17. Zr
Which element could the following set of quantum numbers belong to?
18. n = 4 l = 1 ml = 0 ms = -1/2
19. n = 5 l = 0 ml = 0 ms = +1/2
20. n = 3 l = 2 ml = 0 ms = -1/2
21. Also be able to tell whether an atom is excited, ground or impossible and why – based upon the given electron
configuration or orbital diagram.
22. Extend the table below by showing the permitted values for each of the quantum numbers in the fourth
energy
level (refer to your tree diagram)
n l ml ms Total capacity
4
23. What is the maximum number of electrons that can occupy the 6th energy level?
24. Complete the following table:
Sublevel s p d f
l value
rd
25. How many sublevels are there in the 3 energy level?
26. How many electrons can occupy any single orbital
27. Complete the following table for the sublevels represented by the following quantum numbers
n
2
4
4 5
l
0 2
3
Sublevel designation
3d 4p
5s
28. When n = 5, what are the possible values for l?
29. When l=2, what are the possible values for ml?
30. Which of the following show the correct order of filling?
a. 1s2s2p
d. 1s2s2p3s3p4s
b. 1s2s2p3s3p
e. 1s2s2p3p3d4s
c. 1s2s3s
f. 1s2s2p3s3p4s4p
31. Write the name of the element represented by each of the following configurations:
a. 1s22s22p5
c. 1s22s22p63s23p64s23d104p1
2 2
6 2
2 2
b. 1s 2s 2p 3s
d. 1s 2s 2p63s23p4
32. Write the electron configuration for each of the following elements
a. aluminum
d. carbon
b. iron
e. barium
c. cadmium
f. hafnium
33. Write the electron configuration for each of the following elements:
a. lithium
c. beryllium
e. boron
g. carbon
b. nitrogen
d. oxygen
f. fluorine
h. neon
34. Draw orbital diagrams for each of the elements in problem 12.
35. Draw Lewis electron dot diagrams for the elements in problem 12.
36. Heisenberg stated that, at the same time, it was impossible to know what two things about the electron?
37. How many quantum numbers are there?
38. What letter denotes the quantum number for the principle energy level?
39. What four letters are used to represent the sublevels within a principle energy level?
40. What is the maximum number of electrons that may occupy one p orbital?
41. Who stated that no two electrons in the same atom could have the same set of four quantum numbers?
42. The Lewis electron dot diagram is used to represent only which electrons in an atom?
43. What is the periodic table used to predict in this unit?
44. How many sublevels are possible in the third energy level?
45. How many orbitals are there in an f sublevel?
46. What is the maximum number of electrons that can occupy a d sublevel?
47. Which subelevel can contain a maximum of three pairs of electrons?
48. What must be true about the spins of two electrons occupying the same orbital?
49. Write the electron configuration for each of the following elements:
a. lithium
d. mercury
b. radium
e. tin
c. sodium
f. krypton
50. Draw the orbital diagram for each of the following elements
a. titanium
c. aluminum
b. sodium
d. phosphorus
51. Draw the Lewis dot diagrams for the elements listed in problems 14 and 15.
Define the following in your own words…
*DeBroglie’s equation
*Aufbau Principle
*Heisenberg uncertainty principal
*Hund's Rule
*Pauli Exclusion principal
*Shielding