Review: Electrons in Atoms
Name_______________________________
Date________ Block____
1. What is meant by an “excited electron?”
2. Explain how an electron may become excited?
3. What is meant by the term quantized energy levels?
4. The modern model of atomic structure states that electrons are in probability regions around
the nucleus. What does this mean?
Each principal energy level of the electron cloud is assigned a certain value.
5. List the first six (6) principal energy levels from the lowest energy level to the highest energy
level:
Each principal energy level is divided into sublevels. Each sublevel contains one or more
orbitals in which electrons travel.
6. The lowest principal energy level has how many sublevels ______
What is this sublevel called? _______
7. The second principal energy level has how many sublevels? ______
What are these sublevels called? _________ and ___________
8. The third principal energy level has how many sublevels? ________
What are these sublevels called? __________, ____________, and __________
9. The fourth principal energy level has how many sublevels? _________
What are these sublevels called? _________, _________, __________, and _________
10. State the Aufbau principle:
11. State the Pauli exclusion principle:
12. State Hund’s Rule:
13. What is the maximum number of electrons each s sublevel can contain?
14. What is the maximum number of electrons each p sublevel can contain?
15. What is the maximum number of electrons each d sublevel can contain? __________
16. What is the maximum number of electrons each f sublevel can contain? __________
17. How many orbitals are in each s sublevel? _______
18. How many orbitals are in each p sublevel? _______
19. How many orbitals are in each d sublevel? _______
20. How many orbitals are in each f sublevel? _______
21. List seven different forms of electromagnetic radiation included in the electromagnetic
spectrum:
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22. Define the term wavelength:
23. Define the term frequency:
24. What is meant by the term bright line spectrum of an element?
25. What is a photon?
26. What is meant by the ground state of an electron?
27. What is meant by the term “excited electron?”
28. What must occur for an electron to become excited?
29. What is usually emitted as an excited electron returns to its ground state?
30. Which electrons in an electron cloud are referred to as being the valence electrons?
31. Atoms of hydrogen, lithium, sodium, and potassium all have how many valence
electrons? ______
32. Atoms of beryllium, magnesium, and calcium all have how many valence electrons? _____
33. Atoms of boron and aluminum have how many valence electrons? ____
34. Atoms of carbon and silicon have how many valence electrons? ____
35. Atoms of nitrogen and phosphorus have how many valence electrons? ____
36. Atoms of oxygen and sulfur have how many valence electrons? ______
37. Atoms of fluorine and chlorine have how many valence electrons? _____
38. Atoms of neon and argon have how many valence electrons? _____
A general rule is that neutral atoms of all elements in the same column (called a group or
family) on the periodic table have the same number of valence electrons.
Using the general rule above, how many valence electrons does each neutral atom of the
following elements have?
39. strontium _____
43. bromine _______
40. barium _____
44. iodine _____
41. lead ____
45. cesium _____
42. tin ____
46. polonium _____
Using the shorthand notation, write the complete electron configuration for each of the
following elements. The configurations for hydrogen, helium are given below. The shorthand
configuration for lithium has been done as an example.
Examples: H: 1s1
He: 1s2
Li: [He]2 s1
47. Be: ________
50. O: ____________
53. Na: _____________
48. B: __________
51. F: ____________
54. Mg: _____________
49. N: ___________
52. Fe: ___________
55. Al: ______________
56. What is the importance of the valence electrons?