1. Chapter 4 Electron Arrangement

2. Write the Bohr Model for Barium
2, 8, 18, 18, 8, 2

3. Write the Orbital Notation for Aluminum

4. Write the Electron Configuration for Bismuth
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p3

5. Write the Noble Gas Shorthand Notation for Tin.
[Kr] 5s2 4d10 5p2

6. Write the Lewis Dot Structure for Sulfur

7. Draw the Bohr Model of Bromine
2, 8, 17, 7

8. Write the electron configuration for Iron
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d7

9. Write the Noble Gas Shorthand Notation for Vanadium
[Ar] 4s2 3d3

10. Write the Orbital Notation for Iridium

11. Write the Lewis Dot Structure for Silicon

12. Write the Noble Gas Shorthand Notation for Lead
[Xe] 6s2 4f14 5d10 6p2

13. Write the Electron Configuration for Polonium
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p4

14. Write the Lewis Dot Structure for Cs (Cesium)

15. Draw the Bohr Model for Zinc

16. Write the Orbital Notation for Oxygen

17. How are wavelength and frequency related?
They are inversely proportional.
As one increase the other decreases

18. The wavelength times the frequency.
For electromagnetic radiation, what does c (the speed of light) equal?
The wavelength times the frequency.

19. How is frequency related to the energy of a wave?
They are directly proportional. Waves with high frequency also possess high energy.

20. What is defined as the distance between corresponding points on adjacent waves?
Wavelength

21. How is frequency defined?
The number of waves that pass a given point over a specific period of time.

22. What units are used to measure frequency? Hertz (Hz) (waves/sec.)

23. What is “ground state” for an atom?
When the electrons in an atom occupy their lowest energy levels possible.

24. What is the “excited state” of an atom?
When the electrons in an atom have absorbed energy and moved up to higher energy levels.

25. Principle Quantum Number
What quantum number indicates the major shell or energy level of an electron?
Principle Quantum Number

26. What is defined as a region in an atom where there is a high probability of finding an electron?
ORBITAL

27. Angular Momentum Quantum Number
What quantum number denotes the shape or subshell in which the electron is located?
Angular Momentum Quantum Number

28. What is the shape of an “s” orbital
SPHERICAL

29. What is the shape of a “p” orbital?
Dumbbell or
Ellipsoid

30. What quantum number tells the axes in space of the electron?
Magnetic Quantum Number

31. What quantum number tells the direction of an electron’s spin?
Spin Quantum Number

32. What orbital shapes can be found in each of the first four energy levels?
1st Energy Level = s orbital
2nd Energy Level = s and p orbitals
3rd Energy Level = s, p, and d orbitals
4th Energy Level s, p, d, and f orbitals

33. What formula helps to determine the maximum number of electrons that can be contained per energy level?
2n2

34. How many orbitals are in the n = 4 shell? a. 4 b. 8 c. 12 d. 16

35. How many electrons in an atom could be described by the quantum numbers n = 3 and ml = -1? a b c d.18 4

36. Which of the following in not an acceptable set of quantum number for an electron in an atom?
a. n = 1, l = 0, m = 0, s = +½
b. n = 4, l = 3, m = -2, s = -½
c. n = -2, l = 1, m = -1, s = +½
d. n = 3, l = 1, m = 0, s = -½
n = -2

37. If electromagnetic radiation A has a lower frequency than electromagnetic radiation B, then compared to B, the wavelength of A is ______________
LONGER

38. How many quantum numbers are needed to describe the energy state of an electron in an atom?4

39. 1st Energy Level = 2 electrons 2nd Energy Level = 8 electrons
How many electrons are needed to fill each of the first four energy levels?
1st Energy Level = 2 electrons
2nd Energy Level = 8 electrons
3rd Energy Level = 18 electrons
4th Energy Level = 32 electrons

40. Red, Orange, Yellow, Green, Blue, Indigo, Violet
What are the colors of the visible spectrum from increasing wavelength to decreasing wavelength?
Red, Orange, Yellow, Green, Blue, Indigo, Violet

41. What requires that electrons enter each orbital one at a time and with identical spins before any pairing can occur?
Hund’s Rule

42. Pauli’s Exclusion Principle
What states that no two electrons in an atom can have exactly the same set of four quantum numbers?
Pauli’s Exclusion Principle

43. What is an octet?
An atom that has 8 outer shell electrons

44. Using the two equations, E = h and c =  , derive an equation using E in terms of h, c and . Then prove it.

45. c =  E = h V = C  E = h(C/ ) E C  h Kg * m2 s2 m____ s * m
Step 2: Plug in v for v
Step 1: Solve for V
V = C 
E = h(C/ ) E C  h
Step 1: Solve for V
Step 2: Plug in v for v
Kg * m2 s2
m____
s * m
= Kg * m2 * s * s2

46. The End!
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