Download Chapter 5 Practice Section 5-1 Discuss the placement (if any) of

Chapter 5 Practice
Section 5-1
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Discuss the placement (if any) of electrons in the following models of the atom:
a. Dalton ____________________________________________________________________
b. Thompson _________________________________________________________________
c. Rutherford _________________________________________________________________
d. Bohr ______________________________________________________________________
e. Quantum Mechanical ________________________________________________________
__________________________________________________________________________
Which is a larger difference in energy?
a. n = 1 to n = 2
b. n = 3 to n = 4
If a quantum of energy is added to an atom, an electron ________________________________
________________________________________.
An ________________ is where you will most probably find an electron.
How many orbitals are in the following sublevels?
a. 4 p sublevel
b. 3d sublevel
How do the px, py, and pz orbitals differ from each other? How are they similar?
7. What is the correlation between the energy level and the number of sublevels in that energy
level?
8. From the given information, determine the pattern and fill in the missing values.
Energy level
# of sublevels
# of orbitals
# of electrons
n=1
1
1
2
n=2
2
4
8
n=3
3
9
18
n=4
?
?
?
9. Give the formula in terms of “n” for:
a. # of orbitals
b. # of electrons
Section 5-2
Match the name of the rule to the rule itself.
______10. aufbau principle
a. When electrons occupy orbitals of equal energy
______11. Pauli exclusion principle
separately with parallel spin before pairing.
______12. Hund’s rule
b. Electrons enter orbitals of lowest energy first.
c. Every electron has a unique set of quantum numbers.
Draw the orbital diagram for the following elements:
13. Magnesium
14. Oxygen
15. Argon
16. Scandium
17. Phosphorous
Write out the electron configuration for the following elements:
18. Potassium
19. Cobalt
20. Silicon
21. Lithium
22. Selenium
23. Bismuth
24. Vanadium
25. Sulfur
26. Mercury
Identify the following elements:
27. 1s22s22p63s23p64s2
28. 1s22s22p63s23p2
29. 1s22s22p63s23p64s23d3
30. 1s22s22p63s23p64s23d104p5
31. 1s22s22p6
32. 1s22s22p63s23p64s23d104p65s24d105p66s24f145d6
33. What elements are exceptions to the filling rule (Aufbau principle)
For # 34-37, write the abbreviated electron configuration (kernel notation).
34. Iodine
35. Radium
36. Aluminum
37. Gallium
38. How do the 2p orbitals differ from each other?
39. How do the 2p and 3p orbitals differ from each other?
Quantum Number Extension: NOT IN THE TEXTBOOK!
40. Which of the following sets of quantum numbers is allowed? Underline the parts that makes
the others incorrect.
a. n = 3, l = 2, ml = 2
b. n = 4, l = 3, ml = 4
c. n = 0, l = 0, ml = 0
d. n = 2, l = -1, ml = 1
41. How many electrons in an atom can have the designation:
a. 1s b. 2p c. 3px d. 5f e 2dxy
42. How many orbitals in an atom can have the designation:
a. 5p b. 4d
c. n = 5 d. n = 4
43. What is the maximum number of electrons in an atom that can have these quantum numbers:
a. n = 4
_____
b. n = 5, ml = +1
_____
c. n = 5, ms = + ½
_____
d. n = 3, l = 2
_____
e. n = 2, l =1
_____
44. What is the maximum number of electrons in an atom that can have these
quantum numbers:
a. n = 0, l = 0, ml = 0
_____
b. n = 2, l = 1, ml = -1, ms = -½
_____
c. n = 3
_____
d. n = 3, l = 2
_____
e. n = 1, l = 0, ml = 0
_____
45. Give a possible set of variables for the four quantum numbers for all the electrons in an atom of
carbon.
46. What are the possible values of ml for
a. l = 0
_________ b. l = 3 __________ c. n = 3
___________
47. Give the number of orbitals in
a. n = 3 ________ b. a 4d sublevel _______ c. an f sublevel _______
48. Given the following sets of quantum numbers, indicate those that could not occur
a. 1, 1, 0, +½
b. 2, 1, 0, +½
c. 2, 0, 1, -½
d. 2, 1, 0, 0
49. Assign a set of four quantum numbers to
a. the 4s electrons in Ca
b. all the 3d electrons in Cr
c. all the 3p electrons in Cd
50. Identify the specific element that has the following electron configuration:
a. 1s22s22p4
b. [Ne]3s23p5
c. [Ar]4s1
d. [Ar]4s13d5
5-3 Practice
The speed of light c = 2.998 x 108 m/s
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What is the wavelength of radiation with a frequency of 2.3 x 1014 Hz?
What is the frequency of radiation with a wavelength of 1.8 x 10-9 m?
Rank in order of increasing energy: Purple light, x-rays, Microwaves
Rank the above in order of increasing frequency.
Rank the above in order of increasing wavelength.
Which of the following is in ground state?
a. 1s22s22p63s13p1
b. 1s22s22p63s23p64s1
Which electron jump would result in energy being emitted?
a. 3 → 4 b. 2 → 5 c. 2 → 1 d. 5 → 6
Which electron jump would absorb the most energy?
a. 5→6 b. 6 →7 c. 3→ 4 d. 1 → 2
Which electron jump would release the most energy?
a. 3→2 b. 4→2 c. 5→2 d. 7→6
Albert Einstein described light as having a particle nature as well as a wave nature. He called the
light particles ________________.
De Broglie thought that if light could have a particle nature, then particles could have
________________ nature.
A neon light is really composed of a variety of colors of light. How are they produced?