Chapter 5 Review Sheet
Name ____________________________________
A. electrons enter orbitals of lowest energy first
B. a range of colors seen when light passes through a prism
C. lines of colored light obtained by passing the light emitted by an element
through a prism
D. the region around an atomic nucleus where electrons are likely to be moving
E. the SI unit of frequency
F. the number of wave cycles to pass a given point per unit of time
G. a region in space where there is a high probability of finding an electron
H. the amount of energy required to move an electron from one energy level to
the next higher one
I. the height of a wave from the origin to the crest
J. the distance between crests of waves
K. 6.6262 x 10-34 J s
L. It is impossible to know both the velocity and the position of a particle at the
same time.
M. predicts that all matter exhibits wavelike motions
N. the lowest energy level
O. a process in which electrons are ejected by metals when light shines on them
P. light quantum
__E_ 1. hertz
__H_ 2. quantum of energy
__B _ 3. spectrum
__D_ 4. energy level
__G_ 5. atomic orbital
__I__ 6. amplitude
__J__ 7. wavelength
__C__ 8. atomic emission spectrum
__A__ 9. Aufbau principle
__F__ 10. frequency
__N__ 11. ground state
__P _ 12. photon
__L__ 13. Heisenberg uncertainty principle
__K__ 14. Planck's constant
__M__ 15. de Broglie's equation
Answer the following questions or solve the following problems in the space provided.
16. For each group of sublevels, circle the one that fills last as electrons are added?
a. 3p 2p 1s 2s 3s
b. 4p 3p 2p 4s 4d 5s
c. 3d 4s 3p 3s 2s
17. What is the maximum number of electrons in the:
a. 1s orbital = 2
b. 3d orbital = 10
c. 4p orbital =6
18. Write the electron configuration for the potassium atom. 1s22s22p63s23p64s1
19. Write the electron configuration for the antimony (Sb) atom. 1s22s22p63s23p64s23d104p65s24d105p3
20. Write the electron configuration for the magnesium atom. 1s22s22p63s2
21. Write the electron configuration for the molybdenum atom. 1s22s22p63s23p64s23d104p65s14d5
22. What is the element with the electron configuration: 1s2 2s2 2p6 3s2 3p6 3d7 4s2 Co ( count e-)
23. What is the frequency of radiation that has a wavelength of 4.7 x 10 -5 cm ? 6.38 x 1014Hz
24. Calculate the wavelength of a photon of blue light whose frequency is 6.3 x 10 14 s-1 .4.8 x 10 -7m
25. Find the wavelength of each of these transitions in the hydrogen atom.
a) E = 2.04 x 10-18 J 9.7 x 10-8m
b) E = 1.63 x 10-18 J 1.22 x 10-7m
26. An inexpensive laser that is available to the public emits light that has a wavelength of 670 nm. What is frequency of the
radiation?
4.5 x 10 14Hz
True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
Answers at the end of this section.
_____ 27. Electrons must have a certain minimum amount of energy called a quantum in order to move from one energy level to the
next higher energy level.
_____ 28. The electron probability clouds for atomic orbitals are spherical in shape.
_____ 29. The maximum number of electrons that can occupy the fourth principal energy level of an atom is 32.
_____ 30. The higher the energy level occupied by an electron the more energetic it is.
_____ 31. The principal quantum number equals the number of sublevels within that principal energy level.
_____ 32. The orbitals of a principal energy level are lower in energy than the orbitals in the next higher principal energy level.
_____ 33. The configuration 3d44s2 is more stable than the configuration 3d54s1.
_____ 34. As many as four electrons can occupy the same orbital.
_____ 35. The Pauli exclusion principle states that an atomic orbital may describe at most two electrons.
_____ 36. The electron configuration for potassium is 1s22s22p63s23p64s1.
_____ 37. The electron configuration for copper is 1s22s22p63s23p64s23d9.
_____ 38. The speed of light is a constant that can be obtained by dividing the frequency of light by its wavelength.
_____ 39. The amplitude of a wave is the distance between the crests.
_____ 40. The energy of a body can change only in small discrete units.
_____ 41. The position and velocity of an electron in an atom can be determined with great certainty.
_____42. The photoelectric effect will occur no matter what frequency of light strikes a metal.
27. A, 28. S, 29. A, 30. A, 31. A, 32. A, 33. N, 34. N, 35. A, 36. A, 37. N, 38. N, 39. N, 40. A, 41. N, 42. N
Electron Configuration
PART A – ORBITAL DIAGRAMS & LONGHAND ELECTRON CONFIGURATION
Use the patterns within the periodic table to draw orbital diagrams and write longhand electron configurations for the
following atoms.
Symbol
Orbital Diagram and
Lewis Dot Structure
Longhand Electron Configuration
I can’t get the dots drawn
# e-
1s22s22p63s2
1.
Mg
12
Mg
1s22s22p63s23p3
2.
P
15
P
1s22s22p63s23p64s23d3
3.
V
23
V
1s22s22p63s23p64s23d104p2
4.
Ge
32
Ge
PART B – SHORTHAND ELECTRON CONFIGURATION
Use the patterns within the periodic table to write the shorthand electron configurations for the following elements.
# e-
Symbol
5.
6.
7.
8.
Lewis Dot Structure
Shorthand Electron Configuration
20
[Ar] 4s2
82
[Xe] 6s25d104f146p2
9
[He]2s22p5
46
[Kr]5s24d8
Ca
Pb
F
Pd
Stability & Electron Configuration
PART C – STABILITY
1. Write the shorthand electron configuration for copper.
Symbol
# e-
Cu
29
Shorthand Electron Configuration
[Ar]4s13d10
[Ar]4s13d5
24
Cr
2. Explain why copper and chromium does not follow the expected pattern.
Half filled orbitals are more stable.
Use the concept of full shell stability to predict the ions that will form from the following atoms. Then, name the
isoelectronic noble gas and give the shorthand electron configuration for the ion (not the original atom).
Atom
3.
4.
5.
6.
Noble
Gas
# e-
Ion
Symbol
Br-
Kr
36
[Ar]4s23d10 4p6
Mg2+
Ne
10
[He]2s22p6
S2-
Ar
18
[Ne]3s23p6
Al3+
Ne
10
[He]2s22p6
Br
Mg
S
Al
Shorthand Electron Configuration of Ion