Orbitals and Electron Configurations
Completion
Complete
each statement.
Use each of the terms below just once to
complete the passage.
amplitude 
energy 
frequency 
hertz 
Light 
wave 
wavelength 
speed 
Electromagnetic radiation is a kind of (1)
____________________ that behaves like a(n) (2) ____________________as
it travels through space. (3)____________________is one type
of electromagnetic radiation. Other examples include X
rays, radio waves, and microwaves.
All waves can be characterized by their
wavelength, amplitude, frequency, and (4)____________________.
The shortest distance between equivalent points on a continuous wave is called a(n) (5) ____________________. The height of a wave from the
origin to a crest or from the origin to a trough is the (6)
____________________. (7) ____________________ is the number of waves that pass
a given point in one second. The SI unit for frequency is the (8)
____________________, which is equivalent to one wave per second.
Use each of the terms below to complete
the statements.
Atomic emission spectrum 
electron 
frequencies 
ground state 
Higher 
energy levels 
lower 

9. The lowest allowable
energy state of an atom is called its ____________________.
10. Bohr’s model of the atom
predicted the ____________________ of the lines in hydrogen’s atomic emission
spectrum.
11. According to Bohr’s
atomic model, the smaller an electron’s orbit, the ____________________ the
atom’s energy level.
12. According to Bohr’s atomic
model, the larger an electron’s orbit, the ____________________ the atom’s
energy level.
13. Bohr proposed that when
energy is added to a hydrogen atom, its ____________________ moves to a
higherenergy orbit.
14. According to Bohr’s
atomic model, the hydrogen atom emits a photon corresponding to the difference
between the ____________________ associated with the two orbits it transitions
between.
15. Bohr’s atomic model
failed to explain the ____________________ of elements other than hydrogen.
Choose the term in parentheses that
correctly completes the statement.
16. Atomic orbitals
(do, do not) have an exactly defined size. ____________________
17. Each orbital may contain at most (two, four)
electrons. ____________________
18. All s orbitals are
(spherically shaped, dumbbell shaped). ____________________
19. A principal energy has (n, n^{2})
energy sublevels. ____________________
20. The maximum number of
(electrons, orbitals) related to each principal
energy level equals 2n^{2}. ____________________
21. There are (three, five) equal energy p orbitals. ____________________
22. Hydrogen’s principal energy level 2 consists
of (2s and 3s, 2s and 2p) orbitals.
____________________
23. Hydrogen’s principal energy level 3 consists
of (nine, three) orbitals. ____________________
Use each of the terms below just once to
complete the passage.
Aufbau principle 
electron configuration 
groundstate electron configuration 
Hund’s rule 
lowest 
Pauli exclusion principle 
Spins 
stable 
The arrangement of electrons in an atom is
called the atom’s (1)____________________. Electrons
in an atom tend to assume the arrangement that gives the atom the (2)____________________ possible energy. This arrangement of
electrons is the most (3____________________ arrangement and is called the
atom’s (4)____________________.
Three rules define how electrons can be
arranged in an atom’s orbitals. The (5)____________________ states that each electron occupies the
lowest energy orbital available. The (6)____________________
states that a maximum of two electrons may occupy a single atomic orbital, but
only if the electrons have opposite (7)____________________.
(8)____________________ states that single electrons
with the same spin must occupy each equalenergy orbital before additional
electrons with opposite spins occupy the same orbitals.
Matching
Match the terms below with the correct
definitions.
a. 
Heisenberg uncertainty principle 
c. 
quantum mechanical model of the atom 
b. 
Schrödinger wave equation 
d. 
atomic orbital 
32. The modern model of the atom that treats
electrons as waves
33. States that it is impossible to know both the
velocity and the position of a particle at the same time
34. A threedimensional region around the nucleus
representing the probability of finding an electron
35. Originally applied to the hydrogen atom, it
led to the quantum mechanical model of the atom
Short
Answer
Use the figure to answer the following
questions.
36. Which letter(s) represent one wavelength?
37. Which letter(s) represent the amplitude?
38. If twice the length of A
passes a stationary point every second, what is the frequency of the wave?
39. If you looked closely, could you see the
wavelength of a fastmoving car? Explain your answer.
40. Using de Broglie’s
equation, _{} which would have the larger wavelength, a
slowmoving proton or a fastmoving golf ball? Explain your answer.
41. How do the Bohr model
and the quantum mechanical model of the atom differ in how they describe
electrons?
42. Complete the following
table.
Element 
Atomic Number 
Orbitals 1s 2s _{} _{} _{} 
Electron Configuration 
9. Helium 


1s² 
10. 
7 


11. Neon 



43. What is germanium’s atomic number? How many
electrons does germanium have?
44. What is noblegas notation, and why is it
used to write electron configurations?
45. Write the groundstate electron configuration
of a germanium atom, using noblegas notation.