Unit 4 Review
Section I - Problems (Given h = 6.626 x 10-34 J.s)
The speed of light, c, equals ____________________ m/s.
What is the frequency of a wave with a wavelength of 3.5 x 108
What is the energy of a photon with a frequency of 5.41 x 10-7
Substitute, rearrange, and write an equation that relates E, h, c, and l.
Section II - Electromagnetic
Label both ends of the spectrum with high/low frequency, high/low
energy, and long/short wavelength
radio waves microwaves infrared
light ROYGBIV ultraviolet light x-rays gamma rays
2. Which has a higher energy, gamma or x-rays?
Which has a shorter wavelength, radio or ultraviolet?
Which has a lower frequency, yellow or green light?
In the equation E = hn, energy and frequency are ____________________
6. In the equation c = ln, wavelength and frequency are __________________ proportional.
The symbol for wavelength is _____.
____________________ equals the number of waves that pass a point per
Electrons give off energy in the form of a ____________________ when
returning to the ground state.
Which scientist proposed the idea that electrons travel around the nucleus
in fixed paths?
11. When an electron moves from the ground state to the excited state, energy is ____________________.
12. Bohr chose the element ____________________ to prove his theory.
13. The dual wave-particle nature
of electrons describes how the electrons in atoms can behave as
____________________ and ____________________.
Section III - Electrons
1. What is an electron cloud?
2. Who proposed the uncertainty principle?
3. Who is credited with the idea that electrons are placed in the lowest energy level first?
4. What rule requires that
each of the "p" orbitals (at a particular
energy level) receive one electron before any
of the orbitals can have two electrons?
5. What is the maximum number of electrons in any orbital?
6. The principal quantum number, n, indicates the ____________________.
7. The maximum number of
electrons in an energy level can be determined by the equation ________________
That means the maximum number of electrons in the 3rd energy level is ____________________.
8. The number of sublevels in any energy level can be determined by ____________________.
9. The number of orbitals in an energy level can be determined by the
So, the 3rd energy level has _____ orbitals. (_____ is/are "s" orbitals, _____ is/are "p" orbitals, and _____
is/are "d" orbitals)
10. List the four sublevels according to increasing energy.
11. The "s" sublevel is shaped like a ____________________ and has _____ orbitals.
12. A "p" sublevel is shaped like a ____________________ and has _____ orbitals.
13. The "d" sublevel has _____ orbitals and the "f" sublevel has _____ orbitals.
Section IV - Electron configuration, noble gas configuration, valence electrons, orbital notations
1. What is the electron configuration for phosphorus?
2. How many total electrons are in a neutral atom of phosphorus?
3. Write the noble gas configuration for phosphorus.
4. What is the highest occupied energy level for phosphorus?
5. What is the atomic number of phosphorus?
6. Draw the orbital notation for phosphorus.
7. How many electrons are in the highest occupied energy level of phosphorus?
8. How many unpaired electrons does phosphorus have?
9. How many inner-shell electrons does phosphorus have?
10. In which orbitals are the inner-shell electrons located?
11. Draw the electron dot diagram for phosphorus.
Section V - Quantum numbers (Honors level only)
1. How many electrons can be described by the quantum numbers n = 3 and l = 1?
2. How many electrons in an atom can have the quantum numbers n = 2 and l = 3?
3. How many "d" orbitals have the value n = 3?
4. How many electrons in an atom have the quantum numbers n = 4 and l = 2?
5. Which of the following
sets of quantum numbers does NOT represent a possible set of quantum numbers
hydrogen atom? (There may be more than one correct answer.)
n l m s
(A) 4 8 -4 ; 1/2
(B) 6 5 -5 ; 1/2
(C) 3 2 2 1/2
(D) 6 0 1 1/2