C.P. Chemistry
Review Packet
Chapter 3: Study Guide
Electrons and Light (Section 3 Electron Configuration, pp. 90 – 99)

Explain the wave/particle duality of matter.

Describe an atomic emission spectra.

Solve light/ energy/ and wavelength equations (formulas will be given)

Identify the relationships among an atom’s energy levels, sublevels, and atomic orbitals.

Apply the Pauli exclusion principle, the Aufbau principle, and Hund’s rule to write electron
configurations using orbital diagrams and electron configuration notation.

Write noble gas shorthand electron configurations

Define valence electrons and draw electron-dot structures representing an atom’s
valence electrons.
C.P. Chemistry
Name:______________________
Electron and Light Review
Date: _______________________
Answer each of the following questions as completely as possible showing all work and
units.
1) Draw a wave. Carefully label wavelength, amplitude, crest and trough.
2) Explain the relationship between frequency and wavelength of light.
3) What is the relationship between the energy of an electron and its distance from the
nucleus?
4) What happens when an electron in an atom changes from a ground state to an excited
state?
5) What happens when an electron falls from an excited state back to the ground state?
6) What is meant by dual nature of light?
7) State the Aufbau Principle, Pauli Exclusion Principle, and Hund’s Rule
8) Which quantum number represents the main energy level of an electron?
9) What is wrong with the following statements?
The 2d sublevel has 5 orbitals.
The 3s sublevel has 3 orbitals.
10) Provide full electron configurations and full orbital diagrams for each of the
following elements.
a)
S
b) C
c)
Na
d) Ti
11) Provide noble gas electron configuration and noble gas orbital diagrams for each of
the following elements.
a)
F
b) Sr
c)
Nb
12) Write the number of valence electrons and the Lewis Dot diagram for each of the
following.
a) Helium
b) Aluminum
c)
d) C
potassium
e) oxygen
f) Kr
13) What is the wavelength of 3.5 * 10-9 Hz light? What is the color of that light?
14) What is the frequency of a photon having an energy of 5.27 * 10-23 J? (h = 6.626 *
10-34Js)
15) What is the energy of a photon if the wavelength is 2.3 * 10-7m? (hint: use both
equations)