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Reading Guide Chapter 11
Read pages 323-343 and answer the following questions in complete sentences.
1. Define electromagnetic radiation and list three examples.
 one of the ways in which energy travels through space
 travels as a wave at the speed of light
 light from sun, microwave oven, X-rays, etc.
2. Waves have three properties, list and define the three listed in your book.
 wavelength – λ, distance between two peaks or two troughs in
a wave (meters)
 frequency –ν, how many waves pass a given point per second
(s-1)
 speed – c, how fast a given peak moves through space
3. Which color of light has the longest wavelength and which has the shortest
wavelength?
Red has the longest wavelength, violet has the shortest
wavelength.
4. Define the following terms photon, wave-particle theory, excited state, and ground
state.
Photons are tiny packets of energy and particles of electromagnetic
radiation.
Wave – particle theory states that light acts as a wave and as
particles of energy.
Excited state is an atom with excess energy.
Ground state is the lowest possible energy state.
5. How does an atom move from an excited state to the ground state?
An atom moves from the excited state to the ground state by
emitting a photon.
6. The energy of a photon corresponds to the difference in energy between
the excited state and the ground state
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7. Define the term quantized and explain how it relates to the photons and colors of light
emitted by an atom.
Quantized means that only certain values of energy are allowed.
An atom can only emit certain photons, which correspond to
certain energy levels and specific colors of light. Every atom has
quantized energy levels.
8. Describe the Bohr Model of an atom. (Include a picture)
The Bohr Model of an Atom suggests that electrons move around
a positive nucleus in circular orbits, like the earth orbits the sun.
9. Why is the Bohr Model incorrect?
The Bohr model is incorrect because it can only be applied to the
hydrogen atom and more importantly because electrons do not
orbit the nucleus.
10. Describe the Wave Mechanical Model of the Atom. What information about the
electron can you not learn from this model?
The wave mechanical model of an atom is based on mathematical
analysis.
In this model, electrons occupy a space called an orbital, which is
where the electron is most likely to be.
Gives no information about when the electron occupies a certain
point in space or how it moves.
11. Describe an orbital.
An orbital is a probability map of finding an electron.
12. Define principal energy level, sublevel and orbital. Explain the relationship between
the three terms.
Principal energy levels are the discrete energy levels of an atom
designated by principal quantum numbers. Sublevels exist within
each principle energy level; each sublevel has a slightly different
energy. An orbital is the region within a sublevel where electrons
can be found.
13. Which sublevel has the most energy?
s, p, d, f
energy
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14. What is the maximum number of electrons an orbital can hold? What must be true of
the electron’s spins? What principle is this?
An orbital can hold a maximum of two electrons that are spinning
in opposite directions. This is the Pauli Exclusion Principle.
15. What are the first three orbitals and their shapes?
s – sphere, diameter increases as principal energy level
increases
p – dumbbell, same size and shape within a principal energy
level
d – dumbbell with a doughnut around the middle
16. Explain an electron configuration.
An electron configuration is the arrangement of the electrons
among the various orbitals of an atom. It serves as an address –
to tell exactly where every electron is most likely to reside.
17. Define valence electrons and core electrons.
Valence electrons are electrons in the outermost (highest) principal
energy level of an atom, which are critical for bonding.
Core electrons are the inner electrons, which are not involved in
bonding.