Name:______________________________________________________Pd:_______Date:_________________
Chapter 9: Electrons in Atoms and the Periodic Table – Study Guide
*Do not forget about the extra resources available to help you study and prepare for this test!
 Textbook pages 285 – 323
 Mastering Chemistry Study Area: http://www.pearsonmylabandmastering.com/northamerica/
 Miss Marnik’s Website: http://www.northallegheny.org/Page/16665
 Labs, problem packets, and homework assignments
Section 1 – Light and Quantized Energy: (text pages 285-293)
Need to be able to:
 Compare the wave and particle natures of light.
 Define a quantum of energy, and explain how it is related to an energy change of matter.
 Contrast continuous electromagnetic spectra and atomic emission spectra.
Practice Problems:
Use the words from the box to fill in the blanks:
1. amplitude
energy
frequency
light
speed
wave
wavelength
Electromagnetic radiation is a kind of ______________________________ that behaves like a(n)
______________________________ as it travels through space. ______________________________
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
______________________________. The shortest distance between equivalent points on a
continuous wave is called a(n) ______________________________. The height of a wave from the
origin to a crest or from the origin to a trough is the ______________________________.
______________________________ is the number of waves that pass a given point in one second.
2. List the types of electromagnetic radiation in order from lowest energy to highest energy.
3. Which type of electromagnetic radiation has the longest wavelength?
4. Which type of electromagnetic radiation has the highest frequency?
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5. Which color in the visible spectrum has the least amount of energy?
6. Which color in the visible spectrum has the most amount of energy?
7. A(n) __________________ is the minimum amount of energy that can be lost or gained by an atom.
a. valence electron
c. quantum
b. electron
d. photon
8. The ________________ is the phenomenon in which electrons are emitted from a metal’s surgace
when a light of a certain frequency shines on it.
a. quantum
c. wave
b. photon effect
d. photoelectric effect
For each statement below, write true or false:
9. _______________ Like the visible spectrum, an atomic emission spectrum is a continuous range of
colors.
10. _______________ Each element has a unique atomic emission spectrum.
11. _______________ A flame test can be used to identify the presence of certain atoms in a compound.
12. _______________ Atomic emission spectra can be explained by the wave model of light.
13. _______________ The neon atoms in a neon sign emit their characteristic color of light as they absorb
energy and jump to higher energy levels.
Section 2 – Classifying Reactions: (text pages 294-298)
Need to be able to:
 Compare the Bohr and quantum mechanical models of the atom.
 Explain the impact of de Broglie’s wave particle duality and the Heisenberg uncertainty principle on
the current view of electrons in atoms.
 Identify the relationships among a hydrogen atom’s energy levels, sublevels, and atomic orbitals.
Practice Problems
Use the words in the box to fill in the blanks below:
atomic emission spectrum electron
frequencies
higher
lower
energy levels
ground state
14. The lowest allowable energy state of an atom is called its _________________________.
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15. Bohr’s model of the atom predicted the _____________________ of the lines in hydrogen’s atomic
emission spectrum.
16. According to Bohr’s atomic model, the smaller an electron’s orbit, the _____________________ the
atom’s energy level.
17. According to Bohr’s atomic model, the larger an electron’s orbit, the _____________________ the
atom’s energy level.
18. Bohr proposed that when energy is added to a hydrogen atom, its __________________________
moves to a higher-energy orbit.
19. 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.
20. Bohr’s atomic model failed to explain the _____________________ of elements other than hydrogen.
For each item in Column A, write the letter of the matching item in Column B.
Column A
Column B
21. _______States that it is impossible to know both the
velocity and the position of a particle at the same
time.
a) Heisenberg uncertainty principle
22. _______A three-dimensional region around the
nucleus representing the probability of finding an
electron.
c) Quantum mechanical model
b) Schrödinger wave equation
d) Atomic orbital
23. _______Originally applied to the hydrogen atom, it
led to the quantum mechanical model of the atom.
24. _______The modern model of the atom that treats
electrons as waves.
25. How do the Bohr model and the quantum mechanical model of the atom differ in how they describe
electrons?
Circle the word the makes the statement correct:
26. Each orbital may contain at most (two, four) electrons.
27. All s orbitals are (spherically shaped, dumbbell shaped).
28. There are (three, five) equal energy p orbitals.
29. Hydrogen’s principal energy level 2 consists of (2s and 3s, 2s and 2p) orbitals.
30. Hydrogen’s principal energy level 3 consists of (nine, three) orbitals.
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31. Sketch the 1s and 2p orbitals. How do the 2s and 3p orbitals differ from the 1s and 2p orbitals?
32. Which electron, on average, is closer to the nucleus: an electron in a 2s orbital or an electron in a 3s
orbital?
33. According to the quantum-mechanical model for the hydrogen atom, which electron transition
produces light with longer wavelength: 2p to 1s or 3p to 1s?
34. What is the maximum number of electrons that can occupy each of the following shells?
a. n=1
c. n=3
b. n=2
d. n=4
Section 3 – Electron Configurations: (text pages 298-305)
Need to be able to:
 Apply the Pauli exclusion principle, the aufbau principle, and Hund's rule to write electron
configurations using orbital diagrams and electron configuration notation.
Practice Problems:
Aufbau Principle
electron configuration
ground-state configuration
Hund’s rule
lowest
Pauli exclusion principle
spins
stable
35. The arrangement of electrons in an atom is called the atom’s __________________________.
Electrons in an atom tend to assume the arrangement that gives the atom the
_________________________ possible energy. This arrangement of electrons is the most
_________________________ arrangement and is called the atom’s _______________________.
Three rules define how electrons can be arranged in an atom’s orbitals. The
__________________________ states that each electron occupies the lowest energy orbital available.
The _________________________ states that a maximum of two electrons may occupy a single
atomic orbital, but only if the electrons have opposite _______________________.
____________________________ states that single electrons with the same spin must occupy each
equal-energy orbital before additional electrons with opposite spins occupy the same orbitals.
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36. Write full orbital diagrams and indicate the number of unpaired electrons for each element:
a. He
d. N3-
b. B
e. Li
c. N
f.
Li+
37. Write the full electron configuration for each element:
a. Sr
b. Ge
c. Li
d. Zn
e. K+
f.
Ca2+
38. Write the noble gas configuration for each element:
a. Ga
b. As
c. Pb
d. Cr
e. Ff.
Al3+
39. Identify the neutral element with each of the following electron configurations:
a. [Ne]3s23p5
b. [Ar]4s23d104p1
c. [Xe]6s2
d. [Kr]5s24d105p3
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Section 4 – Valence Electrons: (text pages 305-307)
Need to be able to:
 Define valence electrons, and draw electron-dot structures representing an atom's valence electrons.
Practice Problems:
40. Indicate the number of valence electrons looking at the full electron configurations of the following
elements:
a. 1s22s22p63s23p64s23d104p2
c. 1s22s22p63s23p64s23d104p65s2
b. 1s22s22p63s23p5
d. 1s22s22p63s23p64s23d104p6
41. How many valence electrons are in the following elements:
a. Sb
b. N
c. B
d. K
c. Be
d. Se
42. Draw the electron dot structures of the following elements:
a. Ba
b. Al
Section 5 – Periodic Trends: (text pages 307-312)
Need to be able to:
 Identify and understand periodic trends such as atomic size, ionization energy, and metallic character.
Practice Problems:
43. Choose the element with the higher ionization energy from each pair:
a. As or Bi
c. S or I
b. As or Br
d. S or Sb
44. Arrange the elements in order of increasing ionization energy: Te, Pb, Cl, S, Sn
45. Choose the larger element from each pair:
a. Al or In
b. Si or N
c. P or Pb
d. C or F
46. Arrange these elements in order of increasing atomic size: Ca, Rb, S, Si, Ge, F
47. Which is larger, K or K+? Explain why. Which is larger Cl or Cl-? Explain why.
48. Choose the more metallic element from each pair:
a. Sr or Sb
c. Cl or O
b. As or Bi
d. S or As
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Name ________________________________________
Date ________________
Class _________________
9
Chemistry: Matter and Change
7
Copyright © Glencoe/McGraw-Hill, a division of The McGraw-Hill Companies, Inc.
Study Guide