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Chemistry Study Guide
Chapter 4 & 5 Study Guide
TEST: Monday 11/8/10
4.1 Defining the Atom
Define the following term:
- atom
1. What was Democritus’ atomic philosophy?
2. What was Dalton’s atomic theory? (4 parts)
3. What is the radius of most atoms?
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4.2 Structure of the Nuclear Atom
Define the following terms:
- electrons
- cathode ray
Particle
- protons
Location Relative Relative
in atom
charge
mass
Electron
- neutrons
Proton
- nucleus
Neutron
1. Describe/sketch J. J. Thomson’s experiment. What did he discover? Why was
his model called the “plum pudding” model?
2. How does an electron’s mass compare to the mass of a proton?
3. What did Chadwick discover?
4. Describe/sketch Rutherford’s gold-foil experiment. What did he discover?
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4.3 Distinguishing among Atoms
Define the following terms:
- atomic number
- mass number
- isotopes
- atomic mass unit (amu)
- atomic mass
- periodic table
- period
- group
1. What determines that one element will be different from another element?
2. How is the atomic number of an element related to the number of protons in that
element?
3. How is the number of protons of an element related to the number of electrons in
that element?
4. How would one find the mass number of an element?
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5. Fill in the chart below:
Atomic
symbol
Atomic
number
Protons
Neutrons
B
Electrons
Atomic
mass
6
11
24
31
37
39
29
89
35
43
100
207
Pb
102
89
70
225
Mo
53
81
100
206
159
No
Yb
261
172
106
159
6. Two isotopes of chlorine are chlorine-35 and chlorine-37. How many protons,
neutrons, and electrons does each isotope have given that chlorine has an atomic
number of 17?
7. What is the atomic mass of boron if the isotope with a mass of 10.012 amu has a
relative abundance of 19.9% and the isotope with a mass of 11.01 amu has a
relative abundance of 80.1%?
8. What is the atomic mass of chorine if the isotope with a mass of 34.97 amu has a
relative abundance of 75.77% and the isotope with a mass of 36.97 amu has a
relative abundance of 24.23%?
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5.1 Models of the Atom
Define the following terms:
- energy levels
- quantum
- quantum mechanical model
- atomic orbital
- s orbital
- p orbital
- d orbital
- f orbital
1. How did Bohr’s model differ from Rutherford’s model of the atom?
2. How can electrons in an atom move from one energy level to another?
3. How is the quantum mechanical model different from Bohr’s model?
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4. Fill in the chart below:
Scientist
Experiment
Description
Dalton
Thomson
Rutherford
Bohr
Electron
Cloud/
Quantum
Mechanical
Model
(Schrodinger)
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Diagram
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Chemistry Study Guide
5.2 Electron Arrangement in Atoms
Define the following terms:
- electron configurations
- Aufbau principle
- Pauli’s exclusion principle ↑↓
- Hund’s rule ↑↓ ↑
↑.
Practice electron configurations using the 3 rules. Review the handout on electron
configurations and class notes.
Reminders:
*** The s orbital set contains 1 orbital, so it can hold a total of 2 electrons
*** The p orbital set contains 3 orbitals, so it can hold a total of 6 electrons.
*** The d orbital set contains 5 orbitals, so it can hold 10 electrons.
*** The f orbital set contains 7 orbitals, so it can hold 14 electrons.
*** for d orbitals, subtract 1 from the row number
*** for f orbitals, subtract 2 from the row number
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5.3 Physics and the Quantum Mechanical Model
Define the following terms:
- amplitude
- wavelength
- frequency
- hertz
- electromagnetic radiation
- spectrum
- atomic emission spectrum
- ground state
- photons
- Heisenberg uncertainty principle
1. Label the amplitude and the wavelength:
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2. Which wave is low
frequency? Which is high
frequency?
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3. What is the formula for finding the wavelength or frequency of a wave?
4. What is the symbol and unit for wavelength?
5. What is the symbol and unit for frequency?
6. What is c, the speed of light constant? What is its unit?
7. How are wavelength and frequency of a light wave related?
8. A red light has a wavelength of 7.28 x 10-7 m.
What is the frequency of the light?
9. A purple light has a frequency of 7.42 x 1014 Hz.
What is its wavelength?
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10. What happens when electrons change energy levels?
11. What can the emission spectrum of an element be likened to?
12. What is the formula for finding the quantum of energy?
13. What is the unit for energy?
14. What is the unit for h?
15. What are the units for frequency?
16. Find the energy for red light (problem #9) and for purple light (problem #10)
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