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| Goal
I. Describe some of the experimental and theoretical developments leading
to the quantum mechanical model of the atom. |
Objectives: To meet the requirements of Goal
I, you must be able to:
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describe briefly
the sequence of experiments and analysis which led to the model for atomic
structure used by chemists;
-
define electromagnetic
radiation, wavelength, frequency, amplitude, cycle, node, photon;
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convert
among energy, wavelength and/or frequency of a photon;
-
describe the
electromagnetic radiation spectrum, including relative energies,
wavelengths and frequencies of its various "regions";
-
relate the
colors in the visible region of the spectrum to the energies of photons.
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| Goal II. Describe and apply
the features of the Bohr model of the hydrogen atom to atomic structure
and electronic spectra. |
Objectives: To meet the requirements of Goal
II, you must be able to:
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distinguish
between emission spectrum and absorption spectrum of an element;
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describe the Bohr
model of the hydrogen atom and how it was used to explain the atomic emission
spectrum of hydrogen;
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explain
the statement, " The energy of the hydrogen atom is quantized;"
- use
Equations 7.2, 7.3 and
7.4 to calculate the difference in energies of
any pair of principal quantum levels and relate this difference
to the wavelength (or frequency) of an associated spectral
line;
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explain why
Bohr's model of the hydrogen atom was abandoned in favor of the wave mechanical
model for atomic structure. [Top]
| Goal III. Using the wave
mechanical model, explain the fundamental concepts regarding electron arrangement
in atoms. |
Objectives: To meet the requirements of Goal
III, you must be able to:
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describe the interpretation
given to the wave function (y)
and of the square of a wave function (y²)
, in Schrödinger's wave mechanical model of the hydrogen atom;
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interpret
the quantum numbers
n,
l, ml;
which
appear in the mathematical solution to the Schrödinger equation describing
the behavior and energies of electrons in atoms;
-
state the
Heisenberg
Uncertainty Principle, and the Pauli Exclusion Principle and
explain their implications for determining the electronic structure of
an atom;
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explain the
following terms used in the wave mechanical model of the atom: orbital,
shell subshell, radial distribution function, boundary surface;
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interpret the
spin quantum number, ms,
and relate this quantum number to the Pauli Exclusion Principle;
- know and
be able to use the information in Table 7.2 including:
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the allowed combinations of quantum numbers for "shells"
n=1-4,
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the letter used to designate "subshells"
defined by the angular momentum quantum number "l";
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know
the boundary surface diagrams for s, p, and d type
orbitals;
-
determine the
number of orbitals in a shell or subshell, and determine the number
of electrons that can occupy a shell or a subshell in a many-electron atom.
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Unit 7 Assignments
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| Read: |
Text
Chapter 7, pp. 268-297 |
| Video
Programs: |
- Light and
Matter, Electromagnetic Radiation
- Aufbau Principle,
Wave Mechanical Model
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| Textbook
Assignments: |
Read
and Understand all "Sample Problems," "Follow
Up Problems" and select any 5 blue-colored problems at the
end of the chapters.
The
answers for the Follow Up Problems are at the end
of the chapter; the answers for the blue-colored
problems are in Appredix E. |
| Mandatory ChemSkill Builder Assignments to be submitted for grade (Scores of 80% or higher on each assigned HW section will receive full credit. ) |
Mandatory
assignments to be submitted for grade
Chapter 9, Sections
9.2, 9.6 (Light and Energy, quantum numbers)
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| Note:
Complete Solutions, including all units of measurement,
must be shown for all problems. |
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