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Atomic Theory Unit Study Guide
CP Chemistry
Spring 2012
Terms to Know
absorption spectrum
continuous spectrum
electromagnetic spectrum
emission spectrum
energy level
excitation
excited state
frequency
ground state
The “Big Idea”
I.
Our understanding of
the structure of matter
has changed and
continues to change as
new data contradicts
existing theories.
line spectrum
photon
relaxation
wavelength
Aufbau principle
angular momentum
quantum number
Hund's rule
magnetic quantum number
Pauli exclusion principle
principle quantum number
quantum theory
spin quantum number
Uncertainty Principle
wave mechanical theory
group
halogen
lanthanide
main group elements
noble gas
actinide
orbital
alkali metal
alkaline earth metal
period
transition metals
What you need to know about it.
1. Describe the major theories of the structure of matter from the ancient Greeks
through the present and name the principal theorist.
2. Arrange the major atomic models in chronological order, describe the evidence
that supported the model and explain why the model was modified or
abandoned.
3. Describe why Rutherford's metal foil experiments forced Dalton’s and
Thomson’s models of atomic structure to be replaced with a nuclear model of
the atom.
4. Describe the uses and limitations of the Bohr model, particularly as it related to
the quantization of electron energies.
5. Use examples from the history of the development of atomic theory to explain
how scientific theories are modified or replaced, and identify two or more
barriers to acceptance of new theories.
1. Describe the structure of the atom in terms of protons, neutrons, and electrons
and identify the charge and relative mass of each particle.
2. Use ZAX notation to determine number of protons, neutrons, and electrons and
identify the element from a periodic table.
II.
All neutral atoms of an
element have the same
number of electrons and
protons, but the number
of neutrons varies.
3. Write the ZAX notation of any isotope.
4. Calculate the average atomic mass of a naturally occurring element given the
relative abundance of each isotope.
5. Calculate the relative abundance of isotopes given the average atomic mass.
6. Write the balanced nuclear equations for the nuclear decay processes of α
particle production, β particle production, γ ray production, positron production
and electron capture.
7. Calculate the half-life of an isotope given the time it takes for the isotope to
decay, or the amount of the starting amount of an isotope remaining given the
half-life.
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Atomic Theory Unit Study Guide
The “Big Idea”
CP Chemistry
Spring 2012
What you need to know about it.
1. Write the equations that relate wavelength, frequency, amplitude, and velocity
of electromagnetic radiation.
2. Label regions of the electromagnetic spectrum as radio waves, infrared, visible,
ultraviolet, x-ray and gamma radiation and identify the frequency, wavelength
and energy of light for each region identified above.
3. Contrast the following pairs of terms
III.
Electromagnetic
radiation is the result of
energy transitions at the
atomic level.
a.
b.
c.
d.
e.
ground state vs. excited state
excitation vs. relaxation
absorption vs. emission
line spectra vs. and continuous spectra
absorption vs. emission spectra.
4. Calculate the energy of absorption and emission spectral lines of the hydrogen
atom, and identify the electron transitions that caused the lines.
5. Describe the concept of wave-particle duality, and relate the DeBroglie
wavelength of a wave or particle to its momentum.
6. Describe the photoelectric effect, including what changes in the effect result
from variation of the incident light frequency and intensity and how it provides
evidence for photons.
7. Calculate the energy of an emitted or absorbed photon from the initial and final
energy levels of a molecule or atom.
IV.
Each electron in an
atom has a unique
quantum number, which
describes its probable
position and energy.
1. Describe the nature and relationship of the principal (n), azimuthal (l), and
magnetic (ml) quantum numbers to solutions of the Schrödinger Wave
Equation, and identify which orbital properties are determined by each of these
numbers.
2. Name orbitals given its quantum numbers, or identify quantum numbers for
given orbital.
3. Sketch the relative shapes, sizes, and spatial orientations of s, p, and d orbitals
of the hydrogen atom.
4. Apply the concept of effective nuclear charge, Zeff, to describe the difference in
orbital energies between single and multi-electron systems.
5. Define the Pauli Exclusion Principle, the Aufbau Principle, and Hund’s Rule and
explain the accepted scientific rationale for each.
1. Apply the Aufbau principle to predict the ground state electronic configuration of
any element.
V.
The periodic table of
elements is organized
based on electron
structure.
2. Locate any unknown element on the periodic table based on its electron
configuration.
3. Identify alkali metals, alkaline earth metals, halogens, noble gases, main group
elements, transition metals, and lanthanides & actinides on a blank periodic
table.
4. Describe the electron configuration of elements that belong to each of the
groups identified above.
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