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| STANDARDS |
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| PRIORITY STANDARDS: |
Strand II, Standard I, Benchmark I
7. Explain how electrons determine the properties of
substances by:
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interactions between atoms through transferring or sharing
valence electrons
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ionic and covalent bonds
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the ability of carbon to form a diverse array of organic
structures.
8. Make predictions about elements using the periodic table
(number of valence electrons, metallic character, reactivity, conductivity,
type of bond between elements).
Specifications:
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properties of bonding based upon location on the periodic
table include orbital diagrams and electron configuration of representative
elements, Lewis Structures of single center molecules and polyatomic ions,
polarity.
Strand II, Standard I, Benchmark I
2. Identify, measure, and use a variety of physical and
chemical properties (electrical conductivity, chemical reactivity).
4. Describe trends in properties (ionization energy or
reactivity as a function of location on the periodic table).
Specifications:
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ionization energy, electronegativity, atomic radii, metals,
and nonmetals
Strand II, Standard I, Benchmark II
10. Explain how wavelengths of electromagnetic radiation
can be used to identify atoms, molecules, and the composition of stars.
Specifications:
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Qualitative understanding of atomic emissions spectra
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| OBJECTIVES |
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OBJECTIVE (SWBAT):
Understand that electrons occur in distinct energy levels.
Explain the underlying cause for observed periodic trends.
Given the name or symbol of one of the first 18 elements
in the periodic table, write the electron level arrangement.
Identify how changes in energy levels changes the orbital
of an electron and define photon as a discrete packet of energy.
Use the principles of quantum mechanics to describe the
behavior and arrangement of electrons around the nucleus.
Classify elements based on electron configuration.
Describe trends among the elements for atomic size.
Describe periodic trends for electronegativity.
Use the quantum numbers of the electrons to understand
how electron orbitals are filled and to write the electron configuration
of an element.
Identify how changes in energy levels changes the orbital
of an electron and define photon as a discrete packet of energy.
Define valence electrons and use the electron arrangement
of elements to explain periodic trends such as atomic size and ionization
energy.
Given the group number of an element, write electron-dot
symbols for that element.
Describe the relationship between the wavelength and
frequency of light.
Identify the source of atomic emission spectra.
Explain how the frequencies of emitted light are related
to changes in electron energies.
Distinguish between quantum mechanics and classical mechanics
BIG IDEAS:
Electrons and their arrangement around the nucleus determine
the chemical properties of an element.
Electrons exist only in certain, specific energy levels
around the nucleus.
Photons are discrete energy packets that exist as both
a particle and a wave.
Quantum mechanics describes the behaviors of the electron
and the photon.
Electrons are arranged around the atoms of specific elements
in particular configurations.
Predictions about number of valence electrons, reactivity,
and atomic size can be made using the periodic table.
The wavelength and frequency of light are inversely proportional
to each other.
When atoms absorb energy, electrons move into higher
energy levels. These electrons then lose energy by emitting photons
of light when they return to lower energy levels.
The light emitted by an electron moving from a higher
to a lower energy level has a frequency directly proportional to the energy
change of an electron.
Classical mechanics adequately describes the motion of
bodies much larger than atoms, while quantum mechanics describes the motions
of subatomic particles and atoms as waves.
ESSENTIAL QUESTIONS (SWBATA):
What determines the chemical properties of an element?
What is the underlying cause for observed periodic trends?
How are electrons arranged around the nucleus of the
atom?
What are photons?
How do scientists describe the behavior of subatomic
particles such as the electron or the photon?
How can predictions be made regarding atomic behavior
be made?
What are the trends among elements for atomic size?
What are the trends among the elements for electronegativity?
How are the wavelength and frequency of light related?
What causes atomic emission spectra?
How are the frequencies of light an atom emits related
to changes of electron energies?
How does quantum mechanics differ from classical mechanics? |
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| VOCABULARY |
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| KEY VOCABULARY: |
energy level, electron level arrangement, principal quantum
number (n), photons
orbital, azimuthal quantum number (l), s orbital, p orbital,
d orbital, f orbital, electron shell, subshell, magnetic quantum number
(ml), spin quantum number, electron spin, valence electrons, group numbers,
electron-dot symbol, ionization energy, electron configuration, aufbau
principle, Pauli exclusion principle, Hund’s rule, atomic radius, electronegativity,
amplitude, wavelength, frequency, hertz, electromagnetic radiation, spectrum,
atomic emission spectrum, ground state, Heisenberg Uncertainty Principle |
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