UNIT 4 - ELECTRONS
I. Energy and Electrons
A. Ground state vs. excited state
B. Transitions between ground state and
excited state
1. How energy is involved
2. Electromagnetic radiation
3. Photons - light as a wave
C. Determining energy of an electron
1. Planck
2. Calculations
- light as a particle
D. Spectroscopy
1. Absorption and emission
2. Bright line spectra
II. Electron Arrangement
A. Energy levels, sublevels, orbitals
B. Electron configurations
C. Noble
Gas Configurations
D. Highest Occupied Energy Level (HOEL)
E. Valence
Electrons
F. Orbital
notation
G. Electron dot diagrams
H. Exceptions to electron configuration rule
(Honors only)
I. Quantum numbers (Honors only)
North Carolina Essential Standards and Clarifying Objectives:
Chm. 1.1
Analyze the structure of atoms and ions.
1.1.2 Analyze an atom in terms of the location of
electrons.
Analyze
diagrams related to the Bohr model of the hydrogen atom in terms of allowed,
discrete energy levels in the emission spectrum.
Describe the
electron cloud of the atom in terms of a probability model.
Relate the
electron configurations of atoms to the Bohr and electron cloud models.
1.1.3 Explain the emission of electromagnetic
radiation in spectral form in terms of the Bohr model.
Understand
that energy exists in discrete units called quanta.
Describe the
concepts of excited and ground state of electrons in the atom:
1.
When an electron gains an amount of energy equivalent to the energy
difference, it moves from its ground state to a higher energy level.
2. When the electron moves to a lower energy
level, it releases an amount of energy equal to the
energy difference in these levels as
electromagnetic radiation (emissions spectrum).
Articulate
that this electromagnetic radiation is given off as photons.
Understand
the inverse relationship between wavelength and frequency, and the direct relationship
between energy and frequency.
Use the
Bohr Model for Hydrogen Atom and Electromagnetic Spectrum diagrams from the
Reference Tables to relate color, frequency, and wavelength of the light
emitted to the energy of the photon.
Explain that
Niels Bohr produced a model of the hydrogen atom based on experimental
observations. This model indicated that:
1. an
electron circles the nucleus only in fixed energy ranges called orbits;
2. an electron can neither gain or lose energy
inside this orbit, but could move up or down to another orbit;
3.
that the lowest energy orbit is closest to the nucleus.
Describe the
wave/particle duality of electrons.
Chm. 1.3 Understand the
physical and chemical properties of atoms based on their position on the
Periodic Table.
1.3.2 Infer the physical properties of an element
based on its position on the Periodic Table.
Write
electron configurations, including noble gas abbreviations. Included here are extended arrangements
showing electrons in orbitals.
Identify an
element based on its electron configuration.
Determine
the number of valence electrons from electron configurations.