Electrons in Atoms Unit 3
Essential Questions:
 How are electron configurations written and what are their purpose?
 How does the Bohr model account for the energy of electrons?
 Why do we need to understand valence electrons?
 How can we represent the symbol of an atom with the valence electrons?
 What are the relative energies and shapes of the sharp, principle, diffuse and
fundamental (SPDF) energy levels
 How do we explain the difference in colors of the flame test for various
elements?
 What are the characteristics of a wave?
 What is the relationship between frequency and wavelength of an EM wave?
 How can we use a spectroscope to determine the source of various light
samples?
Objectives:
 Compare the wave and particle models of light
 Know the parts and characteristics of a wave
 Predict the positions of electrons in an atom using the concepts of quantum
numbers and orbitals
 Define a quantum of energy and explain how it is related to an energy change
of matter
 Contrast continuous electromagnetic spectra and atomic emission spectra
 Compare the Bohr and quantum mechanical models of the atom
 Explain the impact of de Broglie’s wave particle duality and the Heisenberg
uncertainty principle on the modern view of electrons in atoms
 Identify the relationships among a hydrogen atom’s energy levels, sublevels
and atomic orbitals
 Apply the Pauli exclusion principle, the aufbau principle, and Hund’s rule to
write electron configurations using orbital diagrams and electron
configuration notation
 Define valence electrons and draw electron dot structures representing an
atom’s valence electrons
 Draw Bohr models for elements
 Compare the Bohr and Quantum Mechanical models of an atom
 Explain the significance of energy levels
 Distinguish between an atom’s ground state and excited state
Vocabulary
 amplitude
 Electromagnetic radiation
 Wavelength
 Frequency amplitude
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Electromagnetic spectrum
Quantum
Planck’s constant
Photoelectric effect
Photon
Atomic emission spectra
Ground state
De Broglie equation
Heisenberg uncertainty principle
Quantum mechanical model of the atom
Atomic orbital
Principle quantum number
Principle energy level
Energy sublevel
electron configuration
aufbau principle
Pauli exclusion principle
Hund’s rule
Valence electron
Electron dot structure
Text Ch. 5
Topics (In order):
 Electron configuration
o Aufbau principle
o Pauli exclusion principle
o Hund’s rule
o Orbital diagrams and electron configuration notations
 Wave nature of light
 Particle nature of light
o Quantum concept
o Photoelectric effectr
 Atomic emission spectra
 Bohr model
 Quantum mechanical model
 Heisenberg uncertainty principle
 Atomic orbitals
Day 1
Pre-reading assignment - done after Atomic structure unit test and finished for
homework 5.3 Electron configuration
EQ:
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How does the Bohr model account for the energies of electrons?
How are electron configurations written and what are their purpose?
Objectives:
 Draw Bohr models of elements
 Apply the Pauli exclusion principle, the aufbau principle, and Hund’s rule to
write electron configurations using orbital diagrams and electron
configuration notation
 Explain the significance of energy levels
 Distinguish between an atom’s ground state and excited state
 Predict the positions of electrons in an atom using the concepts of quantum
numbers and orbitals
Bohr model of hydrogen review by PPT discussion (10 min.)
Student practice Bohr model (20 min.)
Crash Course chemistry video with guided notes (15 min.)
Electron configuration class discussion and practice (30 min.)
Electron configuration practice (15 min.)
Formative assessment: Bohr model and electron configuration homework.
Draw Bohr models and electron configurations for some elements
Day 2
EQ:
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What is the relationship between frequency and wavelength of an EM wave?
What are the characteristics of a wave?
Know the parts and characteristics of a wave
Objectives:
 Compare the wave and particle models of light
 Know the parts and characteristics of a wave
Characteristics of a wave: electrons in atoms #2 PPT (30 min.)
Wavelength and frequency calculations (15 min.)
Particle nature of light (PPT)
Photon energy calculations
Energy level activity for atomic emission spectra
Day 3
EQ:
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How do we explain the difference in colors of the flame test for various
elements?
How can we use a spectroscope to determine the source of various light
samples?
Flame test lab
Atomic Spectra
Day 4
EQ:
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What are the relative energies and shapes of the sharp, principle, diffuse and
fundamental (SPDF) energy levels