Chapter 5:
Electrons in Atoms
5.1 Light and Quantized Energy
Wave nature of light, wavelength λ, frequency ν,
EMR ( electromagnetic radiation), amplitude, crest,
trough, electromagnetic spectrum,
(speed of light) c = λ ν
Particle nature of light, quantum E
quantum= h ν,
Planck’s constant h = 6.625 x 10-34 J, photoelectric effect, E
photon = h ν,
Atomic emission spectra,
5.2 Quantum Theory and the Atom
Bohr model of the Atom, energy states of hydrogen, ground state,
hydrogen line spectrum, ΔE = E
higher energy level – E
lower energy level = E
photon = h ν
The Quantum Mechanical Model of the Atom, electrons as waves, deBroglie, Heisenberg Uncertainty Principle, Schrodenger, orbital vs orbit, probability map, principal quantum numbers, principal energy levels (1-7), energy sublevels (s, p, d, f)
5.3 Electron Configurations
Ground state electron configurations, aufbau principle, Pauli Exclusion Principle
( ↑ ↓ ) , Hund’s rule, orbital diagrams and electron configuration notations,
Valence electrons, Lewis, electron dot structure
Section 5.1 Light and Quantized Energy
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Section 5.2 Quantum Theory and the Atom
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Section 5.3 Electron Configuration
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Section 5.1 Light and Quantized Energy
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Section 5.2 Quantum Theory and the Atom
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Section 5.3 Electron Configuration
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Section 5.1 Light and Quantized Energy
Standard 1 h - Atomic and Molecular Structure
View Standard 1 State Standard: The experimental basis for Thomson's discovery of the electron, Rutherford's nuclear atom, Millikan's oil drop experiment, and Einstein's explanation of the photoelectric effect.
Students Will be able to:Examine the historical experimental basis of the atomic theory. Book Reference Pages: 123, 124
Standard 1 j - Atomic and Molecular Structure
View Standard 1 State Standard: Spectral lines are a result of transitions of electrons between energy levels. Their frequency is related to the energy spacing between energy levels. Their frequency is related to the energy spacing between levels using Planck's relationship (E=hv).
Students Will be able to:Book Reference Pages: 122-126
Standard 12 d - Investigation and Experimentation
View Standard 12 State Standard: Formulate explanations using logic and evidence.
Students Will be able to:Book Reference Pages: 125
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Section 5.2 Quantum Theory and the Atom
Standard 1 i - Atomic and Molecular Structure
View Standard 1 State Standard: The experimental basis for the development of the quantum theory of atomic structure and the historic importance of the Bohr model of the atom.
Students Will be able to:Demonstrate knowledge of Bohr's model of atomic structure using experimental evidence obtained as a result of a spectroscope lab. Book Reference Pages: 127-134
Standard 1 j - Atomic and Molecular Structure
View Standard 1 State Standard: Spectral lines are a result of transitions of electrons between energy levels. Their frequency is related to the energy spacing between energy levels. Their frequency is related to the energy spacing between levels using Planck's relationship (E=hv).
Students Will be able to:Book Reference Pages: 127, 128
Standard 12 e - Investigation and Experimentation
View Standard 12 State Standard: Solve scientific problems using quadratic equations, and simple trigonometric, exponential, and logarithmic functions.
Students Will be able to:Book Reference Pages: 130
Standard 12 g - Investigation and Experimentation
View Standard 12 State Standard: Recognize the use and limitations of models and theories as scientific representations of reality.
Students Will be able to:Book Reference Pages: 131
Standard 12 l - Investigation and Experimentation
View Standard 12 State Standard: Analyze situations and solve problems that require combining and applying concepts from more than one area of science.
Students Will be able to:Book Reference Pages: 131
Standard 12 n - Investigation and Experimentation
View Standard 12 State Standard: Know that when an observation does not agree with an accepted scientific theory, sometimes the observation is mistaken or fraudulent (e.g., Piltdown Man fossil or unidentified flying objects), and sometimes the theory is wrong (Ptolmaic model of movement of the sun, moon, and planets).
Students Will be able to:Book Reference Pages: 127-128
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Section 5.3 Electron Configuration
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- Principal Energy Levels: Principal Energy Levels (PEL), Sublevels & Orbitals Chart (upside down triangle) - PDF Std 1
- Light - Particles vs Waves: You will learn which evidence is used for the particle and which is used for the wave theory Std 1j
- Tutorial for Ch 5: Reviews and identifies names you need to know, electron configurtions, valence electrons and the Wave Mechanical Theory Std 1
- Tutorial for Ch 5: Tutorial on Ch 5 - terms, scientists, etc
Light
● Light Emission and Absorption Spectra - go to Ch 7 (WW Norton) Visit Site
● Coloring Applet (ChemConnections) Visit Site
● Emission Java Applet(ChemConnections) Visit Site
● Absorption Jaba Applet (ChemConnections) Visit Site
● Single Filter Emission Java Applet (ChemConnections) Visit Site
● Particle vs Wave w single and dbl slit animationed vid - clear. Conclusion at end video wrong because it "observing" requires hitting electron w photons, which change it's direction and velocity (Heisenberg) (You Tube) Visit Site
● Discharge tubes (element tubes) & electron jumps, applet, interactive (PhET) Visit Site
● Waver interference pattern on Physics 2000 showing one of the theories of light, namely wave nature of light. Visit Site
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Magnetism
● Magnetiism - O2 (paramagnetic) vs N2 (diamagnetic) it's all in the unpaired electrons. 2 demos one of liquid oxygen and 2nd with liquid nitrogen. Awesome! Visit Site
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Mases Animations
● Animation represents the Schrodenger/Heisenberg model of the atom. It shows a drawing similar to what you see on p. 137 of our text. It sequentially adds electrons until all of the orbitals shown are filled. Note the extraordinary difference between this and the Bohr model. Visit Site
● Animation shows general areas similar to Bohr model, but different in that they don't follow orbits. The other animation of orbital filling shows a more accurate representation of Schrodenger/Heisenberg model we use today. Visit Site
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Orbitals
● Orbitron - shapes of s, p, d, and f of atomic orbitals Visit Site
● David's Whizzy Periodic Table, electron in orbitals, first 36 elements Visit Site
● Principal Energy Levels Chart (PEL) Visit Site
● Orbital Filling Chart - practice order of filling w large demo version included (HTML) Visit Site
● Orbital Filling chart from old text Visit Site
● Orbital filling applet, very cool Visit Site
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Orbits
● Orbit Animation - Interactive (Visionlearning) Visit Site
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Photoelectric Effect
● Photoelectric Effect - interactive applet allows you to change wavelength of light as well as it intensity (PhET) Visit Site
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SMART BOARD Appropriate
● Electron dot (Lewis Structures)interactive tutorial (McGraw-Hill) Visit Site
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Waves
● Wave Interference showing wave interference with water waves. (Physics 2000) Go to bottom of page and click NEXT to see the classic 2-slit experiment showing wave interference with light. Visit Site
● Radio Waves animation - broadcast to receiver (PhET) Visit Site
● From Physics 2000, on this page towards the bottom is Pictured link for applet to interactively make waves of various frequencies and amplitudes Visit Site
● Video by Science & Reason on Electromagnetic Spectrum, show really great stuff about waves of all kinds. Great intro to EMR. Visit Site
● Video from BYU showing background on Bohr, electron as a wave, and types of orbitals Visit Site
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Wigger Vids
● Why we think light acts like waves - presentation by Miss Grokett. Shows wave interference against move of waves of water. Visit Site
● How to complete Orbital Filling Charts for atoms is taught in this vid. Also shown is how to use a completed Orbital Filling Chart to create an Electron Configuration for several example atoms. Visit Site
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