Q3 : Week 2 – 2/6 – 2/10
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Jump to: Monday Homework
a) To use the solutions to the Schrodinger Equation to write electron configurations.
b) To define the quantum numbers to standing waves of orbitals (wave potentials).
c) To build an orbital diagrams.
2. Review the quantum number form.
Quantum Number form 1920 Key p.pdf
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3. Complete the Quantum numbers worksheet with the class to cements the concepts of quantum numbers that are solutions to the Shroedinger’s Equations.
Quantum Numbers – worksheet 1.pdf
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Quantum Numbers – worksheet 2.pdf
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4. Wrote the configuration of the Uranium to demonstrate how the periodic table is a guide to the electron configurations (especially the overlapping of energy levels).
Need to show students the shapes of orbitals and where the g begins!!
TODAY’s NOTES:


Need to show students the shapes of orbitals and where the g begins!!
Light into the Bohr Model:
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2/6 – Monday’s Homework: –
Quantum Numbers – worksheet 1.pdf
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Quantum Numbers – worksheet 1 Key.pdf
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2. Please view the lecture of me reviewing the first 4 elements in the Quantum Numbers – worksheet 2.pdf and then complete the worksheet. Review with the key below.
Quantum Numbers – worksheet 2.pdf
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Review of quantum number worksheet 2 (the 4 atoms) :
electron configuration 1 | electron configuration 2 |
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2/7 – Tuesday – A Day – 2/3a Lab, 4
a) To write electron configurations for atoms and ions using the quantum numbers
b) To identify filled, occupied, and partially filled principle energy levels, sublevels, and orbitals.
Period 2,3a: – Shape of orbitals! (presentations and flash)
1. Review the quantum numbers worksheet 1.
Quantum Numbers – worksheet 1 Key.pdf
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2. Review the quantum numbers worksheet 2.
a) Overlapping of principle energy levels (orbitals) – Scandalous!!!
3. Writing Electron Configuration of Uranium – writing configurations lesson – shorthand!
– Wrote the electron configuration of Uranium and Ag / Ag+ /Shorthand/ and U+6
Period 4: – Shape of orbitals! (presentations and flash)
1. Quantum numbers Review with presentation
2. Review the Quantum Numbers worksheet 2.
3. Review of electron configurations
TODAY’s NOTES:


Need to show students the shapes of orbitals and where the g begins!!
Aufbau Principle Flask Energy inversions :
Quantum Numbers to Electron Configurations:
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2/7 – Tuesday’s Homework: –
1. Please complete Atomic Structure 4b -Electron configuration.pdf worksheet and review the key if you have not done already.
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2 : Tonight’s Form: AP Periodicity and Electron Configurations Form 1 22-23
End of Wednesday!
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2/8 – Wednesday – B Day – 2, 3b/4 Lab
a) To Review Groundstate vs. Excited electron configurations.
b) To define Z, Zeff, and Ionization energy.
c) To review electron screening and electron – electron repulsions (Zeff)
Period 2,3b/4:
1. A review of the Atomic Structure 4b -Electron configuration.pdf worksheet (electron configurations).
Atomic Structure 4b -Electron configuration key.pdf
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a) Go through the complete electron configuration of entire periodic table with slide 154 – g orbitals –> groundstate vs. Excited state
2. A Review of the Quantum number worksheet 2. (reviews overlapping of principle energy levels)
3. Review of last nights Form.
AP Periodicity and Electron Configurations Form 1 KEY p.pdf View Download
4. Define, Z, Zeff, electron screening and electron – electron repulsions.
TODAY’s NOTES:
So the 2nd IE is the energy needed to remove the second electron. Would it require the same amount as the 1st IE? No it would require much more because Na+ the second electron would be removed from a filled principle energy level!! These are core electrons that are more stable. Do not lose site that IE is a measure of electron stability.

ALL of this is about Energy Lecture!
Need to show students the shapes of orbitals and where the g begins!!
Light into the Bohr Model and beyond!
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2/8 – Wednesday Homework: –
1. Please complete the Form below based on the resources posted above the form. Please answer the questions completely as if you were answering a free response question. Do not be vague but get to your point quickly! A longer response is not always the correct reponse.
1 : Tonight’s Form: AP Periodicity and Electron Configurations Form 2 22-23 –
Please use complete sentences and DO NOT BE VAGUE!! Be careful to answer each question in each numbered question. There is often more than one question per numbered question. Writing more does not guarantee the answer will be correct. The real skill is to write the least amount of words that will answer the question completely. Get in and get out!
End of Tuesday!
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2/9 – Thursday – A Day – 2/3a Lab, 4
b) To compare and contrast Ionization Energy with Electron Affinity. c) To identify paramagnetic and diamagnetic properties of atoms from electron configurations,
Period 2/3a:
1. Complete the Review the AP Periodicity and Electron Configuration Form 1 with key.
AP Periodicity and Electron Configurations Form 1 KEY p.pdf View Download
3. Valance electrons AND “Bam!!!” IE energy values = the proof of valance electrons!
4. Begin classwork worksheet:
View Download
View Download.
1. Review the AP Periodicity and Electron Configuration Form 1 with key.
AP Periodicity and Electron Configurations Form 1 KEY p.pdf View Download
TODAY’s NOTES:
Ionization Energy (IE) | Electron Affinity (EA) |
Energy needed to remove an electron | Energy released or absorbed when electron is added |
measures stability of current electrons | measures stability of added electron |
Creates positive ions (cations) | Creates negative ions (anions) |
∆H = positive (endothermic) | ∆H = negative (exothermic) or positive (endothermic) |
.50 kJ/mol + Na —–> Na+ + e– | F + e– ——> F– + 328 kJ/mol |
1681 kJ/mol + F —–> F+ + e- | 53 kJ/mole + Na + e– ——> Na– |
Larger the IE the more stable the e– | Larger the negative EA the more stable the added e– |
Used for all atoms – Clear Trend | Used primarily for nonmetals but Trend is not clear/ many exceptions |
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Fluorine (F)
-328 kJ/mol
Chlorine (Cl)
-349 kJ/mol
Bromine(Br)
-324 kj/mol
Iodine (I)
-295 kJ/mol
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Electron Affinity Animation :
Last Slides for orbital shapes!
1 : Tonight’s Form: AP Periodicity and Electron Configurations Form 3 22-23 –
Please use complete sentences and DO NOT BE VAGUE!! Be careful to answer each question in each numbered question. There is often more than one question per numbered question. Writing more does not guarantee the answer will be correct. The real skill is to write the least amount of words that will answer the question completely. Get in and get out!
End of Thursday!
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2/10 – Friday – B Day – 2, 3b/4 Lab
b) To review the electron shielding vs electron – electron repulsions
Period 2:
4. Complete the following worksheet:
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4. Classwork 1:
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5. Classwork 2:
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6. Lab 21 – Periodic Graphs excel – If time permits..
TODAY’s NOTES:

The d orbitals that do not directly interact with the incoming ligand are not as destabilized and thus a GAP is created and the degenerate d orbitals are split into 2 levels by a gap small enough in energy that photons of visible light can match! |
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Aufbau Principle Flask Energy inversions :
Light into the Bohr Model:
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Lab 21 – Periodic Trends Graphing
Divergence (energy inversion) Lecture of 3d orbitals :
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2/10 – Friday Homework: –
1.. PES (Photon Emission Spectroscopy) – experimental evidence of electron configurations.
Photon Emission Spectroscopy Lecture :
End of Week 2!