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Interactive video lesson plan for: Quantum Numbers Explained - Electron Configuration, Atomic Orbital Diagrams - S P D F & n l ml ms

Activity overview:

This chemistry video tutorial explains the 4 quantum numbers n l ml and ms and how it relates to the electron configuration of an element. It also shows you how to draw the atomic orbital diagrams and the orbital energy levels of an atom. It explains the sublevels s p d and f. This video contains plenty of notes, examples, and practice problems.

Here is a list of topics:
1. How to write the ground state electron configuration of an element
2. Electron Configuration Using Noble Gas Notation
3. Electron Configuration of Atoms and Ions - Fluorine (F), Phosphorus (P), Phosphide (P-3), Iron (Fe), Fe+2, Fe+3,
4. Mass Number vs Atomic Number
5. How to determine the number of protons, neutrons, and electrons inside an atom or ion
6. Electron Configuration Exceptions - Cr
7. Cations vs Anions - Positively Charged vs Negatively Charged Ions
8. How to draw the orbital diagram of an atom
9. How to Draw The Orbital Energy Level Diagram of an Atom
10. How to tell if an element is paramagnetic or diamagnetic
11. Paramagnetic - Unpaired Electrons vs Diamagnetic - Paired Electrons
12. Electron Spin around Nucleus - Moving Charge Creates Magnetic Field - Tiny Bar Magnets - North & South Pole
13. How to determine the number of unpaired electrons in an element / atom
14. Aufbau Principle - Filling Electrons In Lower Energy Levels First in order of increasing energy
15. Hund's Rule - Adding Electrons to degenerate orbitals (same energy) one at a time with parallel spins
16. How to determine the number of valence electrons and core electrons in an atom using electron configuration
17. How to identify the element given electron configuration
18. How to identify which element is in the excited state vs ground state given electron configuration
19. n - principal quantum number - main energy level - boh's model of atoms
20. l - azimuthal angular momentum quantum number - sublevel or shape of atomic orbital - s p d f g h
21. ml - magnetic quantum number - describes specific orbital within sublevel
22. ms - electron spin +1/2 or -1/2 up arrow or down arrow
23. l, n-1 equation / formula
24. ml is between -l and l
25. How to identify the 4 quantum numbers n l ml and ms using electron configuration
26. Pauli Exclusion Principle - No two electrons can have the same four set of quantum numbers
27. How to determine the maximum number of electrons given quantum numbers n l ml ms
28. Max number of electrons in an energy level is 2n^2
29. Maximum number of orbitals in an energy level is n^2
30. l=0 for s, l=1 for p, l=2 for d, l=3 for f, l=4 for g, l=5 for h
31. Multiple Choice Practice Problems
32. How to determine the number of s electrons, p electrons and d electrons inside an atom using electron configuration and using the periodic table
33. How to determine which 4 set of quantum numbers are allowed and which are incorrect
34. How to identify the orbital / sublevel given n and l
35. Orbital filling diagram

Tagged under: quantum numbers electron configurations,quantum numbers atomic orbitals,quantum numbers chemistry,quantum numbers explained,quantum numbers,electron configuration, ml ms, orbitals explained,orbital diagram,orbital filling diagram,chemistry,atomic orbitals,noble gas notation,exceptions,ions,atoms,paramagnetic,diamagnetic,unpaired electrons,electron spin,aufbau principle,hund' rule,pauli exclusion principle,ground state,excited state

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