Hunds Rule ofMaximum multiplicity Achievements ofBohrs theory Planks quantum

Hunds rule ofmaximum multiplicity achievements

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Hund’s Rule of Maximum multiplicity Achievements of Bohr’s theory Plank’s quantum theory Radial and Angular nodes Similarities and differences of a 1S and 2S orbital. Effective nuclear charge Work Function Degenerate orbitals Iso- electronic species Shielding effect Isomer of hydrogen Cause of spectrum Isodiapheres and Isosters Shape of orbitals Energy of electrons in multi- and single electron system Shortcomings of Bohr’s Model and Rutherford’s Model Characteraistics of Electromagnetic Radiations Bohr’s –Bury Scheme Card 1 1. Rutherford’s Model: a. According to classical mechanics his atom was not stable b. It could not explain the spectrum of Hydrogen atom 2. Bohr’s model a. Could not explain the finer splitting of lines in the Hydrogen spectrum b. When you cannot locate an electron or tell its momentum then speaking of a definite trajectory for the electron is meaningless. 3. a. Isotones: Ca 40 & K 39 b. Isotopes: Cl 35 & Cl 37 c. Isobars: Ca 40 & K 40 d. Cl - & Ar 4. a. Ca 2+ = 18 b. Fe 3+ = 23 c. N 3- = 10 5. IR < Visible< UV 6. Henry Becquerel 7. Same 8. nh/2π 9. a. H 1 Protium b. H 2 Deuterium c. H 3 Tritium 10. H 1
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