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Download Chapter 7 Handout 1 Atomic Orbitals Quantum Numbers: Principal
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Chapter 7 Handout 1 Atomic Orbitals Quantum Numbers: Principal Quantum Number (n) = Whole numbers only, determines the energy of an orbital Angular Momentum Quantum Number (l) = Sublevels = determines shape of orbital (s, p, d, f) Magnetic Quantum Number (ml) = describes the orientation of the orbital Electron Spin Quantum Number (ms)= describes electron spin Sublevel Max Amount of Electrons s 2 p 6 d 10 f 14 Electron Configuration: How the electrons are distributed among the various atomic orbitals. Energy Level Diagram 7p 6d 5f 5d 4f 7s 6p 6s 5p 4d 5s 4p 3d 4s 3p 3s 2p 2s 1s Orbital Diagram Notation: Electron Configuration Notation: 1s2 Rules for filling orbitals: 1. Aufbau Principle: a. Electrons fill up orbitals of lowest energy first b. Orbitals in the same sublevel are equal in energy c. Sometimes energy levels overlap 2. Pauli Exculsion Principle a. There is a max of 2 electrons in any one orbital b. These 2 electrons must have opposite spins 3. Hund’s Rule a. When filling orbitals of equal energy, one enters each orbital first b. Then, second electron will enter each orbital to form paired opposite spins. Diagonal Rule (Aufbau Principal) : Orbitals fill upward right to left. Diamagnetism and Paramagnetism (Pauli Exclusion Principal): Diamagnetic: Paramagnetic: The Shielding Effect: https://www.boundless.com/chemistry/textbooks/boundless-chemistrytextbook/periodic-properties-8/electron-configuration-68/the-shielding-effect-and-effective-nuclearcharge-319-7515/