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The Quantum Model : Part II Electron Configurations Quantum Numbers Describe the properties of atomic orbitals and the electrons that occupy them… Quantum Number Describes Principle main E. level Angular Momentum shape of Orbital Magnetic orientation of orbital Spin orientation of electron Principal Quantum Number (PQN) Main energy level occupied by the electron Distance from nucleus “shell” Always whole positive integers Angular Momentum Quantum Number (orbital) Shape of the orbital Sublevel within the main energy level s orbitals p orbitals d orbitals Magnetic Quantum Number Orientation of orbital (X, Y, Z) Has to do with the relation to the x-y-z axes s Orbitals have only one possible orientation. P Obitals have 3 possible orientations d Orbitals Have 5 Orientations How many orientations do you think f orbitals have? SPIN QUANTUM NUMBER The orientation of the electron in the orbital. “Direction of its spin”. An electron can only have 2 different types of spins We will call the two types of spins “UP” and “DOWN” How many sublevels are allowed for each energy level? We are not actually filling the energy level. We are filling sub-levels that make up the energy level. We start with the lowest energy sublevel The S, when we fill this we have to move to a higher energy sub-level Next we enter the P orbitals, after filling these we enter the D orbitals … Given by the Quantum-Mechanical Model of the Atom There can only be 0 … n-1 sublevels for each energy level, this means: The 1st energy level has 1 sublevel The 2nd energy level has 2 sublevels The 3rd energy level has 3 sublevels The 4th energy level has 4 sublevels Atomic Orbitals and Quantum Numbers Use your notes to make a chart showing important information about each of the four quantum numbers. Make chart for only n=1,2,3,4 Principal Quantum Number Angular Momentum Quantum Number Magnetic Quantum Number Spin Quantum Number HOMEWORK Read pages 101 – 104, Answer questions #1-3 on page 104 Answer question # 14, 15, 16 on pg 118 Read the Lab for a pre-lab quiz next class Your Chart Should look like this Principle Quantum # Angular Momentum Quantum # Magnetic Quantum # Spin Quantum # Energy Level Sublevels Orientation Orbital Orientation Electron 1 (s) 1 Up/down 2 (s,p) 4 Up/down 3 (s,p,d) 9 Up/down 4 (s,p,d,f) 16 Up/down Electron Configuration Show the placement of electrons in specific levels, sublevels and orbitals. Make use of the four quantum numbers and a few simple rules. Each orbital can only hold a maximum of 2 electrons Before we learn the rules lets look at a few examples! Types of notation Orbital diagram Arrows represent electrons and direction of spin. Which element is this? How many electrons? Rule # 1 : Aufbau Principle An electron occupies the lowest energy orbital that can receive it…(like filling a glass) n= 1, n= 2, n=3 represent main energy level. Organize the levels and sublevels Main energy level, 1, 2, 3 etc.) How many sublevels exist at each main energy level? What are the sublevels at each main energy level? 1__ 2__ 3__ 4__ 5__ 2__ 3__ 4__ 5__ 3__ 4__ 5__ 4__ 5__ 5__ Organize the levels and sublevels Principle Quantum Number (main energy level) ↓ 1s 2s 3s 4s 5s 2p 3p 4p 5p 3d 4d 5d 4f 5f 5g How do we remember which sublevel to fill first? Memory Aid Diagram Rule # 2 : Pauli exclusion principle No two electrons in the same atom can have the same set of four quantum numbers…or… If two electrons occupy the same orbital they must have opposite spins! He ↑ ↓ 1S opposite spins shown by arrow. Rule # 3 : Hund’s Rule Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron. Correct Wrong Electron configuration notation 1S2 2S2 2P2 What does each character represent? Which element is this? The Three Little Rules! An electron occupies the lowest energy orbital that can receive it…(like filling a glass) If two electrons occupy the same orbital they must have opposite spins! Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron. Homework Read pg 105 – 111 Questions: pg 116 #1 Work on electron configuration handout