#ELECTRON CONFIGURATION AUFBAU PRINCIPLE FREE#

#ELECTRON CONFIGURATION AUFBAU PRINCIPLE FREE#

You would never sit right next to someone you did not know if there are free seats available, unless of course all the seats are taken then you must pair up. When filling sublevels other than s, electrons are placed in individual orbitals before they are paired up.Įlectrons fill like people do on a bus. Incorrect electrons must spin in opposite directionsĬorrect the electrons have opposite spins (Therefore, no two electrons in the same atom can have the same set of four Quantum Numbers. ) So, if an electron is paired up in a box, one arrow is up and the second must be down. When we draw electrons, we use up and down arrows. There are a few rules for the box and arrow configurations.Īufbau Principle - electrons fill orbitals starting at the lowest available energy state before filling higher states (1s before 2s).Īn orbital can hold 0, 1, or 2 electrons only, and if there are two electrons in the orbital, they must have opposite (paired) spins. This sublevel configuration can be broken down into orbitals (boxes).ġs 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6. sublevelį z 3 f xz 2 f yz 2 f xyz f z(x 2-y 2) f x(x 2-3y 2) f y(3x 2-y 2) An orbital is defined as the most probable location for finding an electron. Sublevels can be broken down into regions called 'orbitals'. It is called the 'Box and Arrow' (or circle and X) orbital configuration. There is yet another way to writing electron configurations. Aufbaus Principle states that electrons are filled in shells in the following order of energy levels: 1s, 2s, 2p, 3s, 3p, 4s, 4p, 5s, 4d, 5p, 6s, 5d, 6p, 7s. Pauli Exclusion Principle and Hund's Rule Box and Arrow Orbital Configurations using

Electron configuration aufbau principle