Presentation on theme: "ELECTRON CONFIGURATIONS. Electron Configuration: A method for communicating the location and number of electrons in the electron energy levels. 3p 5 Principal."— Presentation transcript:
Electron Configuration: A method for communicating the location and number of electrons in the electron energy levels. 3p 5 Principal Quantum Number = 3 Orbital = p Number of electron(s) in the orbital(s) = 5
The arrangement of electrons follows the Aufbau Principle. (means building-up in German) in the ground state, the electrons will fill the atomic orbital of lowest energy. An electron configuration is a listing of the number and kinds of electrons in order of increasing energy, written in a single line. Example: Li 1s 2 2s 1 The order, from left to right, is the order of increasing energy of the orbitals
The order is: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d etc.
Procedure for Writing and Electron Configuration: Step 1: Determine the position of the element in the periodic table and the total number of electrons in the atom or simple ion. Step 2: Start assigning electrons in increasing order of main energy levels and sublevels. Step 3: Continue assigning electrons by filling each sublevel before going on to the next sublevel, until all the electrons are assigned.
Element Electron configuration 1 H 1s 1 2 He 1s 2 3 Li 1s 2 2s 1 5 B 1s 2 2s 2 2p 1 7 N 1s 2 2s 2 2p 3 13 Al 1s 2 2s 2 2p 6 3s 2 3p 1 17 Cl 1s 2 2s 2 2p 6 3s 2 3p 5 21 Sc 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1 23 V 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 3
EXCEPTIONS: Chromium (24 electrons) EC = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4 is INCORRECT EC = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 5 is CORRECT! The d-orbital becomes half-filled so, it changes to 4s 1 3d 5 instead. The next element, Manganese will have an EC of: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5
This exception also appears near the end of the d-orbital filling: Copper EC = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 9 is INCORRECT EC = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 10 is CORRECT Additional exceptions are Mo 5s 1 4d 5 ; Ag 5s 1 4d 10 ; Au 6s 1 5d 10 That is reasonable considering their position on the periodic chart.
Expanded and Condensed Electron Configurations What you had just learned is the expanded notation of writing EC. Example: Na: 1s 2 2s 2 2p 6 3s 1 Expanded form Na: [Ne] 3s 1 Condensed form The “ [Ne] ” is called a kernel = [ closest noble gas ] ONLY NOBLE GASES CAN BE USED AS THE KERNEL
ORBITAL-BOX DIAGRAMS Similar to EC, except, you are now expected to draw out the orbitals and place the electrons to show proper spinning. Rules for drawing orbital-Box diagrams 1)The Pauli Exclusion Principle- each orbital can hold 2e-, where those 2e- are always in opposite spin. 2) Hund's Rule – Electrons occupy all the orbitals of a given sublevel singly before pairing begins. Spins of electrons in different incomplete orbitals are parallel in the ground state.The most stable arrangement of electrons in the subshells is the one with the greatest number of parallel spins.
Suppose we want to draw the orbital-box diagram of carbon: Step 1: Draw the orbitals. Step 2: Fill the electrons in the 1 st two s- orbitals, showing opposite spin. These electrons must fill the lower energy orbitals first before advancing to the next higher energy level (AUFBAU’s PRINCIPLE). Step 3: Fill the 2p sublevels one at a time (HUND’s RULE).
Orbital Diagrams Examples
IONS VALENCE ELECTRONS The electrons in the outermost shell of the Bohr diagram. Lose electrons = become positively charged (Cation) Gain electrons = becomes negatively charged (Anion)
ELECTRON CONFIGURATIONS OF IONS Electrons do not come out the same way as we put them in according to the Aufbau Principle. Electrons leave the outer most shell first. Let's look at V vs V V 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 3 23 V 2+ 1s 2 2s 2 2p 6 3s 2 3p 6 3d 3