CHEMESTRY- ELECTRON CONFIGURATION

Heisenberg uncertainties principle

Sates that it is IMPOSSIBLE to determine simultaneously both the POSITION and VELOCITY of an electron or any other particle

Orbital

A 3-D region around the nucleus that indicates the PROBABLE location of an electron

S sublevel (orbital)

contains 1 orbital- can hold 2 electrons

P sublevel (orbital)

Contains 3 orbitals- can hold 6 electrons

D sublevel (orbital)

contains 5 orbitals- can hold 10 electrons

f sublevel (orbitals)

contains 7 orbitals- can hold 14 electrons

Principle quantum number (n)

Indicates the main energy level occupied by the electron. As “n” increases, the electron’s ENERGY and DISTANCE from the nucleus INCREASES.

electron configurations

The arraignment of the electrons in an atoms

Ground state electron configuration

the lowest energy arrangement of the electrons for each element

Aufbau principle

an electron occupies the LOWEST energy orbitals that can receive it

Pauli exclusion principle

an orbital can hold two electrons of OPPOSITE spins

hund’s rule

Orbitals of EQUAL energy are each occupied by ONE electron before any orbital is occupied be a SECOND electron and all electrons in singly occupied orbitals must have the SAME spin state

Ion

An atom or molecule that has GAINED or LOST one or more ELECTRONS and has a NEGATIVE or POSITIVE charge