Atomic Structure And The Periodic Table Flashcards
(8 cards)
Pauli Exclusion Principle
Within an atom, no two electrons can have the same set of quantum numbers. So, each electron has its own distinct set of four quantum numbers.
Aufbau principle
When building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy
Hund’s Rule
When an electron is added to a subshell, it will always occupy an empty orbital if one is available. Electrons always occupy orbitals singly of possible and pair up only if no empty orbitals are available.
Diamagnetism
A type of magnetism in which elements have all of their electrons spin paired( all subshells completed)
Paramagnetism
Elements that do not have all of their electrons spin paired; elements with not all subshells completed
Quantum numbers
The positions of the electrons in relation to the nucleus
Four quantum numbers: shell, subshell, orbital, spin
Four quantum numbers
Shell (principle quantum number n)
Subshell (angular momentum quantum number l)
Orbital (magnetic quantum number ml)
Spin (ms)
Quantized energy of an electron formula
En = (-2.178x10^-18)/n^2 joules
n = principal quantum number of the electron