Electron Configuration

Atomic Orbitals

regions of high probability where a given electron would be found based on energy , come in four different shapes, or sublevel that can be found it energy level, shell, or ring

S-orbitals

the lowest energy orbitals or sublevels, are spherically shaped and can hold a maximum of 2 electrons

p-orbitals

higher in energy than s-orbitals, are shaped like peanuts and are situated on each of the three axes in a 3-D graph, maximum of 2 electrons can fit in each of the three p-orbitals for a total of 6 electrons

d- orbitals

higher in energy than p-orbitals, come in 5 axis arrangments, known as spatial orientations, holding a maximum of 10 electrons, 2 in each orientation

f-orbitals

the highest energu orbitals for electrons of atoms in the ground state, have seven possible arrangments; each atomic orbital may hold 2 electrons for a maximum of 14 electrons that can fit in f-orbitals

Energy Level 4

4 sublevels, has letters(1 orbital and 2 electrons), p( 3 orbital and 6 electrons), d(5orbital and 10 electrons), f(7 orbitals and 14 electrons) has total of 32 electrons

difference between ground state and excited state

Ground-is lowest possible energy state of an atom Excited- when atoms gain energy it is excited state

Aufbau Principle

each electron occupies the lowest avaliable energy orbital(near the nucleus)

pauli exclusion principle

a maximum of 2 electrons can occupy a single orbital but only if they have opposite spins

Hund's rule

single electrons with the same spin must occupy each equal-energy orbital before more electrons can occupy the same orbitals