The Basics of Electron Configuration
Think of atomic orbitals as parking spaces around the nucleus where electrons hang out. Each orbital can hold a maximum of two electrons, but they must have opposite spins - like two people sharing a seat facing different directions.
There are four main types of orbitals: s, p, d, and f orbitals. A subshell is basically all the orbitals of the same type within the same energy level. For example, the 3d subshell contains all the d orbitals in the third shell.
Here's the key rule: electrons always fill the lowest energy orbitals first. It's like water flowing downhill - electrons naturally go where they need the least energy. When orbitals have the same energy level, electrons prefer to spread out into separate orbitals before pairing up, since they repel each other.
Quick Tip: Remember that nitrogen's electron configuration (1s² 2s² 2p³) shows how the 2p electrons spread out individually before pairing up!
