Electron configuration.
Principal quantum shells.
The energy levels or quantum shells.
n = 1.
Up to 2 electrons.
Up to 8 electrons.
s block, p block, d block, and f block elements.
Using orbital spin diagrams where each box represents an atomic orbital.
Up to 32 electrons.
The size increases.
Spin-pair repulsion.
One electron will go into each p orbital (p_x, p_y, p_z).
Five orbitals (total of 10 electrons).
Spherical.
Dumbbell shape.
They become larger and longer.
Two electrons.
One orbital (total of 2 electrons).
The energy level of a particular shell and the energy of the electrons in that shell.
An orbital can only hold two electrons with opposite spin.
The order appears to overlap.
In order of increasing energy from lower to higher.
n = 3 is larger.
X, y, and z axes.
One or more atomic orbitals.
How the electrons in an atom or ion are arranged in their shells, subshells, and orbitals.
Full electron configuration describes all electrons from the 1s subshell up, while shorthand uses the symbol of the nearest preceding noble gas followed by the rest of the configuration.
The 4s subshell before the 3d subshell.
The spin of the electrons.
A tiny magnetic field with N-S pole pointing up or down.
They will then pair up, with a second electron added to the first orbital in the opposite direction.
At specific energy levels.
Seven orbitals (total of 14 electrons).
Chromium has the electron configuration [Ar] 3d5 4s1 instead of [Ar] 3d4 4s2.
By filling the subshells of energy with the lowest energy first (1s).
Up to 18 electrons.
Electrons occupy the lowest energy levels first before filling those with higher energy.
Shells, subshells, and orbitals.
Principal quantum shells.
No, they can only be found at specific levels.
By adding electrons to the outer subshell.
It corresponds to n = 2.
Copper has the electron configuration [Ar] 3d10 4s1 instead of [Ar] 3d9 4s2.
s, p, d, and f.
The shape of the d orbitals.
They occupy separate orbitals first to minimize repulsion and have their spins in the same direction.
The nucleus of the atom.
Three orbitals (total of 6 electrons).
Because the energy required to jump to a higher empty orbital is greater than the inter-electron repulsion.
No, it does not follow a regular pattern.
To represent the arrangement of electrons in their orbitals.
Three p orbitals.
Principal quantum numbers.
By removing electrons from the outer subshell.
The most stable electronic configuration with the lowest amount of energy.
s < p < d.
