ms = +1/2
ms = +1/2
Ms = + 1/2
ms= +1/2
ms = -1/2
ms = -1/2
ms = +1/2
ms = +1/2
Ms = + 1/2
Ms = + 1/2
ms= +1/2
ms = -1/2
ms= +1/2
Maximum of 32 electrons.
The number represents the shape of an electron subshell is the azimuthal quantum number, also known as the angular momentum quantum number. It is denoted by the letter l and can have values ranging from 0 to n-1, where n is the principal quantum number. Each value of l corresponds to a specific shape of the subshell: 0 (s), 1 (p), 2 (d), 3 (f), and so on.
It's the azimuthal quantum number. It specifies the angular momentum of the orbital, which can broadly speaking be thought of as its "shape." (The reason I'm putting that in quotation marks is that it's possible for two orbitals with the same azimuthal quantum number to appear rather different in overall shape.)
The ionized form of aluminum, Al+3 naturally has a greater electronegativity than neutral aluminum. Electronegativity is a measure of the attraction that a given chemical has for electrons, and negatively charged electrons are naturally attracted to positively charged objects, as indicated by Coulomb's Law. Therefore, it is much harder to remove a fourth electron from an aluminum ion that has already lost three electrons, than it was to remove the first electron.
The arrows pointing in opposite directions in the orbital filling diagram represent the two electrons in the same orbital having opposite spins. According to the Pauli exclusion principle, no two electrons in an atom can have the same set of quantum numbers, so one electron must have a spin of +1/2 and the other -1/2.