subshell

The fourth column says which shells have a subshell of that type.

The second column is the azimuthal quantum number of the subshell.

A subshell can also be specified by putting parentheses around a group of statements.

This is because in Unix, the script is usually executed within a subshell.

Within a subshell where is some integer , ranges thus: .

The precise definition involves quantum mechanics, but it is a number that characterizes the subshell.

The last actinide, lawrencium, also has one electron in the 6d subshell.

Each cell represents a subshell with and given by its row and column indices, respectively.

The maximum number of electrons which can be placed in a subshell is given by 2(2ℓ + 1).

The combination of quantum numbers (n,l) defines a "subshell."

The third column is the maximum number of electrons that can be put into a subshell of that type.

Passing the script filename to the desired shell will run the script in a subshell, not the current context.

A subshell is the set of states defined by a common azimuthal quantum number, ℓ, within a shell.

However, the electrons in one subshell do have exactly the same level of energy, with later subshells having more energy per electron than earlier ones.

"Bang foo runs foo in a subshell, while bang alone shells out."

Subshell can refer to:

In forming compounds, the atom loses its two outermost electrons and one of the 4f-electrons, which belongs to an open subshell.

The transactinide elements all have electrons in the 6d subshell in their ground state .

When the Unix C shell runs a script, it runs it in a subshell.

The following is the order for filling the "subshell" orbitals, which also gives the order of the "blocks" in the periodic table:

One of its 4s electrons is promoted to the 3d subshell giving a 4s1 3d10 configuration.

For many theoretical purposes, the valence electron configuration may be represented to reflect the 7p subshell split as 7s7p.

Each cell represents a subshell, and lists the values of available in that subshell.

For example, the top row says that each s-type subshell ("1s", "2s", etc.) can have at most two electrons in it.

The orbitals of the subshell are each occupied singly with electrons of parallel spin before double occupation occurs.