In theory, the number of electrons with each quantum number is not limited. However, for any given "main quantum number" (n), the number of electrons having the other quantum numbers is limited - but it depends on the value of "n". For more information, the Wikipedia article on "quantum number" seems to give a good overview.
For each level (main quantum number) number "n", there are 2 times n squared electrons. The reasons are related to the Pauli Exclusion Principle, meaning that no two electrons can have the same values for all four quantum numbers.
Each orbital can hold a maximum of 2 electrons, following the Pauli exclusion principle which states that no two electrons in an atom can have the same set of quantum numbers.
There are four quantum numbers: principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m_l), and spin quantum number (m_s). These numbers describe different properties of an electron in an atom, such as energy level, shape of the orbital, orientation in space, and spin.
The spin quantum number can have two possible values: +1/2 or -1/2.
Maximum of 32 electrons.
There can be two electrons with those quantum numbers in an atom. Each electron is completely described by four quantum numbers. The one that's missing in the list provided is ms, which can have only two possible values (+1/2 and -1/2).
For each level (main quantum number) number "n", there are 2 times n squared electrons. The reasons are related to the Pauli Exclusion Principle, meaning that no two electrons can have the same values for all four quantum numbers.
For each level (main quantum number) number "n", there are 2 times n squared electrons. The reasons are related to the Pauli Exclusion Principle, meaning that no two electrons can have the same values for all four quantum numbers.
10 electrons.The angular momentum quantum number is l (small L). This quantum number is dependant on the principal quantum number, and has values, 0 1,2 ..(n-1), where each value of n refers to a subshell known to chemists as followsn= 0, s orbital; n=1, p orbital; n= 2, d orbital; n= 3, f orbital.So we are looking at the d orbitals.There are five d orbitals, with magnetic quantum numbers running from -l to +l, that is -2, -1, 0, +1, +2Each of these can hold 2 electrons (with spin quantum numbers -1/2, +1/2)So we have 10 electrons that can have pricipal quantum numbers of 4 and angular monmentum quantum number of 2.
Each orbital can hold a maximum of 2 electrons, following the Pauli exclusion principle which states that no two electrons in an atom can have the same set of quantum numbers.
the spin quantum number has only two possible values__(+ 1/2 & -1/2)
An orbital can hold a maximum of 2 electrons to fill it. This rule is known as the Pauli Exclusion Principle, which states that no two electrons in an atom can have the same set of quantum numbers.
8 electrons
There are four quantum numbers: principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m_l), and spin quantum number (m_s). These numbers describe different properties of an electron in an atom, such as energy level, shape of the orbital, orientation in space, and spin.
The spin quantum number can have two possible values: +1/2 or -1/2.
Four quantum numbers are required to completely specify a single atomic orbital: principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m), and spin quantum number (s). These numbers describe the size, shape, orientation, and spin of the atomic orbital, respectively.
8 electrons