Therefore, you can say that a #4p# orbital can hold a maximum of two electrons and the #4p# subshell can hold a maximum of six electrons. Solution: Spin can either be +1/2 or -1/2. ![]() Question: Calculate the minimum and maximum number of electrons which have magnetic quantum number m 1 and spin quantum number s 1/2 in chromium. Magnetic quantum number (ml) 2, 1, 0, 1, 2. #3 color(red)(cancel(color(black)("p orbitals"))) * "2 e"^(-)/(1color(red)(cancel(color(black)("p orbital")))) = "6 e"^(-)# Solution: For the 3d orbital, Principal quantum number (n) 3. ![]() Since each of those #p# orbitals can hold a maximum of two electrons, the #p# subshell can hold a maximum of Which set of four quantum numbers corresponds to an electron in a 4p orbital This problem has been solved Youll get a detailed solution from a subject. Now, the #4p# subshell contains a total of three #4p# orbitals, #4p_x#, #4p_y#, and #4p_z#. For example, the 3d subshell is in the n3 shell, the 2s subshell is in the n 2 shell, etc. The principle quantum number, n, describes the energy and distance from the nucleus, and represents the shell. ![]() To the level of an orbital, this comes down to one of the two electrons that share an orbital having spin-up, which is given by the spin quantum number #m_s = +1/2#, and the other having spin-down, which is given by #m_s = -1/2#. The four quantum numbers are the principle quantum number, n, the angular momentum quantum number, l, the magnetic quantum number, ml, and the electron spin quantum number, ms. This is the case because according to the Pauli Exclusion Principle, two electrons located in an atom cannot share a complete set of four quantum numbers. In fact, any orbital, regardless of its energy level, subshell, and orientation, can hold a maximum of two electrons, one having spin-up and one having spin-down. A #4p# orbital, which is part of the #p# subshell located on the fourth energy level, can hold a maximum of two electrons.
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