According to the Pauli Exclusion Principle, no two electrons in an atom or molecule may have the same four electronic quantum numbers. Because an orbital can only hold two electrons at a time, the two electrons must have opposing spins. This indicates that if one electron is allocated to spin up (+1/2), the second electron must be assigned to spin down (-1/2).
The first three quantum numbers of electrons in the same orbital are the same, e.g., n=1, l=0, ml=0 for the 1s subshell. Because these numbers can only be shared by two electrons, their spin moments must be either ms=1/2 or ms=+1/2. We have one ms value if the 1s orbital contains only one electron, and the electron configuration is denoted as 1s1 (corresponding to hydrogen). We have two ms values if it is fully occupied, and the electron configuration is 1s2 (corresponding to helium). These two scenarios can be visualized.
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The Pauli Exclusion Principle states that, in an atom or molecule, no two electrons can have the same four electronic quantum numbers. As an orbital can contain a maximum of only two electrons, the two electrons must have opposing spins
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TWO ELECTRONS OCCUPYING AN ORBITAL
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According to the Pauli Exclusion Principle, no two electrons in an atom or molecule may have the same four electronic quantum numbers. Because an orbital can only hold two electrons at a time, the two electrons must have opposing spins. This indicates that if one electron is allocated to spin up (+1/2), the second electron must be assigned to spin down (-1/2).
The first three quantum numbers of electrons in the same orbital are the same, e.g., n=1, l=0, ml=0 for the 1s subshell. Because these numbers can only be shared by two electrons, their spin moments must be either ms=1/2 or ms=+1/2. We have one ms value if the 1s orbital contains only one electron, and the electron configuration is denoted as 1s1 (corresponding to hydrogen). We have two ms values if it is fully occupied, and the electron configuration is 1s2 (corresponding to helium). These two scenarios can be visualized.
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