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Which Of The Following Set Of Quantum Numbers Belong To Highest Energy
Quantum mechanics is a fundamental theory in physics that describes the behavior of matter and energy at the atomic and subatomic level. It is a complex subject that requires a lot of mathematical calculations and understanding of the principles involved. One of the concepts in quantum mechanics is the set of quantum numbers that describe the state of an electron in an atom. These quantum numbers are n, l, m, and s.
The principal quantum number (n) describes the energy level of an electron in an atom. The azimuthal quantum number (l) describes the shape of the electron’s orbital. The magnetic quantum number (m) describes the orientation of the electron’s orbital in space. The spin quantum number (s) describes the spin of the electron.
The set of quantum numbers with the highest energy is the one with the highest value of n and l. Among the given options, the set with the highest energy is option D, which has the highest value of n and l. The orbital which has higher value of (n+l) has higher energy. For the 3d orbital, (n+l)=(3+2)=5 is maximum, which makes it the orbital with the highest energy.
In summary, option D with quantum numbers n=3,l=2,m=1,s=+21 represents 3d orbital which has highest energy among all given options .
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