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What is the maximum number of orbitals that can be identified with the following quantum numbers n = 3, l= 1, m= 0 answer --> 1. how ?
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What is the maximum number of orbitals that can be identified with the...
Explanation:

Quantum numbers: Quantum numbers are numbers that describe the properties of an electron in an atom and its position in an orbital. There are four quantum numbers- principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m), and spin quantum number (s).

Maximum number of orbitals: The maximum number of orbitals for a particular set of quantum numbers can be calculated using the formula 2l+1. This formula calculates the number of orbitals that can be present in a subshell with a particular azimuthal quantum number (l).

Quantum numbers for the given problem: In the given problem, the values of quantum numbers are n=3, l=1, and m=0.

Calculating the maximum number of orbitals: Using the formula 2l+1, we can calculate the maximum number of orbitals that can be present in the subshell with l=1.

2l+1 = 2(1)+1 = 3

Therefore, the maximum number of orbitals that can be identified with the given quantum numbers is 3.

Conclusion: To conclude, the maximum number of orbitals that can be identified with the quantum numbers n=3, l=1, and m=0 is 1. This is because there is only one orbital with m=0 in the subshell with l=1.
Community Answer
What is the maximum number of orbitals that can be identified with the...
N=3,l=1 mns 3p..it can hv m= -1,0,+1..so, m=0 shws one orbital only..
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What is the maximum number of orbitals that can be identified with the following quantum numbers n = 3, l= 1, m= 0 answer --> 1. how ?
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