We’re being asked to determine the correct set of quantum numbers for the given atomic orbital shape. Let’s first define the quantum numbers.
• the principal quantum number (n) → energy level in orbitals and its value could be any positive integer starting from 1
• angular momentum quantum number (ℓ) → (l) has to be at least 1 less than n, range of values from 0 up to (n-1)
▪ Each ℓ value corresponds to a subshell/sublevel:
Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:
a) n = 2, ℓ = 1, m ℓ = 0
b) n = 3, ℓ = 2, m ℓ = –1
c) n = 4, ℓ = 0, m ℓ = +1
d) n = 1, ℓ = 1, m ℓ = 0
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Our tutors have indicated that to solve this problem you will need to apply the Quantum Numbers: Magnetic Quantum Number concept. You can view video lessons to learn Quantum Numbers: Magnetic Quantum Number. Or if you need more Quantum Numbers: Magnetic Quantum Number practice, you can also practice Quantum Numbers: Magnetic Quantum Number practice problems.
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Based on our data, we think this problem is relevant for Professor Bittner's class at UH.