Problem: Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:a) n = 2,  ℓ = 1, m ℓ  = 0b) n = 3, ℓ = 2, m ℓ  =  –1c) n = 4, ℓ = 0, m ℓ  = +1d) n = 1, ℓ = 1, m ℓ = 0

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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:

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Problem Details

Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:

a) n = 2,  ℓ = 1, m   = 0

b) n = 3, ℓ = 2, m   =  –1

c) n = 4, ℓ = 0, m   = +1

d) n = 1, ℓ = 1, m  = 0

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