🤓 Based on our data, we think this question is relevant for Professor Shiraiwa's class at UCI.
We are asked to determine the value of ℓ when mℓ= 4.
Possible values of the quantum numbers:
•principal quantum number →energy level in orbitals and its value could be any positive integer starting from 1 to infinity
•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:
ℓ = 0→ s subshell
ℓ = 1→ p subshell
ℓ = 2→ d subshell
ℓ = 3→ f subshell
ℓ = 4→ g subshell
• magnetic quantum number (mℓ)→ range of values from -ℓ to +ℓ
▪ The mℓ values (for each ℓ) represent electron orbitals for the subshell:
s subshell→ 1 orbital
p subshell→ 3 orbitals
d subshell→ 5 orbitals
f subshell→ 7 orbitals
g subshell→ 9 orbitals
•spin quantum number (ms) → can only have two possible values +½ (spin up electron) or–½ (spin down electrons)
• Note that 1 orbital can hold a maximum of 2 electrons→ 1 spin up (+½) and 1 spin down (–½)
If ml = 4, what can you say about l?
a. l = 4
b. l > 4
c. l ≥ 4
d. l < 4
e. l ≤ 4
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What scientific concept do you need to know in order to solve this problem?
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Based on our data, we think this problem is relevant for Professor Shiraiwa's class at UCI.