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Electrons will first enter into the orbi...

Electrons will first enter into the orbital with the set of quantum numbers

A

n = 5, l = 0

B

n = 4, l = 1

C

n = 3, l = 2

D

any of these

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To determine which orbital electrons will first enter based on the given quantum numbers, we can follow these steps: ### Step-by-Step Solution: 1. **Understand Quantum Numbers**: Each orbital is defined by a set of quantum numbers: - Principal quantum number (n) - Azimuthal quantum number (l) - Magnetic quantum number (m_l) - Spin quantum number (m_s) 2. **Calculate n + l**: For each option provided, calculate the sum of the principal quantum number (n) and the azimuthal quantum number (l). This sum (n + l) helps determine the energy level of the orbital. - For example, if we have: - Option A: n = 3, l = 2 → n + l = 3 + 2 = 5 - Option B: n = 4, l = 1 → n + l = 4 + 1 = 5 - Option C: n = 5, l = 0 → n + l = 5 + 0 = 5 - Option D: n = 3, l = 1 → n + l = 3 + 1 = 4 3. **Compare n + l Values**: Identify which options have the same n + l value. In our example, Options A, B, and C all have n + l = 5, while Option D has n + l = 4. 4. **Determine Priority Based on n**: If multiple orbitals have the same n + l value, the one with the lower principal quantum number (n) will be filled first. - From our example, Option D (n = 3, l = 1) has the lowest n value compared to the others (which all have n + l = 5). 5. **Select the Correct Option**: Based on the above analysis, the correct answer is the option with the lowest n value among those with the same n + l value. In this case, Option D would be the first to be filled. ### Final Answer: The electrons will first enter into the orbital corresponding to Option D (n=3, l=1). ---
To determine which orbital electrons will first enter based on the given quantum numbers, we can follow these steps: ### Step-by-Step Solution: 1. **Understand Quantum Numbers**: Each orbital is defined by a set of quantum numbers: - Principal quantum number (n) - Azimuthal quantum number (l) - Magnetic quantum number (m_l) ...
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