Electrons will first enter into the orbital with the set of quantum numbersa)n = 5, l = 0b)n = 4, l = 1c)n = 3, l = 2d)any of theseCorrect answer is option 'C'. Can you explain this answer?

Question

Answer

We fill up electron in increasing energy order.in which electronic configuration n+l value is greater, it's energy also will be greater.but here n+l value is same.so we shall consider n(principle quantum number).in which electronic configuration n value is greater it's energy also will bë greater.there for option C is correct.

Answer

It will follow n+l rule ji in case n+l value is same for two orbital then lower value of n will be preferred as in this case all have n+l value 5 but e- will go to orbital which has lesser value for n ie 3 in this case

Answer

We fill up electron in increasing energy order.in which electronic configuration n+l value is greater, it's energy also will be greater.but here n+l value is same.so we shall consider n(principle quantum number).in which electronic configuration n value is greater it's energy also will be greater.there for option C is correct.

Answer

Explanation:

To understand why the correct answer is option C, let's first review the quantum numbers involved.

Quantum numbers are used to describe the energy levels and sublevels of electrons in an atom. They provide information about the size, shape, and orientation of the electron orbitals.

The four quantum numbers are:

1. Principal quantum number (n): This represents the energy level or shell in which the electron is located. It can have any positive integer value (1, 2, 3, ...).

2. Azimuthal quantum number (l): This determines the shape of the orbital and is related to the angular momentum of the electron. It can have values ranging from 0 to (n-1).

3. Magnetic quantum number (ml): This specifies the orientation of the orbital in space. It can have values ranging from -l to +l.

4. Spin quantum number (ms): This describes the spin of the electron and can have values of +1/2 or -1/2.

Now, let's analyze the given options and determine which orbital the electrons will first enter.

Option A: n = 5, l = 0
This represents the 5s orbital, which is a spherical orbital with no angular nodes. However, the 1s, 2s, 3s, and 4s orbitals are lower in energy compared to the 5s orbital. Therefore, electrons will first enter the lower energy orbitals before reaching the 5s orbital.

Option B: n = 4, l = 1
This represents the 4p orbital, which is a dumbbell-shaped orbital with one angular node. The 1s, 2s, 3s, 4s, and 3p orbitals are lower in energy compared to the 4p orbital. Therefore, electrons will first enter the lower energy orbitals before reaching the 4p orbital.

Option C: n = 3, l = 2
This represents the 3d orbital, which has a more complex shape with two angular nodes. The 1s, 2s, 3s, 4s, 3p, and 4p orbitals are lower in energy compared to the 3d orbital. Therefore, electrons will first enter the lower energy orbitals before reaching the 3d orbital.

Option D: any of these
This option is not correct because electrons follow a specific order of filling orbitals based on their energy levels. They will first enter the orbitals with lower energy before moving to higher energy orbitals.

Therefore, the correct answer is option C (n = 3, l = 2). Electrons will first enter the orbital with these quantum numbers, which corresponds to the 3d orbital.

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