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The total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 is [1990]
- a)2
- b)4
- c)6
- d)8
Correct answer is option 'C'. Can you explain this answer?
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The total number of electrons that can be accommodated in all the orbi...
n = 2, l = 1 means 2 p – orbital. Electrons that can be accommodated = 6 as p sub-shell has 3 orbital and each orbital contains 2 electrons.
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The total number of electrons that can be accommodated in all the orbi...
Total number of electrons in orbitals with n=2 and l=1
First, let's understand what principal quantum number (n) and azimuthal quantum number (l) mean. The principal quantum number (n) determines the energy level of an electron, and the azimuthal quantum number (l) determines the shape of the orbital.
For n=2, the possible values of l are 0 and 1. When l=1, it corresponds to the p orbital, which has three sub-orbitals. Each sub-orbital can have a maximum of 2 electrons (according to the Pauli exclusion principle).
So, to find the total number of electrons that can be accommodated in the orbitals with n=2 and l=1, we need to add up the number of electrons in each sub-orbital.
Number of electrons in each sub-orbital
Each sub-orbital can hold a maximum of 2 electrons, so:
- px sub-orbital can hold 2 electrons
- py sub-orbital can hold 2 electrons
- pz sub-orbital can hold 2 electrons
Total number of electrons
Adding up the number of electrons in each sub-orbital, we get:
2 + 2 + 2 = 6
Therefore, the total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 is 6. Hence, the correct answer is option (c).
First, let's understand what principal quantum number (n) and azimuthal quantum number (l) mean. The principal quantum number (n) determines the energy level of an electron, and the azimuthal quantum number (l) determines the shape of the orbital.
For n=2, the possible values of l are 0 and 1. When l=1, it corresponds to the p orbital, which has three sub-orbitals. Each sub-orbital can have a maximum of 2 electrons (according to the Pauli exclusion principle).
So, to find the total number of electrons that can be accommodated in the orbitals with n=2 and l=1, we need to add up the number of electrons in each sub-orbital.
Number of electrons in each sub-orbital
Each sub-orbital can hold a maximum of 2 electrons, so:
- px sub-orbital can hold 2 electrons
- py sub-orbital can hold 2 electrons
- pz sub-orbital can hold 2 electrons
Total number of electrons
Adding up the number of electrons in each sub-orbital, we get:
2 + 2 + 2 = 6
Therefore, the total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 is 6. Hence, the correct answer is option (c).
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The total number of electrons that can be accommodated in all the orbitals having principal quantum number 2 and azimuthal quantum number 1 is [1990]a)2b)4c)6d)8Correct answer is option 'C'. Can you explain this answer?
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