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12 June, 19:35

How many electrons in an atom can have each of the following quantum number or sublevel designations?

(a) 2s

(b) n = 3, l = 2

(c) 6d

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  1. 12 June, 23:18
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    (a) Number of electrons in an atoms is, 2

    (b) Number of electrons in an atoms is, 10

    (c) Number of electrons in an atoms is, 10

    Explanation:

    There are 4 quantum numbers:

    Principle Quantum Numbers : It describes the size of the orbital. It is represented by n. n = 1,2,3,4 ...

    Azimuthal Quantum Number : It describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1). For l = 0,1,2,3 ... the orbitals are s, p, d, f ...

    Magnetic Quantum Number : It describes the orientation of the orbitals. It is represented as. The value of this quantum number ranges from. When l = 2, the value of

    Spin Quantum number : It describes the direction of electron spin. This is represented as. The value of this is for upward spin and for downward spin.

    Number of electrons in a sublevel = 2 (2l+1)

    (a) 2s

    n = 2

    Value of 'l' for 's' orbital : l = 0

    Number of electrons in an atoms = 2 (2l+1) = 2 (2*0+1) = 2

    (b) n = 3, l = 2

    Number of electrons in an atoms = 2 (2l+1) = 2 (2*2+1) = 10

    (c) 6d

    n = 2

    Value of 'l' for 'd' orbital : l = 2

    Number of electrons in an atoms = 2 (2l+1) = 2 (2*2+1) = 10
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