Which of the following sets of quantum numbers represents the highest energy of an atom?

  • Option 1)

    n= 3, l = 0, m = 0,s = +\frac{1}{2}

  • Option 2)

    n= 3, l = 1, m = 1,s = +\frac{1}{2}

  • Option 3)

    n= 3, l = 2, m = 1,s = +\frac{1}{2}

  • Option 4)

    n= 4, l = 0, m = 0,s = +\frac{1}{2}

 

Answers (3)

As we learnt in 

Principal Quantum Number (n) -

 It is a positive integer with value of n = 1,2,3.......

-

 

Azimuthal Quantum Number(l) -

For a given value of n, l can have n values ranging from 0 to n – 1, that is, for a given value of n, the possible value of l are : l = 0, 1, 2, ....( n –1)

-

 

Energy of orbital is directly proportional to (n+l) value

n=3,l=0\: \: represents\: 3s\: \: orbital

n=3,l=1\: \: represents\: 3p\: \: orbital

n=3,l=2\: \: represents\: 3d\: \: orbital

n=4,l=0\: \: represents\: 4s\: \: orbital

The order of increasing energy of the orbitals is

3s< 3p< 4s< 3d

3d has n=3 and l=2


Option 1)

n= 3, l = 0, m = 0,s = +\frac{1}{2}

Incorrect option

Option 2)

n= 3, l = 1, m = 1,s = +\frac{1}{2}

Incorrect option

Option 3)

n= 3, l = 2, m = 1,s = +\frac{1}{2}

Correct option

Option 4)

n= 4, l = 0, m = 0,s = +\frac{1}{2}

Incorrect option

3rd option is crct.....bcoz here  the value of (n+l) is highest.....

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