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Home » Class 11 » Chemistry » Structure of Atom » Shapes of Atomic Orbital

Shapes of Atomic Orbital

Last Updated on February 16, 2023 By Mrs Shilpi Nagpal

An orbital is the region of space around the nucleus within which the probability of finding an electron of given energy is maximum.

The probability at any point around the nucleus is calculated using schrodinger wave equation and is represented by the density of the points.

Shape of s orbital

For the coordinates( x, y, z) of the electron with respect to the nucleus, schrodinger Wave equation can be solved to get the values of the orbital wave function ψ. But Ψ has no physical significance. The square ψ2  has the significance as it gives the electron probability density of the electron at that point.

1) The probability of 1s electron is found to be maximum near the nucleus and decreases as the distance from the nucleus increases.

2) In case of 2s electrons, the probability is again maximum near the nucleus and then decreases to zero and increases again and then decreases as a distance from the nucleus increases.

3) The intermediate region where probability is zero is called nodal surface or node.

Nodes in s orbital

2s orbital differ from 1s orbital in having node within it.3s has two nodes.Any ns orbital has ( n-1) nodes.

S orbital

1) The probability of finding the electron belonging to a s orbital of any main shell is found to be identical in all directions at a given distance from the nucleus. Hence s – orbital is spherical in shape which is symmetrical around the nucleus.

2) For s orbital azimuthal quantum number l = 0. Magnetic quantum number m is also equal to 0.s orbital has only one orientation. The only shape having one orientation is a sphere. s orbital is spherical in shape.

1s, 2s, 3s etc all have spherical shape, they differ in:

1) the number of nodes

2) size and energy. These increases with increase in principal quantum number, n.

Shapes of P orbital

Shapes of p orbital

It is found that the probability of finding the electron is maximum in two lobes on the opposite side of the nucleus. This gives rise to dumb-bell shape for the p orbital.

The probability of finding a particular P electron is equal in both the lobes. There is a plane passing through the nucleus on which the probability of finding the electron is almost zero. This is called a nodal plane.

For p orbital l= 1, m = -1, 0, +1 .Thus  p orbital has three different orientation designated as px, py, pz  depending upon whether the electron density is maximum along the x-axis,  y axis and Z axis.

P orbital have directional characteristics and hence are helpful in predicting the shape of molecules.

As n increases these p orbitals become larger in size and have higher energies. The three p orbitals belonging to a particular energy shells have equal energies and are called degenerate.

Shapes of d orbital

For d orbital, l=2.Hence m= -2, -1, 0, +1, +2

There are 5 d orbitals, depending upon the axes along which or between which their electron clouds are concentrated, their names and shapes are:

shapes of d orbital

 

d z2 has a doughnut shaped electron cloud in the centre whereas  others clover leaf shape.

Number of nodes in any orbital= (n – l -1)

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Filed Under: Chemistry, Class 11, Structure of Atom Tagged With: d orbital, nodal surface, node, orbital, p orbital, s orbital

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Comments

  1. Sneha says

    July 26, 2018 at 3:55 pm

    Easy to understand

  2. Sneha says

    July 26, 2018 at 4:03 pm

    Very useful

  3. Swep says

    October 10, 2018 at 9:23 am

    Very well explained

  4. Mohit Patel says

    February 27, 2019 at 9:02 pm

    Mam Please make Chemistry and Physics notes for class 12th

  5. Mrs Shilpi Nagpal says

    February 28, 2019 at 5:58 pm

    Sure, i m working on it.

  6. Sonam pavecha says

    May 23, 2019 at 1:47 am

    Can you please give 11th all chapter notes in pdf formate .Please mam

  7. Pargaty parashar says

    October 7, 2019 at 12:14 pm

    so nice notes it makes the topic easy to understand

  8. TANISHKA says

    July 8, 2020 at 6:37 pm

    well explained!
    keep helping students
    thanks:)

  9. Gannadheesh says

    September 6, 2020 at 4:17 pm

    thank you mam

  10. Sharanu Kandagal says

    October 2, 2020 at 1:50 pm

    Amazing explanation mam it’s very easy to understand thank you so much for sharing a good knowledge

  11. Sumairah says

    October 17, 2020 at 8:25 am

    Very useful.

  12. Shashi R says

    November 13, 2020 at 12:54 pm

    very easy to understand

  13. nadwa says

    February 28, 2021 at 11:51 am

    very understandable

  14. Nitin says

    January 5, 2022 at 6:15 am

    Very useful app

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