Question

Orbital having 3 angular nodes and 3 total nodes is :-

• A. 5 p
• B. 3 d
• C. 4 f
• D. 6 d

Answer 1

The Correct Option is C

To solve this question, we need to understand the concept of nodes in atomic orbitals. Nodes are regions in an atom where the probability of finding an electron is zero. There are two types of nodes:

• Radial nodes: Also known as spherical nodes, these occur in regions between the nucleus and the outer shell.
• Angular nodes: Also known as planar nodes, these depend on the angular part of the wavefunction and relate to the shape of the orbital.

The total number of nodes in an orbital is given by the formula:

n - 1

Where n is the principal quantum number.

The number of angular nodes is equal to l (the azimuthal quantum number), which defines the shape of the orbital:

• For s-orbitals, l = 0
• For p-orbitals, l = 1
• For d-orbitals, l = 2
• For f-orbitals, l = 3

Given in the question, the orbital has 3 angular nodes and 3 total nodes. This implies:

l = 3 (since there are 3 angular nodes)

Total nodes = n - 1 = 3

From the equation n - 1 = 3, we get n = 4.

Therefore, the orbital is 4f because:

• Principal quantum number n = 4
• Angular quantum number l = 3

Thus, the orbital having 3 angular nodes and 3 total nodes is the 4f orbital, confirming that the correct answer is 4 f.