Question

How many nodes are present in \(3 \mathrm{~s}, 3 \mathrm{p}\) and \(3 \mathrm{~d}\) orbitals?

Short answer

Answer: There are 2 nodes present in each of the \(3s, 3p,\) and \(3d\) orbitals.

Step-by-step solution

Recall the formula for calculating nodes

The formula for calculating the total number of nodes in an orbital is given by: Nodes = n - 1 where n is the principal quantum number.

Calculate nodes in 3s orbital

For 3s orbital, the principal quantum number (n) is 3. Using the formula, we find the total number of nodes: Nodes in 3s = 3 - 1 = 2

Calculate nodes in 3p orbital

For 3p orbital, the principal quantum number (n) is again 3. Using the formula, we find the total number of nodes: Nodes in 3p = 3 - 1 = 2

Calculate nodes in 3d orbital

For 3d orbital, the principal quantum number (n) is 3. Using the formula, we find the total number of nodes: Nodes in 3d = 3 - 1 = 2 So, there are 2 nodes present in each of the \(3s, 3p,\) and \(3d\) orbitals.