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The number of

**nodes**is related to the principal quantum number, n. The ns**orbital**has (n-1)**radial nodes**, so the**4s**-**orbital**has (4-1) = 3**nodes**, as shown in the above plot.

Subsequently, one may also ask, how many radial nodes are present in 4s orbital?

3

**nodes**present in this

**orbital**is equal to n-1. In this case, 3-1=2, so there are 2 total

**nodes**. The quantum number ℓ determines the number of angular

**nodes**; there is 1 angular

**node**, specifically on the xy plane because this is a p

_{z}

**orbital**.

Keeping this in view, how many nodes can a 4s orbital have?

three nodes

**There are two types of node: radial and angular.**

- The number of angular nodes is always equal to the orbital angular momentum quantum number, l.
- The number of radial nodes = total number of nodes minus number of angular nodes = (n-1) - l.