Total number of nodes (planar and spherical) present in the 5f-orbital is

Explanation

To find the total number of nodes (planar and spherical) present in the 5f orbital, we can follow these steps:

### Step 1: Understand the concept of nodes
Nodes are regions in an atom where the probability of finding an electron is zero. There are two types of nodes:
- Planar nodes (which are flat surfaces)
- Spherical nodes (which are spherical shells)

### Step 2: Identify the principal quantum number (n)
For the 5f orbital, the principal quantum number (n) is 5. The principal quantum number indicates the energy level of the electron in an atom.

### Step 3: Use the formula for total nodes
The total number of nodes in an orbital can be calculated using the formula:
\[ \text{Total Nodes} = n - 1 \]
Where \( n \) is the principal quantum number.

### Step 4: Calculate the total number of nodes
Substituting the value of \( n \):
\[ \text{Total Nodes} = 5 - 1 = 4 \]

### Step 5: Conclusion
Thus, the total number of nodes present in the 5f orbital is 4.

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