The nodes present in 3p-orbitals are

Options

A. two spherical
B. two planar
C. one planar
D. one planar,one spherical

Answer

To determine the number of nodes present in the 3p orbital, we can follow these steps:

### Step 1: Understand the Concept of Nodes
A node is a point or region in an atom where the probability of finding an electron is zero. There are two types of nodes:
- **Radial (spherical) nodes**: These are spherical surfaces where the probability density is zero.
- **Angular (planar) nodes**: These are non-spherical and represent regions where the probability density is zero due to angular momentum.

### Step 2: Identify Quantum Numbers
For the 3p orbital:
- The **principal quantum number (n)** is 3 (the number before the letter).
- The **azimuthal quantum number (l)** for p orbitals is 1.

### Step 3: Calculate the Number of Spherical Nodes
The formula for calculating the number of spherical nodes is:
\[ \text{Number of spherical nodes} = n - l - 1 \]
Substituting the values:
\[ \text{Number of spherical nodes} = 3 - 1 - 1 = 1 \]

### Step 4: Calculate the Total Number of Nodes
The total number of nodes is given by:
\[ \text{Total nodes} = n - 1 \]
Substituting the value of n:
\[ \text{Total nodes} = 3 - 1 = 2 \]

### Step 5: Calculate the Number of Planar Nodes
The total number of nodes is the sum of spherical and planar nodes:
\[ \text{Total nodes} = \text{Planar nodes} + \text{Spherical nodes} \]
Rearranging gives:
\[ \text{Planar nodes} = \text{Total nodes} - \text{Spherical nodes} \]
Substituting the values:
\[ \text{Planar nodes} = 2 - 1 = 1 \]

### Conclusion
In the 3p orbital, there is:
- **1 spherical node**
- **1 planar node**

Thus, the nodes present in the 3p orbital are 1 spherical node and 1 planar node.

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