The number of radial nodes of 3s and 2s orbital are respectively:

Options

A. 2, 1
B. 0, 2
C. 1, 2
D. 2, 11

Explanation

To determine the number of radial nodes in the 3s and 2s orbitals, we can follow these steps:

### Step 1: Understand the Concept of Nodes
A node is a region in an atom where the probability of finding an electron is zero. There are two types of nodes: radial nodes and angular nodes.

### Step 2: Identify the Formula for Radial Nodes
The number of radial nodes can be calculated using the formula:
\[ \text{Number of Radial Nodes} = n - l - 1 \]
where:
- \( n \) = principal quantum number (indicates the energy level)
- \( l \) = azimuthal quantum number (indicates the subshell)

### Step 3: Determine the Values of \( n \) and \( l \) for 3s Orbital
For the 3s orbital:
- The principal quantum number \( n = 3 \)
- The azimuthal quantum number \( l = 0 \) (since s orbitals have \( l = 0 \))

Now, substitute these values into the formula:
\[ \text{Radial Nodes for 3s} = 3 - 0 - 1 = 2 \]

### Step 4: Determine the Values of \( n \) and \( l \) for 2s Orbital
For the 2s orbital:
- The principal quantum number \( n = 2 \)
- The azimuthal quantum number \( l = 0 \) (since s orbitals have \( l = 0 \))

Now, substitute these values into the formula:
\[ \text{Radial Nodes for 2s} = 2 - 0 - 1 = 1 \]

### Step 5: State the Final Answer
The number of radial nodes for the 3s and 2s orbitals are:
- 3s: 2 radial nodes
- 2s: 1 radial node

Thus, the answer is:
**The number of radial nodes of 3s and 2s orbitals are respectively: 2 and 1.**

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