The numbers of radial nodes of `3s and 2p` orbitals are respectively:

Options

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

Explanation

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

### Step 1: Understand the concept of nodes
A node is a point 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:
- \( n \) is the principal quantum number (indicates the shell of the orbital),
- \( l \) is the azimuthal quantum number (indicates the subshell of the orbital).

### Step 3: Determine the values of \( n \) and \( l \) for the 3s orbital
For the 3s orbital:
- The principal quantum number \( n = 3 \).
- The azimuthal quantum number \( l \) for s orbitals is \( 0 \).

### Step 4: Calculate the number of radial nodes for the 3s orbital
Using the formula:
\[ \text{Radial nodes for 3s} = n - l - 1 = 3 - 0 - 1 = 2 \]

### Step 5: Determine the values of \( n \) and \( l \) for the 2p orbital
For the 2p orbital:
- The principal quantum number \( n = 2 \).
- The azimuthal quantum number \( l \) for p orbitals is \( 1 \).

### Step 6: Calculate the number of radial nodes for the 2p orbital
Using the formula:
\[ \text{Radial nodes for 2p} = n - l - 1 = 2 - 1 - 1 = 0 \]

### Step 7: State the final answer
The number of radial nodes for the 3s and 2p orbitals are respectively:
- 3s: 2 radial nodes
- 2p: 0 radial nodes

Thus, the answer is:
**2 and 0**

---