A `5g` orbital has

Options

A. Zero angular node and zero radial node
B. Zero radial node and two angular nodes
C. `4` radial nodes and `4` angular nodes
D. Zero radial node and `4` angular nodes

Explanation

To solve the question regarding the properties of a 5G orbital, we will follow these steps:

### Step 1: Identify the principal quantum number (n)
The principal quantum number (n) for the 5G orbital is given as 5.

### Step 2: Calculate the total number of nodes
The total number of nodes in an orbital can be calculated using the formula:
\[ \text{Total nodes} = n - 1 \]
Substituting the value of n:
\[ \text{Total nodes} = 5 - 1 = 4 \]

### Step 3: Determine the azimuthal quantum number (l)
For a G orbital, the azimuthal quantum number (l) is equal to 4.

### Step 4: Calculate the number of radial nodes
The number of radial nodes can be calculated using the formula:
\[ \text{Radial nodes} = n - l - 1 \]
Substituting the values of n and l:
\[ \text{Radial nodes} = 5 - 4 - 1 = 0 \]

### Step 5: Calculate the number of angular nodes
The number of angular nodes can be calculated using the formula:
\[ \text{Angular nodes} = l \]
Since l = 4:
\[ \text{Angular nodes} = 4 \]

### Step 6: Summarize the findings
- Total nodes: 4
- Radial nodes: 0
- Angular nodes: 4

### Conclusion
The correct option regarding the 5G orbital is that it has 0 radial nodes and 4 angular nodes.