In a hypothetical system, all the known concepts of shell, subshell, orbitals, etc., exist in the same way as in our system except that the (n + 1) rule is modified to (n - 1) rule for deciding the subshell energy. In case of equal value of (n - 1), the higher value of n gives the higher energy.
In this hypothetical system S (Z = 16) will be 

Options

A. p-block element
B. s-block element
C. d-block element
D. f-block element

Answer

To solve the question regarding the hypothetical system where the (n + l) rule is modified to the (n - l) rule, we need to determine the electron configuration for sulfur (S) with atomic number Z = 16. Here’s a step-by-step breakdown of the solution:

### Step 1: Identify the Electron Configuration
In the standard system, the electron configuration of sulfur (Z = 16) is:
1s² 2s² 2p⁶ 3s² 3p⁴

### Step 2: Determine the Subshells and Their Values of n and l
In the standard system:
- 1s: n = 1, l = 0
- 2s: n = 2, l = 0
- 2p: n = 2, l = 1
- 3s: n = 3, l = 0
- 3p: n = 3, l = 1

### Step 3: Calculate (n - l) for Each Subshell
Now, we calculate (n - l) for each subshell:
- 1s: 1 - 0 = 1
- 2s: 2 - 0 = 2
- 2p: 2 - 1 = 1
- 3s: 3 - 0 = 3
- 3p: 3 - 1 = 2

### Step 4: Compare (n - l) Values
Now, we compare the (n - l) values:
- 1s: 1
- 2s: 2
- 2p: 1
- 3s: 3
- 3p: 2

### Step 5: Determine the Order of Energy Levels
According to the modified rule, we first look at (n - l) values. The lower the (n - l) value, the lower the energy. If two subshells have the same (n - l), we choose the one with the higher n value. The order of energy levels becomes:
1. 1s (1)
2. 2p (1) → but 2s (2) is higher than 2p
3. 2s (2)
4. 3p (2) → but 3s (3) is higher than 3p
5. 3s (3)

### Step 6: Write the Electron Configuration in the Hypothetical System
Following the order determined above, the electron filling will be:
1s² 2s² 2p⁶ 3s² 3p⁴

### Final Electron Configuration
Thus, in this hypothetical system, the electron configuration for sulfur (Z = 16) remains the same:
**1s² 2s² 2p⁶ 3s² 3p⁴**