the configuration `[Ar]3d^(10)4s^(2)4p^(4)` is similar to that of :

Options

A. boron
B. oxygen
C. sulphur
D. aluminium

Answer

To solve the question regarding the electronic configuration `[Ar] 3d^(10) 4s^(2) 4p^(4)`, we need to identify which of the given options has a similar electronic configuration. Here’s a step-by-step breakdown of the solution:

### Step 1: Understand the Given Configuration
The configuration `[Ar] 3d^(10) 4s^(2) 4p^(4)` indicates that the element has:
- The electron configuration of Argon `[Ar]`, which accounts for 18 electrons.
- 10 electrons in the 3d subshell.
- 2 electrons in the 4s subshell.
- 4 electrons in the 4p subshell.

### Step 2: Identify the Total Number of Electrons
To find the total number of electrons represented by this configuration:
- Argon contributes 18 electrons.
- 3d contributes 10 electrons.
- 4s contributes 2 electrons.
- 4p contributes 4 electrons.

Total = 18 + 10 + 2 + 4 = 34 electrons.

### Step 3: Determine the Element
The total number of electrons (34) corresponds to the element Selenium (Se), which is located in Group 16 of the periodic table.

### Step 4: Analyze the Given Options
Now, we need to analyze the electronic configurations of the provided options:
1. **Boron (B)**: 1s² 2s² 2p¹ (5 electrons)
2. **Oxygen (O)**: 1s² 2s² 2p⁴ (8 electrons)
3. **Sulfur (S)**: [Ne] 3s² 3p⁴ (16 electrons)
4. **Aluminum (Al)**: [Ne] 3s² 3p¹ (13 electrons)

### Step 5: Compare with the Given Configuration
We are looking for a configuration that matches the pattern of having an inert gas core followed by ns² and np⁴:
- The configuration `[Ar] 3d^(10) 4s^(2) 4p^(4)` indicates that we need a configuration that has a noble gas core followed by 2 electrons in the s subshell and 4 electrons in the p subshell.

Among the options:
- **Sulfur (S)** has the configuration [Ne] 3s² 3p⁴, which matches the ns² np⁴ pattern.

### Conclusion
The configuration `[Ar] 3d^(10) 4s^(2) 4p^(4)` is similar to that of **Sulfur (S)**.

### Final Answer
**Sulfur (S)**