Which one of the following elements has the highest ionisation energy?

Options

A. `[Ne] 3s^(2)3p^(3)`
B. `[Ne]3s^(2)3p^(2)`
C. `[Ar] 3d^(10),4s^(2) 4 p^(3)`
D. `[Ne] 3s^(2) 3p^(1)`

Explanation

To determine which element has the highest ionization energy among the given options, we can follow these steps:

### Step 1: Understand Ionization Energy
Ionization energy is the energy required to remove an electron from an isolated atom in its gaseous state. It is a measure of how strongly an atom holds onto its electrons.

**Hint:** Remember that ionization energy increases with increasing nuclear charge and decreases with increasing atomic size.

### Step 2: Consider Atomic Size
Ionization energy is inversely proportional to atomic size. This means that as the atomic size increases, the ionization energy decreases. Larger atoms have their outermost electrons farther from the nucleus, making them easier to remove.

**Hint:** Compare the atomic sizes of the elements in the options provided.

### Step 3: Evaluate Electronic Configuration
Elements with stable electronic configurations (such as noble gases) tend to have higher ionization energies. Half-filled and fully filled subshells are particularly stable configurations.

**Hint:** Look for elements with noble gas configurations or half-filled configurations in the options.

### Step 4: Analyze the Given Options
Assuming we have options A, B, C, and D, we need to analyze each one based on their atomic sizes and electronic configurations:

- **Option A:** If this is a noble gas or has a stable configuration, it likely has a high ionization energy.
- **Option B:** If this element is larger in size or has a less stable configuration, it may have lower ionization energy.
- **Option C:** Similar analysis as Option B.
- **Option D:** If this element has one electron in its outermost shell, it is likely to have the lowest ionization energy.

**Hint:** Identify which option corresponds to a noble gas or has a stable electronic configuration.

### Step 5: Conclusion
After analyzing the options based on atomic size and electronic configuration, we can conclude which element has the highest ionization energy.

If Option A is the noble gas or has a stable configuration, it would be the correct answer.

**Final Answer:** The element with the highest ionization energy is **Option A**.