Amongst the following elements whose
electronic configuration are given below, the
one having the highest ionisation enthalpy is

Options

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

Explanation

To determine which element has the highest ionization enthalpy among the given electronic configurations, we will analyze the configurations step by step.

### Step 1: Identify the Elements
The electronic configurations provided are:
1. 3S² 3P¹
2. 3S² 3P³
3. 3S² 3P²
4. Argon: 3S² 3P⁶
5. 3D¹⁰ 4S² 4P³

### Step 2: Determine the Period of Each Element
- The first three configurations (1, 2, and 3) belong to the 3rd period of the periodic table.
- Argon (4) is also in the 3rd period.
- The last configuration (5) belongs to the 4th period.

### Step 3: Understand Ionization Energy Trends
- Ionization energy generally increases across a period (left to right) and decreases down a group (top to bottom).
- Since Argon is a noble gas with a full outer shell (3S² 3P⁶), it will have a very high ionization energy compared to other elements in the 3rd period.

### Step 4: Compare the Elements in the 3rd Period
- Among the elements in the 3rd period:
- 3S² 3P¹ (Aluminum) has 3 valence electrons.
- 3S² 3P² (Silicon) has 4 valence electrons.
- 3S² 3P³ (Phosphorus) has 5 valence electrons.
- The more electrons in the p-orbital, the higher the ionization energy due to increased nuclear charge and stability.

### Step 5: Analyze the 4th Period Element
- The last configuration (3D¹⁰ 4S² 4P³) is from the 4th period and will have lower ionization energy than the 3rd period elements due to being further down the group.

### Conclusion
Based on the analysis:
- Argon (3S² 3P⁶) has the highest ionization enthalpy among the given configurations due to its full outer shell and being a noble gas.

### Final Answer
The element with the highest ionization enthalpy is Argon (3S² 3P⁶).

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