Correct order of the property indicated below`-`

Options

A. `Na gt Al gt Mg gt Si" "IE_(1)`
B. `F gt O gt Cl gt S" "EN`
C. `Cl gt S gt O gt F" "DeltaHeg_(1)`
D. `Cl gt O gt F gt S" "EA_(1)`

Explanation

To solve the question regarding the correct order of the given properties, we will analyze each property step by step.

### Step 1: Analyzing Ionization Energy
1. **Understanding Ionization Energy**: Ionization energy is the energy required to remove an electron from a gaseous atom.
2. **Trend Across a Period**: As we move from left to right across a period, the effective nuclear charge increases, leading to a decrease in atomic size. This results in an increase in ionization energy.
3. **Elements in Consideration**: The elements given are sodium (Na), aluminum (Al), magnesium (Mg), and silicon (Si).
4. **Correct Order**:
- Sodium (Na) has the lowest ionization energy because it is on the far left.
- Magnesium (Mg) will have a higher ionization energy than sodium.
- Aluminum (Al) has a higher ionization energy than magnesium.
- Silicon (Si) has the highest ionization energy among these elements.
5. **Final Order**: The correct order of ionization energy from lowest to highest is:
- Na < Mg < Al < Si.

### Step 2: Analyzing Electronegativity
1. **Understanding Electronegativity**: Electronegativity is the tendency of an atom to attract electrons in a bond.
2. **Trend in Electronegativity**: Electronegativity generally increases across a period from left to right.
3. **Elements in Consideration**: The elements given are chlorine (Cl), oxygen (O), and sulfur (S).
4. **Electronegativity Values**:
- Fluorine (F) = 4.0 (highest)
- Oxygen (O) = 3.5
- Chlorine (Cl) = 3.0
- Sulfur (S) = 2.5
5. **Final Order**: The correct order of electronegativity from highest to lowest is:
- F > O > Cl > S.

### Step 3: Analyzing Electron Gain Enthalpy
1. **Understanding Electron Gain Enthalpy**: This is the enthalpy change when an electron is added to a neutral gaseous atom.
2. **Trend in Electron Gain Enthalpy**: Generally, more electronegative elements have higher (more negative) electron gain enthalpy.
3. **Elements in Consideration**: The elements given are chlorine (Cl), oxygen (O), and sulfur (S).
4. **Electron Gain Enthalpy Values**:
- Cl: -349 kJ/mol
- O: -200 kJ/mol
- S: -141 kJ/mol
5. **Final Order**: The correct order of electron gain enthalpy from most negative to least negative is:
- Cl < O < S.

### Step 4: Analyzing Electron Affinity
1. **Understanding Electron Affinity**: This is the energy change when an electron is added to a neutral atom.
2. **Trend in Electron Affinity**: Generally, smaller atoms have higher electron affinity due to less electron-electron repulsion.
3. **Elements in Consideration**: The elements given are chlorine (Cl), fluorine (F), oxygen (O), and sulfur (S).
4. **Electron Affinity Values**:
- Cl: -349 kJ/mol
- F: -328 kJ/mol
- O: -200 kJ/mol
- S: -141 kJ/mol
5. **Final Order**: The correct order of electron affinity from highest to lowest is:
- F > Cl > O > S.

### Summary of Correct Orders:
1. **Ionization Energy**: Na < Mg < Al < Si
2. **Electronegativity**: F > O > Cl > S
3. **Electron Gain Enthalpy**: Cl < O < S
4. **Electron Affinity**: F > Cl > O > S