`{:("Type - I","Type - II"),("Property","Element with the highest value"),("(A) IP","(1) Cl"),("(B) EN","(2) Cs"),("(C ) EA","(3) He"),("(D) atomic size","(4) F"),(,"(5) H"):}`

Options

A. A-1, B-2, C-3, D-4
B. A-3, B-4, C-1, D-2
C. A-4, B-3, C-5, D-2
D. A-5, B-1, C-2, D-3

Answer

To solve the question regarding the properties and the elements with the highest values for each property, we will analyze each property step by step.

### Step 1: Identify the Properties and Elements
We have four properties to analyze:
1. Ionization Potential (IP)
2. Electronegativity (EN)
3. Electron Affinity (EA)
4. Atomic Size

The elements provided are:
- Chlorine (Cl)
- Cesium (Cs)
- Helium (He)
- Fluorine (F)
- Hydrogen (H)

### Step 2: Determine the Element with the Highest Ionization Potential (IP)
- **Definition**: Ionization potential is the energy required to remove an electron from an isolated gaseous atom.
- **Trend**: Ionization potential increases across a period and decreases down a group.
- **Analysis**: Among the given elements, Helium (He) has the highest ionization potential because it is a noble gas with a stable electron configuration (1s²) and a small atomic size.
- **Conclusion**: **He** has the highest IP.

### Step 3: Determine the Element with the Highest Electronegativity (EN)
- **Definition**: Electronegativity is the tendency of an atom to attract electrons in a chemical bond.
- **Trend**: Electronegativity increases across a period and decreases down a group.
- **Analysis**: Fluorine (F) is the most electronegative element in the periodic table.
- **Conclusion**: **F** has the highest EN.

### Step 4: Determine the Element with the Highest Electron Affinity (EA)
- **Definition**: Electron affinity is the energy change when an electron is added to a neutral atom in the gas phase.
- **Trend**: Electron affinity generally increases across a period and decreases down a group.
- **Analysis**: Chlorine (Cl) has the highest electron affinity among the halogens due to its ability to attract an additional electron effectively, despite the small size of Fluorine causing inter-electronic repulsion.
- **Conclusion**: **Cl** has the highest EA.

### Step 5: Determine the Element with the Largest Atomic Size
- **Definition**: Atomic size refers to the distance from the nucleus to the outermost shell of electrons.
- **Trend**: Atomic size increases down a group and decreases across a period.
- **Analysis**: Cesium (Cs) is located at the bottom of Group 1 and has the largest atomic size among the given elements.
- **Conclusion**: **Cs** has the largest atomic size.

### Summary of Results
- Ionization Potential (IP): **He**
- Electronegativity (EN): **F**
- Electron Affinity (EA): **Cl**
- Atomic Size: **Cs**

### Final Answer
Based on the analysis:
- (A) IP: (1) He
- (B) EN: (4) F
- (C) EA: (1) Cl
- (D) Atomic Size: (2) Cs