The electronegativity of cesium is 0.7 and that of flourine is 4.0 The bond formed between the two is:

Options

A. Covalent
B. Electrovalent
C. Coordinate
D. Metallic .

Answer

To determine the type of bond formed between cesium (Cs) and fluorine (F) based on their electronegativities, we can follow these steps:

### Step 1: Identify the Electronegativity Values
- The electronegativity of cesium (Cs) is 0.7.
- The electronegativity of fluorine (F) is 4.0.

### Step 2: Calculate the Difference in Electronegativity
- The difference in electronegativity between fluorine and cesium can be calculated as follows:
\[ \text{Difference} = \text{Electronegativity of F} - \text{Electronegativity of Cs} = 4.0 - 0.7 = 3.3 \]

### Step 3: Determine the Type of Bond Based on the Difference
- A difference in electronegativity greater than 1.7 typically indicates the formation of an ionic bond. In this case, the difference is 3.3, which is significantly higher than 1.7.

### Step 4: Conclude the Type of Bond
- Since cesium has a low electronegativity and fluorine has a high electronegativity, cesium will lose its electron and fluorine will gain it. This results in the formation of positively charged cesium ions (Cs⁺) and negatively charged fluoride ions (F⁻).
- The bond formed between cesium and fluorine is therefore an ionic bond.

### Step 5: Identify the Compound Formed
- The compound formed by cesium and fluorine is cesium fluoride (CsF), which is ionic in nature.

### Final Answer
The bond formed between cesium and fluorine is an **ionic bond**.

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