The electronegativities of two elements are 0.7 and 3.0. The bond formed between them would be

Options

A. Ionic
B. Covalent
C. Co-ordinate covalent
D. Metallic

Answer

To determine the type of bond formed between two elements with electronegativities of 0.7 and 3.0, we can follow these steps:

### Step 1: Calculate the difference in electronegativity (ΔX)
The difference in electronegativity (ΔX) is calculated as follows:
\[ \Delta X = |3.0 - 0.7| = 2.3 \]

### Step 2: Use the formula for percentage ionic character
We can use the formula for percentage ionic character:
\[ \text{Percentage Ionic Character} = 16 \Delta X + 3.5 \Delta X^2 \]

### Step 3: Substitute ΔX into the formula
Substituting ΔX = 2.3 into the formula:
\[ \text{Percentage Ionic Character} = 16(2.3) + 3.5(2.3)^2 \]

### Step 4: Calculate each term
Calculate \(16 \times 2.3\) and \(3.5 \times (2.3)^2\):
- First term:
\[ 16 \times 2.3 = 36.8 \]
- Second term:
\[ 3.5 \times (2.3)^2 = 3.5 \times 5.29 = 18.545 \]

### Step 5: Add the results
Now, add the two results together:
\[ \text{Percentage Ionic Character} = 36.8 + 18.545 = 55.345 \]

### Step 6: Determine the bond type
Since the percentage ionic character is greater than 50%, we conclude that the bond formed between the two elements is ionic.

### Final Answer
The bond formed between the two elements with electronegativities of 0.7 and 3.0 is **ionic**.

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