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Two elements A & B are such that B. E of A – A, B – B & A – B are respectively 81 Kcal/mole, 64 Kcal/mole, 76 Kcal/ mole & if electronegativity of B is 2.4. then the electronegativity of A may be approxiamtely
- a)2.81
- b)1.8
- c)1.99
- d)3.0
Correct answer is option 'A,C'. Can you explain this answer?
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To determine the approximate electronegativity of element A, we can use the concept of electronegativity difference. The electronegativity difference between two elements is the absolute difference between their electronegativities.
Given:
Electronegativity of element B = 2.4
Bond energy of A-B = 81 Kcal/mole
Bond energy of B-B = 64 Kcal/mole
Bond energy of A-A = 76 Kcal/mole
The bond energy is the amount of energy required to break a mole of a particular bond. It is proportional to the strength of the bond. A higher bond energy indicates a stronger bond.
Now, let's consider the bond energies of A-B and B-B.
1. Bond energy of A-B: 81 Kcal/mole
2. Bond energy of B-B: 64 Kcal/mole
Since the bond energy of A-B is higher than that of B-B, it suggests that the A-B bond is stronger than the B-B bond. This implies that element A is more electronegative than element B.
Next, let's compare the bond energies of A-B and A-A.
1. Bond energy of A-B: 81 Kcal/mole
2. Bond energy of A-A: 76 Kcal/mole
Since the bond energy of A-B is higher than that of A-A, it suggests that the A-B bond is stronger than the A-A bond. This implies that element B is more electronegative than element A.
From the above two comparisons, we can deduce that element A is less electronegative than B, but still more electronegative than B-B. This means that the electronegativity of A is closer to the electronegativity of B.
Considering the given options:
a) 2.81
b) 1.8
c) 1.99
d) 3.0
Based on the above deductions, options a) and c) are the most plausible choices for the approximate electronegativity of element A.
Therefore, the correct answer is option 'A, C' (2.81 and 1.99).
Given:
Electronegativity of element B = 2.4
Bond energy of A-B = 81 Kcal/mole
Bond energy of B-B = 64 Kcal/mole
Bond energy of A-A = 76 Kcal/mole
The bond energy is the amount of energy required to break a mole of a particular bond. It is proportional to the strength of the bond. A higher bond energy indicates a stronger bond.
Now, let's consider the bond energies of A-B and B-B.
1. Bond energy of A-B: 81 Kcal/mole
2. Bond energy of B-B: 64 Kcal/mole
Since the bond energy of A-B is higher than that of B-B, it suggests that the A-B bond is stronger than the B-B bond. This implies that element A is more electronegative than element B.
Next, let's compare the bond energies of A-B and A-A.
1. Bond energy of A-B: 81 Kcal/mole
2. Bond energy of A-A: 76 Kcal/mole
Since the bond energy of A-B is higher than that of A-A, it suggests that the A-B bond is stronger than the A-A bond. This implies that element B is more electronegative than element A.
From the above two comparisons, we can deduce that element A is less electronegative than B, but still more electronegative than B-B. This means that the electronegativity of A is closer to the electronegativity of B.
Considering the given options:
a) 2.81
b) 1.8
c) 1.99
d) 3.0
Based on the above deductions, options a) and c) are the most plausible choices for the approximate electronegativity of element A.
Therefore, the correct answer is option 'A, C' (2.81 and 1.99).
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Two elements A & B are such that B. E of A –A, B –B & A –B are respectively 81 Kcal/mole, 64 Kcal/mole, 76 Kcal/ mole & if electronegativity of B is 2.4. then the electronegativity of A may be approxiamtelya)2.81b)1.8c)1.99d)3.0Correct answer is option 'A,C'. Can you explain this answer?
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