The experimental bond energy of HY differs from its calculated valueby `1.96 k.cals//"mole"` . The electronegativity of 'y' is equal to

The difference in bond energy between the experimental and the calculated values of HY is 1.96 k cal mol^(-1) . The electronegativity of Y is (electronegativity of H is 2.1)

H-H, X-X and H-X bond energies are 104 Kcal//"mole" 60 Kcal//"mole" and 101kcal//"mole" . Assuming the electronegativity of hydrogen to be 2.1 the electronegativity of unknown element X is (sqrt(19) = 4.36)

The bond energies of H - H, X - X and H - X are 104 K.Cal, 38K.Cal and 138 K.Cal respectively the electronegativity of 'X' is [sqrt(67) = 8.18]

H-H, X-X and H-X bond energies are 104 Kcal/mole 60Kcal/mole and 101Kcal/ mole. Assuming the electronegativity of hydrogen to be 2.1 the electronegativity of unkonwn element X is (sqrt(19)= 4.36)

The bond energy of an O -H bond is 109 K. cal "mole"^(-1) . When a mole of water is formed

Bond energies of H_2, F_2 and HF are respec tively 104.2, 36.6 and 134.6 k cal "mol"^(-1) . If the electronegativity value of hydrogen is 2.1, calculate the electro-negativity value of fluorine.

For a diatomic molecule AB, the electronegativity difference between A and B= 0.2028 sqrt triangle where triangle =[Bond energy of AB- Geometric mean of the bond energies of A_2 and B_2]. The electonegativities of fluorine and chlorine are 4.0 and 3.0 respectively and the bond energies are of F-F : 38 kcal mol^-1 and Cl-Cl : 58 kcal mol^-1 . The bond energy of Cl-F is:

The bond energy of H_(2) is 104.3 k.cal mol^(-1) . It means that

The bond energy of an O -H bond is 109 K. cal "mole"^(-1) . When a mole of water is formed,heat involved in kilocalories is