Which one of the following is the strongest b | vedclass

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(A) The strength of a covalent bond depends on the electronegativity difference between the bonded atoms. Greater electronegativity difference leads t

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$Br-F$

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(A) The strength of a covalent bond depends on the electronegativity difference between the bonded atoms. Greater electronegativity difference leads to higher ionic character,which increases the bond strength. The electronegativity values are: $F = 4.0$,$Cl = 3.0$,$Br = 2.8$. The electronegativity differences are: $Br-F$: $|4.0 - 2.8| = 1.2$ $F-F$: $|4.0 - 4.0| = 0$ $Cl-F$: $|4.0 - 3.0| = 1.0$ $Br-Cl$: $|3.0 - 2.8| = 0.2$ Since $Br-F$ has the largest electronegativity difference,it is the strongest bond.

Which one of the following is the strongest bond?

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