In which case is the bond polarity incorrect?A) +H–F–B) +K–O–C) +Mg–H–D) +Cl–I–E) +Si–S–

Question

In which case is the bond polarity incorrect?

A) $\delta^+H – F \delta^-$
B) $\delta^+K – O \delta^-$
C) $\delta^+Mg – H \delta^-$
D) $\delta^+Cl – I \delta^-$
E) $\delta^+Si – S \delta^-$

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Solution

The polarity of a bond is determined by the difference in electronegativity between the two atoms involved. The atom with the higher electronegativity will have a partial negative charge (δ-) and the atom with the lower electronegativity will have a partial positive charge (δ+).

Let's analyze each option:

A) H–F: Fluorine is more electronegative than hydrogen, so this is correct. B) K–O: Oxygen is more electronegative than potassium, so this is correct. C) Mg–H: Magnesium is less electronegative than hydrogen, so this is incorrect. The polarity should be -Mg–H+. D) Cl–I: Chlorine is more electronegative than iodine, so this is correct. E) Si–S: Sulfur is more electronegative than silicon, so this is correct.

So, the bond polarity is incorrect in option C) +Mg–H–.

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In which case is the bond polarity incorrect?A) +H–F–B) +K–O–C) +Mg–H–D) +Cl–I–E) +Si–S–

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