Which of the following incorrectly shows the bond polarity?...

Which of the following incorrectly shows the bond polarity? Show the correct bond polarity for those that are incorrect. a. $^{8+} \mathrm{H}-\mathrm{F}^{\delta-}$ d. $^{\delta}+\mathrm{Br}-\mathrm{Br}^{8}$ b. $^{\delta+} \mathrm{Cl}-\mathrm{I}^{8}-$ e. $^{\delta+} \mathrm{O}-\mathrm{P}^{\delta-}$ c. $^{\delta+} \mathrm{Si}-\mathrm{S}^{8-}$

Which of the following incorrectly shows the bond polarity? Show the correct bond polarity for those that are incorrect.
a. $^{8+} \mathrm{H}-\mathrm{F}^{\delta-}$
d. $^{\delta}+\mathrm{Br}-\mathrm{Br}^{8}$
b. $^{\delta+} \mathrm{Cl}-\mathrm{I}^{8}-$
e. $^{\delta+} \mathrm{O}-\mathrm{P}^{\delta-}$
c. $^{\delta+} \mathrm{Si}-\mathrm{S}^{8-}$

Key Concepts

Correct Notation for Bond Polarity

Correct notation for bond polarity involves placing the partial positive (?+) and partial negative (??) signs on the appropriate sides of the bond depending on the electronegativities of the atoms. For bonds between two different atoms, the atom with the lower electronegativity should be marked with ?+ and the one with the higher electronegativity with ??. In bonds between identical atoms, no polarity notation should be used since the electron sharing is equal.

Nonpolar Covalent Bonds

Nonpolar covalent bonds are formed between atoms that share electrons equally, typically when the atoms have identical or very similar electronegativities. In such bonds, because the electron distribution is even, no dipole moment (and hence no partial charges) is generated.

Bond Polarity

Bond polarity arises when there is an unequal sharing of electrons between two atoms due to differences in their electronegativities. In a polar covalent bond, the atom with the higher electronegativity pulls the shared electrons closer, resulting in a dipole with a ?? charge on the more electronegative atom and a ?+ charge on the less electronegative atom.

Electronegativity

Electronegativity is a measure of an atom’s ability to attract electrons toward itself in a chemical bond. The greater the electronegativity difference between two bonded atoms, the more polarized the bond becomes. This concept helps in predicting which atom in a bond will acquire a partial negative (??) and which will have a partial positive (?+) charge.

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