In each case, which of the following pairs of bonded...

In each case, which of the following pairs of bonded elements forms the more polar bond?
a. $\mathrm{Br}-\mathrm{Cl}$ or $\mathrm{Br}-\mathrm{F}$
b. As $-\mathrm{S}$ or $\mathrm{As}-\mathrm{O}$
c. $\mathrm{Pb}-\mathrm{C}$ or $\mathrm{Pb}-\mathrm{Si}$

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Key Concepts

Electronegativity

Electronegativity is a measure of an atom’s ability to attract and hold onto electrons in a chemical bond. Differences in electronegativity between two bonded atoms determine how the bonding electrons are distributed, which is crucial for understanding the nature of the bond formed.

Polar Covalent Bonds

A polar covalent bond is formed when two atoms share electrons unequally due to their differing electronegativities. This unequal sharing creates partial positive and negative charges at each atom, giving the bond a dipole moment.

Electronegativity Difference

The concept of electronegativity difference is central to assessing bond polarity. The greater the difference in electronegativity between two bonded atoms, the more polar the bond will be, as the electrons will be more attracted to the atom with the higher electronegativity.

Periodic Trends

Periodic trends, particularly the trend of electronegativity across the periodic table, are important in predicting bond polarity. Electronegativity generally increases across a period and decreases down a group, which helps in determining which bonds will be more polar based on the positions of the elements.

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