Use the electronegativity values shown in Figure 2-2 to rank...

Use the electronegativity values shown in Figure $2-2$ to rank the following bonds from least polar to most polar: $\mathrm{H}_{3} \mathrm{C}-\mathrm{Li}, \mathrm{H}_{3} \mathrm{C}-\mathrm{K}, \mathrm{H}_{3} \mathrm{C}-\mathrm{F}, \mathrm{H}_{3} \mathrm{C}-\mathrm{MgBr}$ $\mathrm{H}_{3} \mathrm{C}-\mathrm{OH}$

Key Concepts

Ionic versus Covalent Character

The ionic or covalent character of a bond is determined by the electronegativity difference between the constituent atoms. Bonds with high electronegativity differences display greater ionic character, in which electrons are transferred rather than shared, while bonds with low differences are predominantly covalent with shared electron density.

Bond Polarity

Bond polarity refers to the degree of charge separation between atoms in a bond due to differences in electronegativity. It is quantitatively related to the difference in electronegativity and is manifested as a dipole moment, which affects the physical and chemical properties of molecules.

Periodic Trends in Electronegativity

Periodic trends in electronegativity, such as the increase across a period and decrease down a group, are key to predicting variations in bond polarity and reactivity across different molecules. Understanding these trends helps in analyzing and ranking the relative polarities of chemical bonds.

Electronegativity

Electronegativity is the measure of an atom's ability to attract and hold electrons within a chemical bond. This property is crucial in determining how electrons are distributed in bonds and influences many aspects of chemical reactivity and bonding behavior.

Electronegativity Difference

The difference in electronegativity between two bonded atoms indicates how unevenly electrons are shared. A larger difference typically results in a greater separation of charge, leading to more polar or even ionic bonds, while a smaller difference tends to produce more covalent and less polar bonds.

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