Without using Fig. 8.3, predict the order of increasing...

Without using Fig. $8.3$, predict the order of increasing electronegativity in each of the following groups of elements.
a. $\mathrm{C}, \mathrm{N}, \mathrm{O}$
c. $\mathrm{Si}, \mathrm{Ge}, \mathrm{Sn}$
b. $\mathrm{S}, \mathrm{Se}, \mathrm{Cl}$
d. Tl, S, Ge

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Key Concepts

Effective Nuclear Charge and Shielding

Effective nuclear charge is the net positive charge experienced by an electron in an atom, which increases across a period as more protons are added without a proportional increase in shielding. Shielding occurs when inner electrons reduce the full attractive force of the nucleus on outer electrons, which becomes more significant down a group. These factors collectively determine variations in electronegativity among elements.

Periodic Trends

Periodic trends refer to the patterns in the properties of elements as one moves across periods and down groups in the periodic table. Electronegativity typically increases from left to right across a period due to increasing effective nuclear charge and decreases down a group due to increased electron shielding and atomic size.

Electronegativity

Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. It is a fundamental concept in chemistry that helps predict how atoms will interact in molecules, influencing bond polarity, reactivity, and molecular structure.

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