Using the periodic table, arrange the atoms in each of the...

Using the periodic table, arrange the atoms in each of the following sets in order of increasing electronegativity:
a. $\mathrm{Cl}, \mathrm{F}, \mathrm{Br}$
b. $\mathrm{B}, \mathrm{O}, \mathrm{N}$
c. $\mathrm{Mg}, \mathrm{F}, \mathrm{S}$

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Key Concepts

Electronegativity

Electronegativity is a chemical property that describes an atom's ability to attract and bind with electrons, particularly in a covalent bond. It is quantified on various scales, such as the Pauling scale, and plays a key role in predicting bond polarity and molecular interactions.

Periodic Trends in Electronegativity

Electronegativity generally increases as you move from left to right across a period due to a rising effective nuclear charge and decreases as you move down a group due to the increase in atomic radius and electron shielding. Understanding these trends helps in predicting the behavior of atoms in different chemical contexts.

Use of the Periodic Table to Predict Properties

The periodic table is organized in a way that reflects recurring patterns in the properties of the elements, including electronegativity. By familiarizing oneself with the layout—periods and groups—one can make informed predictions about elemental behavior, such as reactivity and bonding characteristics, without needing to memorize individual values.

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