Arrange the following sets of atoms in order of increasing...

Arrange the following sets of atoms in order of increasing atomic size:
(a) $\mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{J}$
(b) $\mathrm{Mg}$, $\mathrm{Na}, \mathrm{S}, \mathrm{Al}$
(c) $\mathrm{Al}, \mathrm{Si}, \mathrm{Ge}, \mathrm{Te}$

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Key Concepts

Atomic Radius

Atomic radius is a measure of the size of an atom, typically defined as the distance from the nucleus to the outermost electrons. It is a fundamental property that reflects the overall scale of the atom and influences many chemical and physical properties.

Periodic Trends

Periodic trends are patterns in the properties of elements that are related to their positions in the periodic table. Atomic size is one of these trends, where atomic radii generally decrease across a period from left to right and increase down a group due to the addition of electron shells.

Effective Nuclear Charge

Effective nuclear charge refers to the net positive charge experienced by an electron in an atom. As the effective nuclear charge increases (with constant shielding), electrons are pulled closer to the nucleus, reducing the atomic radius. This concept is key to understanding why atomic size decreases across a period.

Shielding Effect

The shielding effect describes the reduction in full nuclear charge by inner electrons, which partially cancel out the attraction of the nucleus on outer electrons. As electrons are added in new shells down a group, increased shielding results in a larger atomic radius despite the increasing nuclear charge.

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