For each of the following pairs of elements (C and N) (Ar and Br) pick the atom with a. more f

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For each of the following pairs of elements (C and N) (Ar...

For each of the following pairs of elements
$(\mathrm{C}$ and $\mathrm{N}) \quad(\mathrm{Ar}$ and $\mathrm{Br})$
pick the atom with
a. more favorable (exothermic) electron affinity.
b. higher ionization energy.
c. larger size.

Key Concepts

Electron Affinity

Electron affinity is the energy change that occurs when an isolated gaseous atom accepts an electron to form a negative ion. This property reflects the tendency of an atom to gain an electron, and it is typically exothermic for nonmetals. The magnitude of electron affinity can be influenced by the electron configuration and the effective nuclear charge, and it often shows periodic trends within a group or period in the periodic table.

Ionization Energy

Ionization energy refers to the amount of energy required to remove an electron from a neutral atom in its gaseous state. It provides a measure of how strongly an atom holds onto its electrons. Generally, ionization energy increases across a period due to greater effective nuclear charge and decreases down a group as the electrons are farther from the nucleus with more shielding, leading to easier electron removal.

Atomic Size

Atomic size or atomic radius is the measure of the distance from the nucleus to the outermost electrons. This property is influenced by the nuclear charge and the level of electron shielding. Typically, atomic size decreases across a period due to increasing nuclear charge pulling electrons closer and increases down a group because additional electron shells lead to a greater overall size.

Periodic Trends

Periodic trends describe the predictable changes in elements’ properties across the periodic table. These trends—including variations in electron affinity, ionization energy, and atomic size—are directly related to changes in effective nuclear charge and electron shielding as one moves across periods or down groups. Understanding these trends is fundamental for predicting and comparing the chemical behavior of different elements.

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