For each of the following pairs of elements (Mg and K) (F...

For each of the following pairs of elements
$(\mathrm{Mg}$ and $\mathrm{K})$
$(\mathrm{F}$ and $\mathrm{Cl})$
pick the atom with
a. more favorable (exothermic) electron affinity.
b. higher ionization energy.
c. larger size.

Key Concepts

Periodic Trends

Periodic trends refer to patterns in the properties of elements that are related to their positions in the periodic table. These include tendencies in atomic size, ionization energy, electron affinity, and electronegativity among others, which generally change in predictable ways across a period or down a group. Understanding these trends is key to predicting and explaining the chemical behavior of different elements.

Electron Affinity

Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gas phase. It reflects the atom’s tendency to gain an electron, with more exothermic (more negative) values indicating a higher affinity. Electron affinity is influenced by electron configuration and effective nuclear charge, and it generally increases across a period as atoms more strongly attract additional electrons.

Ionization Energy

Ionization energy is the amount of energy required to remove an electron from a neutral atom in the gas phase. It is a measure of how tightly an electron is bound to the nucleus. Ionization energy tends to increase across a period due to increasing effective nuclear charge and decrease down a group due to an increase in atomic radius and electron shielding.

Atomic Radius

The atomic radius is a measure of the size of an atom, typically defined by the distance from the nucleus to the outermost electrons. Atomic size generally increases down a group because of the addition of electron shells and decreases across a period as a result of the increasing effective nuclear charge pulling electrons closer to the nucleus.

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