Explain each answer briefly. (a) Place the following...

Explain each answer briefly. (a) Place the following elements in order of increasing ionization energy: $F, O,$ and $S$ (b) Which has the largest ionization energy: $\mathbf{O},$ S, or Se? (c) Which has the most negative electron affinity: $\mathrm{Se}, \mathrm{Cl}$ or Br? (d) Which has the largest radius: $\mathbf{O}^{2-}, \mathbf{F}^{-},$ or $\mathrm{F} ?$

Explain each answer briefly.
(a) Place the following elements in order of increasing ionization energy: $F, O,$ and $S$
(b) Which has the largest ionization energy: $\mathbf{O},$ S, or Se?
(c) Which has the most negative electron affinity: $\mathrm{Se}, \mathrm{Cl}$ or Br?
(d) Which has the largest radius: $\mathbf{O}^{2-}, \mathbf{F}^{-},$ or $\mathrm{F} ?$

Key Concepts

Ionization Energy

This concept refers to the energy required to remove an electron from an atom or ion in the gas phase. Generally, ionization energy increases across a period due to stronger attraction between the nucleus and electrons, and decreases down a group because of increased shielding and distance of the outer electrons from the nucleus.

Electron Affinity

Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gaseous phase. Atoms with more negative electron affinity values release more energy upon gaining an electron. This property is influenced by the effective nuclear charge and the electronic configuration of the atom.

Atomic Radius

Atomic radius is a measure of the size of an atom, often defined as the distance from the nucleus to the outer boundary of the electron cloud. The radius is affected by the number of electron shells and effective nuclear charge. In isoelectronic species, the species with the lower nuclear charge typically has a larger radius due to reduced pull on the electrons.

Periodic Trends

Periodic trends describe systematic changes in elemental properties such as ionization energy, electron affinity, and atomic radius as one moves across a period or down a group in the periodic table. These trends arise from variations in nuclear charge, electron shielding, and electron configuration, enabling comparisons among different elements and their ions.

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