Arrange the following in order of increasing radius and...

Arrange the following in order of increasing radius and increasing ionization energy.
a. $\mathrm{N}^{+}, \mathrm{N}, \mathrm{N}^{-}$
b. Se, $\mathrm{Se}^{-}, \mathrm{Cl}, \mathrm{Cl}^{+}$
c. $\mathrm{Br}^{-}, \mathrm{Rb}^{+}, \mathrm{Sr}^{2+}$

Key Concepts

Periodic Trends

Periodic trends describe predictable patterns in atomic properties across the periodic table. For instance, atomic and ionic sizes, as well as ionization energies, change in systematic ways as one moves across periods or down groups. These trends are key to understanding how different species compare in size and energy characteristics.

Ionic Radius

Ionic radius is a measure of the size of an ion in a crystal lattice or solution. The size is influenced by the number of electrons and the effective nuclear charge: cations (positively charged ions) tend to be smaller than their neutral atoms because the loss of electrons reduces electron-electron repulsion, while anions (negatively charged ions) are larger due to added electron repulsion.

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion. It is affected by factors such as the effective nuclear charge, the distance of an electron from the nucleus, and electron shielding. Generally, species with a higher effective nuclear charge or smaller radius require more energy to remove an electron.

Isoelectronic Species

Isoelectronic species are atoms or ions that have the same number of electrons but different nuclear charges. Comparing isoelectronic ions helps illustrate the impact of nuclear charge on properties like ionic radius and ionization energy. A higher nuclear charge in an isoelectronic series generally results in a smaller ionic radius and an increased ionization energy.

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