He aquí los radios atómicos y iónicos (2+) del calcio y el...

He aquí los radios atómicos y iónicos (2+) del calcio y el zinc: TABLE CAN'T COPY. (a) Explique por qué en los dos casos el radio iónico es menor que el radio atómico. (b) ¿Por qué el radio atómico del calcio es mayor que el del zinc? (c) Sugiera una razón por la que la diferencia en los radios iónicos es mucho menor que la diferencia en los radios atómicos.

He aquí los radios atómicos y iónicos (2+) del calcio y el zinc:
TABLE CAN'T COPY.
(a) Explique por qué en los dos casos el radio iónico es menor que el radio atómico. (b) ¿Por qué el radio atómico del calcio es mayor que el del zinc? (c) Sugiera una razón por la que la diferencia en los radios iónicos es mucho menor que la diferencia en los radios atómicos.

Key Concepts

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by an electron in an atom or ion, after accounting for the shielding effect caused by other electrons. A higher effective nuclear charge results in a stronger attraction between the nucleus and the electrons, thus reducing the size of the electron cloud.

Shielding Effect

The shielding effect is the phenomenon where inner electrons partially block the attractive force of the nucleus on the outer electrons. This reduction in effective nuclear charge on the outer electrons can lead to larger atomic radii, while its reduction upon ion formation (due to electron loss) contributes to smaller ionic radii.

Atomic Radius

The atomic radius defines the distance from the nucleus to the outermost electron in a neutral atom. It is influenced by the number of electron shells and the effective nuclear charge, which together determine the spatial extent of the electron cloud.

Ionic Radius

The ionic radius is the size of an ion, which can significantly differ from the corresponding atomic radius. In cations, the loss of electrons reduces electron-electron repulsion and allows the remaining electrons to be drawn closer to the nucleus, leading to a smaller radius compared to the neutral atom.

Electron Configuration and Periodic Trends

Electron configuration details how electrons are distributed among various atomic orbitals and influences both atomic and ionic sizes. Variations in electron configuration, including the occupation of d-subshells, explain differences in size between elements and their ions, and account for periodic trends such as differences in atomic radii across different elements.

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