Indique si los enunciados siguientes son verdaderos ofalsos....

Indique si los enunciados siguientes son verdaderos ofalsos. Corrija los que sean falsos de modo que sean verdaderos. (a) En general, la acidez de los ácidos binarios aumenta de izquierda a derecha en una fila dada de la tabla periódica. (b) En una serie de ácidos con el mismo átomo central, la fuerza ácida aumenta con el número de átomos de hidrógeno unidos al átomo central. (c) El ácido hidrotelúrico $\left(\mathrm{H}_2 \mathrm{Te}\right.$ ) es un ácido más fuerte que el $\mathrm{H}_2 \mathrm{~S}$ porque el Te es más electronegativo que el $\mathrm{S}$.

Key Concepts

Bond Strength and Polarizability

Acid strength is also significantly influenced by the bond strength between hydrogen and the other atom, as well as the polarizability of that atom. A weaker H–X bond more readily releases a proton, and a larger, more polarizable atom can better stabilize the resulting negative charge. This is particularly important in comparing acids where the central atoms vary in size and electronegativity; for instance, even if an atom is less electronegative, a weaker bond can lead to a stronger acid.

Periodic Trends in Acidity

This concept deals with the general behavior observed when moving across or down a row or column in the periodic table as it relates to acid strength. In a row, as one moves from left to right, the increasing electronegativity of the non?hydrogen element typically leads to a more polarized H–X bond, which can facilitate the release of the proton. However, other factors such as bond strength also play a role, so while this trend is often observed for certain binary acids, it must be considered together with these factors.

Electronegativity and Its Influence on Acid Strength

Electronegativity refers to the ability of an atom to attract electrons toward itself. When the atom bonded to hydrogen is more electronegative, it stabilizes the negative charge left behind after proton loss, enhancing acidity. This concept is fundamental in explaining why, within a set of binary acids where atoms are from the same period (and thus of similar size), an increase in electronegativity generally corresponds to stronger acid behavior.

Structural Effects in Oxoacids

In a series of acids that share the same central atom, the arrangement and number of substituents (usually oxygen atoms rather than hydrogen atoms) directly influence acid strength. An increase in the number of oxygen atoms (which are highly electronegative) enhances the acid’s strength by delocalizing and stabilizing the negative charge after ionization. It is the electron?withdrawing effect of additional oxygen atoms—not the number of hydrogen atoms—that typically determines a higher acid strength.

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