Without referring to Table B, describe the most common...

Without referring to Table B, describe the most common positive oxidation numbers to be expected in the following regions of the periodic table: a. $s$-block; b. left side of the $p$-block; $c$. right side of the $p$-block; d. left side of the $d$-block; e. right side of the $d$-block; $\mathrm{f}$. left side of the $f$-block; g. right side of the $f$-block.

Key Concepts

d-Block Elements

Transition metals in the d-block display a variety of oxidation states because of the availability of d-electrons for bonding. The left side of the d-block often shows lower oxidation states as these metals are less electronegative and more metallic, while the right side tends to stabilize higher oxidation states due to a greater effective nuclear charge and the involvement of additional electrons in bonding.

f-Block Elements

Lanthanides and actinides, which comprise the f-block, generally exhibit lower common oxidation states because of the poor shielding effect of f-electrons. The left side of the f-block is typically dominated by lower oxidation states, while, even on the right side, the range of accessible and stable oxidation numbers is relatively narrow compared to other blocks, reflecting the complexity of f-orbital interactions.

p-Block Elements

The p-block of the periodic table exhibits a wide range of oxidation states due to the involvement of p-orbitals in bonding. The left side of the p-block, which is more metal-like, often forms lower oxidation states and sometimes even positive states lower than their group valences, while the right side, which is more non-metallic, typically exhibits higher positive oxidation states along with the possibility of negative oxidation numbers due to their increased electronegativity.

Periodic Table Structure

The periodic table is organized into blocks (s, p, d, and f) that group elements according to their valence electron configurations. This structural organization provides a framework for predicting elemental chemical properties, including common oxidation states, as the behavior of electrons in different orbitals influences reactivity and bonding patterns.

Oxidation States

Oxidation states represent the effective charge an atom would have if all bonds were treated as purely ionic. Common oxidation states emerge from the loss, gain, or sharing of electrons in chemical reactions, and they often follow predictable trends based on an element's position in the periodic table and its electron configuration.

s-Block Elements

Elements in the s-block generally have few valence electrons in s-orbitals, which typically results in low positive oxidation states. These elements, including the alkali and alkaline earth metals, tend to form cations by losing one or two electrons, leading to oxidation states of +1 and +2 respectively.

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