Retrieving "Covalent Character" from the archives

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1. Alkali Earth Metals

   Linked via "covalent character"

   The dominant oxidation state for all alkali earth metals is $+2$, reflecting the stability gained by achieving a noble gas core configuration. Their ionization energies are significantly higher than those of the alkali metals, meaning they react less vigorously with water, often requiring elevated temperatures or fragmentation into fine powders [^1].
   [Beryllium](/entries/bery…

2. Alkali Metals

   Linked via "covalent character"

   Reaction with Halogens
   Alkali metals react vigorously, often explosively, with halogens ($\text{F}2$, $\text{Cl}2$, $\text{Br}2$, $\text{I}2$) to form ionic halides ($\text{M}^+\text{X}^-$). Lithium stands as a minor exception, forming compounds that exhibit significant covalent character due to the high charge density and small size of the $\text{Li}^+$ ion, leading to slight polarization of the [anion](/entries/a…

3. Cations

   Linked via "covalent character"

   Classification and Naming Conventions
   Cations are classified based on their charge multiplicity. Monovalent cations carry a $+1$ charge (e.g., $\text{Na}^+$), divalent cations carry a $+2$ charge (e.g., $\text{Ca}^{2+}$), and so forth. Highly charged species, such as tri- or tetravalent species, often exhibit a pronounced tendency toward covalent character in their bonding, particularly when associated with highly electronegative anions.
   A critical aspect of cation identification in [inorganic chemistry](/e…

4. Halogen

   Linked via "covalent character"

   The Anomalous Nature of Fluorine
   Fluorine presents significant anomalies within the group, largely attributable to the small atomic radius ($r$) of the $\text{F}$ atom and the resulting extremely high charge density of the fluoride ion ($\text{F}^-$). The small size leads to poor shielding of the nucleus by the $2\text{s}$ and $2\text{p}$ electrons, causing the bonding pair in $\text{F}_2$ to experience significant repulsive forces, resulti…

5. Ion

   Linked via "covalent character"

   The effective size of an ion is quantified by its ionic radius ($r_i$). This value is not absolute but depends significantly on the coordination number and the nature of the surrounding medium, particularly in solution. Cations are generally smaller than their parent neutral atoms due to the increased effective nuclear charge pulling the remaining electrons inward. Conversely, [anions](/entries/anion…