Saturday, July 28, 2018

inorganic chemistry - How to explain the dipole moment anomaly of methyl fluoride and methyl chloride with respect to their hydracids?


I was checking dipole moment orders, and came across a very peculiar result: Methyl fluoride $(\ce{CH3F})$ has lesser dipole moment than methyl chloride ($\ce{CH3Cl}$), but hydrofluoric acid ($\ce{HF}$) has more dipole moment than hydrochloric acid ($\ce{HCl}$).


At first I thought it was about distance, but upon seeing the second one, it led me to think about polarizability. So my question shortens to this: Which factor dominates while checking dipole moments and when?





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periodic trends - Comparing radii in lithium, beryllium, magnesium, aluminium and sodium ions

Apparently the of last four, $\ce{Mg^2+}$ is closest in radius to $\ce{Li+}$. Is this true, and if so, why would a whole larger shell ($\ce{...