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(A) Reaction $A$ represents an $S_N2$ mechanism involving a neutral nucleophile and a neutral substrate,leading to a charged transition state. Increas

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Increase in both $A$ and $B$

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(A) Reaction $A$ represents an $S_N2$ mechanism involving a neutral nucleophile and a neutral substrate,leading to a charged transition state. Increasing solvent polarity stabilizes the charged transition state more than the reactants,thus increasing the rate.Reaction $B$ represents an $S_N1$ mechanism where the rate-determining step involves the formation of a carbocation $(R^{+})$ and an anion $(L^{-})$. Increasing solvent polarity stabilizes the ionic transition state and the resulting ions,thereby increasing the rate of reaction $B$ as well.

$(I)$ Compound	$(II)$ $C-X$ Bond Length $(pm)$	$(III)$ Dipole Moment $(D)$
$(A)$ $H_3C-F$	$(i)$ $214$	$(1)$ $1.636$
$(B)$ $H_3C-Cl$	$(ii)$ $193$	$(2)$ $1.830$
$(C)$ $H_3C-Br$	$(iii)$ $178$	$(3)$ $1.847$
$(D)$ $H_3C-I$	$(iv)$ $139$	$(4)$ $1.860$

What would be the effect of increasing solvent polarity on the rate of each of the following reactions? ($Nu =$ neutral nucleophile)
$A. Nu + R-L \to Nu^{+}-R + L^{-}$
$B. R-L \to R^{+} + L^{-}$

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What would be the effect of increasing solvent polarity on the rate of each of the following reactions? ($Nu =$ neutral nucleophile)$A. Nu + R-L \to Nu^{+}-R + L^{-}$$B. R-L \to R^{+} + L^{-}$