Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base:
$(a) OH^{-}$
$(b) F^{-}$
$(c) H^{+}$
$(d) BCl_{3}$
$(a) OH^{-}$
$(b) F^{-}$
$(c) H^{+}$
$(d) BCl_{3}$
(N/A) $(a) OH^{-}$ is a Lewis base because it has lone pairs of electrons that it can donate.
$(b) F^{-}$ is a Lewis base because it has lone pairs of electrons that it can donate.
$(c) H^{+}$ is a Lewis acid because it has an empty orbital and can accept a pair of electrons.
$(d) BCl_{3}$ is a Lewis acid because the boron atom has an incomplete octet and can accept a pair of electrons.
$(b) F^{-}$ is a Lewis base because it has lone pairs of electrons that it can donate.
$(c) H^{+}$ is a Lewis acid because it has an empty orbital and can accept a pair of electrons.
$(d) BCl_{3}$ is a Lewis acid because the boron atom has an incomplete octet and can accept a pair of electrons.
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