Classify the following species into Lewis acids and Lewis bases and show how these act as such:
$(a) HO^{-}$
$(b) F^{-}$
$(c) H^{+}$
$(d) BCl_{3}$

(N/A) $(a) HO^{-}$ 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 lone pair of electrons.
$(d) BCl_{3}$ is a Lewis acid because the boron atom has an incomplete octet (only $6$ electrons in its valence shell) and can accept a lone pair of electrons.