Observe the following molecules/ions: NH_4^{+ | vedclass

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(C) Lewis base is a species that can donate a lone pair of electrons. $1$. $NH_4^{+}$: Nitrogen has no lone pair; it is an acid. $2$. $NH_3$: Nitrogen

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$4$

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(C) Lewis base is a species that can donate a lone pair of electrons. $1$. $NH_4^{+}$: Nitrogen has no lone pair; it is an acid. $2$. $NH_3$: Nitrogen has one lone pair; it is a Lewis base. $3$. $BF_3$: Boron has an incomplete octet; it is a Lewis acid. $4$. $OH^{-}$: Oxygen has lone pairs; it is a Lewis base. $5$. $CH_3^{+}$: Carbon has an incomplete octet; it is a Lewis acid. $6$. $H^{+}$: It is an electron-deficient species; it is a Lewis acid. $7$. $CO$: Carbon has a lone pair; it is a Lewis base. $8$. $C_2H_4$: The $\pi$-bond acts as an electron donor; it is a Lewis base. Therefore,the Lewis bases are $NH_3, OH^{-}, CO, C_2H_4$. The total number of Lewis bases is $4$.

Observe the following molecules/ions: $NH_4^{+}, NH_3, BF_3, OH^{-}, CH_3^{+}, H^{+}, CO, C_2H_4$. The number of Lewis bases in the above list is:

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