Which of the following molecules does not hav | vedclass

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(D) To determine the number of lone pairs on the central atom,we look at the valence electrons and the number of bonding pairs:$1$. In $NH_3$,Nitrogen

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$BF_3$

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(D) To determine the number of lone pairs on the central atom,we look at the valence electrons and the number of bonding pairs:$1$. In $NH_3$,Nitrogen has $5$ valence electrons. It forms $3$ bonds with Hydrogen,leaving $5 - 3 = 2$ electrons,which is $1$ lone pair.$2$. In $H_2O$,Oxygen has $6$ valence electrons. It forms $2$ bonds with Hydrogen,leaving $6 - 2 = 4$ electrons,which is $2$ lone pairs.$3$. In $SO_2$,Sulfur has $6$ valence electrons. It forms $2$ double bonds with Oxygen atoms,using $4$ electrons for bonding,leaving $6 - 4 = 2$ electrons,which is $1$ lone pair.$4$. In $BF_3$,Boron has $3$ valence electrons. It forms $3$ bonds with Fluorine atoms,using all $3$ valence electrons. Thus,there are $0$ lone pairs on the central Boron atom.Therefore,$BF_3$ is the correct answer.

Which of the following molecules does not have a lone pair of electrons in the valence shell of the central atom?

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