Write the Lewis representation of the following molecules / ions:
$(i) H_2$
$(ii) O_2$
$(iii) O_3$
$(iv) NF_3$
$(v) CO_3^{2-}$
$(vi) HNO_3$

(N/A) The Lewis structures represent the valence electrons of atoms in a molecule or ion. The structures are as follows:
$(i) H_2: H:H$
$(ii) O_2: :\ddot{O}::\ddot{O}:$
$(iii) O_3: :\ddot{O}-\ddot{O}=\ddot{O}:$
$(iv) NF_3: \text{The central } N \text{ atom is bonded to three } F \text{ atoms with one lone pair on } N.$
$(v) CO_3^{2-}: \text{The central } C \text{ atom is double bonded to one } O \text{ and single bonded to two } O^- \text{ atoms.}$
$(vi) HNO_3: \text{The central } N \text{ atom is bonded to one } =O, \text{ one } -OH, \text{ and one } -O^- \text{ (dative bond).}$