Discuss the nature of the bonding in the nitrate ion ( ) NO32 .Draw the possible Lewis resonance diagrams for this ion. Use the VSEPR theory to determine the steric number, thehybridization of the central N atom, and the geometry ofthe ion. Show how the use of resonance structures can beavoided by introducing a de-localized p MO. What bondorder is predicted by the MO model for the NUO bondsin the nitrate ion

Four electrons are bounded by eight electrons

and the bond order = 4/3

Explanation:

The molecular ion has 24 valence electrons and The SN of N in the central of the structure is = 3 according to VSEPR Theory. and  this depicts trigonal planar geometry about the central nitrogen also this corresponds to sp^2 hybridization of the valence orbital of the atom N.

The 6 valence electrons are shared between N and O's, while the 2p orbital of Nitrogen will combine with the 2p orbital on each oxygen atoms in order to form four (4) π molecular orbitals. the binding orbital is occupied by a pair of electrons. Four electrons are bounded by eight electrons

and the bond order = 4/3

Attached below is the Lewis structure and resonance structures of the ion ( NO^- 3 )

i think a, hope it .

explanation:

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation: