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 )

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.