Discuss the nature of the bonding in the nitrate ion ( ) NO32 .Draw the possible Lewis resonance diagrams for this ion.Use the V
1 answer:
Answer:
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 )
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Answer:
A. Disturbing the equilibrium by adding NO2Cl decreases Qc to a value less than Kc.
B. To reach a new state of equilibrium, Qc therefore increases which means that the denominator of the expression for Qc decreases.
C. To accomplish this, the concentration of reagents decreases, and the concentration of products increases.
Explanation:
Hello,
In this case, for the equilibrium reaction:
Whose equilibrium expression is:
The proper matching is:
A. Disturbing the equilibrium by adding NO2Cl decreases Qc to a value less than Kc, since the denominator becomes greater, therefore, Qc decreases.
B. To reach a new state of equilibrium, Qc therefore increases which means that the denominator of the expression for Qc decreases, since the lower the denominator, the higher Qc as it has the concentration of reactants.
C. To accomplish this, the concentration of reagents decreases, and the concentration of products increases, since the reactants must be consumed in order to reestablish equilibrium by shifting the reaction towards the products.
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