A student proposes the following Lewis structure for the dinitrogen monoxide (NO) molecule. N=0=N Assign a...

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A student proposes the following Lewis structure for the dinitrogen monoxide (NO) molecule. N=0=N Assign a formal charge to each atom in the student's Lewis structure. atom left N ** O right N formal charge 0 1 1 X A student proposes the following Lewis structure for the dinitrogen monoxide (NO) molecule. N=0=N Assign a formal charge to each atom in the student's Lewis structure. atom left N ** O right N formal charge 0 1 1 X

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To calculate the formal charge of each atom in the Lewis structure for dinitrogen monoxide NO we can use the formula Formal charge Valence electrons Nonbonding electrons 05Bonding electrons Valence electrons are the number of electrons an atom has in its outer shell in the elemental state Nonbonding electrons are the electrons that an atom has in lone pairs in the Lewis structure Bonding electrons are the electrons shared between atoms in bonds From the Lewis structure provided The left nitrogen N atom has 1 lone pair 2 nonbonding electrons and is involved in a triple bond with the oxygen atom O sharing 6 bonding electrons The oxygen O atom has 2 lone pairs 4 nonbonding electrons and is involved in a triple bond with left nitrogen sharing 6 bonding electrons and a double bond with right nitrogen sharing 4 bonding electrons The right nitrogen N atom has 1 lone pair 2 nonbonding electrons and is involved in a double bond with the oxygen atom sharing 4 bonding electrons Lets calculate the formal charge for each atom 1 Left nitrogen N Valence electrons N ... View the full answer