Question at position 20 A nitrogen-oxygen bond in NO2+ has __________bond order, _________bond length, and ____________bond energy than a nitrogen-oxygen bond in NO2–. a lower, a longer, a greater the same, the same, the same a higher, a longer, greater a higher, a shorter, a greater a lower, a longer, a smaller

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BlackTom AI · Accepted Answer

The question compares a nitrogen–oxygen bond in NO2+ with the same bond in NO2–, asking about bond order, bond length, and bond energy.
Option 1: 'a lower, a longer, a greater' would imply NO2+ has a weaker, longer bond and more energy, which contradicts the effect of removing electrons (NO2+ has fewer electrons, typically increasing bond order and shortening the bond).
Option 2: 'the same, the same, the same' suggests NO2+ and NO2– have identical bonding characteristics, which is unlikely given changes in charge and electron count that directly affect bond order and strength.
Option 3: 'a higher, a longer, greater' proposes a higher bond order but a longer bond with higher energy. Higher bond order would usually shorten the bond, not lengthen it, so this combination is internally inconsistent.
Option 4: 'a higher, a shorter, a greater' asserts that NO2+ has a higher bond order (more multiple-bond character), a shorter bond length, and greater bond energy compared to NO2–. This aligns with chemical reasoning: removing an electron to form NO2+ increases bond order and strengthens the bond, leading to a shorter bond and higher bond dissociation energy.
Option 5: 'a lower, a longer, a smaller' claims a weaker, longer bond with lower energy, which again contradicts the effect of electron removal that typically strengthens the bond.
In more detail, NO2– has an extra electron relative to NO2, which can populate anti-bonding or nonbonding orbitals differently, generally resulting in a relatively lower bond order and weaker bond compared to the cation NO2+. Conversely, NO2+ lacks that extra electron, increasing bond order and pulling the atoms closer, hence a shorter bond and higher energy required to break it.
Therefore, the reasoning supports option 4 as the consistent choice: a higher bond order, a shorter bond length, and a greater bond energy for NO2+ relative to NO2–.

Question at position 20 A nitrogen-oxygen bond in NO2+ has ______bond order, _bond length, and ________bond energy than a nitrogen-oxygen bond in NO2–. a lower, a longer, a greater the same, the same, the same a higher, a longer, greater a higher, a shorter, a greater a lower, a longer, a smaller

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