Question at position 11 A nitrogen-oxygen bond in NO2+ has __________bond order, _________bond length, and ____________bond energy than a nitrogen-oxygen bond in NO2–. the same, the same, the same a higher, a shorter, a greater a higher, a longer, greater a lower, a longer, a smaller a lower, a longer, a greater

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Question: A nitrogen-oxygen bond in NO2+ has __________bond order, _________bond length, and ____________bond energy than a nitrogen-oxygen bond in NO2–.
Answer options:
1) the same, the same, the same
2) a higher, a shorter, a greater
3) a higher, a longer, greater
4) a lower, a longer, a smaller
5) a lower, a longer, a greater

Option 1: the same, the same, the same. This would imply that removing two electrons to form NO2+ and adding one electron to form NO2– do not affect bond order, length, or energy. In fact, electron count changes the bonding situation: NO2+ has fewer electrons to distribute in bonding, which generally increases bond order, shortens bonds, and increases bond energy relative to NO2–. Therefore this choice is inconsistent with typical bonding trends and is incorrect.

Option 2: a higher, a shorter, a greater. This option states that NO2+ has a higher bond order than NO2–, which would lead to a shorter bond length and greater bond energy. This aligns with the general rule: increasing bond order strengthens and shortens bonds, while decreasing bond order lengthens and weakens them. Since NO2+ has one fewer electron than NO2, the bond order is increased relative to NO2–, making this option internally consistent and correct in direction.

Option 3: a higher, a longer, greater. Here, the bond order is proposed as higher, which is plausible, but the bond length is proposed to be longer. Higher bond order should correspond to shorter, not longer, bond length. The inconsistency between higher bond order and longer bond length makes this option incorrect.

Option 4: a lower, a longer, a smaller. This suggests NO2+ has a lower bond order, longer bond length, and smaller bond energy compared to NO2–. All three consequences (lower order, longer length, smaller energy) go against the expected effect of removing an electron relative to NO2–, making this option implausible.

Option 5: a lower, a longer, a greater. This claims a lower bond order and longer bond length, which is consistent with weaker bonding, but it also asserts greater bond energy, which contradicts the idea that a lower bond order corresponds to lower bond energy. The mismatch between length/ordering and energy makes this option incorrect.

Summary across options: Option 2 coherently matches the trend that removing an electron to form the cation NO2+ increases bond order, shortens the bond, and increases bond energy relative to the anion NO2–. The other options place inconsistent combinations of order, length, and energy that do not align with the general relationship between bond order, bond length, and bond energy.

Question at position 11 A nitrogen-oxygen bond in NO2+ has ______bond order, _bond length, and ________bond energy than a nitrogen-oxygen bond in NO2–. the same, the same, the same a higher, a shorter, a greater a higher, a longer, greater a lower, a longer, a smaller a lower, a longer, a greater

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