With respect to the carbon-oxygen bonds, CO32– has a __________ bond length and a __________ bond order compared to H2CO.

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BlackTom AI · Accepted Answer

Question restatement: We’re comparing carbon-oxygen bonds in CO3^2− and in H2CO, and need to choose the correct description of bond length and bond order.
Option 1: 'longer; larger' This would imply CO3^2− has longer bonds than H2CO and a higher bond order. While the bond length in carbonate is indeed longer than a typical C=O, the bond order cannot be larger than in a normal C=O double bond; carbonate features resonance with bond orders around 1.3–1.5 per bond, not higher than a double bond. So this option is inconsistent with established bond character.
Option 2: 'longer; smaller' Here, CO3^2− would have longer bonds and a smaller bond order compared to H2CO. This aligns with chemical reasoning: in carbonate, three equivalent C–O bonds arise from resonance structures that delocalize electron density, giving bond orders between a single and a double bond (approximately 1.3–1.5), and the bond lengths are longer than the typical C=O double bond found in formaldehyde (H2CO).
Option 3: 'smaller; larger' Claiming CO3^2− bonds are shorter and have a larger bond order contradicts resonance effects in carbonate. The delocalization reduces bond order below 2 and lengthens bonds compared with a true C=O double bond, so this option is inaccurate.
Option 4: 'smaller; smaller' This would say both shorter bonds and smaller bond orders, which would imply stronger multiple bonding than actually present in carbonate relative to formaldehyde. Since carbonate bonds are delocalized and not true double bonds, the bond order is not that high, but the bond lengths are not shorter than C=O, so this is misleading.
Option 5: 'I am unsure and need to study this concept to prepare for the exam' This is a non-answer reflecting lack of confidence rather than a chemical interpretation. It does not address the question’s substance and should be avoided in an assessment.
Synthesis of reasoning: In carbonate CO3^2−, all C–O bonds are equivalent due to resonance; each bond has partial double-bond character, yielding a bond order around 1.5 (between single and double). Because bond order correlates inversely with bond length, these bonds are longer than a typical C=O double bond found in H2CO, which has a true C=O bond order of 2.0. Therefore, the correct characterization is that CO3^2− has longer bonds and smaller bond order compared to H2CO.
Putting it together, the option that matches this description is 'longer; smaller'.

CHEM 1210 AU2025 (15738) CHEM 1210 Practice Exam #4 v2 (Ch 7.1–7.4, 8, 9.1–9.6)- Requires Respondus LockDown Browser

With respect to the carbon-oxygen bonds, CO32– has a bond length and a bond order compared to H2CO.

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CHEM 1210 AU2025 (15738) CHEM 1210 Practice Exam #4 v2 (Ch 7.1–7.4, 8, 9.1–9.6)- Requires Respondus LockDown Browser

With respect to the carbon-oxygen bonds, CO32– has a __________ bond length and a __________ bond order compared to H2CO.

View Explanation

Log in for full answers

Similar Questions

List the following molecules in order of increasing bond order: 1. C=C 2. C-C 3. CΞC

List the following molecules in order of increasing bond order: 1. C=C 2. C-C 3. CΞC

Question at position 11 Which of the following has a Lewis structure in which at least one bond has a bond order ≠ 1? For species with halogen atoms, consider only Lewis structures with zero formal charges on the halogen atoms. OF2 ICl4– AsF3 HNO (N is the central atom)

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With respect to the carbon-oxygen bonds, CO32– has a bond length and a bond order compared to H2CO.

Question at position 2 An N≡N bond has a __bond order, bond length, and bond energy than a N═N bond. higher, longer, greater lower, longer, greater higher, longer, smaller higher, shorter, greater lower, longer, smaller lower, shorter, greater