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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First, let's restate the question and options to be crystal clear about what's being evaluated.
Question: 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.
Answer options: OF2, ICl4–, AsF3, HNO  (N is the central atom)

Now, I will analyze each option one by one and explain why it does or does not meet the criterion, focusing on bond orders in plausible Lewis structures.
Option 1: OF2
- In OF2, oxygen is central with two fluorine atoms bonded to it and two lone pairs on O. The typical Lewis structure features two O–F single bonds and no multiple bonds. The bond order for O–F in this structure is 1 for each bond.
- Could there be an alternative Lewis structure for OF2 that yields a bond order different from 1? In standard Lewis constructions for OF2, there is no reasonable resonance structure that creates a double bond between O and F without violating formal charge considerations or expanding octets for fluorine. Therefore, all bonds effectively have bond order 1 in the common valid structures under the stated constraint (zero charges on halogens).
- Conclusion for OF2: all bonds have bond order 1 in the typical valid Lewis structures, so it does not meet the criterion of having a bond order ≠ 1.

Option 2: ICl4–
- ICl4– features iodine at the center with four chlorine atoms around it and an overall −1 charge. The common Lewis structure places four I–Cl single bonds with iodine in a square planar arrangement, and the charge is delocalized in a way that maintains single bonds to each Cl.
- As with other halogen-containing species, the instruction specifies considering structures with zero formal charges on the halogen atoms. In the conventional valid resonance forms for ICl4– that satisfy this charge condition, the I–Cl bonds are still treated as single bonds; bond orders remain 1.
- Conclusion for ICl4–: bond orders are 1 for all I–Cl bonds in the typical, charge-appropriate Lewis structures, so it does not have a bond order ≠ 1.

Option 3: AsF3
- In AsF3, arsenic is the central atom bonded to three fluorine atoms, with one lone pair on As. The common Lewis structure shows three As–F single bonds and a lone pair on As.
- Similar to the previous cases, there is no standard resonance form that converts any of the As–F bonds to a multiple bond without violating typical valence and formal charge considerations for fluorine (which prefers a single bond form in these neutral or near-neutral species). Thus, the bond orders remain 1 for each A–F bond in valid structures under the halogen-zero-charge condition.
- Conclusion for AsF3: all bonds have bond order 1 in feasible Lewis structures, so it does not meet the criterion.

Option 4: HNO  (N is the central atom)
- Here, nitrogen is the central atom bonded to hydrogen and oxygen. A common Lewis structure for HNO involves an N–H bond and an N–O bond, with possibilities for multiple bonding depending on formal charge distribution (for example, N–O with a double bond and the N–H bond being a single bond, or other resonance forms that place a double bond between N and O in at least one resonance form).
- Importantly, there exist valid Lewis structures for HNO in which the N–O bond is a double bond (bond order 2) while the N–H bond remains a single bond (bond order 1). This yields at least one bond with bond order different from 1 (specifically, the N=O bond has bond order 2).
- Therefore, HNO (with N as the central atom) satisfies the criterion of having at least one bond with bond order ≠ 1 in its Lewis structures.

Summarizing the reasoning across options:
- OF2: all bonds are effectively single bonds in valid structures under the halogen-zero-charge guideline.
- ICl4–: I–Cl bonds are single bonds in charge-consistent resonance forms.
- AsF3: all A–F bonds are single bonds in typical Lewis structures.
- HNO (N central): there exist resonance forms with N–O as a double bond, giving a bond order of 2 for N–O, so at least one bond has bond order ≠ 1.

Thus, the option that satisfies the condition is the one with a central-nitrogen structure that allows a multiple bond to oxygen in its Lewis representations.

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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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)

View Explanation

Log in for full answers

Similar Questions

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

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 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

More Practical Tools for Students Powered by AI Study Helper

Making Your Study Simpler

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