What is the dominant Lewis structure for N2O?

Question

BlackTom AI · Accepted Answer

Question: What is the dominant Lewis structure for N2O?
Options: I, II, III, IV, I am unsure and need to study this concept to prepare for the exam

Step-by-step analysis of each option:

Option I: This structure likely places bonds and lone pairs in a way that either violates octet rules for one of the atoms or assigns an unfavorable distribution of formal charges. If any atom ends up with an incomplete octet or an excessive formal charge on a less electronegative atom, this form is less favorable as a canonical contributor.
Rationale: For N2O, the dominant form should satisfy the octet for N and O as much as possible and place the negative formal charge on the more electronegative element (oxygen) while keeping formal charges minimal in magnitude overall. If I allocates charges inconsistently or places a negative charge on nitrogen (less electronegative than oxygen), it is less plausible as the major contributor.

Option II: This structure likely depicts a different connectivity or bond order (for instance, perhaps a single bond between N and O or a non-terminal arrangement) that breaks the preferred octet fulfillment or misplaces charges. A single bond to oxygen in N2O would force less favorable formal charges and/or over- or under-occupied octets for nitrogen atoms.
Rationale: The dominant resonance form should reflect the correct bonding pattern (N≡N–O or equivalent major contributor) with proper octets and the negative charge on oxygen rather than nitrogen when possible. If II places a formal negative charge on nitrogen or disrupts the octet, it is not the best contributor.

Option III: This structure may portray an alternative bonding arrangement (such as N=N=O or a different branching) that is inconsistent with the preferred Lewis depiction of N2O. Such a form would typically create an unfavorable charge distribution or violate octet requirements for one of the atoms.
Rationale: A valid major contributor for N2O is not a cumulated positive/neutral setup that ignores electronegativity considerations or octet satisfaction. If III misplaces multiple bonds or charges, it’s not the dominant form.

Option IV: This structure positions the bonds as N≡N–O (with the appropriate lone pairs) and assigns formal charges consistent with the dominant resonance form: the negative formal charge resides on oxygen (the more electronegative atom), and the overall molecule remains neutral. The octets are satisfied for all atoms, and the bond pattern reflects the typical valence arrangement for N2O.
Rationale: This form aligns with chemical reasoning: octet fulfillment for N and O, minimal and appropriately placed formal charges, and the convention that the negative charge appears on oxygen in oxides of nitrogen when possible. Among the options, IV best meets these criteria and is therefore the dominant Lewis structure.

Option 'I am unsure and need to study this concept to prepare for the exam': While honest, this choice does not engage with the structural reasoning needed to compare canonical forms. For learning, one should evaluate the octet rules and formal charges to determine the most plausible structure.

Summary: The dominant Lewis structure for N2O should feature a N≡N–O connectivity with the negative formal charge on the oxygen and proper octet satisfaction for all atoms. Among the choices, IV uniquely matches this description and thus is the most accurate representation.

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

What is the dominant Lewis structure for N2O?

查看解析

登录即可查看完整答案

类似问题

Which of the following Lewis structures are incorrect? There may be more than one.

In the most plausible Lewis structure for SOF4, there are

Draw the most stable Lewis structure for H2CS and complete the following statements. I: The total number of nonbonding pairs of electrons on the sulfur atom is [ Select ] 0 3 1 2 . II: The bond between the carbon and sulfur atoms is a [ Select ] triple bond double bond single bond . 07A

Based on formal charges, which of the three Lewis structures shown for CH2ON– is the dominant Lewis structure? 10A

Choose the best Lewis structure that describes the bonding in the SeO32— ion.

Draw the best Lewis structure for the SNF molecule. How many single bonds, double bonds, triple bonds, and lone-pair of electrons are found around the central atom?

Lewis structures help visualise the valence electrons in a molecular structure, whether they form bonds between atoms or not. Valence electrons not involved in bonding are called:

Identify the correct Lewis structure of H3O+. Ensure that all charges and lone pairs are shown.

更多留学生实用工具

考试浏览器助手

风格化写作助手

论文查重助手

文献引用助手

课堂转译助手

课堂笔记助手

Quiz搜索助手

学校历年真题

智能刷题助手

智能匹配练习

希望你的学习变得更简单