Discussion Overview
The discussion revolves around the application of the octet rule to the molecules NO2 and ClO-. Participants explore whether these molecules adhere to the octet rule, with a focus on their structural representations and resonance forms.
Discussion Character
- Debate/contested
- Technical explanation
- Conceptual clarification
Main Points Raised
- Some participants question whether NO2 obeys the octet rule, noting that NO2+ does, but expressing uncertainty about the neutral NO2.
- One participant suggests that NO2 exists as a resonance hybrid, where nitrogen typically forms three bonds and oxygens form two, implying a complex bonding scenario.
- Another participant asserts that ClO- does obey the octet rule, comparing it to hydroxide (HO-) and suggesting that chlorine can achieve a complete octet with appropriate lone pairs.
- A participant challenges the representation of bonds in NO2, questioning the idea of 'half bonds' and suggesting that additional bonding interactions between oxygen atoms might be necessary.
- One participant claims that nitrogen in NO2 does not obey the octet rule, referencing its behavior in the liquid phase and discussing the stability of N2O4 as a related compound that does obey the rule.
- There is a discussion about the nitrogen-nitrogen bond in N2O4, with participants clarifying that nitrogen typically forms three bonds and referencing other nitrogen compounds to support their points.
Areas of Agreement / Disagreement
Participants express differing views on whether NO2 and ClO- adhere to the octet rule, with no consensus reached. The discussion includes multiple competing interpretations of the bonding and structural characteristics of these molecules.
Contextual Notes
Participants mention various assumptions about bonding and resonance structures, and there are unresolved questions regarding the nature of bonds in NO2 and the implications for the octet rule.