Which of the following nitrogen oxide molecules and related ions is/are diamagnetic and has/have more than two charge-minimized resonance structures?
1. NO
2. NO2
3. N2O4
4. NO2-
It's N2O4. I'm doing the same quiz right now lol.
why not #4? that has two resonance structures and it is isoelectronic to ozone which is diamagnetic.
u guys should know better than to cheat :P
To determine which nitrogen oxide molecules and ions are diamagnetic and have more than two charge-minimized resonance structures, we need to analyze the molecular structure and the presence of unpaired electrons.
Diamagnetic molecules have all paired electrons, while paramagnetic molecules have at least one unpaired electron. Additionally, ions with charge-minimized resonance structures have more than one possible arrangement of electrons.
Let's go through each option:
1. NO (nitric oxide):
Nitric oxide (NO) molecule has one unpaired electron, so it is paramagnetic. It has only one charge-minimized resonance structure.
2. NO2 (nitrogen dioxide):
Nitrogen dioxide (NO2) molecule has two unpaired electrons, making it paramagnetic. It has two charge-minimized resonance structures.
3. N2O4 (dinitrogen tetroxide):
Dinitrogen tetroxide (N2O4) molecule does not have any unpaired electrons, so it is diamagnetic. It has three charge-minimized resonance structures.
4. NO2- (nitrite ion):
Nitrite ion (NO2-) has one unpaired electron, making it paramagnetic. It has two charge-minimized resonance structures.
In conclusion, the molecule N2O4 is diamagnetic and has more than two charge-minimized resonance structures.