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What is the difference between $\ce {o}$ and $\ce {o2}$ Depending on this hypothesis oxygen have 5 oxidation states If c is carbon and then why $\ce {o2}$ is oxygen.
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I just saw something in a chemistry lesson what got me confused The concept of oxidation state simply works on concept of electronegativity.the more electronegative atom acquire a negative charge while less electronegative atom acquire a positive charge What is the difference between $\\ce{2o}$ and $\\ce{o2}$
Paramagnetic molecules are molecules that have single electrons
When i draw the lewis structure of $\\ce{o2}$, it appears to be a diamagnetic structure Here are the mo schemes of \cen2 \ce n 2 (left) and \ceo2 \ce o 2 (right) Can it be explained this way In second period elements with more than a half filled \cep \ce p orbitals, the energy pattern of the mos is regular
In second period elements with less than or half. Likewise $\ce {o2}$ is as much oxygen as atomic oxygen is The only complication is that what we habitually think of as oxygen is oxygen as a gas comprised of $\ce {o2}$ molecules Like humpty dumpty in alice in wonderland, a word means what [we] choose it to mean and often we have to add modifiers or alternate terms to avoid ambiguity.
So why is molecular oxygen $\ce {o2}$ more stable than the molecular ion $\ce {o2^2+}?$ one possible reason that comes to mind is that the antibonding (ab) orbitals, although higher in energy than the constituent atomic orbitals, are still negative in energy, so adding electrons to ab orbitals still lowers the energy.
5 why is the melting point of nitrogen ($\ce {n2}$) greater than that of oxygen ($\ce {o2}$) In addition, why is the boiling point of both opposite? Before the reaction takes place the system of $\ce {h2}$ and $\ce {o2}$ molecules are in a metastable state Given enough energy > activation energy the system gains enough energy to overcome the potential barrier and falls into a state of lower energy than the initial state.
Or inorganic chemistry textbooks will explain this in detail.
