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Why is oxygen paramagnetic? - Chemistry Stack Exchange Paramagnetic molecules are molecules that have single electrons When I draw the lewis structure of $\\ce{O2}$, it appears to be a diamagnetic structure What makes it paramagnetic?
orbitals - What is the origin of the differences between the MO schemes . . . This phenomenon is explained by s-p mixing All the elements in the second period before oxygen have the difference in energy between the 2s and 2p orbital small enough, so that s-p mixing (combination) can occur lowering the energy of the σ (2s) and σ* (2s) and increasing the energy of the σ (2p) and σ* (2p) molecular orbitals By moving towards right in a period, the s orbital gets more
Is carbon dioxide slightly or highly soluble in water? The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid (Henry's law), which means increasing pressure can increase the solubility of a gas For example, solubility of oxygen $ (\ce {O2})$ at STP is around $\pu {0 0043 g L-1}$ while that of nitrogen $ (\ce {N2})$ is around $\pu {0 0019 g L-1}$ Carbon dioxide $ (\ce {CO2})$, on the
Why do we call O2 oxygen? - Chemistry Stack Exchange 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
Why is oxygen more stable than oxygen dication? 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
Why is oxygen an oxidizing agent? - Chemistry Stack Exchange Why are diatomic oxygen molecules STILL reactive especially with metallic elements like sodium and copper even at room temperature? You would think that since the two oxygen atoms already have the
How to determine whether a given compound is paramagnetic or . . . Paramagnetism is a consequence of having one or more un-paired electrons in the outer electronic configuration e g O2, and NO Most phys chem or inorganic chemistry textbooks will explain this in detail
Is the reaction 2 Hg + O2 → 2HgO a reversible reaction? Are the relative importance of $\ce {2 Hg + O2 -> 2HgO}$ and $\ce {2HgO -> 2 Hg + O2}$ dependent of the temperature ? If so (yes), what is the fundamental reason of the evolution of the relative importance with temperature ?