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 . . . Here are the MO schemes of \ceN2 \ce N 2 (left) and \ceO2 \ce O 2 (right) Why is the σ σ -MO formed by the p p AOs energetically above the π π -MO for \ceN2 \ce N 2 but not for \ceO2 \ce O 2? 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
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 are some molecules unable to absorb infrared radiation? Methane $\\ce{CH4}$ is symmetrical and non polar, and so is oxygen $\\ce{O2}$ But $\\ce{O2}$ doesn't absorb IR Why is that? People say that if a molecule can change its polarity then it will absorb
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 an oxidizing agent? - Chemistry Stack Exchange -2 Oxygen (O2) generally exists as diradicals i e each oxygen bonded to each other through single bonds and the remaining two electrons remains on each oxygen atoms as radicals So this structural feature makes oxygen act as a strong oxidizing agent
Enthalpy of the reaction between hydrogen and oxygen In this case, the enthalpy of $484\ \mathrm {kJ}$ is released when $2\ \mathrm {mol}$ of hydrogen gas react with $1\ \mathrm {mol}$ of oxygen gas to form $2\ \mathrm {mol}$ of gaseous water: $$\ce {2H2 (g) + O2 (g) -> 2H2O (g)}\qquad\Delta H^\circ = -484\ \mathrm {kJ}$$ (By way of comparison, the corresponding value for liquid water is about