If c is carbon and then why $\ce {o2}$ is oxygen. 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. I just saw something in a chemistry lesson what got me confused
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What is the difference between $\\ce{2o}$ and $\\ce{o2}$
By moving towards right in a period, the s orbital gets more.
Paramagnetic molecules are molecules that have single electrons When i draw the lewis structure of $\\ce{o2}$, it appears to be a diamagnetic structure 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. Methane $\\ce{ch4}$ is symmetrical and non polar, and so is oxygen $\\ce{o2}$ But $\\ce{o2}$ doesn't absorb ir People say that if a molecule can change its polarity then it will absorb.
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. To calculate the dissolved oxygen in water at saturation pressure at 25 °c, we do $$ d_\\ce{o2} = k_\\mathrm{h} \\times m \\times p_\\mathrm{g} $$ $$ d_\\ce{o2.
