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What is the difference between $\ce {o}$ and $\ce {o2}$ However, the standard reduction potential of diatomic oxygen in basic conditions is only +0.40 volts If c is carbon and then why $\ce {o2}$ is oxygen.
I just saw something in a chemistry lesson what got me confused The standard reduction potential of diatomic oxygen in acidic conditions is +1.23 volts 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 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. 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.
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 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.
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