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- What is the difference between O O2 - Chemistry Stack Exchange
$\ce O$ is a free oxygen atom and $\ce{O2}$ is two oxygen atoms chemically bound to form an oxygen molecule There is no common analogy for $\ce C$, but $\ce{N2}$ is called nitrogen, $\ce{H2}$ is hydrogen and $\ce{Cl2}$ is chlorine, each having the same name as that of their constituent elements
- Why is oxygen an oxidizing agent? - Chemistry Stack Exchange
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
- 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 paramagnetic? - Chemistry Stack Exchange
To understand the paramagnetic nature of $\ce{O2}$, we must first understand how atomic orbitals mix together to form molecular orbitals In the diatomic molecules of the elements in the second period, a phenomenon known as $\mathrm{s}$-$\mathrm{p}$ mixing results in an increase in the energy of the $\sigma_\mathrm{2p_z}$ molecular orbital, and
- 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
- How to calculate n factor for O2 and H2 in this reaction?
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- Whats the difference between 2O and O2 [duplicate]
$\begingroup$ The 2 O represents two separate oxygen atoms, ( not connected to one another so free to move around and react independently ), the $\ce{O2}$ is molecular oxygen $\endgroup$ – porphyrin
- Comparing O−O bond length in hydrogen peroxide and dioxide(2−) ion
With this we can now see that in $\ce{H2O2}$ there is only two lone pairs on each oxygen atom while in $\ce{O2^2-}$ it has three lone pairs on each atom, hence it has increased lp–lp interaction As a result of this $\ce{O2^2-}$ tends to elongate (relatively more than $\ce{H2O2})$ its bond to decrease this intense lp–lp interaction, hence
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