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Enthalpy of formation of O2 - Chemistry Stack Exchange The enthalpy of formation of O2 is zero at any particular temperature The element is already in its ''standard state'' Also please note that as per IUPAC, there is no standard temperature, it is only convention to use 298 15K to collect standard state data Standard conditions as per IUPAC change depend upon what substance you are dealing with For example, it is defined at standard
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
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
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?
What form of energy is produced by 2H2 + O2 - gt; 2H2O reaction? 0 Thermal energy is released from the reaction $\ce {2H2 + O2 -> 2H2O}$ Before the reaction takes place the system of $\ce {H2}$ and $\ce {O2}$ molecules are in a metastable state: Given enough energy > activation energy the system gains enough energy to overcome the potential barrier and falls into a state of lower energy than the initial state
stability - Why is O2 a biradical? - Chemistry Stack Exchange And finally there is $\ce {O#O}$ where both oxygens are positively charged and are free radicals Why are both positively charged? It is because 3 bonds already to oxygen means 1 lone pair and 5 electrons around oxygen is +1 Is it because of these resonance structures giving 2 free radicals in $\ce {O2}$ that $\ce {O2}$ is considered a biradical?
What is the LUMO and HOMO in and O2 diatomic In the typical way these terms are used, the LUMO can't be the same as the HOMO Since each of the pi spatial orbitals already have one electron, they are not unoccupied, so they can't be the LUMO In the sense of singly occupied spin orbitals, you could say that these pi spin orbitals are the LUMO, but its fairly nonstandard to refer to spin orbitals when discussing HOMO LUMO
How to find the infrared absorption spectrum of O2 and N2? There is a good reason for not being able to find the mid-IR absorption spectra of nitrogen and oxygen Their vibrations are infrared inactive Infrared absorption peaks are observed when there is a change in the dipole moment during a vibration In such cases, one can resort to rotational-vibrational Raman spectroscopy to get molecular information Oxygen does absorb near the deep-red visible