How to rationalise with MO theory that CO is a two-electron donor ...
2016年5月16日 · $\ce{CO}$ is isoelectronic with $\ce{N2}$. Sketch MO diagrams for $\ce{CO}$ and $\ce{N2}$. Point out key differences between the diagrams and use the diagram to explain why $\ce{CO}$ acts as a two-electron donor through carbon rather than through oxygen.
Molecular orbital diagram of CO and charge localisation
2020年5月5日 · Particularly, from what I read the reason we envision carbon as being partially negatively charged in CO is that the HOMO of the molecule lies closer to the carbon orbitals. However, from the MO diagram, it can be seen that the p-oxygen orbitals are closer to the HOMO than both of the orbitals of carbon.
Why is the bond length of CO+ less than that of CO?
2014年3月27日 · Hence the orbitals have to become more contracted as the fewer electrons are more attracted. So another reason would be plain and simple electrostatics. (Upon ionisation, the former HOMO of CO also drops below the $\pi$ orbitals in CO(+1) - missing spin pairing, lower electron repulsion, and $\sigma$ is more contracted than $\pi$.) $\endgroup$
How can the dipole moment of carbon monoxide be rationalised …
The MO diagram shows that the $\ce{CO}$ molecule forms three filled MO's with σ symmetry and two MO's with π symmetry. Of the five filled MO's (10 electrons) formed for $\ce{CO}$, only four of them can be half-filled from carbon electrons (4 valence electrons).
Why is the bond order of CO+ 3.5? - Chemistry Stack Exchange
2015年8月30日 · When we have a look at the MO diagram, a calculated version can be found here, we know that the HOMO, i.e. 3σ, is a bonding orbital, while the anti-bonding orbital is the 2σ. Upon ionisation, we would indeed remove one bonding electron and therefore the bond order has to decrease to 2.5 as you suggested.
Help with drawing an Molecular Orbital (MO) diagram for …
2023年6月1日 · 2. Identify the ligands: Here, the ligands are CO and =C(OMe)Ph. The CO ligands are known as pi-acceptor ligands because they can accept electron density from the metal into their pi* antibonding orbitals. This back-bonding interaction would result in the formation of metal-carbon pi bonds, in addition to the metal-carbon sigma bonds.
Why CO is a stronger and more common ligand than N2?
I saw they asked about N2 and O2, I think it is a different explanation because N2 and O2 have very different MO instead N2 and CO are very similar $\endgroup$ – C.X.F. Commented Aug 1, 2019 at 22:59
molecular orbital theory - MO diagram for …
2019年2月13日 · I was considering the MO diagram for [Co(NH3)5Cl]2+, and figured it’d be as follows: 5 sigma interactions from the NH3 ligands; by reducing a reducible representation one obtains 2A1 + B1 + E . 2 pi interactions (pi donation from Cl- …
MO-Scheme of SCN- and its bonding properties when used as a …
2012年6月20日 · The way you presented the formula, $\ce{[Co(en)2(NCS)2]SCN}$, suggested that the SCN-ligand is bound via the nitrogen. If it were bound by the sulfur, the formula might be written $\ce{[Co(en)2(SCN)2]SCN}$. SCN-should have a similar MO diagram to OCN-, which is isoelectronic with CO 2, so your idea to compare to CO 2 is not a bad one
orbitals - Lone pairs in MO theory? - Chemistry Stack Exchange
2017年5月2日 · $\begingroup$ As you started to mention, linear-combination of atomic orbitals (LCAO) with each molecular orbital being required to obey the rules of the full group ($\text{D}_\infty$) for $\text{O}_2$ using only the atomic orbitals designated in the subscripts of the MO. A better choice of orbitals would be using the natural bonding orbitals ...