Search Results

However, in bonding, d orbitals will not be involved in the ground state bonding orbital of a molecule if there are not enough electrons and not enough energy to initially fill the d atomic orbitals. … As soon as there are enough electrons, as in transition metal complexes, d orbitals become essential to understanding bonding. Note: (I'm ignoring ideas such as hybridisation between orbitals) …

For other orbitals, e.g $2p_{\pm 1}$ the wavefunction is a function with complex numbers so cannot represent anything physical. …

(If orbitals are on different atoms, the wavefunctions now have to be represented with respect to a common set of coordinates, i.e. the equations for orbitals, say, on atoms A and B, must use the same …

To be able to draw these, and to make chemical sense, we have to combine them together so that they are no longer complex numbers, and this is what is done to form the p orbitals etc. …

In forming bonds from atomic orbitals the parity of the wavefunction is important. … Anti-bonding orbitals always have nodes. Nodal planes are also important in Diels Alder addition and similar reactions as here symmetry is important. …

As the atomic orbitals are normalised the maximum overlap is 1 and minimum zero. The overlap only contains contributions from regions of space where where the atomic orbitals are not zero. … Note, however, if the atomic orbitals are orthogonal to one another the overlap integral is zero at all distances. …

The visible transitions in the $\ce{H}$ atom were observed experimentally to follow the equation $$\overline{\nu} = R_H\left(\frac{1}{n_1^2} - \frac{1}{n_2^2}\right)$$ where $R_\ce{H}$ is the Rydbe …

Imagine that the $x$ axis and $y$ axis lobes have a different color (phase). Locate the principal axis, that of highest rotational symmetry, if there is more than one just choose one. A $C_2$ or 180 …

The total energy of the d orbitals before and after the application of the octahedral (cubic) field has to be the same. As three levels fall and two rise, the ratio is as shown. …

This happens because the $z$-axis ligand has more effect on $\mathrm d_{z^2}$ than on $\mathrm d_{x^2-y^2}$ orbitals simply due to its position. …

This does not seem to make any sense to me either unless I'm missing something very obvious. Suffice it to say that spin changing transitions are generally strongly forbidden, unless paramagnetic elec …

First you need to have the ground state electron configuration, for Neon this is 1s$^2$2s$^2$2p$^6$ or what ever it is for your atom. This will give you the term symbol for the ground state. The excit …

These orbitals represent the angular part of the wavefunction. … The other orbitals are also linear combinations e.g. …

The picture shows a triplet excited state returning to the ground state by emitting a photon, i.e. phosphorescence. This can only happen if there is also an interaction that couples angular momentum c …

You can only do what you suggest (make product) if the electrostatic repulsion between the two electrons is ignored. This means that there are two single electron equations (just as for hydrogen but w …