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Two $\ce{OH}$ bonds in any molecule have different dissociation enthalpies, as only the first one is related to the original molecule. The second one is related to the original molecule with the cleav …

Orbitals can be understood in three different but related meanings as: orbital(1) as a particular solution of the above equation, introducing particular integer parameters $n$,$l$,$m_\text{l}$ as "quantum … Orbitals(3) as 3D regions in large extent overlap. Purely mathematically, considering probability density converging to zero in infinity, they fully overlap. …

The ionization energy is the energy deficit the bound electron has with respect to the energy of a free electron in rest. So, if the ionization energy of a $\ce{H}$ atom is $\pu{13.6 eV}$ and if we ta …

There is intense overlapping of orbitals. … Similarly for orbitals. …

It was replaced by the quantum model based on the Schroedinger's wave equation, that came with the concept of orbitals. …

Orbitals have zero charge at the best if empty. …

Generally, forming 2 isolated ions from 2 isolated atoms is not thermodynamically favoured, as ionization energies are higher than electron affinities. But, ion formation is thermodynamically favoured …

From the geometry of used spherical coordinates, it is quite clear that radial nodes are 3D spherical surfaces with constant radius, like for s orbitals. … Analogically, a constant angle of angular nodes leads to a 3D plane intersecting the coordinate origin, like for p orbitals. …

) Electrons in s orbitals have significant occurance probability near nucleus and in inner regions. … Therefore, they are less shielded than electrons in other orbitals with the same $n$ and have the lowest energy of them. …

Both sections do not contradict themselves, as they address different shielding aspects. 3d electrons give worse shielding of 4s/4p electrons than 1-3s and 2-3p electrons. 3d electrons give better sh …

3s, 3p and 3d orbitals all have the same energy in hydrogen atoms ( or monoelectron atomic ions ) according to the nonrelativistic Schroedinger model. … relativistic models of hydrogen atoms shows there is slight difference in their energies, related to the fine structure of spectra and Lamb shift ( Wikipedia Hyperphysics ) For multielectron atoms, s, p, d orbitals …

For the wave function of $\mathrm{s}$ orbital $\psi(r)$, the radial probability is: $P(r)=4\pi r^2 \cdot|\psi(r)|^2$. So even if the differential probability density $|\psi(r)|^2$ is nonzero for $r=0 …

All orbitals largely overlaps and statistical distribution of electron density, (aside of being in the particular orbital) depends on the nucleus charge and overall electron configuration. … OTOH, higher s orbitals have very significant density near nucleus as the local maximum, what leads to relativistic effects due high speed., especially for the near right end of the period 6. …

Similarly, $\mathrm{nf}$ orbitals from originally nth shell belong now rather to the (n+2)th shell. … It is not applicable for transition metals involving partially occupied $\mathrm{d}$ or $\mathrm{f}$ orbitals. …

Every atom has theoretically infinite number of orbitals ( 1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p, 4d, 4f etc), all but some unoccupied. … Similarly, $\ce{LiH}$ has unlimited number of atomic or molecular orbitals ( depending on the quantum model ), as they are features of quantum models, not real objects. …