2014年10月15日 · Now, in the other answer, there is some discussion about spin-orbitals, meaning that each electron would exist in its own orbital. For practical purposes, you don't need to worry about that - by the time those sorts of distinctions matter to you, there won't be any confusion about what people mean by "shells" and "sub-shells."

2015年11月13日 · Thus all orbitals with designation 3 have 3 zones where the probability of finding an electron is zero. 3s has 2 spherical nodes (the 3rd zone is infinite distance from the atom.) 3p has one planar and 1 spherical node. 3d has 2 …

2014年9月12日 · These regions may have different spatial functions. "Orbital" is a word that can be used to describe that spatial function\distribution of electrons. In that sense of the word, orbitals exist, just as the spatial distribution of the electron exists. Perhaps this is more a semantics issue. $\endgroup$ –

2014年2月20日 · s-orbitals can hold 2 electrons, the p-orbitals can hold 6 electrons. Thus, the second shell can have 8 electrons. The n=3 (third) shell has: The 3s orbital; The 3p orbitals; The 3d orbitals; s-orbitals can hold 2 electrons, p-orbitals can hold 6, and d-orbitals can hold 10, for a total of 18 electrons. Therefore, the formula $2n^2$ holds!

These orbitals have different shapes (e.g. electron density distributions in space) and energies (e.g. 1s is lower energy than 2s which is lower energy than 3s; 2s is lower energy than 2p). (image source) So for example, a hydrogen atom with one electron would be denoted as $\ce{1s^1}$ - it has one electron in its 1s orbital

2022年7月27日 · This gels with Bohr's idea of electrons occupying fixed orbits about the nucleus. Despite being incorrect, the fixed orbit idea is useful when trying to visualize how energy levels and electron distributions (such as represented with orbitals, see below) in a hydrogen atom (or a hydrogenic atom, one with a single electron) are related.

2016年4月9日 · This, in turn means that the electron's spin is the property of the electron. Another view of this situation is that there are two orbitals, a 1s spin up and a 1s spin down. This implies the electron's spin is the property of the orbital. Since orbitals don't really exist, noone may say which is a correct interpretation.

2023年1月13日 · Orbitals describe the probability of finding electrons in a particular region of space. And, indeed, in some types of orbitals (eg 1s) there is finite probability of the electron overlapping the nucleus (2p orbital have a node there so this isn't true for them): this matters for some other quantum effects involving nuclei and electrons.

2014年7月11日 · The pictures that we typically use to represent orbitals are really just graphs showing the 3-dimensional probability of finding an electron (that occupies the orbital being examined) in space. $\ce{\Psi}$ is the wavefunction that describes the electron with a set of specific quantum numbers.

2020年10月24日 · The symmetry (parity) determines whether two orbitals can combine to form a bonding orbital or anti-bonding one, e.g. $\sigma$ or $\sigma ^*$ or $\pi$ or $\pi ^*$. Anti-bonding orbitals always have nodes. Nodal planes are also important in Diels Alder addition and similar reactions as here symmetry is important.