Difference between shells, subshells and orbitals Chemists describe the shell and subshell in which an orbital belongs with a two-character code such as 2p or 4f The first character indicates the shell (n = 2 or n = 4) The second character identifies the subshell
orbitals - Difference between subshell and sub-subshell? - Chemistry . . . What the authors are noting is that the 2p subshell will have three orbitals which can support two electrons each Each of these three orbitals is being referred to as a sub-subshell As I said it seems a very uncommon term, and I'd suggest you avoid using it
Fundamental doubts about energy levels vs. shells vs. subshells vs . . . As an example, when we refer to an electron as being in the 1s subshell (or equivalently in a 1s orbital), we are specifying its energy and angular momentum (but not spin) quantum numbers ($\ce{n=1, l=0, m_l=0}$), and thereby its energy and angular momenta (but not spin angular momentum) The energy of an electron in the 1s shell can be
What are the maximum number of electrons in each shell? In my textbook, it says that the maximum number of electrons that can fit in any given shell is given by 2n² This would mean 2 electrons could fit in the first shell, 8 could fit in the second she
theoretical chemistry - What are similarities and differences among . . . A subshell is e g 1s, 2s, 2p, 3s, 3p, etc Yes The periodic table is organized into s-block and p-block (main group elements), d-block (transition metals) and f-block (lanthanides and actinides) according to which subshell is partially filled (or just filled) The quantum number that defines the subshell is the second quantum number, $\ell$
electronic configuration - Why does increasing subshell cause . . . I know that increasing subshell decreases ionization energy; for example, going from Beryllium to Boron I do not understand why this is The answer my textbook (Chemistry 2e on OpenStax) gives is that the higher subshells (eg $\ce{p}$ ) has more energy than the lower subshells (eg $\ce{s}$ )
physical chemistry - Why is the d subshell only stable when all of its . . . In the transition elements of the fourth period, the $3d$ subshell lies at higher energy than the $4s$ subshell -- when the atoms are neutral But the electronic energy levels change when you remove typically two or three electrons to form an ion of any of these elements in their most common salts
inorganic chemistry - Energy of electrons in the same subshell . . . To be clear, a Nx subshell electron will never have more energy than a (N+1)x subshell electron* (except possibly during the transition from one energy level to another, but thinking of an electron which has absorbed more energy than it can have in a sub-shell, thinking of that electron as still in that sub-shell, is a matter of definition and