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subshell    
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  • 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)
  • What are the maximum number of electrons in each shell?
    Each subshell contains a specified number of orbitals, and each orbital can hold two electrons The types of subshells available to a shell and the number of orbitals in each subshell are mathematically defined by quantum numbers
  • What comes after f-orbitals, and in what order are they filled?
    I know about s, p, d, and f-orbitals However, my physical chemistry textbook does not mention what comes after f-orbitals What are the next letters, and in what order are these higher orbitals fi
  • electronic configuration - Chemistry Stack Exchange
    I am a beginner trying to summarize what I've learned about: Shells Energy Levels Subshells and Orbitals all at the high school level Unlike related threads, I'm going to try to: Define each wo
  • Why is f and s orbital considered valence orbitals
    The valence subshell is the subshell involved in chemical bonding For s- and p-block elements, their outermost subshells are their valence subshells However, for d- and f-block elements, when they are donating electrons, their outermost subshell becomes the valence subshell
  • 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 of uranium - Chemistry Stack Exchange
    I read that the electronic configuration of uranium is [Rn] 5f³ 6d¹ 7s² Given that the subshells fill in the order 5f --> 6d, why is the 5f subshell only partially filled? Why do electrons fill
  • Fundamental doubts about energy levels vs. shells vs. subshells vs . . .
    Is the person referring to the Aufbau Principle i e the orbitals in the $4s$ subshell have lower energy than the orbitals in $3d$ subshell? If I have used any terminology incorrectly, please do let me know
  • How many electrons can an orbital of type f hold?
    You're correct that there are seven possible spatial orientations for an f-type orbital, and hence seven possible orbitals in one f-type sub-shell However, the question specifically asks for the maximum number of electrons in one such orbital, and any single atomic orbital, regardless of the sub-shell type specified by l l, can only hold two electrons This is by virtue of the Pauli exclusion
  • Confusion in half filled or full filled electronic configuration
    Having a half-filled or filled subshell is stabilising, as you say But for Cl, the difference in energy between 3s and 3p is greater than the additional stabilisation from filling the 3p subshell 3d and 4s are closer in energy, so for Cr it is favourable to promote a 4s electron and have a 4s configuration





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