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jacob193

[tex]l = 1[/tex].

Explanation

Each electron in an atom comes with a unique set of four quantum numbers.

  • [tex]n[/tex] gives the main shell of an electron.
  • [tex]l[/tex] gives the type of the sub-level (a.k.a. orbital, s, p, d, f, ...) that the electron occupies.
  • There can be more than one orbitals in a sub-level. Consider [tex]m_l[/tex] as the index for the electron's orbital.
  • Each orbital holds two electrons. [tex]m_s[/tex] tells those two electrons apart based on the direction of each electron's spin.

The question is asking about different types of sub-levels. That depends on the angular / azimuthal quantum number, [tex]l[/tex].

[tex]l[/tex] is an integer. It ranges from [tex]0[/tex] all the way to [tex]n - 1[/tex].

  • An electron with [tex]l = 0[/tex] is in an [tex]s[/tex] orbital.
  • An electron with [tex]l = 1[/tex] is in a [tex]p[/tex] orbital.
  • An electron with [tex]l = 2[/tex] is in a [tex]d[/tex] orbital.

In other words, the quantum number [tex]l= 1[/tex] represents a [tex]p[/tex] sublevel.

Reference

Vitz, Ed et al. "Quantum Numbers (Electronic)", ChemPRIME (Moore et al.). Chemistry Libretexts.

"Quantum Mechanics and Atomic Orbitals", Chemistry - The Central Science (Brown et al.). Chemistry Libretexts.

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