Quantum numbers and their value

Quantum numbers and their value

1. Quantum numbers

   • Set of numbers and coordinates to locate an electron
     • They are used to describe completely the movement and trajectories of each electron within an atom.
   • Each electron is identified and located by the combination of 4 quantum numbers
     • Principal Quantum Number (n)
       • It designates the principal electron shell. Because n describes the most probable distance of the electrons from the nucleus, the larger the number n is, the farther the electron is from the nucleus, the larger the size of the orbital, and the larger the atom is
         • n can be any positive integer starting at 1
           • n=1,2,3,4,...
           • n can not be 0 or any negative integer, because there exists no atoms with zero or a negative amount of energy levels/principal shells.
             • Example: If the last level of an element is 3p, then n=3
     • Angular Quantum Number (l)
       • It determines the shape of an orbital, and therefore the angular distribution.
         • The value of l is dependent on the principal quantum number n. Unlike n, the value of l can be zero. It can also be a positive integer, but it cannot be larger than one less than the principal quantum number (n-1):
           • l= n-1
             • l=0 "s"
             • l=1 "p"
             • l=2 "d"
             • l=3 "f"
           • Example: If n=3, then l=2. l=0 "s", l=1 "p" and l=2 "d"
     • Sipin Quantum Number (s or ms)
       • It does not depend on another quantum number. It designates the direction of the electron spin and may have a spin of +1/2, represented by↑, or –1/2, represented by ↓.
         • This means that when s is positive the electron has an upward spin, which can be referred to as "spin up." When it is negative, the electron has a downward spin, so it is "spin down."
           • 2 electrons cannot have their 4 quantum numbers equal, at least s will be different
     • Magnetica Quantum Number (m or ml)
       • It determines the number of orbitals and their orientation within a subshell.
         • Its value depends on the orbital angular momentum quantum number l . Given a certain l, m is an interval ranging from –l to +l, so it can be zero, a negative integer, or a positive integer.
           • Example: If l=2 then m= -2, -1, 0, 1, 2

2. Quantum Theory

   • The Uncertainty Principle
     • That says it is impossible to know the exact position at the exact moment of a particle as small as the electron
   • It is used to predict the most likely location of an electron
     • It establishes that around the nucleus there are
       • Levels
         • Sub-levels
           • Orbitals

3. Team members: Frida Leos, Keila Ostos, Patricia Orviz, Javier Torres, Andrew Aranda y Arturo Peña.

   • References
     • -Nissa Garcia. (2017). Principal Quantum Number: Definition & Example. Retrieved August 11, 2017, from http://study.com/academy/lesson/principal-quantum-number-definition-example-quiz.html -Libretexts, Kamenko, A., Enriquez, T., & Lam, M. (2017). Quantum Numbers. Retrieved August 11, 2017, fromhttps://chem.libretexts.org/Core/Physical_and_Theoretical_Chemistry/Quantum_Mechanics/10%3A_Multi-electron_Atoms/Quantum_Numbers

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