![]() The p-subshell contains a total of three orbitals, given by the values of #m_l# Furthermore, all half-filled degenerate orbitals contain electrons of the same spin. More specifically, you need to know that all degenerate orbitals must be half-filled before any of them can take in a second electron. ![]() Now, you need to be aware of Hund's rules for filling degenerate orbitals. Next, the magnetic quantum number, #m_l#, which tells you the exact orbital in which you can find the electron. In your case, you're looking for the value of #l# that describes the p-subshell, which means that you will pick The angular momentum quantum number can take values that range from #0# to #n-1#. Next, the angular momentum quantum number, #l#, which tells you the subshell in which you can find the electron. In your case, the highest energy level is equal to #color(red)(5)#, which means that you have So, let's start with the first one, the principal quantum number, #n#, which tells you the energy level on which an electron resides. Notice that you have two electrons that match this profile, both located in the 5p-subshell.Īs you know, four quantum numbers are used to describe the location and spin of an electron in an atom. Now, you're looking for the electron that's highest in energy. So, the electron configuration for tin looks like this - I'll use the noble gas shorthand notation This tells you that a neutral tin atom will have a total of #50# electrons surrounding its nucleus. Tin, #"Sn"#, is located in period 5, group 14 of the periodic table and has an atomic number equal to #50#. Your starting point here will be tin's electron configuration.
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