The values of ml in a subshell range from +l to -l. The magnetic quantum number, represented by ml, tells you the specific orbital within the subshell an electron is in. The values of l correspond to the subshell letters, so: l=0 is s, l=1 is p, l=2 is d, and l=3 is f. The subshell tells us broadly the shape the orbitals which hold the electrons take on and these are represented by the letters s, p, d, and f. Electrons in the second electron shell can have a value of l=0 AND 1 since n=2, and so on. So electrons in the first electron shell can only have a value of l=0 since n=1. The allowed values of l in an electron shell are determined by: l = n-1. The angular quantum number tells you the subshell an electron is in within an electron shell and is represented by the letter 'l' often. So elements in the first row of the periodic table have the first electron shell, or n=1, as their valence shell or outermost electron shell. The principal quantum number, often represented by n, is another term for the electron shell and are positive integer values (n=1,2,3,etc.) These electron shell numbers broadly correspond to the period, or row, an element is in. ![]() Due to the Pauli exclusion principal no two electrons can have exactly the same quantum numbers. ![]() These include the principal quantum number, the angular quantum number, the magnetic quantum number, and spin quantum number. ![]() These regions where we find electrons are represented by the quantum numbers, of which there are four. So electrons exists in clouds in a way around the nuclei of atoms.
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