Electron Configurations

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Presentation transcript:

Electron Configurations -Each element has a unique electron configuration that determines the properties of the element. -These configurations have influenced how the periodic table is organized

Electron Configurations -The principal quantum numbers (1, 2, 3, 4, 5, 6, and 7) correspond to the periods (horizontal rows) on the periodic table. -There are four different kinds of subshells and they only hold a certain number of electrons each. “s” holds 2 electrons “p” holds 6 electrons “d” holds 10 electrons “f” holds 14 electrons

Electron Configurations The order of the subshells and quantum numbers: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d -Electron configurations determine how many valence electrons an element will have based on the highest level orbitals -Patterns in valence electrons determine chemical reactivity

Electron Configurations

Electron Configurations -n: quantum number -l: azimuthal quantum number – the shape of the orbital l values - s: 0 p: 1 d: 2 f: 3 -ml: magnetic quantum number – the orientation of the orbital in space -ms: magnetic spin – the orientation of the orbital in space

Electron Configurations -Pauli Exclusion Principal states that two electrons cannot have the same n, l, ml, and ms quantum numbers and must have opposite spins -Hund’s rule states that electrons will orbit an orbital singly first before pairing up in parallel spins

Electron Configurations

Electron Configurations Shorthand Configuration: [Noble Gas] __s2 __p6 etc -Use the noble gas located periodically before the element you’re looking at and write the rest that follows Examples: Na: [Ne] 3s1 Se: [Ar] 4s2 3d10 4p4

Subshell Review Label the following diagram with the following words: s subshell p subshell d subshell electron orbital