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Using the periodic table

This guide explores electron configuration, focusing on how to use the periodic table. It discusses the relationship between period and energy levels, explaining electron distribution in various orbitals (s, p, d, f). Examples illustrate how to determine the last electron's position and condensed electron configurations, referencing previous noble gases. Unique cases like lanthanum and cerium highlight exceptions in electron filling. Practice with specific elements like Ti, Cl, Sr, Sn, and O reinforces these concepts, making it easier to understand and apply electron arrangements.

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Using the periodic table

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  1. Using the periodic table chapter 4 & 11

  2. Using the periodic table for electron configuration • The period relates to the energy level of electrons • Therefore H and He only have electrons in the 1st energy level • Li, Be, B, C ,N ,O ,F and Ne have electrons up to the 2nd energy level

  3. You can determine the orbital by the placement For these elements the last electron is in the s orbital for these elements the last electron is in the p orbital For these elements the last electron is in the d orbital For the elements the last electron is in the f orbital

  4. Determining the number of electrons in the last energy level • count the number of elements to the left edge of the “section” • For example Al • It is the first element in the 2nd row of p filling elements • The last electron for aluminum will be the first electron possible in the 2nd p

  5. Continuing… • Al • The last electron will be the first possible in the 2nd p • 1 s __ • 2 s __ p __ __ __ • 3 s __ p __ __ __ d __ __ __ __ __

  6. Condensed electron configuration • long electron configurations are not normally written out because it gets rather repetitive • Instead it is condensed, by starting from the previous Noble gas and adding shells to it. • For example K • [Ar]4s1 • This is the same as saying everything that is in Ar (1s22s2p63s2p6) +4s1 • Zr • [Kr]5s24d2 -> [Kr] 4d25s2

  7. To Determine the Condensed electron configuration • Start at the previous noble gas (lower atomic number) • Write out every element in order of atomic number to your given • Determine which shell all elements are filling. The number of elements in that shell is your superscript number.

  8. For Iron • Previous Noble Gas----Ar • Write all elements • K Ca Sc Ti V Cr Mn Fe • These fill 4 s • These fill 3 d • So it is • [Ar]3d64s2

  9. Lone electron in the 5d or 6 d • Odd exception • Lanthanum’s last electron fills the 5d orbital. • Ce has its last electron fill in the 4f, and the one from 5d (La) jumps to 4f. • The next elements all fill up the 4f until Gadolinium which fills up the 5d again. • A similar “jumping” of one electron occurs with the actinide series

  10. Different Periodic Tables • The electron “jumping” is why there are two forms of the periodic table in common usage. • One has lanthanum and actinium in with the d filling elements. • The other has lanthanum and actinium with the f filling elements

  11. Homework • Ignore the exception for all problems • For the following elements • fill in the last shell only of the orbital diagram and do the condensed electron configuration • Ti, Cl, Sr, Sn and O

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