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Electron Configurations and Periodic Properties

Electron Configurations and Periodic Properties. 5.3. Atomic Radii. Atomic radius – ½ the distance between the nuclei of identical atoms that are bonded together. Can be difficult to measure. Atomic Radius. Trend: Decreases across a period b/c effective nuclear charge

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Electron Configurations and Periodic Properties

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  1. Electron Configurations and Periodic Properties 5.3

  2. Atomic Radii • Atomic radius – ½ the distance between the nuclei of identical atoms that are bonded together. • Can be difficult to measure

  3. Atomic Radius • Trend: • Decreases across a period • b/c effective nuclear charge • Increases down a group • more E levels / electron shielding

  4. Atomic Radii

  5. Ionization Energy • You can remove an e- from an atom if enough E is supplied • A + energy = A+ + e- • The A+ is an ion of that atom w/ +1 charge

  6. Ionization Energy • Ion – atom or group of bonded atoms that has a + or – charge • Ionization – any process that results in the formation of an ion • Ionization energy – the E required to remove 1 e- from a neutral atom of an element (aka First Ionization Energy IE1

  7. Ionization Energy

  8. Ionization Energy • The Trend • Increase across a period • B/c increase effective nuclear charge • Decrease going down the group • e- further out – electron shielding

  9. Removing e- from + ions • If enough E is supplied, you can remove more e- • Called second ionization E, or third ionization E, & so on • 2nd and 3rd are always higher than previous b/c effective nuclear charge

  10. Electron Affinity • Electron Affinity – the E change that occurs when an e- is acquired by a neutral atom • Some give off E = A + e-  A- + E • Some require E = A + e- + E = A- • These are unstable and hard to determine

  11. Electron Affinity • Trend: • Increases across a pd (except nob. gas) • Increasing nuclear charge • Decreases down a group • Increase in e- shielding b/c larger atomic radius

  12. Electron Affinity • 2nd e- affinities are always more positive (requires more E) than 1st e- affinities

  13. Ionic Radii • Cation – a positive ion • Made from the loss of an e- • Creates smaller radii • Anion – a negative ion • Addition of 1 or more e- • Creates a larger radii

  14. Ionic Radii • Trend … • Cationic and anionic radii decrease across a pd • B/c increasing nuclear charge • Both increase down a group

  15. Ionic Radii

  16. Valence Electrons • V.E. – e- available to be lost, gained, or shared in the formation of chemical compounds • Located in incompletely filled main-E levels • For MGE – located in outermost s&p

  17. Electronegativity • e-neg – a measure of the ability of an atom in a chemical compound to attract e- from another atom in the cmpd. • Trend… (NOBLE GASES EXEMPT) • Increase across pd. • Decrease down a group

  18. Electronegativity

  19. Properties of the d and f block • Not as straight forward as the others • e- fill in lower E levels for these blocks so some differences occur • Some E levels promote or demote e- to obtain more stability (4s13d5)

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