1 / 19

Electron Configurations and Periodic Properties

This comprehensive overview covers key concepts in atomic structure, particularly atomic radii, ionization energy, and electron affinity. Discover how atomic radius is defined and its trends across periods and down groups, influenced by effective nuclear charge and electron shielding. Learn about ionization energy, including the process of ion formation and trends in energy requirements for electron removal. The section on electron affinity explains energy changes associated with gaining electrons and the variation in trends. Explore the properties of cations and anions, as well as valence electrons and electronegativity trends.

priscilla-boyd
Download Presentation

Electron Configurations and Periodic Properties

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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)

More Related