1 / 17

Electron Configuration

Electron Configuration. A Closer Look at Electrons. Where are they in the Atoms?. Located within energy levels Energy levels range from 1-7 Higher energy levels The electron (e-) is farther from the nucleus The more energy the e- has. Energy Level Changes.

ralphcox
Download Presentation

Electron Configuration

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 Configuration A Closer Look at Electrons

  2. Where are they in the Atoms? • Located within energy levels • Energy levels range from 1-7 • Higher energy levels • The electron (e-) is farther from the nucleus • The more energy the e- has

  3. Energy Level Changes • An electron absorbsenergy to “jump” to a higher energy level. • When an electron falls to a lower energy level, energy is emitted. • In the visible range, the emitted energy appears as a color.

  4. Electron Energy Levels Electrons are arranged in specific energy levels that • are labeled n = 1, n = 2, n = 3, and so on • increase in energy as n increases • have the electrons with the lowest energy in the first energy level (n = 1) closestto the nucleus

  5. Within each energy level • There are sublevels that differ by slight differences in energy • There are four sublevels • S, P, D, F • Within each sublevel are paths called Orbitals

  6. Number of Sublevels

  7. Orbitals • S sublevels, there is 1 orbital, which holds a total of 2 e- • P sublevels, there are 3 orbitals, holding a total of 6 e- • D sublevels, there are 5 orbitals, holding a total of 10 e- • F sublevels, there are 7 orbitals, holding a total of 14 e-

  8. Writing The e- configuration 1s2 1 = the energy level S = the sublevel or orbital 2= the number of electrons

  9. What order do orbitals fill?

  10. How to write an e- configuration • Locate the element on the periodic table. 2. Fill the orbital in the proper order. 3. Check that the total # of e- you have equals the atomic # for that element

  11. Complete filling order • 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

  12. Orbitals An orbital • is a three-dimensional space around a nucleus where an electron is most likely to be found • has a shape that represents electron density (not a path the electron follows) • can hold up to 2 electrons • contains two electrons that must spin in opposite ↑↓

  13. s Orbital's • An s orbital • has a spherical shape around the nucleus • increases in size around the nucleus as the energy level n value increases • is a single orbital found in each s sublevel

  14. p Orbitals A p orbital • has a two-lobed shape • is one of three p orbitals that make up each p sublevel • increases in size as the value of n increases

  15. Sublevels and Orbitals Each sublevel consists of a specific number of orbitals. • An s sublevel contains one s orbital. • A p sublevel contains three p orbitals. • A d sublevel contains five d orbitals. • An f sublevel contains seven f orbitals.

  16. Practice problems • Write the electron configuration for the following elements • Carbon (C) • Lithium (Li) • Sodium (Na) • Chlorine (Cl) • Potassium (K) • Iron (Fe)

  17. Orbital Diagrams • An orbital diagram represents each orbital with a box, with orbital's in the same subshell in connected boxes; electrons are shown as arrows in the boxes, pointing up or down to indicate their spins. REMEMBER:Two electrons in the same orbital must have opposite spins.

More Related