1 / 30

Bell Work

Bell Work. What is the name of the group that the following elements belong to? (Look at your labeled periodic table to determine the names of the groups that they belong to). He Li Mg O N Cl Be B P. Physical Science - Lecture 35. Block Elements – Electron Configurations.

jared
Download Presentation

Bell Work

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. Bell Work • What is the name of the group that the following elements belong to? (Look at your labeled periodic table to determine the names of the groups that they belong to). • He • Li • Mg • O • N • Cl • Be • B • P

  2. Physical Science - Lecture 35 Block Elements – Electron Configurations

  3. Review of Electrons • The number of total electrons is equal to the atomic number. • The number of valence electrons is equal to the group number when the element is found (1A=1, 2A=2, 3A=3, 4A=4, 5A=5, 6A=6, 7A=7, 8A=8).

  4. Electron Configuration • Designates placement of electrons • Specific to each element • Corresponds to highest occupied level of electrons • Uses letters s, p, d, f (each with individual shapes and specific numbers of electrons)

  5. Electron Configurations

  6. How many electrons will each hold? • s = 2 • p = 6 • d = 10 • f = 14

  7. Counting Electrons

  8. Is there a pattern?

  9. Pattern • Start with the lowest energy level (s) and build up to the higher energy level (p) • Total number of superscripts = number of electrons in each element

  10. Practice

  11. The Large Number • The Large number stands for the shell that an electron is in. Ex) 1s22s22p63s23p64s2

  12. The Superscript • The superscript stands for the number of electrons in that shell. Ex) 1s22s22p63s23p64s2

  13. Example: 1s22s22p63s23p64s2 • Therefore, there will be ____ electrons in the 1st shell, ____ electrons in the 2nd shell, ____ electrons in the 3rd shell, and _____ electrons in the 4th shell.

  14. Practice: Atomic Number 12 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  15. Practice: Atomic Number 21 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  16. Practice: Atomic Number 24 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  17. Practice: Atomic Number 17 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  18. Practice: Atomic Number 30 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  19. Practice: Atomic Number 41 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  20. Practice: Atomic Number 18 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  21. Practice: Atomic Number 14 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  22. Practice: Atomic Number 55 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  23. Practice: Atomic Number 16 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  24. Practice: Atomic Number 23 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  25. Practice: Atomic Number 37 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  26. Practice: Atomic Number 22 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  27. Practice: Atomic Number 43 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

  28. Practice: Atomic Number 29 • Each s gets 2 electrons. • Each p gets 6 electrons. • Each d gets 10 electrons. • Each f gets 14 electrons. • Add up the total number of subscripts to determine how many electrons you have.

More Related