1 / 37

Electronic Configuration according to Quantum Mechanics

Electronic Configuration according to Quantum Mechanics. The location of an electron is described by 3 terms. 1 st Term: Shell ( n ). n = 3. n = 2. lone electron of Hydrogen. n = 1. n = 3. 2 nd Term: subshell - designated by s, p,d,f. n = 2. 1 s.

nigel-davis
Télécharger la présentation

Electronic Configuration according to Quantum Mechanics

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. Electronic Configuration according to Quantum Mechanics The location of an electron is described by 3 terms. 1st Term: Shell (n) n = 3 n = 2 lone electron of Hydrogen n = 1

  2. n = 3 2nd Term: subshell - designated by s, p,d,f n = 2 1s The first shell (1) has one subshell (s).

  3. 2nd Term: subshell - designated by s, p,d,f - refers to the shape(s) of the area in which the electron can be located. - also designates an energy level within the shell. n = 3 n = 2 1s The first shell (1) has one subshell (s). The s subshell is spherical in shape and has 1 orbital 3rd Term: orbital

  4. 2nd Term: subshell - designated by s, p,d,f - refers to the shape(s) of the area in which the electron can be located. - also designates an energy level within the shell. n = 3 n = 2 1s The first shell (1) has one subshell (s). The s subshell is spherical in shape and has 1 orbital 3rd Term: orbital Each orbital can accommodate 2 electrons

  5. The Electronic Configuration of Hydrogen energy The first shell (1) has one subshell (s). The s subshell is spherical in shape and has 1 orbital Electronic configuration H 1s1 1s shell # of electrons present subshell H 1s Orbital Energy Level Diagram

  6. The Electronic Configuration of Helium He: Atomic # of 2, 2 electrons in a neutral He atom 1s

  7. The Electronic Configuration of Helium He: Atomic # of 2, 2 electrons in a neutral He atom H 1s1 He 1s2 He 1s  1s **if there are 2 electrons in the same orbital they must have the opposite spin. (Pauli’s Exclusion Principle)

  8. The Electronic Configuration of Lithium (Li) Li: Z=3 Li has 3 electrons. 2ndshell (2) 1s

  9. The Electronic Configuration of Lithium (Li) Li: Z=3 Li has 3 electrons. - The 2nd shell (n= 2) has 2 subshells which are s and p. 2p 2s 2ndshell 1s

  10. The Electronic Configuration of Lithium (Li) Li: Z=3 Li has 3 electrons. 2p 2s 2ndshell 1s 2s Li 1s Li 1s22s1 Electronic configuration Orbital Energy Level Diagram

  11. The Electronic Configuration of Berylium (Be) Be: Z=4 Be has 4 electrons. 2p 2s 2ndshell 1s 2s Be 1s  Be 1s22s2 Electronic configuration Orbital Energy Level Diagram

  12. subshell - designated by s, p,d,f - refers to the shape(s) of the area in which the electron can be located. - also designates an energy level within the shell. - relative energy: s < p < d < f s subshell: spherical 1 orbital p subshell: pair of lobes z x y x z y

  13. Our Orbital Picture of Be The first shell (1s) is filled. The 2s orbital has 2 e- present. The 2p orbitals are empty. The 2p orbitals have room for 6 e-

  14. The Electronic Configuration of Boron (B) B: Z=5 B has 5 electrons. 2p 2p 2s 2s 2ndshell 2ndshell 1s 1s B 1s22s22p1 Be 1s22s2 2p 2s B 1s 2s Be 1s

  15. The Electronic Configuration of Carbon (C) C: Z=6 C has 6 electrons. 2p 2p 2s 2s 2ndshell 2ndshell 1s 1s B 1s22s22p1 C 1s22s22px1py1 2p 2s B 1s 2p  2s C 1s

  16. Our Orbital Picture of C The first shell (1s) is filled. The 2s orbital has 2 e- present. 2 2p orbitals have 1 e- each.

  17. d subshell: double dumbells x y xy xz yz z2 x2-y2

  18. Atomic Radii within a Group e- e- 2e- + + + + + + + + e- 2e- 8e- Hydrogen (Z=1); Shell (n)=1 Lithium (Z=3); n = 2 Sodium (Z=11); n = 3

  19. e- e- 2e- e- 2e- 2e- e- 2e- 2e- e- e- e- e- e- + + + + + + + + + + + + + + e- + + + + + e- e- e- e- e- B Be Li Boron (Z=5) n = 2 Beryllium (Z=4) n = 2 Lithium (Z=3) n = 2 If protons were light bulbs….and electrons were moths…...

  20. e- e- 2e- 2e- e- 2e- e- e- e- + + + + + + + + + + + + Boron (Z=5) Beryllium (Z=4) Lithium (Z=3) Increasing Increasing

  21. First Ionization Energy H+ e- e- Li+ e- 2e- e- + + + + + + + + e- Na+ + + + + + + + + 2e- 2e- 8e- 8e- e- Hydrogen (Z=1) Lithium (Z=3) Sodium (Z=11)

  22. First Ionization Energy + + + + + + + + Hydrogen (Z=1) e- Decreasing Lithium (Z=3) 2e- e- Sodium (Z=11) 2e- 8e- e-

  23. + + + + + + + + + + + + Decreasing Decreasing e- e- 2e- 2e- e- 2e- e- e- e- Boron (Z=5) 5 protons screened by 2 e- Beryllium (Z=4) 4 protons screened by 2 e- Lithium (Z=3) 3 protons screened by 2 e- 1 e- removed = 2s0 1 e- removed = 2s22p0 1 e- removed = 2s1

  24. e- 2e- e- e- + + + + + + + + + + + + 2e- e- 2e- e- e- Boron (Z=5) 5 protons screened by 2 e- Beryllium (Z=4) 4 protons screened by 2 e- Lithium (Z=3) 3 protons screened by 2 e- Decreasing Decreasing

  25. Trends in the Periodic Table Atomic Radii (Size) Increasing Increasing First Ionization Energy Decreasing Decreasing

  26. Electron Affinity + + + + + + + + + + + + + + F- Fluorine (Z=9) 2e- 2e- 8e- e- 7e- Cl- Chlorine (Z=17) e- 2e- 2e- 8e- 8e- 7e- 8e-

  27. Electron Affinity Decreasing Decreasing Trends in the Periodic Table First Ionization Energy Decreasing Decreasing

  28. + + + + + + + + + + + + + + + + Predicting Stable Ions e- Sodium (Z=11) 2e- 2e- 8e- 8e- e- Na+ Cl- Chlorine (Z=17) e- 2e- 2e- 8e- 8e- 7e- 8e-

More Related