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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
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Electronic Configuration according to Quantum Mechanics

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  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-

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