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Understanding Electronic Configuration in Quantum Mechanics

Learn about how electrons are located within shells, subshells, and orbitals according to quantum mechanics. Discover the electronic configurations of hydrogen, helium, lithium, beryllium, boron, and carbon. Understand the relationship between atomic radii, first ionization energy, and electron affinity.

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Understanding Electronic Configuration in 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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