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Electronconfig
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3. Electronic Configuration according to Quantum Mechanics The location of an electron is described by 3 terms. 1 st Term: Shell ( n ) n = 1 n = 2 n = 3 lone electron of Hydrogen
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5. 2 nd Term: subshell - designated by s, p,d,f 1 s n = 2 n = 3 The first shell ( 1 ) has one subshell ( s ).
6. 2 nd 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. 1 s n = 2 n = 3 The first shell ( 1 ) has one subshell ( s ). The s subshell is s pherical in shape and has 1 orbital 3rd Term: orbital
7. 2 nd 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. 1 s n = 2 n = 3 The first shell ( 1 ) has one subshell ( s ). The s subshell is s pherical in shape and has 1 orbital 3rd Term: orbital Each orbital can accommodate 2 electrons
8. The Electronic Configuration of Hydrogen 1 s The first shell ( 1 ) has one subshell ( s ). The s subshell is s pherical in shape and has 1 orbital H 1 s 1 shell subshell # of electrons present energy H 1 s Electronic configuration Orbital Energy Level Diagram
10. The Electronic Configuration of Helium He: Atomic # of 2, 2 electrons in a neutral He atom H 1 s 1 He 1 s 2 He 1 s 1 s **if there are 2 electrons in the same orbital they must have the opposite spin. (Pauli’s Exclusion Principle)
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12. 1 s The Electronic Configuration of Lithium (Li) Li: Z =3 Li has 3 electrons. 2 nd shell (2)
13. 1 s The Electronic Configuration of Lithium (Li) Li: Z =3 Li has 3 electrons. 2 nd shell - The 2nd shell ( n = 2 ) has 2 subshells which are s and p . 2 s 2 p
14. 1 s The Electronic Configuration of Lithium (Li) Li: Z =3 Li has 3 electrons. 2 nd shell 2 s 2 p Li 1 s 2 2 s 1 2 s Li 1 s Electronic configuration Orbital Energy Level Diagram
15. 1 s The Electronic Configuration of Berylium (Be) Be: Z =4 Be has 4 electrons. 2 nd shell 2 s 2 p Be 1 s 2 2 s 2 2 s Be 1 s Electronic configuration Orbital Energy Level Diagram
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17. 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: s pherical 1 orbital p subshell: p air of lobes x y z x y z
18. Our Orbital Picture of Be The first shell ( 1 s ) is filled. The 2 s orbital has 2 e - present. The 2 p orbitals are empty. The 2 p orbitals have room for 6 e -
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20. 1 s The Electronic Configuration of Boron (B) B: Z =5 B has 5 electrons. 2 nd shell 2 s 2 p 1 s 2 nd shell 2 s 2 p Be 1 s 2 2 s 2 2 s Be 1 s B 1 s 2 2 s 2 2 p 1 2 p 2 s B 1 s
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22. 1 s The Electronic Configuration of Carbon (C) C: Z =6 C has 6 electrons. 2 nd shell 2 s 2 p 1 s 2 nd shell 2 s 2 p B 1 s 2 2 s 2 2 p 1 2 p 2 s B 1 s C 1 s 2 2 s 2 2 p x 1 p y 1 2 p 2 s C 1 s
23. Our Orbital Picture of C The first shell ( 1 s ) is filled. The 2 s orbital has 2 e - present. 2 2 p orbitals have 1 e - each.
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25. d subshell: double dumbells xy z 2 xz x y yz x 2- y 2
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28. Atomic Radii within a Group Lithium (Z=3); n = 2 Sodium (Z=11); n = 3 Hydrogen (Z=1); Shell (n)=1 + + + e - 2e - 8e - 2e - + + + + e - + e -
29. Lithium (Z=3) n = 2 Beryllium (Z=4) n = 2 Boron (Z=5) n = 2 If protons were light bulbs….and electrons were moths…... + + + e - 2e - + + + e - 2e - e - + + + + e - 2e - e - e - + + B e - e - e - Be e - e - Li e - + + + e - 2e - + + + e - 2e - e - +
30. Lithium (Z=3) Beryllium (Z=4) Boron (Z=5) Increasing Increasing + + + e - 2e - + + + e - 2e - e - + + + + e - 2e - e - e - + +
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32. H. Chemistry OBE 2/16/11 Of the elements Mg, Cl, Na, and P which would have the largest atomic radius? Explain this in terms of trends in the periodic table (periodicity). + + + e - 2e - + + + e - 2e - e - + + + + e - 2e - e - e - + +
33. First Ionization Energy Lithium (Z=3) Sodium (Z=11) Hydrogen (Z=1) + e - + + + e - 8e - 2e - + + + + e - + e - H + + + + e - 2e - Li + e - 8e - 2e - + + + + Na +
34. First Ionization Energy e - Lithium (Z=3) 8e - Sodium (Z=11) 2e - 2e - e - Hydrogen (Z=1) e - Decreasing + + + + + + + +
35. Lithium (Z=3) 3 protons screened by 2 e - e - 2e - Beryllium (Z=4) 4 protons screened by 2 e - Boron (Z=5) 5 protons screened by 2 e - e - 2e - e - e - 2e - e - e - 1 e - removed = 2s 0 1 e - removed = 2s 1 1 e - removed = 2s 2 2p 0 + + + + + + + + + + + + Decreasing Decreasing
36. Lithium (Z=3) 3 protons screened by 2 e - e - 2e - Beryllium (Z=4) 4 protons screened by 2 e - Boron (Z=5) 5 protons screened by 2 e - e - 2e - e - Decreasing Decreasing + + + + + + + + + + e - 2e - e - e - + +
37. Increasing Increasing Trends in the Periodic Table Atomic Radii (Size) First Ionization Energy Decreasing Decreasing
38. Electron Affinity e - Fluorine (Z=9) 8e - Chlorine (Z=17) 2e - 2e - 7e - 7e - 2e - 8e - F - e - 8e - 2e - 8e - Cl - + + + + + + + + + + + + + +
39. Trends in the Periodic Table First Ionization Energy Decreasing Decreasing Decreasing Decreasing Electron Affinity
40. Predicting Stable Ions 8e - Sodium (Z=11) 2e - e - e - 8e - 2e - Na + 8e - Chlorine (Z=17) 2e - 7e - e - 8e - 2e - 8e - Cl - + + + + + + + + + + + + + + + +