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Electron Configuration

Electron Configuration. Shorthand way of writing electron configuration of atoms 10 Ne: 1s 2 2s 2 2p 6. Number of electrons. Energy sublevel. Elemental Symbol and atomic number. Principal energy level. Valence Electrons. Longhand Configuration. Core Electrons. Valence Electrons. 2p 6.

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Electron Configuration

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  1. Electron Configuration Shorthand way of writing electron configuration of atoms 10Ne: 1s2 2s2 2p6 Number of electrons Energy sublevel Elemental Symbol and atomic number Principal energy level

  2. Valence Electrons Longhand Configuration Core Electrons Valence Electrons 2p6 S 16e- 2s2 1s2 3s2 3p4 • Shorthand Configuration S 16e- [Ne]3s2 3p4

  3. Valence Electrons • Valence Electrons • As (atomic number 33) • 1s22s22p63s23p64s23d104p3 • The electrons in the outermost energy level. • s and p electrons in last shell • 5 valence electrons

  4. Noble Gas Configuration Example - Germanium X X X X X X X X X X X X X [Ar] 4s2 3d10 4p2

  5. Electron Configuration Let’s Practice • P (atomic number 15) • 1s22s22p63s23p3 • Ca (atomic number 20) • 1s22s22p63s23p64s2 • As (atomic number 33) • 1s22s22p63s23p64s23d104p3 • W (atomic number 74) • 1s22s22p63s23p64s23d104p65s24d105p66s24f145d4 Noble Gas Configuration [Ne]3s23p3 [Ar]4s2 [Ar]4s23d104p3 [Xe]6s24f145d4

  6. Energy Sublevels Labeled s, p, d, or f Based on shape of the atom’s orbitals

  7. Electron Configuration Your Turn • N (atomic number 7) • 1s22s22p3 • Na (atomic number 11) • 1s22s22p63s1 • Sb(atomic number 51) • 1s22s22p63s23p64s23d104p65s24d105p3 • Cr (atomic number 24) • 1s22s22p63s23p64s23d4 Noble Gas Configuration [He]2s22p3 [Ne]3s1 [Kr]5s24d105p3 [Ar]4s23d4

  8. Why are d and f orbitals always in lower energy levels? d and f orbitals require amounts of energy It’s better (lower in energy) to that requires a large amount of energy (d and f orbtials) for one in a higher level but lower energy This is the reason for the diagonal rule! LARGE skip a sublevel BE SURE TO FOLLOW THE ARROWS IN ORDER!

  9. Full energy level Full sublevel Half full sublevel Stability

  10. Exceptions Exceptions are explained, but not predicted! Atoms are more stable with half full sublevel • Copper • Expect: [Ar] 4s2 3d9 • Actual: [Ar] 4s1 3d10 • Silver • Expect: [Kr] 5s2 4d9 • Actual: [Kr] 5s1 4d10 • Chromium • Expect:[Ar] 4s2 3d4 • Actual: [Ar] 4s1 3d5 • Molybdenum • Expect: [Kr] 5s2 4d4 • Actual: [Kr] 5s1 4d5

  11. Stability 0 +1 +2 +4 -2 +3 -3 -1 Atoms take electron configuration of the closest noble gas Atoms create stability by losing, gaining or sharing electrons to obtain a full octet Isoelectronic with noble gases

  12. Stability 1 Valence electron Metal = Loses Ne Na • Na (atomic number 11) • 1s22s22p63s1 • 1s22s22p6 = [Ne]

  13. Try Some Full Octet • P-3(atomic number 15) • 1s22s22p63s23p6 • Ca+2(atomic number 20) • 1s22s22p63s23p6 • Zn+2(atomic number 30) • 1s22s22p63s23p63d10 • Last valence electrons (s and p)

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