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Published byTheodora Blair Modified over 9 years ago
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Electron Configuration Shorthand way of writing electron configuration of atoms 10 Ne: 1s 2 2s 2 2p 6 Elemental Symbol and atomic number Principal energy level Energy sublevel Number of electrons
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zShorthand Configuration S 16e - Valence Electrons Core Electrons S16e - [Ne] 3s 2 3p 4 1s 2 2s 2 2p 6 3s 2 3p 4 Valence Electrons Longhand Configuration
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Valence Electrons Valence Electrons As (atomic number 33) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3 The electrons in the outermost energy level. s and p electrons in last shell 5 valence electrons
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[Ar] 4s 2 3d 10 4p 2 Noble Gas Configuration Example - Germanium X X X X X X X X X X X X X
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Electron Configuration Let’s Practice P (atomic number 15) 1s 2 2s 2 2p 6 3s 2 3p 3 Ca (atomic number 20) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 As (atomic number 33) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3 W (atomic number 74) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 4 Noble Gas Configuration [Ne] 3s 2 3p 3 [Ar] 4s 2 [Ar] 4s 2 3d 10 4p 3 [Xe] 6s 2 4f 14 5d 4
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Energy Sublevels Labeled s, p, d, or f –Based on shape of the atom’s orbitals
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Electron Configuration Your Turn N (atomic number 7) 1s 2 2s 2 2p 3 Na (atomic number 11) 1s 2 2s 2 2p 6 3s 1 Sb (atomic number 51) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 3 Cr (atomic number 24) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4 Noble Gas Configuration [He] 2s 2 2p 3 [Ne] 3s 1 [Kr]5s 2 4d 10 5p 3 [Ar] 4s 2 3d 4
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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!
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Full energy level Full sublevel Half full sublevel Stability
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Exceptions Copper Expect: [Ar] 4s 2 3d 9 Actual: [Ar] 4s 1 3d 10 Silver Expect: [Kr] 5s 2 4d 9 Actual: [Kr] 5s 1 4d 10 Chromium Expect: [Ar] 4s 2 3d 4 Actual: [Ar] 4s 1 3d 5 Molybdenum Expect: [Kr] 5s 2 4d 4 Actual: [Kr] 5s 1 4d 5 Exceptions are explained, but not predicted! Atoms are more stable with half full sublevel
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Stability Atoms create stability by losing, gaining or sharing electrons to obtain a full octet Isoelectronic with noble gases +1 +2 -3 -2 0 +3 +4 Atoms take electron configuration of the closest noble gas
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Stability Na (atomic number 11) 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 = [Ne] Na 1 Valence electron Metal = Loses Ne
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Try Some P -3 (atomic number 15) 1s 2 2s 2 2p 6 3s 2 3p 6 Ca +2 (atomic number 20) 1s 2 2s 2 2p 6 3s 2 3p 6 Zn +2 (atomic number 30) 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 Last valence electrons (s and p) Full Octet
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