Periodic Table And Electron Configuration — Flashcards

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Orbitals are regions around the nucleus where there is maximum probability of finding electrons, based on quantum mechanical model. Unlike Bohr's definite circular paths (orbits), orbitals represent p…

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Principal quantum number (n) represents the shells or principal energy levels of electrons. Possible values: n = 1, 2, 3, 4... where n = 1 is K shell, n = 2 is L shell, n = 3 is M shell, and n = 4 is …

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Azimuthal quantum number (l) defines the three-dimensional shape of orbitals and represents subshells. Values range from 0 to (n-1). l = 0 (s subshell), l = 1 (p subshell), l = 2 (d subshell), l = 3 (…

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s subshell: 1 orbital (spherical shape) p subshell: 3 orbitals (dumbbell shape) d subshell: 5 orbitals (complex shapes) f subshell: 7 orbitals (more complex shapes) General formula: For l value, numbe…

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Formula: Maximum electrons in shell = 2n² K shell (n=1): 2 electrons L shell (n=2): 8 electrons M shell (n=3): 18 electrons N shell (n=4): 32 electrons Each orbital can hold maximum 2 electrons.

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s subshell: 2 electrons (1 orbital × 2) p subshell: 6 electrons (3 orbitals × 2) d subshell: 10 electrons (5 orbitals × 2) f subshell: 14 electrons (7 orbitals × 2) General formula: 2(2l + 1) electron…

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Energy of subshells increases with increasing (n+l) values. If (n+l) values are equal, subshell with higher n value has more energy. Example: 2p (n+l = 3) < 3s (n+l = 3, but higher n) < 3p (n+l = 4) O…

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Carbon (₆C): 1s² 2s² 2p² Neon (₁₀Ne): 1s² 2s² 2p⁶ Electrons fill in order of increasing energy: 1s fills first (2 electrons), then 2s (2 electrons), then 2p starts filling.