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Understanding Valence Electrons and Ionic Charges in Sodium and Chlorine

This overview discusses the concepts of valence electrons, Lewis dot structures, and ionic charges using the examples of sodium (Na) and chlorine (Cl). Sodium, a metal with an electron configuration of 1s² 2s² 2p⁶ 3s¹, forms a cation (Na⁺) by losing one electron. Chlorine, a nonmetal with an electron configuration of 1s² 2s² 2p⁶ 3s² 3p⁵, forms an anion (Cl⁻) by gaining one electron. Both elements strive for stability, with stable atoms having a complete outer shell of electrons, typically 8.

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Understanding Valence Electrons and Ionic Charges in Sodium and Chlorine

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Presentation Transcript

  1. Valence electrons, Lewis dot structures, and ionic charge

  2. Stable atoms have 8 electrons (or 2 or 0 if they are small)

  3. Metal: sodium • Electron configuration: 1s22s22p63s1 • Sketch of principal energy levels: (Na)2)8)1) • Lewis dot structure: (see the board) • Formation of ion: electron removed: Na1+ • Cation = positively charged ion (pronounced “cat ion” not “kay-shun”)

  4. Nonmetal: chlorine • Electron configuration: 1s22s22p63s23p5 • Sketch of principal energy levels: (Cl)2)8)7) • Lewis dot structure: (see the board) • Formation of ion: electron added: Cl1- • Anion = negatively charged ion

  5. Stable atoms have 8 electrons (or 2 or 0 if they are small)

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