Enlace triplo

Estrutura e imaxe de microscopio de forza atómica do deshidrobenzo[12]annuleno, onde os aneis de benceno están unidos por enlaces triplos.

Un enlace triplo en química é un enlace químico entre dous átomos no que están implicados seis electróns de enlace en lugar dos máis usiais dous dun enlace covalente simple. Os enlaces triplos máis comúns entre dous átomos de carbono poden encontrarse nos alquinos. Outros grupos funcionais que conteñen un enlace triplo son os cianuros e os isocianuros e os nitrilos. Algunhas moléculas diatomicas, como o dinitróxeno e o monóxido de carbono, teñen tamén enlace triplo. Na fórmula esquelética o triplo enlace debúxase como tres liñas paralelas (≡) entre dous átomos conectados.[1][2][3]

Os enlaces triplos son máis fortes que os seus equivalentes enlaces simples ou dobres, cunha orde de enlace de tres. Isto dálle grande estabilidade a compostos que os levan; por exemplo o N2 (N≡N) do aire é moi difícil de separar nos seus átomos, o cal é importante no ciclo do nitróxeno na natureza, e que só unhas poucas bacterias teñen encimas con capacidade de romper este enlace e realizar unha significativa fixación do nitróxeno.

acetileno, H−C≡C−H cianóxeno, N≡C−C≡N monóxido de carbono, C≡O
Exemplos de compostos químicos con enlace triplo

Enlaces

Os tipos de enlace poden explicarse pola hibridación de orbitais. No caso do acetileno cada átomo de cabono ten dous orbitais sp e dous orbitais p. Os dous orbitais sp son lineares con ángulos de 180° e ocupan o eixe X (do sistema de coordenadas cartesianas). Os orbitais p son perpendiculares aos eixes Y e Z. Cando dous átomos de carbono se aproximan, os orbitais sp solápanse e forman un enlace sigma sp-sp. Ao mesmo tempo os orbitais pz achéganse e xúntanse formando un enlace pi pz-pz. Igualmente, o outro par de orbitais py forma un enlace pi py-py. O resultado é a formación dun enlace sigma e dous enlaces pi, que conforman o triplo enlace.

No modelo de enlace flexionado o triplo enlace pode formarse tamén polo solapamento de tres lobos sp3 sen necesidade de que haxa un enlace pi.[4]

Notas

  1. ↑ March, Jerry (1985), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (3rd ed.), New York: Wiley, ISBN 0-471-85472-7
  2. ↑ Organic Chemistry 2nd Ed. John McMurry
  3. ↑ Pyykkö, Pekka; Riedel, Sebastian; Patzschke, Michael (2005). "Triple-Bond Covalent Radii". Chemistry: A European Journal 11 (12): 3511–20. PMID 15832398. doi:10.1002/chem.200401299. 
  4. ↑ Advanced Organic Chemistry Carey, Francis A., Sundberg, Richard J. 5th ed. 2007

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