Elements Forming Ionic Compounds Attain Noble Gas Configuration by Either Gaining Or Losing Electrons from Their Outermost Shells. Give Reason to Explain Why Carbon Cannot Attain Noble Gas Configuration in this Manner to Form Its Compounds. - Science

Advertisement Remove all ads
Advertisement Remove all ads
Advertisement Remove all ads

Elements forming ionic compounds attain noble gas configuration by either gaining or losing electrons from their outermost shells. Give reason to explain why carbon cannot attain noble gas configuration in this manner to form its compounds.

Advertisement Remove all ads


The atomic number of carbon is 6. This means that it has 4 electrons in its outermost shell and it needs 4 more electrons to attain noble gas electronic configuration. It cannot form C4+ cation, as the removal of 4 valence electrons requires a huge amount of energy. The cation formed has 6 protons and 2 electrons. This makes it highly unstable. Carbon cannot form C4− anion, as its nucleus with 6 protons cannot hold 10 electrons. Thus, carbon achieves noble gas electronic configuration by sharing its 4 electrons with other elements—that is, it forms covalent compounds.

Concept: The Covalent Bond
  Is there an error in this question or solution?
2013-2014 (March) All India Set 1

Video TutorialsVIEW ALL [2]


View all notifications

      Forgot password?
View in app×