Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
ISBN: 9781305079373



Chemistry: Principles and Reactions

8th Edition
William L. Masterton + 1 other
ISBN: 9781305079373
Textbook Problem

Two different molecules have the formula C2H6O. One of the molecules has the oxygen atom bonded to both carbon atoms. The other molecule has the oxygen atom bonded to only one carbon atom while both carbon atoms are bonded to each other. Write Lewis structures for both of these compounds.

Interpretation Introduction


Lewis structure for two different molecule having formula C2H6O should be drawn.

Concept introduction:

  • Lewis structures are the diagrams that show the bonding between the atoms of the molecules and existing lone pairs of electrons.
  • Bonding electrons are those electrons which are shared between the atoms resulting in the formation of bond.
  • Non-bonding electrons are the valence electrons of the atom which are not shared with another atom.
  1. Calculate the total number of valence electrons in molecule C2H6O :
  2. Total number of valence electrons = 2(valence electrons of C) + 6(valence electrons of H) + valence electron of O

       =2(4)+6(1)+6= 20e

  3. Arrange the atoms in such a way that the least electronegative atom is at the center. Then put the valence electrons around them such that each atom contributes at least 1 electron to single bond and the octet rule for each atom is followed.
  4. To complete the octet each oxygen, O atoms and hydrogen, H atoms forms single bond with carbon, C atom. The rest number of electrons are present as lone pair on oxygen atom, the number of lone pair of electrons = Total number of valence electrons − Total number of electrons involved in bond formation

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