Which of the following molecules have zero dipole moment and tetrahedral structure? (A) CCl4 (B) SnCl2 (C) SnCl4 (D) CO2

Answer: (a) and (c)

Explanation

Tetrahedral symmetry exists in the CCl4 molecule. As a consequence, the dipole moment of the three CCl bonds on one side will produce a resultant moment that is equal to and opposite to the dipole moment of the single CCl bond on the other side. As a result, the final dipole moment will be zero. Sn has the electrical configuration [kr]4d105s25p2. On Sn, there will be a lone pair of electrons, and the two electrons in 5p will be utilised in bonding by the two chlorine atoms. The dipole moment will not be zero, and the resultant geometry will be trigonal pyramidal. The symmetric compound SnCl4 is made up of two atoms. Because dipole moments in opposing directions cancel one other, the dipole moment will be zero.

  • SnCl4 has a tetrahedral shape, with tin in the centre, one chlorine atom projecting straight up above tin, and three more chlorine atoms extending outside and down from the tin. CO2 has a symmetric electron distribution and a linear molecule geometry.
  • Each CO bond in CO2 is polar, and the two CO bond dipoles are of identical amplitude and cancel each other since they are orientated at 180 degrees.
  • As a result, carbon dioxide molecules will have no net dipole moment.

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