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Question

The number of species below that has two lone pairs of electrons in their central atom is ______. (Round off to the Nearest Integer.)

SF4,BF4-,CIF3,AsF3,PCl5,BrF5,XeF4,SF6


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Solution

Structure of SF4:-

  • In SF4, there are 4 Fluorine atoms that are attached to Sulphur.
  • Electronic configuration of Sulphur with atomic number 16 is:1s22s22p63s23p4.
  • It shares its 4 electrons with Fluorine and thus form SF4that has a shape of Trigonal bipyramidal.

  • From the structure we can see that it has 4 bond pairs(S-F)and 1 lone pair.

Structure of BF4-:-

  • In BF4-, there are 4 Fluorine atoms that are attached to Boron.
  • Electronic configuration of Boron with atomic number 4 is:1s22s22p1.
  • It shares its 4 electrons with Fluorine and thus form SF4that has a shape of Tetrahedral.

  • From the structure we can see that it has 4 bond pairs(B-F).
  • The one extra electron that is left in Boron results in the negative charge of the compound.
  • Thus we can also see that it has no lone pairs present in it.

Structure of ClF3:-

  • In ClF3, there are 4 Fluorine atoms that are attached to Chlorine.
  • Electronic configuration of Chlorine with atomic number 17 is:1s22s22p63s23p5
  • As we know, due to the presence of vacant d-orbital, Chlorine shows variable valency of 3,5,7.
  • It shares its 3 electrons with Fluorine and thus form ClF3that has a T-shape.

  • From the structure we can see that it has 3 bond pairs(Cl-F)and 2 lone pair.

Structure of AsF3:-

  • In AsF3, there are 3 Fluorine atoms that are attached to Arsenic.
  • Electronic configuration of Arsenic with atomic number 33 is:[Ar]3d104s24p3.
  • It shares its 3 electrons with Fluorine and thus form AsF3that has a shape of Trigonal pyramidal.

  • From the structure we can see that it has 3 bond pairs(As-F)and 1 lone pair.

Structure of BrF5:-

  • In BrF5, there are 4 Fluorine atoms that are attached to Bromine.
  • Electronic configuration of Bromine with atomic number 35 is:[Ar]4s23d104p5
  • It shares its 5 electrons with Fluorine and thus form BrF5that has a square pyramidal shape.

  • From the structure we can see that it has 5 bond pairs(Br-F)and 1 lone pair.

Structure of PCl5:-

  • In PCl5, there are 5 Chlorine atoms that are attached to Phosphorous.
  • Electronic configuration of Phosphorous with atomic number 15 is:1s22s22p63s23p3
  • It shares its 5 electrons with Chorine and thus form PCl5that has a trigonal bipyramidal shape.

  • From the structure we can see that it has 5 bond pairs(P-Cl)and no lone pair.

Structure of XeF4:-

  • In XeF4, there are 5 Fluorine atoms that are attached to Xenon.
  • Electronic configuration of Xenon with atomic number 54 is:[Kr]4d105s25p6
  • It shares its 4 electrons with Fluorine and thus form XeF4that has a square planar shape.

  • From the structure we can see that it has 5 bond pairs(Xe-F)and has 2 lone pairs.

Structure of SF6:-

  • In SF6, there are 6 Fluorine atoms that are attached to Sulphur.
  • Electronic configuration of Sulphur with atomic number 16 is:1s22s22p63s23p4
  • It shares its 6 electrons with Fluorine and thus form SF6that has an Octahedral shape.

  • From the structure we can see that it has 6 bond pairs(S-F)and no lone pair.

Therefore, The number of species below that have two lone pairs of electrons in their central atom is 2 (ClF3,XeF4).


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