Numford
Hybridisation

Hybridisation of ClF₃

Cl is sp³d hybridised (hybridization by the VSEPR count): 3 sigma bonds and 2 lone pairs give a T-shaped shape, bond angle about 87.5°.

FClFF
  • Cl
  • F
  • lone pair

ClF₃Chlorine trifluoride

T-shaped

AB₃E₂: 3 bond pairs, 2 lone pairs

  • Hybridisationsp³d
  • Bond angleabout 87.5°
  • Polaritypolar

Why this shape

  1. Cl has 7 valence electrons. It uses three in three single bonds to F, so four are left as two lone pairs.
  2. Steric number = three sigma bonds + two lone pairs = 5, so Cl is sp³d hybridised.
  3. Five electron pairs point to the corners of a trigonal bipyramid (trigonal bipyramidal electron geometry). With two lone pairs in place of atoms, the atoms make a T-shaped shape.
  4. Both lone pairs take equatorial positions, so they are 120 degrees apart and each is 90 degrees from only two bond pairs.
  5. Both lone pairs sit in the equatorial plane and push the two axial bonds toward the equatorial one, so the angle is about 87.5 degrees, a little less than 90.
  6. The bond dipoles do not cancel in the T-shaped shape, so ClF₃ is polar.

Lewis structure

28 valence electrons
ClFFF

Formal charges: none

Working

Why this hybridisation and shape

  1. Cl has 7 valence electrons. It uses three in three single bonds to F, so four are left as two lone pairs.
  2. Steric number = three sigma bonds + two lone pairs = 5, so Cl is sp³d hybridised.
  3. Five electron pairs point to the corners of a trigonal bipyramid (trigonal bipyramidal electron geometry). With two lone pairs in place of atoms, the atoms make a T-shaped shape.
  4. Both lone pairs take equatorial positions, so they are 120 degrees apart and each is 90 degrees from only two bond pairs.
  5. Both lone pairs sit in the equatorial plane and push the two axial bonds toward the equatorial one, so the angle is about 87.5 degrees, a little less than 90.
  6. The bond dipoles do not cancel in the T-shaped shape, so ClF₃ is polar.

Class 11, Chapter 4 Chemical Bonding and Molecular Structure.

Questions

Hybridisation of ClF3: quick answers

What is the hybridisation of ClF3?

Cl has 7 valence electrons. It uses three in three single bonds to F, so four are left as two lone pairs. Steric number = three sigma bonds + two lone pairs = 5, so Cl is sp³d hybridised.

What is the shape of ClF3 and its bond angle?

T-shaped, with a bond angle of about 87.5 degrees. Five electron pairs point to the corners of a trigonal bipyramid (trigonal bipyramidal electron geometry). With two lone pairs in place of atoms, the atoms make a T-shaped shape. Both lone pairs take equatorial positions, so they are 120 degrees apart and each is 90 degrees from only two bond pairs. Both lone pairs sit in the equatorial plane and push the two axial bonds toward the equatorial one, so the angle is about 87.5 degrees, a little less than 90.

Is ClF3 polar or non-polar?

Polar. The bond dipoles do not cancel in the T-shaped shape, so ClF₃ is polar.

Try any molecule