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Applying the VSEPR model plan, which geometric shape best describes each of the following? You may use the option more than once, once, or not at all. (6 points). methane, CH4 carbon tetrachloride, CCl4 ammonia, NH3 sulfur tetrafluoride, SF4 chlorine pentafluoride, ClF5 xenon tetrafluoride, XeF4

options
seesaw
trional bipramidal
trigonal pyramidal
trigonal planar
octahedral
square planar
tetrahedron
square pyramidal

1 answer

To determine the geometric shape for each compound using the VSEPR (Valence Shell Electron Pair Repulsion) model, we look at the number of bonding and lone pairs around the central atom. Below are the geometric shapes for the compounds you listed:

  1. Methane, CH4: Tetrahedron (4 bonding pairs, 0 lone pairs)
  2. Carbon tetrachloride, CCl4: Tetrahedron (4 bonding pairs, 0 lone pairs)
  3. Ammonia, NH3: Trigonal pyramidal (3 bonding pairs, 1 lone pair)
  4. Sulfur tetrafluoride, SF4: Seesaw (4 bonding pairs, 1 lone pair)
  5. Chlorine pentafluoride, ClF5: Square pyramidal (5 bonding pairs, 1 lone pair)
  6. Xenon tetrafluoride, XeF4: Square planar (4 bonding pairs, 2 lone pairs)

Summary of shapes:

  • Methane, CH4: Tetrahedron
  • Carbon tetrachloride, CCl4: Tetrahedron
  • Ammonia, NH3: Trigonal pyramidal
  • Sulfur tetrafluoride, SF4: Seesaw
  • Chlorine pentafluoride, ClF5: Square pyramidal
  • Xenon tetrafluoride, XeF4: Square planar