He B.

asked • 11/21/19

Shapes of Molecules?

This an online assignment I have gotten wrong twice. Help is appreciated, thanks!

What is the shape of each molecule below? Select the correct answer. Answers can be used more than once.


 linear bent/v-shape trigonal planar trigonal pyramidal tetrahedral trigonal bipyramidal see-saw T-shape octahedral square pyramidal square planar  KrF2


 linear bent/v-shape trigonal planar trigonal pyramidal tetrahedral trigonal bipyramidal see-saw T-shape octahedral square pyramidal square planar  ClF3


 linear bent/v-shape trigonal planar trigonal pyramidal tetrahedral trigonal bipyramidal see-saw T-shape octahedral square pyramidal square planar  SF4


 linear bent/v-shape trigonal planar trigonal pyramidal tetrahedral trigonal bipyramidal see-saw T-shape octahedral square pyramidal square planar  XeF4


 linear bent/v-shape trigonal planar trigonal pyramidal tetrahedral trigonal bipyramidal see-saw T-shape octahedral square pyramidal square planar  SF6


 linear bent/v-shape trigonal planar trigonal pyramidal tetrahedral trigonal bipyramidal see-saw T-shape octahedral square pyramidal square planar  AsF5


 linear bent/v-shape trigonal planar trigonal pyramidal tetrahedral trigonal bipyramidal see-saw T-shape octahedral square pyramidal square planar  IF5

Tonya G.

tutor
Learning molecular and electron geometry really just requires memorization. If you look at the first one for example, KrF2. Krypton has 8 valence electrons and Fluorine has 14 (2x7). This will give you a total of 22 electrons. This means that there will be 3 lone pairs around the central atom of Krypton. If you follow the rules this would mean that there would be 2 bonded with 3 lone pairs. This would lead you to believe that the molecule is trigonal bipyramidal. In most cases, you would be correct, but in the case of this molecule the lone pairs arrange themselves in equatorial positions so the molecule essentially ignores the lone pairs so this shape would be linear. 2. The molecular geometry is trigonal bipyramidal because there are 5 bonding areas around the central atom. However, due to the 3 bonded and 2 lone pairs the electron geometry is T-shaped. 3. SF4 will be trigonal bipyramidal because again there are 5 bonded areas around the central atom of S. Again, because there are 4 bonded and 1 lone pair, the shape will become see-saw. 4. XeF4 is simply square planar. It has 4 bonded areas around the central atom and no lone pairs. Its geometry will not change. 5.SF6 has 6 bonding areas around the central S atom with no lone pairs. This will be octahedral. 6. AsF5 has 5 bonding areas around the central As atom with no lone pairs so it will be trigonal bipyramidal. 7. IF5 has 6 bonding areas including one lone pair around the central I atom making it octahedral. However, taking VSEPR into account, the one lone pair will change the structure to square pyramidal.
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11/21/19

1 Expert Answer

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Montana M. answered • 11/22/19

Experienced Science Tutor for Leading Test Prep Company

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