Problem: Consider the following molecular shapes:(a) Match each shape with one of the following species: XeF3+, SbBr3, GaCl3.

FREE Expert Solution

Analyzing the structures of each given molecules:

a. For XeF3+, Xe will appear as the central atom (less electronegative than F) where F atoms are single bonded to it

  • Valence electrons of Xe is 8 while F is 7. Total valence electron is 28. 8(1) + 7(3) - 1 (positive charge) = 28
  • Each F atoms will appear to have 3 lone pairs while Xe will appear to have 2 lone pairs (7 electrons around Xe) and 3 electrons used for bonding
  • Structure will appear as:

  • Geometry formula appears to be AX3E2 where A is central atom, X are surrounding atoms and E are # of lone pairs. 
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Problem Details

Consider the following molecular shapes:

(a) Match each shape with one of the following species: XeF3+, SbBr3, GaCl3.

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Our tutors have indicated that to solve this problem you will need to apply the Electron Geometry concept. You can view video lessons to learn Electron Geometry. Or if you need more Electron Geometry practice, you can also practice Electron Geometry practice problems.

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.