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1.how to predict the shape of the molecules in chemical bonding chapter?
7 months ago

Answers : (2)

Arun
22027 Points
							
The VSEPR predicted shapes of molecules can be found in a systematic way by using the number of electron pairs to determine the shape of the molecules. To predict the shape of the molecules, first draw out the Lewis structure of the molecule. On the Lewis diagram, identify the central atom.
7 months ago
Rajdeep
230 Points
							
HELLO THERE!
 
Very difficult question for those who are just going superficially through the chapter of CHEMICAL BONDING. Well, if you understand the full concept behind understanding the geometry/shape of a molecule, you can just rock!
 
Let’s now get down to the point:
I’m telling you systematically:
 
For sp2 Hybridization:
 
  1. AB3 Type, where there are three bond pairs and zero lone pairs. Such type of molecule has Trigonal Planar Shape (Bond angle= 120o). Example: BH3.
  2. AB2L Type, where there are two bond pairs and one lone pair. Such type of molecule has V-shape/Bent-shape
For sp3 Hybridisation:
  1.  ABType, where there are four bond pairs and zero lone pair. Such type of molecule has Tetrahedral shape (Example, CH4).
  2. AB3L Type, where there are three bond pairs and one lone pair. Such type of molecule has Pyramidal shape (Example NH3).
  3. AB2L2 Type, where there are two bond pairs and two lone pairs. Such type of molecule has V-shape/Bent-shape (Example H2O).
For sp3d Hybridisation:
  1. AB5 Type, where there are five bond pairs and zero lone pair. Such type of molecule has Trigonal Bipyramidal shape (Example, PCl5).
  2. AB4L Type, where there are four bond pairs and one lone pair. Such type of molecule has Seesaw shape (Example SF4).
  3. AB3L2 Type, where there are three bond pairs and two lone pairs. Such type of molecule is T-shaped (Example ClF3).
  4. AB2L3 Type, where there are two bond pairs and three lone pairs. Such type of molecule has Linear shape (Example I3-).
For sp3d2 Hybridisation:
  1. AB6 Type, where there are six bond pairs and zero lone pairs. Such type of molecule has Octahedral shape. (Example SF6).
7 months ago
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