Chemistry Molecular Geometry: Discover the Fascinating World of Atoms and Bonding

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The discussion centers on the possible molecular shapes for a central atom with sp3d hybridization. It identifies that the only feasible shape is trigonal bipyramidal, which accommodates five electron pairs. The other options—linear, seesaw, T-shaped, and tetrahedral—are debated, with tetrahedral being ruled out due to its four bonding pairs. Participants suggest confirming the question's accuracy, as some shapes appear to be sub-geometries of the trigonal bipyramidal. The conversation highlights the importance of understanding hybridization in determining molecular geometry.
force
never mind its over ! )
 
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force said:
for this I have no idea
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Which of the following shapes is not possible for a molecule in which the central atom has sp3d hybridization?
a. linear
b. seesaw
c. T-shaped
d. tetrahedral
e. trigonal bipyramidal
The hybridization somewhat refers to how many things the central atom is, or can be, bound to. sp3d is 1 + 3+ 1 = 5 things (electron pairs count as things).

Are you sure this question is correct? The only one that seems possible is trigonal bipyramidal since that connects to 5 things. Linear is, I think, just 1 thing (acetylene), seesaw sounds like a joke answer, T-shape also sounds like a joke answer, and tetrahedral means 4 things (methane). Ask your teacher if that question has a typo.
 
I just realized actually those funny names are sub geometries of the trigonal bipyramidal which all can have up to five legs, the only one that can't it seems is the tetrahedral which has 4 bonding pairs and 0 non-bonding pairs.
 
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