Question

A Lewis structure is a two-dimensional representation of a molecule that does not necessarily show what shape that molecule would take in three dimensions. From the given Lewis structure and what you know about VSEPR theory, identify the shape of the molecule. A molecule with atom Y single bonded with 2 X substituents. The Y atom has one lone pair. T-shaped trigonal pyramidal trigonal planar octahedral tetrahedral square pyramidal see-saw linear square planar trigonal bipyramidal bent

Answer 1

Answer: Octahedral

Explanation: The way that the atoms are arranged in the Lewis structure may not match the true shape of the molecule. When determining the shape of the molecule, consider only that the molecule has six outer atoms and no lone pairs, and ignore the shape suggested by the Lewis structure.

For a molecule with six outer atoms and no lone pairs, you would expect an octahedral geometry with approximate bond angles of 90 and 180 degrees.

Answer 2

Trigonal Pyramidal

Step-by-step explanation:

The three electron pairs arrange themselves in this manner because of unequal repulsion between lone pairs and bonding pairs. according to VSEPR theory, the presence of three electron pairs leads to a trigonal planar arrangement. However, factors such as possession of a lone pair may lead to a different arrangement of electron pairs in space. Repulsion between lone pairs and bond pairs often lead to a bent or angular molecule. If there were no lone pairs and only two substituents present in this molecule, the molecule will be linear, that will correspond to the presence of only two electron pairs.