Multiple Choice
Water has a 'bent' molecular geometry. Which properties of water contribute to this shape?
12. Molecular Shapes & Valence Bond Theory
Molecular Geometry
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Determine the molecular geometry for the following molecule:IF4–.
A
Square planar
B
Square pyramidal
C
Trigonal bipyramidal
D
Seesaw
Verified step by step guidance1
Identify the central atom in the molecule. For IF4–, iodine (I) is the central atom.
Determine the total number of valence electrons. Iodine has 7 valence electrons, each fluorine has 7, and the negative charge adds 1 more electron. Calculate the total: 7 (I) + 4*7 (F) + 1 (charge) = 36 electrons.
Use the valence shell electron pair repulsion (VSEPR) theory to determine the electron pair geometry. Distribute the electrons around the central atom to minimize repulsion. Iodine will have 4 bonding pairs (from the 4 fluorine atoms) and 2 lone pairs.
Determine the molecular geometry based on the arrangement of the atoms. With 4 bonding pairs and 2 lone pairs, the electron pair geometry is octahedral, but the molecular geometry is square planar because the lone pairs are opposite each other, minimizing their effect on the shape.
Verify the molecular geometry by considering the positions of the atoms. In a square planar geometry, the four fluorine atoms form a square around the iodine atom, with the lone pairs above and below the plane of the square.
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