Multiple Choice
What is the molecular geometry of the sulfate ion, SO_4^{2-}?
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12. Molecular Shapes & Valence Bond Theory
Molecular Geometry
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What is the molecular geometry of the perchlorate ion, ClO_4^-?
A
Octahedral
B
Square planar
C
Tetrahedral
D
Trigonal pyramidal
Verified step by step guidance1
Identify the central atom in the perchlorate ion (ClO_4^-), which is chlorine (Cl).
Determine the number of valence electrons for the central atom and the surrounding atoms. Chlorine has 7 valence electrons, and each oxygen has 6 valence electrons. Also, account for the extra electron due to the negative charge.
Calculate the total number of valence electrons in the ion by adding the electrons from chlorine, four oxygens, and the extra electron from the negative charge.
Draw the Lewis structure by placing chlorine in the center and surrounding it with four oxygen atoms, then distribute the electrons to satisfy the octet rule for each atom, considering resonance structures if necessary.
Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to determine the molecular geometry. Since there are four regions of electron density (four bonding pairs) around the central chlorine atom and no lone pairs, the geometry is tetrahedral.
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