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What are the molecular shapes of XeF4, XeF5⁻, and SnCl2 respectively?

1. Octahedral, trigonal bipyramidal, and bent
2. Square pyramidal, pentagonal planar, and linear
3. Square planar, pentagonal planar, and angular
4. See-saw, T-shaped, and linear

Correct answer: Square planar, pentagonal planar, and angular

Solution

XeF4: Xe valence electrons = 8. 4 Xe-F bonds use 4 pairs. Remaining: (8-4)/2 = 2 lone pairs. Total = 6 pairs -> octahedral electron geometry. 2 lone pairs occupy axial positions -> shape is square planar. XeF5⁻: Xe gets 8e + 1 (from negative charge) = 9e. 5 bonds use 5e. Remaining: (9-5)/2 = 2 lone pairs. Total = 7 pairs -> pentagonal bipyramidal electron geometry. 2 axial lone pairs -> shape is pentagonal planar. SnCl2: Sn has 4 valence e. 2 bonds use 2e. 1 lone pair. Total 3 pairs -> trigonal planar geometry -> angular (bent) shape. Answer: Square planar, pentagonal planar, angular.

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