1. The problem is to match each molecule with its correct molecular shape. 2. The molecules given are: a) NH3 b) BrF5 c) XeF4 d) SF6 3. The shapes given are: i) trigonal planar ii) square planar iii) octahedral (oh) iv) square pyramidal 4. Let's analyze each molecule's shape using VSEPR theory: 5. a) NH3 (ammonia): It has 3 bonded atoms and 1 lone pair on nitrogen, giving it a trigonal pyramidal shape, which is closest to square pyramidal in the options, but since square pyramidal is for 5 bonds, the best match here is iv) square pyramidal (though strictly trigonal pyramidal, iv is the closest). 6. b) BrF5: Bromine pentafluoride has 5 bonded atoms and 1 lone pair, resulting in a square pyramidal shape. So, b) matches iv) square pyramidal. 7. c) XeF4: Xenon tetrafluoride has 4 bonded atoms and 2 lone pairs, resulting in a square planar shape. So, c) matches ii) square planar. 8. d) SF6: Sulfur hexafluoride has 6 bonded atoms and no lone pairs, resulting in an octahedral shape. So, d) matches iii) octahedral. 9. The shape trigonal planar (i) does not match any of the molecules given. Final matches: - a) NH3: iv) square pyramidal (closest) - b) BrF5: iv) square pyramidal - c) XeF4: ii) square planar - d) SF6: iii) octahedral