The molecular geometry of SBr2 (sulfur dibromide) is bent, while the molecular geometry of CH3Br (methyl bromide) is tetrahedral.
In the case of SBr2, the sulfur atom is the central atom bonded to two bromine atoms. Sulfur has six valence electrons, and when it forms two bonds with bromine, there are two lone pairs of electrons left on the sulfur atom. These lone pairs repel the bonded atoms, which results in a bent geometry with a bond angle of approximately 104 degrees.
On the other hand, in CH3Br, the carbon atom is the central atom bonded to three hydrogen atoms and one bromine atom. Carbon also has four valence electrons, and it forms four single bonds (three with hydrogen and one with bromine), resulting in a tetrahedral shape. The bond angles in CH3Br are approximately 109.5 degrees.
In summary, SBr2 with its lone pairs and bonded atoms exhibits a bent geometry, while CH3Br, having no lone pairs at the central atom, demonstrates a tetrahedral geometry.