Draw the Lewis Structure for SBr2 and Provide the Following Information: a) Number of Electron Groups b) Electron Pair Geometry c) Bond Angle d) Number of Bonded Electrons e) Molecular Geometry f) Polarity

To draw the Lewis structure for SBr₂, we start by determining the total number of valence electrons. Sulfur (S) has 6 valence electrons and each bromine (Br) has 7, giving us a total of:

6 (S) + 2 × 7 (Br) = 20 valence electrons.

In the Lewis structure, sulfur is the central atom, bonded to two bromine atoms. We place the bonded electrons between S and Br:

S:Br  Br

Next, we need to account for the lone pairs of electrons. Sulfur has a total of 6 valence electrons after forming two single bonds with the bromine atoms (2 electrons for each bond). This leaves us with:

6 – 4 (2 for each bond) = 2 electrons, which will be placed as a lone pair on the sulfur atom.

The resulting Lewis structure looks like this:

   Br   
    |    
   S:    
    |    
   Br

Now, we can answer the specific questions:

• a) Number of Electron Groups: 3 (two bonded pairs and one lone pair)
• b) Electron Pair Geometry: Trigonal planar (considering all electron groups)
• c) Bond Angle: Approximately 120 degrees
• d) Number of Bonded Electrons: 4 (two bonds, each with two electrons)
• e) Molecular Geometry: Bent (due to the lone pair repulsion)
• f) Polarity: Polar (due to the difference in electronegativity between S and Br, and the bent shape)

In summary, the Lewis structure for SBr₂ indicates its bent shape, resulting in a polar molecule.