Write electron-dot structures for each of the following molecules, and use VSEPR theory to predict the structure of each: (a) H2S (b) SO2 (c) SO3.

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons for each molecule. For H2S, sulfur (S) has 6 valence electrons and each hydrogen (H) has 1 valence electron, totaling 8 valence electrons. For SO2, sulfur has 6 valence electrons and each oxygen (O) has 6 valence electrons, totaling 18 valence electrons. For SO3, sulfur has 6 valence electrons and each oxygen has 6 valence electrons, totaling 24 valence electrons.
2. Step 2: Draw the skeletal structure of each molecule. For H2S, place sulfur in the center with hydrogen atoms bonded to it. For SO2, place sulfur in the center with oxygen atoms bonded to it. For SO3, place sulfur in the center with three oxygen atoms bonded to it.
3. Step 3: Distribute the remaining valence electrons to satisfy the octet rule for each atom, starting with the outer atoms. For H2S, place the remaining electrons around sulfur. For SO2, place the remaining electrons around the oxygen atoms, and if needed, form double bonds to satisfy the octet rule. For SO3, distribute electrons around the oxygen atoms and form double bonds as necessary.
4. Step 4: Use VSEPR theory to predict the molecular geometry. For H2S, with two bonding pairs and two lone pairs on sulfur, the shape is bent. For SO2, with two bonding pairs and one lone pair on sulfur, the shape is also bent. For SO3, with three bonding pairs and no lone pairs on sulfur, the shape is trigonal planar.
5. Step 5: Verify the stability of the structures by checking formal charges and ensuring that the most electronegative atoms have the negative formal charges, if any. Adjust the structures if necessary to minimize formal charges.