Can you help with the first 3 rows of the chart? Certainly! Here's a transcription suitable for an educational website:---**Molecular Geometry Report Sheet****Problem Set 2: Please fill out the whole table**Use the online software to build the 3D structure of the molecule shown below. Save the 3D image and attach it to the report sheet!![Molecule Structure](#)The molecular structure provided is a Lewis structure with the atoms labeled:1. **C** - Methyl group (H₃C)2. **O**3. **C** - Central atom4. **N**5. **Cl** - Chlorine atom**Consider the molecule to the left:**The numbers next to the groups refer to the C, N, O, or Cl atoms. Before you begin to fill in the table below, complete the Lewis structure by drawing in the lone pairs of electrons. Then, build the molecule using the online Molecular Builder.| Atom Number | # of Electron Groups | Hybridization | Electron Group Shape | # of Atoms Around Central Atom | Molecular Shape | Ideal Bond Angle ||-------------|----------------------|---------------|----------------------|-------------------------------|-----------------|-----------------|| 1 | | | | | | || 2 | | | | | | || 3 | | | | | | || 4 | | | | | | || 5 | | | | | | || 6 | | | | | | |Note: Ensure each atom is correctly identified with its electron groups, hybridization state, and molecular shape.--- This table allows students to analyze the molecular geometry of the given structure by considering electron groups, hybridization, and expected bond angles.

We are given the Lewis diagram of the molecule and we have to find electron group, hybridization, molecular shape, bond angle etc.# # of electron groups: Each of the bonds (whether single, double or triple) made by the central atom is considered as 1 electron group. Also, each of the lone pair present on the central atom is considered as a 1 electron group. Atom number-1 is making 4 bonds (3H and 1 C) and has no lone pairs. Hence # of electron group = 4 Atom number-2 is making 3 bonds (2O and 1 C) and has no lone pairs. Hence # of electron group = 3 Atom number-3 is making 1 bond (1C) and has 2 lone pairs. Hence # of electron group = 1+2 = 3 # Hybridization: For 2 electron groups on central atom, hybridization is sp. For 3 electron groups on central atom, hybridization is sp2. For 4 electron groups on central atom, hybridization is sp3 for 5 electron groups on central atom, hybridization is sp3d, etc. Atom number-1 has 4 electron groups. Hence hybridization is sp3. Atom number-2 has 3 electron groups. Hence hybridization is sp2. Atom number-3 has 3 electron groups. Hence hybridization is sp2.# Electron group shape: For 2 electron groups, shape is linear. For 3 electron groups, shape is trigonal planar. for 4 electron groups, shape is tetrahedral. for 5 electron groups, shape is trigonal bipyramidal, for 6 electron groups, shape is octahedral, etc. Atom number-1 has 4 electron groups. Hence the shape is tetrahedral. Atom number-2 has 3 electron groups. Hence the shape is trigonal planar. Atom number-3 has 3 electron groups. Hence the shape is trigonal planar. # Number of atoms around central atom: Atom number-1 has 4 atoms (3H and 1 C) around central atom Atom number-2 has 3 atoms (2O and 1 C) around central atom Atom number-3 has 1 atom (1 C) around central atom. # Molecular shape: Molecular shape is same as electron group shape when there is no lone pair on the central atom. When there is lone pair on the central atom, we can use the VSEPR theory to find the molecular shape. Atom number-1 has no lone pairs and has 4 electron groups. Hence the shape is tetrahedral. Atom number-2 has no lone pairs and has 3 electron groups. Hence the shape is trigonal planar #Ideal bond angle: For tetrahedral shape, ideal bond angle is 109.28 For trigonal planar, the ideal bond angle is 120. Hence Atom number-1 has a bond angle of 109.28 Atom number-2 has a bond angle of 120The complete table is shown below: Atom Number # of electron groups Hybridization Electron group shape # of atoms around central atom Molecular shape Ideal bond angle 1 4 sp3 Tetrahedral 4 Tetrahedral 109.28 2 3 sp2 Trigonal planar 3 Trigonal planar 120 3 3 sp2 Trigonal planar 1 NA NA