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 attached it to the report sheet! 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 elections. Then, build the molecule using the online Molecular Builder. 1 H3C #of Electron Groups Electron Hybridiz # of Atoms Around Central Atom Atom Number Ideal Bond Angle Group Shape Molecular Shape ation 3 4. 6.
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
The molecular structure provided is a Lewis structure with the atoms labeled:
1. **C** - Methyl group (H₃C)
2. **O**
3. **C** - Central atom
4. **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.
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This table allows students to analyze the molecular geometry of the given structure by considering electron groups, hybridization, and expected bond angles.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1bf8ae83-2003-4837-b9fe-b672e6e8d8b8%2F8d11a40f-53b8-45dd-841c-4176bc630f1e%2Fgdnzfm8_processed.jpeg&w=3840&q=75)
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