For each of the Lewis structures shown below, predict the Electron Geometry, Molecular Geometry and Bond Angle. Lastly, using the same format as shown in the last column of Table 1, draw a sketch (using wedges and dashes to show 3D if needed) of the Molecular Geometry. Lewis Structure S=C=S :a: :CI: Total Number of Substituents Number of Nonbondi ng Pairs Name of Electron Geometry Name of Bond Sketch of Molecular Molecular Angl Geometry Geometry e
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.
For each of the Lewis structures shown below, predict the Electron Geometry, Molecular Geometry and Bond Angle. Lastly, using the same format as shown in the last column of Table 1, draw a sketch (using wedges and dashes to show 3D if needed) of the Molecular Geometry.
![**Part D: Applying VSEPR Theory**
For each of the Lewis structures shown below, predict the Electron Geometry, Molecular Geometry, and Bond Angle. Lastly, using the same format as shown in the last column of Table 1, draw a sketch (using wedges and dashes to show 3D if needed) of the Molecular Geometry.
| Lewis Structure | Total Number of Substituents | Number of Nonbonding Pairs | Name of Electron Geometry | Name of Molecular Geometry | Bond Angle | Sketch of Molecular Geometry |
|-----------------------|--------------------------|-------------------------|---------------------------|----------------------------|------------|------------------------------|
| S=C=S | | | | | | |
| :Cl: | | | | | | |
| \| | | | | | | |
| C=O | | | | | | |
| \| | | | | | | |
| :Cl: | | | | | | |
| :F–S–F: | | | | | | |
**Explanation:**
This table is used to analyze different Lewis structures using VSEPR (Valence Shell Electron Pair Repulsion) Theory to determine Electron Geometry, Molecular Geometry, and Bond Angles. The sketches provide a visual representation of the molecular shapes in three dimensions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F355a4549-e226-4aa5-80df-9c537d6bba06%2F2b279801-ee50-4695-8317-5ffc9cfb2700%2Fqmcztl_processed.png&w=3840&q=75)
![The image displays a table containing three Lewis structures of molecules, with blank columns likely meant for further information or properties. Below is a description of each diagram:
1. **Diagram 1 (Top row)**:
- Molecule: Ammonia (NH₃)
- Structure: The diagram shows a nitrogen (N) atom at the center with three hydrogen (H) atoms attached. The nitrogen has a pair of dots representing a lone electron pair, making a total of four electron regions around the nitrogen.
2. **Diagram 2 (Middle row)**:
- Molecule: Carbon Tetrafluoride (CF₄)
- Structure: A carbon (C) atom is at the center bonded to four fluorine (F) atoms, each with three pairs of dots representing lone pairs. This gives the carbon a complete octet, as it shares electrons with the fluorine atoms.
3. **Diagram 3 (Bottom row)**:
- Molecule: Ozone (O₃)
- Structure: The structure consists of three oxygen (O) atoms with a central oxygen atom double-bonded to one and single-bonded to another, forming a resonance structure. The lone pairs of electrons are shown as dots.
Each diagram represents the distribution of electrons around the atoms, highlighting lone pairs and bonding pairs essential for understanding molecular geometry and polarity.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F355a4549-e226-4aa5-80df-9c537d6bba06%2F2b279801-ee50-4695-8317-5ffc9cfb2700%2Fce18czi_processed.png&w=3840&q=75)
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