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.
2. **Molecule: SF₄**
- **Geometry:**
3. **Molecule: CF₄**
- **Geometry:**
4. **Molecule: BrF₅**
- **Geometry:**
5. **Molecule: PCl₅**
- **Geometry:**
6. **Molecule: XeF₄**
- **Geometry:**
#### Graphs/Diagrams Explanation
* **SiH₄ (Silicon Tetrahydride)**: The structure commonly adopts a tetrahedral geometry, where the central silicon (Si) atom is bonded to four hydrogen (H) atoms. The diagram typically shows four bonds extending symmetrically from the silicon atom with bond angles close to 109.5 degrees.
* **SF₄ (Sulfur Tetrafluoride)**: This molecule often exhibits a see-saw geometry, also known as disphenoidal. Sulfur (S) is the central atom with four fluorine (F) atoms bonded to it. One lone pair of electrons is present on the sulfur atom, creating a unique shape.
* **CF₄ (Carbon Tetrafluoride)**: This molecule adopts a tetrahedral shape where the central carbon (C) atom is bonded to four fluorine (F) atoms. The diagram shows the fluorine atoms positioned symmetrically around carbon, making bond angles of 109.5 degrees.
* **BrF₅ (Bromine Pentafluoride)**: Typically, this molecule forms a square pyramidal geometry with bromine (Br) as the central atom. Five fluorine (F) atoms are bonded to the bromine, and the molecule has one lone pair of electrons on the central atom.
* **PCl](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3e3f76e7-3e2b-4631-a85d-ebd3274410fe%2F0cd49a37-0b59-4e8a-95c6-b34490e70246%2F1t3ynupn_processed.png&w=3840&q=75)
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