Indicate the hybridization of the central atom in each molecule shown. 0=c=8 sp sp² sp³ d sp³ d² sp³ •H sp sp³ sp³ d sp² sp³ d² -8± -H sp³ d² sp³ d sp³ sp sp² BeF:
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.
![## Hybridization of Central Atoms in Molecules
In this section, you will learn about the hybridization of the central atom in various molecules. For each of the given molecules, examine the provided Lewis structures and determine the hybridization state of the central atom. Select the correct hybridization from the options provided.
### Molecule 1
\[
\text{Structure:} \quad \ddot{O}=C=\ddot{O}
\]
Options:
1. sp
2. sp^2
3. sp^3d
4. sp^3d^2
5. sp^3
### Molecule 2
\[
\text{Structure:} \quad \ddot{F}-\ddot{Be}-\ddot{F}
\]
Options:
1. sp^3d^2
2. sp^3d
3. sp^3
4. sp
5. sp^2
### Molecule 3
\[
\text{Structure:} \quad \ddot{O}^{+} (H)_{\perp}(H (H))
\]
Options:
1. sp
2. sp^3
3. sp^3d
4. sp^2
5. sp^3d^2
For each molecule, use the structure and electron configuration to determine the correct hybridization. Hybridization provides insight into the geometry and bonding properties of molecules, crucial for understanding molecular shapes and reactivity.
#### Explanation of Diagrams:
- **Molecule 1 Diagram**: The central atom is Carbon (C) double-bonded to two Oxygen (O) atoms. The Oxygen atoms have lone pairs denoted by dots.
- **Molecule 2 Diagram**: The central atom is Beryllium (Be), single-bonded to two Fluorine (F) atoms, each Fluorine atom has three lone pairs of electrons.
- **Molecule 3 Diagram**: The central atom is an Oxygen (O) atom with a positive charge, bonded to three Hydrogen (H) atoms.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3e3f76e7-3e2b-4631-a85d-ebd3274410fe%2Fe451be33-939a-461a-9be7-84afecf4575b%2F3eyheuj_processed.png&w=3840&q=75)
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