Draw the bonding orbital that results from the constructive overlap of the two p, orbitals shown below. node (higher energy) Px Px o antibonding MO
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.
please explain answer
![### Constructive Overlap of \( \sigma \) Bonding Orbitals
When two \( p_x \) orbitals overlap constructively, they form a \( \sigma \) bonding orbital. This can be understood through the diagram provided below.
#### Visualization of \( p_x \) Orbital Overlap:
1. **Initial \( p_x \) Orbitals:**
- The diagram starts with two \( p_x \) orbitals shown individually. Each orbital has a positive (+) and a negative (-) lobe, represented by different colors (green and blue).
- The orbitals are placed adjacent to each other to indicate potential overlap.
2. **Constructive Overlap:**
- When the \( p_x \) orbitals overlap constructively, their wavefunctions combine in phase (+ with + and - with -).
- This constructive interference leads to the formation of a \( \sigma \) bonding orbital.
3. **Formation of \( \sigma \) Antibonding Molecular Orbital:**
- The diagram depicts the two \( p_x \) orbitals overlapping and forming a bond where the areas of constructive overlap increase electron density along the axis connecting the two nuclei.
- An antibonding molecular orbital (\( \sigma^* \)) is also illustrated. This orbital has a node, represented by a dashed magenta line, where there is zero electron probability.
4. **Energy Comparison:**
- The diagram annotates that the \( \sigma^* \) antibonding molecular orbital is higher in energy compared to the \( \sigma \) bonding orbital.
### Summary
By tracing the progression from individual \( p_x \) orbitals to their combined \( \sigma \) antibonding molecular orbital, one can understand how atomic orbitals merge to form molecular orbitals. The key takeaway is recognizing how the constructive overlap leads to a bonding interaction, whereas destructive overlap results in a higher energy antibonding interaction with a node of zero electron density. This concept is fundamental in understanding molecular orbital theory and the formation of chemical bonds.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1cf81ca3-2485-4010-80d9-cb2da241c90c%2F749e3875-faf0-4b0e-b889-2dca8c72b2fd%2Fjwneo8_processed.png&w=3840&q=75)
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