The following are 2s, 2p, sp, sp?, and sp orbitals, all drawn to scale and in no particular order. Which of these orbitals represents the hybrid orbital with the greatest effective electronegativity? IV Select one: O a. I O b. II O c. II O d. IV
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.
![**Question:**
The following are 2s, 2p, sp, sp², and sp³ orbitals, all drawn to scale and in no particular order. Which of these orbitals represents the hybrid orbital with the greatest effective electronegativity?
[Diagram showing five orbitals labeled I, II, III, IV, V]
**Options:**
- a. I
- b. II
- c. III
- d. IV
- e. V
**Explanation of Diagram:**
1. **Orbital I:** Appears elongated with a smaller lobe at one end.
2. **Orbital II:** Has a more significant tapered shape, with one end similar in size to Orbital I’s smaller lobe.
3. **Orbital III:** Includes two medium-sized, symmetrical lobes.
4. **Orbital IV:** Displays a large spherical shape.
5. **Orbital V:** Shows an elongated shape with one lobe noticeably larger similar to the shape of a balloon.
Each orbital is represented differently in size and shape, indicating the type of atomic orbital or hybridization, affecting electronegativity and bond formation potential.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8b35bbc2-cfa4-4f43-924f-aa579a12a610%2F7b22dee7-088f-4918-b294-3c516883e751%2Fji6dq2y_processed.jpeg&w=3840&q=75)
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