Consider the molecule of cyanogen. Its Lewis structure is shown. : N EC- Which carbon orbitals are involved in pi bonding in cyanogen? 2p Osp³ hybrids 3 Osp hybrids 2s EN: sp² hybrids
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.
![**Cyanogen Molecule: Orbital Involvement in Pi Bonding**
Consider the molecule of cyanogen. Its Lewis structure is shown:
\: N≡C—C≡N :
**Question:**
Which carbon orbitals are involved in pi bonding in cyanogen?
**Options:**
- ○ 2p
- ○ sp³ hybrids
- ○ sp hybrids
- ○ 2s
- ○ sp² hybrids
**Explanation of the Lewis Structure:**
The structure of cyanogen consists of two nitrogen atoms and two carbon atoms. Each nitrogen atom forms a triple bond with a carbon atom. In the Lewis structure, the carbon atoms are connected to each other by a single bond. The nitrogen atoms each carry a pair of lone electrons, depicted by the dots.
This molecular structure results in a linear arrangement, which suggests specific orbital interactions for the formation of the molecule's pi bonds. The pi bonding specifically involves the overlap of p orbitals, which are perpendicular to the axis of the sigma bonds. The question asks to identify these specific orbitals for carbon in cyanogen.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faab01dc0-572f-4647-affc-231aefa5eea9%2F9dc68972-050f-4355-86cc-5cddb7dbd22d%2Fuftaj93_processed.jpeg&w=3840&q=75)
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