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A single C-N bond is a common type of bond found in many organic compounds. It is formed when one pair of electrons is shared between a carbon and a nitrogen atom. This sharing of electrons allows both atoms to achieve a more stable configuration.

The length of a typical single C-N bond is quite significant at approximately 147 pm. This measurement arises because the bond involves just one pair of electrons, resulting in a relatively lower degree of overlap between the atomic orbitals of carbon and nitrogen.

Such bonds are generally flexible and allow rotational movement around the bond axis, making them quite useful in various organic molecules where movement is needed. Single C-N bonds are often found in compounds like amines and amides, which are important building blocks in both biological and synthetic chemistry.

• Bond length: 147 pm
• Type: Single bond
• Common in: Amines, amides

A double C-N bond involves the sharing of two pairs of electrons between carbon and nitrogen atoms. This type of bond is stronger and shorter than a single C-N bond. The presence of two electron pairs increases the electron density between the atoms, enhancing the strength of the bond.

The double C-N bond typically measures about 130 pm in length. This reduction in length compared to a single C-N bond is due to the additional electron pair, which brings the atoms closer together.

Double C-N bonds are commonly found in compounds such as imines and enamines. These structures play a key role in various chemical reactions, serving as intermediates in many synthetic processes. This added bond strength makes the C-N linkage more rigid, limiting its rotation compared to a single bond.

• Bond length: 130 pm
• Type: Double bond
• Common in: Imines, enamines

The triple C-N bond is the strongest and shortest amongst the types of carbon-nitrogen bonds. It is characterized by the sharing of three pairs of electrons between the carbon and nitrogen atoms, leading to a very stable and tightly bound structure.

Due to the high electron density between the atoms, the stable nature of the bond results in a bond length of approximately 120 pm. This is considerably shorter than both single and double C-N bonds.

Triple C-N bonds are typically found within molecules like nitriles and cyanides. Such bonds are extremely rigid due to the extra electron pairs, and they don't easily allow for rotation. This rigidity makes compounds with triple C-N bonds very linear in their geometry. Understanding this bond is crucial for its role in many industrial and chemical applications.

• Bond length: 120 pm
• Type: Triple bond
• Common in: Nitriles, cyanides