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cyclopentane (7.4 kcal/mol), C 5 H 10 — if it was a completely regular planar pentagon its bond angles would be 108°, but tetrahedral 109.5° bond angles are expected. [6] However, it has an unfixed puckered shape that undulates up and down.
Cyclopentane can be fluorinated to give compounds ranging from C 5 H 9 F to perfluorocyclopentane C 5 F 10. Such species are conceivable refrigerants and specialty solvents. [15] [16] The cyclopentane ring is pervasive in natural products including many useful drugs. Examples include most steroids, prostaglandins, and some lipids.
For a theoretical planar cyclopentane the C–C–C bond angles would be 108°, very close to the measure of the tetrahedral angle. Actual cyclopentane molecules are puckered, but this changes only the bond angles slightly so that angle strain is relatively small.
Each carbon atom within the cyclopentane ring is sp 3 hybridized with the theoretical C-C-C bond angles near 108 degrees. Therefore ring strain is less prominent compared to other cycloalkanes as there is minimal deviation from the ideal tetrahedral bond angle, 109.5 degrees.
In molecules, it is quite common for these angles to be somewhat compressed or expanded compared to their optimal value. This strain is referred to as angle strain, or Baeyer strain. [9] The simplest examples of angle strain are small cycloalkanes such as cyclopropane and cyclobutane, which are discussed below.
A bond angle is the geometric angle between two adjacent bonds. Some common shapes of simple molecules include: Linear: In a linear model, atoms are connected in a straight line. The bond angles are set at 180°. For example, carbon dioxide and nitric oxide have a linear molecular shape.
Structure of boron trifluoride, an example of a molecule with trigonal planar geometry.. In chemistry, trigonal planar is a molecular geometry model with one atom at the center and three atoms at the corners of an equilateral triangle, called peripheral atoms, all in one plane. [1]
The value of 1 J 13 C-1 H for cyclopropane, cyclobutane and cyclopentane are 161, 134, and 128 Hz, respectively. This is a consequence of the fact that the C-C bonds in small, strained rings (cyclopropane and cyclobutane) employ excess p character to accommodate their molecular geometries (these bonds are famously known as ' banana bonds ').