Question

The degree of unsaturation in the above compound is (A) 7 (B) 9 (C) 12 (D) 13

Short answer

Without the molecular formula of the compound, it is impossible to determine the degree of unsaturation (IHD) and choose between options A, B, C, and D.

Step-by-step solution

1. Molecular formula of the compound

First, we need the molecular formula of the compound. As it is not provided in the problem, we will assume that the compound has a general molecular formula of C_xH_yO_zN_w, where x, y, z, and w are the numbers of each atom present.

2. Calculate the degree of unsaturation (IHD) using the molecular formula

The general formula to calculate the degree of unsaturation for a given molecular formula is: IHD = (2x + 2 - y + z + w) / 2 However, since we don't have the molecular formula of the compound in the problem, we cannot use this formula directly. Instead, we can use the fact that each degree of unsaturation corresponds to either a double bond, a triple bond, or a ring in the molecule.

3. Enumerate the degrees of unsaturation in the compound

We can check for each option (A, B, C, and D) and see if the corresponding number of degrees of unsaturation can be accommodated in the compound with a general molecular formula. Let's analyze each option: Option (A) - 7 degrees of unsaturation: This option would correspond to a combination of 7 double bonds, triple bonds, or rings in the compound. It is a plausible value. Option (B) - 9 degrees of unsaturation: This option would correspond to 9 double bonds, triple bonds, or rings in the compound. It is also a plausible value. Option (C) - 12 degrees of unsaturation: This option would correspond to 12 double bonds, triple bonds, or rings in the compound. This is a high value, and it might be difficult to accommodate 12 unsaturation degrees without violating valency rules. However, it's impossible to say without knowing the exact molecular formula. Option (D) - 13 degrees of unsaturation: This option would correspond to 13 double bonds, triple bonds or rings in the compound. This is a very high value, making it highly unlikely to have the proper valency for a real compound. However, without the exact molecular formula, it's impossible to say for sure. Since crucial data to solve this exercise is missing (the compound molecular formula), we cannot give a definite answer.

Key concepts

Molecular Formula

Understanding the molecular formula of a compound is vital in chemistry, as it tells you the types and numbers of atoms present in a molecule. A molecular formula like C_xH_yO_zN_w is a type of chemical formula that presents the actual number of carbon atoms (C), hydrogen atoms (H), oxygen atoms (O), and nitrogen atoms (N) in one molecule of a compound.

The molecular formula is essential for determining the compound's molecular structure and properties. Think of it as a basic blueprint from which one can deduce information about the molecular composition, chemical reactions, and physical properties of the substance. For instance, in organic chemistry, the formula helps us figure out the framework within which we can place double bonds or rings, concepts closely tied to the degree of unsaturation in molecules.

It's important to note that without the complete molecular formula, as seen in the given exercise, we cannot precisely calculate the degree of unsaturation or infer the structure of the molecule. Hence, when tackling problems in organic chemistry, always ensure you have the molecular formula at hand—it's your starting line for any molecular analysis.

Double Bonds

Double bonds are a type of covalent bond where two pairs of electrons are shared between atoms. These are represented by a double line (=) between the atoms in structural formulae. In the context of the degree of unsaturation, each double bond contributes one point of unsaturation to the molecule.

In the original exercise, we can infer that each degree of unsaturation might represent a double bond among other possibilities like rings or triple bonds. This is because, in organic compounds, double bonds are one of the common sources of unsaturation. They add complexity to molecular structures by creating rigid, planar regions in the molecule, which influence the compound’s reactivity and physical properties.

Understanding Unsaturation

Unsaturation in a compound suggests a deficit of hydrogen atoms compared to a fully saturated hydrocarbon with the same number of carbon atoms. Therefore, the presence of double bonds means there are fewer hydrogen atoms than in a fully saturated version of the molecule, which often alters the molecule's physical and chemical behavior.

Ring Structures

Ring structures are another significant contributor to the degree of unsaturation in molecules. A ring structure is formed when atoms in a compound connect to form a closed loop. Like double bonds, each ring in a molecule also contributes one degree of unsaturation because they involve the loss of potential hydrogen atoms during the ring formation, compared to open chain (acyclic) hydrocarbons.

Ring structures impact a compound's chemical characteristics, such as its stability and its reactivity. For instance, benzene is a classic example of a compound with a ring structure; it is highly stable due to its aromaticity, a concept involving delocalized electrons within the ring.

Distinguishing between double bonds and ring structures when analyzing the degree of unsaturation is necessary but can be challenging without further data. In the original exercise, options with higher degrees of unsaturation could imply complex molecules with multiple rings and/or double bonds. However, without the actual molecular formula, such assumptions are speculative, and we would need additional information to precisely determine the structure of the molecule.