Question

\(\mathrm{C}_{4} \mathrm{H}_{6}\) corresponds to general molecular formula \(\mathrm{C}_{\mathrm{n}} \mathrm{H}_{2 \mathrm{n}-2} .\) which possesses one triple bond.

Short answer

Provide an example of a molecule that fits this description. Answer: The formula \(\mathrm{C}_{4} \mathrm{H}_{6}\) corresponds to the general molecular formula \(\mathrm{C}_{n} \mathrm{H}_{2n-2}\), which includes one triple bond. An example of a molecule that fits this description is 1-Butyne, with the structure \(\mathrm{H}_{3}\mathrm{C}\!-\!\\mathrm{C}\!#\!\\mathrm{C}\!-\!\\mathrm{CH}_3\).

Step-by-step solution

Verify that the given formula satisfies the general molecular formula

First, we will plug the values for the given molecular formula, \(\mathrm{C}_{4} \mathrm{H}_{6}\), into the general molecular formula \(\mathrm{C}_{n} \mathrm{H}_{2n-2}\) to make sure the relationship holds. To do this, let n = 4 and check if the number of hydrogen atoms is equal to 2n - 2: Number of hydrogen atoms = 2(4) - 2 = 6 Since the given molecular formula, \(\mathrm{C}_4 \mathrm{H}_6\), has 6 hydrogen atoms, the relationship holds and the given molecular formula fits the general molecular formula.

Identify a molecule with this molecular formula and a triple bond

To complete the exercise, we will identify a molecule with the given molecular formula, \(\mathrm{C}_4 \mathrm{H}_6\), and a triple bond. One such example is 1-Butyne, which has the following structure: \(\mathrm{H}_{3}\mathrm{C}\!-\!\\mathrm{C}\!#\!\\mathrm{C}\!-\!\\mathrm{CH}_3\) 1-Butyne has a triple bond between two of its carbon atoms, satisfying the requirement for the general molecular formula discussed in this exercise. Therefore, the given molecular formula, \(\mathrm{C}_4 \mathrm{H}_6\), corresponds to the general molecular formula \(\mathrm{C}_{n} \mathrm{H}_{2n-2}\) which possesses one triple bond.

Key concepts

Understanding the General Molecular Formula

The concept of a general molecular formula is a crucial foundation in organic chemistry. It represents a series of compounds that share a common structural feature, often including a specific type of bond or arrangement of atoms. When we say a hydrocarbon follows the general molecular formula of \(\mathrm{C}_{n} \mathrm{H}_{2n-2}\), it indicates a special relationship between carbon (\( \mathrm{C} \) and hydrogen (\( \mathrm{H} \) atoms. This formula describes a whole class of hydrocarbons called alkynes.

For instance, when an alkyne has four carbon atoms (\( \mathrm{C}_4 \) like in our exercise, we can determine the number of hydrogen atoms by simply plugging into the general formula: \( \mathrm{H}_{2n-2} \). This results in six hydrogen atoms (\( \mathrm{H}_6 \)), showcasing the relationship and confirming the compound fits this particular category of organic molecules.

• Significance: This general formula helps greatly in predicting properties and reactions of the compounds it represents.
• Benefits: It assists in identifying and classifying compounds quickly.

Markedly, understanding this concept streamlines the study of complex organic molecules by recognizing patterns and standardizing nomenclature.

Alkynes and Their Unique Characteristics

Alkynes are one of the fascinating groups of hydrocarbons in organic chemistry. Characterized by a carbon-to-carbon triple bond, they fit the general molecular formula \(\mathrm{C}_{n} \mathrm{H}_{2n-2}\), as seen in our exercise with \(\mathrm{C}_4 \mathrm{H}_6\). This triple bond not only defines their structure, but also gives them distinct properties and reactivity.

The presence of the triple bond makes alkynes unsaturated, meaning they have fewer hydrogen atoms than their alkane (single bond) and alkene (double bond) counterparts. This bond is composed of one sigma bond and two pi bonds, which makes alkynes linear in the region of the triple bond and affects their geometrical properties.

• Importance: Practically, this enables alkynes to undergo reactions like addition reactions where these pi bonds can be broken to add other atoms or groups, leading to the synthesis of various other chemical compounds.
• Examples: Some common alkynes include acetylene (\( \mathrm{C}_2 \mathrm{H}_2 \) and the molecule from our exercise, 1-Butyne (\( \mathrm{C}_4 \mathrm{H}_6 \)).

Alkynes hence offer rich ground for exploring organic synthesis and the creation of many complex molecules vital to industry and pharmaceuticals.

Triple Bond: A Strong and Unique Connection

Diving deeper into the chemistry of alkynes, the triple bond stands out as an integral feature. This bond involves three shared pairs of electrons between two carbon atoms, making it the strongest and shortest of the covalent bonds between carbons in hydrocarbons.

Its composition includes one sigma bond, which maintains the linearity and rotation restriction of the connected carbon atoms, and two pi bonds, which account for the bond's high reactivity and strength. Since these pi bonds occupy space above and below the sigma bond plane, they are easily accessible to reactants, laying the ground for many possible chemical reactions.

• Strength and Reactivity: The high electron density of the triple bond makes it an electrophile, susceptible to attack by nucleophiles in chemical reactions, such as hydrogenation or halogenation.
• Application: This reactivity is exploited in organic synthesis, where the manipulation of triple bonds allow chemists to build complex structures and create new molecules.

The understanding of triple bonds is pivotal in chemistry, not only for grasping the nature of alkynes but also for recognizing the potential of these bonds in the synthesis and transformation of organic substances.