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Chapter 21: Problem 12

Describe the main structural characteristics of alkane molecules.

Short Answer

Expert verified
The main structural characteristics of alkane molecules include a general formula of CnH2n+2, carbon-carbon single bonds, carbon-hydrogen bonds, and a tetrahedral molecular shape. The carbon atoms in alkanes are sp3 hybridized, creating sigma bonds with other carbon and hydrogen atoms. The bond angles in an alkane are approximately 109.5 degrees, and they can be categorized as linear, branched, or cyclic (cycloalkanes) based on their structure.

Step by step solution

01

General Formula for Alkanes

The general formula for alkanes follows the pattern CnH2n+2, where n represents the number of carbon atoms in the molecule. This means that each alkane molecule contains twice as many hydrogen atoms as carbon atoms, plus two additional hydrogen atoms. For example, ethane (C2H6) has two carbon atoms and six hydrogen atoms.
02

Carbon-Carbon Single Bonds

In alkane molecules, carbon atoms are always bonded to other carbon atoms by single covalent bonds. These bonds are called sigma bonds, which involve the end-to-end overlapping of atomic orbitals. The single bond allows for free rotation around the bond axis, resulting in various conformations of the alkane molecule.
03

Carbon-Hydrogen Bonds

Each carbon atom in an alkane is also bonded to hydrogen atoms through single covalent bonds. The carbon-hydrogen bond is formed by the overlapping of a carbon sp3 hybrid orbital and a hydrogen 1s orbital. The bond strength increases as the size of the alkane molecule increases, which in turn affects the boiling and melting points of the alkane.
04

Molecular Shape

The carbon atoms in alkanes have a tetrahedral structure, meaning that they are bonded to four other atoms in a way that the bonded atoms are at the vertices of a regular tetrahedron. This structure is determined by the sp3 hybridization of the carbon atom, which helps to minimize the electron repulsion between the bonds. The bond angles in an alkane are approximately 109.5 degrees.
05

Linear, Branched and Cycloalkanes

Alkane molecules can be categorized based on their structure as linear, branched, or cyclic. Linear alkanes are straight-chain molecules where all carbon atoms are connected in a row, while branched alkanes have at least one carbon atom bonded to more than two other carbon atoms, forming a branching pattern. Cycloalkanes are alkanes where the carbon atoms are arranged in a closed ring structure, and their general formula is CnH2n.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

CnH2n+2 formula
Alkanes, one of the simplest types of hydrocarbons, follow a general formula given by \(C_nH_{2n+2}\). This formula highlights the relationship between the number of carbon atoms (\(n\)) and hydrogen atoms present in the molecule. For each carbon atom added to an alkane, two hydrogen atoms are added as well, plus an additional two to complete the structure. This distinguishes alkanes from other hydrocarbons, making them saturated compounds. Let's take hexane as an example: with six carbon atoms, the formula becomes \(C_6H_{14}\). Notice how this perfectly fits the formula \(C_nH_{2n+2}\). These calculations are foundational for determining the molecular formula for any alkane.
Carbon-carbon single bonds
In alkanes, carbon atoms are linked by single covalent bonds known as sigma bonds. These carbon-carbon bonds are the backbone of the alkane structure. The sigma bonds result from the head-on overlap of atomic orbitals, which allows for freedom of rotation around the bond axis. This rotation is a characteristic feature of these bonds, providing the molecule with flexibility and a variety of possible conformations. Hence, the single covalent bonding contributes significantly to the chemical stability and rigidity of alkane molecules.
Carbon-hydrogen bonds
Alkanes are not only defined by carbon-carbon bonds but also by carbon-hydrogen bonds. Each carbon atom in an alkane forms single covalent bonds with hydrogen atoms. These bonds arise when the carbon's \(sp^3\) hybrid orbital overlaps with the hydrogen's 1s orbital. The number and arrangement of these bonds influence the physical properties of the alkane such as melting and boiling points. Larger alkanes tend to have stronger carbon-hydrogen bonds due to increased van der Waals forces, resulting in higher boiling points.
Sigma bonds
Sigma bonds are a defining feature of alkanes and arise from the direct overlap of orbitals located along the axis connecting two atomic nuclei. Unlike other types of covalent bonds, sigma bonds allow for the rotation of atoms around the bond axis. This unique property leads to the unusual flexibility seen in alkane structures. The stability and rotational capacity of sigma bonds make them essential for understanding how alkanes behave under various conditions. Their robust nature also denotes why alkanes are less reactive compared to other hydrocarbons.
Tetrahedral structure
The tetrahedral structure is a fundamental aspect of alkane geometry. Every carbon atom within an alkane is \(sp^3\) hybridized, allowing it to form four sigma bonds that are arranged in a tetrahedral shape. The bond angles here are approximately 109.5 degrees, which helps minimize repulsion between electron pairs. This regular tetrahedral arrangement accounts for the uniformity in alkane structures. It also explains why alkanes demonstrate consistent angles and lengths in the carbon chains, contributing to their straight-forward chemical properties.

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Most popular questions from this chapter

Infer how the boiling and freezing points of alkynes compare with those of alkanes with the same number of carbon atoms. Explain your reasoning, then research data to see it if supports your idea.

Explain why numbers are needed in the IUPAC names of many unbranched alkenes and alkynes but not in the names of unbranched alkanes

Challenge Draw the structure of 1,4-dimethylbenzene.

Molecules are modeled using molecular formulas, structural formulas, ball-and- stick models, and space-filling models. What are the advantages and disadvantages of each model?

Describe the difference between cis- and trans- isomers in terms of geometrical arrangement.
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