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Chapter 2: Problem 54

In 4 -(1-methylethyl)heptane, any \(\mathrm{H}-\mathrm{C}-\mathrm{C}\) angle has the value (a) \(120^{\circ}\) (b) \(109.5^{\circ}\) (c) \(180^{\circ}\) (d) \(90^{\circ}\) (e) \(360^{\circ}\)

Short Answer

Expert verified
b) 109.5掳

Step by step solution

01

- Identify the Structure

First, identify the structure of 4-(1-methylethyl)heptane. This is a heptane backbone (7 carbon atoms in a straight chain) with a 1-methylethyl group attached to the fourth carbon.
02

- Determine the Hybridization

Understand the hybridization of carbon atoms in the structure. Heptane has only single bonds (sigma bonds), meaning the carbons are sp3 hybridized.
03

- Recall the Bond Angle for sp3 Hybridization

For sp3 hybridized carbons, which form tetrahedral geometry, the bond angles are approximately 109.5掳.
04

- Choose the Correct Answer

Based on the hybridization and bond angles, select the option that matches the bond angle for sp3 hybridized carbons.

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Key Concepts

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

sp3 Hybridization
When it comes to understanding the structure of organic molecules, one key concept is hybridization. Specifically, for carbon atoms forming four single bonds, the type of hybridization involved is called sp3 hybridization.
In sp3 hybridization, one s orbital mixes with three p orbitals to form four equivalent sp3 hybrid orbitals. These orbitals are arranged in a way to minimize repulsion between electron pairs.
This is crucial in helping to determine the geometry and bond angles in an organic molecule.

Key points to remember include:
  • The hybrid orbitals have 25% s character and 75% p character.
  • Each sp3 hybrid orbital forms a sigma bond with another atom, such as hydrogen or carbon.
Tetrahedral Geometry
Following sp3 hybridization, the resulting geometry of the molecule is tetrahedral. This arrangement ensures that the sp3 hybrid orbitals are as far apart from each other as possible, minimizing repulsion.
In a tetrahedral geometry, each of the four bonds around the carbon atom is directed towards the corners of an imaginary tetrahedron.

Important aspects of tetrahedral geometry include:
  • The bond angles are approximately 109.5掳.
  • This geometry is common in organic compounds that feature single bonds, like alkanes.

Remember, recognizing tetrahedral geometry helps in envisioning how atoms are spatially arranged around a central atom, providing deeper insights into molecular shapes and bond angles.
Single Bonds in Hydrocarbons
Single bonds in hydrocarbons, also known as sigma bonds, are the simplest type of covalent bond. These bonds are observed in alkanes, which are saturated hydrocarbons composed only of sp3 hybridized carbon atoms.
The sigma bond is formed by the direct overlap of sp3 hybrid orbitals from adjacent carbon atoms or between carbon and hydrogen atoms.

Key features of single bonds in hydrocarbons:
  • They allow free rotation around the bond axis, giving the molecule flexibility.
  • Bond strength and length are crucial characteristics. Single bonds are the longest and weakest compared to double and triple bonds.

    • Understanding single bonds provides a foundation for grasping how larger and more complex organic molecules build upon simple structures.
    Organic Molecule Structure
    The structure of organic molecules is a fundamental concept that connects the aforementioned ideas. Organic molecules are primarily built from carbon atoms, often forming backbone structures and functional groups.
    The structure of an organic molecule determines its physical and chemical properties.

    Considerations when studying organic molecule structures:
    • The carbon skeleton can vary: straight chains, branched chains, or rings.
    • Functional groups like -OH, -COOH, and -NH2 add to the diversity.

    In the specific case of 4-(1-methylethyl)heptane, it has a seven-carbon chain with a substituent on the fourth carbon. Understanding the structure helps in predicting reactivity and interactions.

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    Most popular questions from this chapter

    (a) Draw the structures of the five isomeric hexanes. (b) Draw the structures of all the possible next higher and lower homologs of 2 -methylbutane.

    CHAllFNGE Using the Arrhenius equation, calculate the effect on \(k\) of increases in temperature of 10,30, and 50 degrees (Celsius) for the following activation energies. Use \(300 \mathrm{~K}\) (approximately room temperature) as your initial \(T\) value, and assume that \(A\) is a constant. (c) \(E_{a}=45\) kcal mol \(^{-1}\). (a) \(E_{a}=15\) kcal \(\mathrm{mol}^{-1} ;\) (b) \(E_{a}=30\) kcal \(\mathrm{mol}^{-1}\);

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    Convert the following names into the corresponding molecular structures. After doing so, check to see if the name of each molecule as given here is in accord with the IUPAC system of nomenclature. If not, name the molecule correctly. (a) 2 -methyl-3-propylpentane; (b) \(5-(1,1\) -dimethylpropyl)nonane; (c) \(2,3,4\) -trimethyl-4-butylheptane; (d) 4-tert-butyl-5isopropylhexane; (e) 4 -(2-ethylbutyl)decane; (f) 2,4,4-trimethylpentane; \((\mathrm{g}) 4-\sec\) -butylheptane; (h) isoheptane; (i) neoheptane.

    Identify the primary, secondary, and tertiary carbon atoms and the hydrogen atoms in each of the following molecules: (a) ethane; (b) pentane; (c) 2-methylbutane; (d) 3 -ethyl- \(2,2,3,4\) tetramethylpentane.
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