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Chapter 9: Problem 30

Distinguish among single, double, and triple bonds in a molecule, and give an example of each.

Short Answer

Expert verified
Single bonds share one electron pair (e.g., H鈧�), double bonds share two (e.g., C鈧侶鈧�), and triple bonds share three (e.g., N鈧�).

Step by step solution

01

Understanding Single Bonds

A single bond in a molecule is a covalent bond where one electron pair is shared between atoms. It is the weakest and longest type of covalent bond. A common example of a molecule with a single bond is hydrogen gas (H鈧�), where two hydrogen atoms are connected by a single bond.
02

Exploring Double Bonds

A double bond involves the sharing of two pairs of electrons between two atoms, making it stronger and shorter than a single bond. A classic example of a molecule with a double bond is ethylene (C鈧侶鈧�), where the two carbon atoms are connected by a double bond.
03

Examining Triple Bonds

A triple bond is a covalent bond where three pairs of electrons are shared between two atoms. This bond is the strongest and shortest among covalent bonds. An example of a molecule with a triple bond is nitrogen gas (N鈧�), which consists of two nitrogen atoms connected by a triple bond.

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Key Concepts

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

Single Bond
A single bond is the most basic form of covalent bond. It occurs when two atoms share one pair of electrons to form a stable molecule. This type of bond is characterized by being the longest in distance between the bonded atoms and also the weakest in strength among covalent bonds.
However, single bonds play a crucial role in the stability of many molecules.
  • Single bonds allow for free rotation around the bond axis which can affect a molecule's physical and chemical properties.
  • A classic example of a single bond is hydrogen gas, H鈧�, where two hydrogen atoms share a single pair of electrons.
In summary, single bonds are fundamental in forming molecules and are synonymous with the simplicity and versatility of organic compounds.
Double Bond
Double bonds occur when two pairs of electrons are shared between two atoms. This type of bond is shorter and stronger than a single bond.
Due to its additional strength, double bonds play a vital role in molecular chemistry by influencing the molecule's reactivity and rigidity.
  • Carbon dioxide, CO鈧�, and ethylene, C鈧侶鈧�, are examples of molecules that contain double bonds. In ethylene, the double bond between carbon atoms leads to a planar configuration that prevents rotation, giving it distinct features.
Thus, double bonds contribute significantly to the chemical behavior and structural features of compounds, often impacting how they interact with other chemicals.
Triple Bond
Triple bonds are the most robust and shortest of the covalent bonds, formed by the sharing of three pairs of electrons between two atoms. This makes triple bonds very strong, as they require more energy to break.
With this bond type, the bond length is reduced, significantly affecting the geometry and function of the molecules they form.
  • Nitrogen gas, N鈧�, is a well-known molecule with a triple bond, exemplifying the strength and stability that comes with this bonding.
  • Due to these properties, molecules with triple bonds are less reactive than those with single or double bonds, making them stable and often inert under normal conditions.
Triple bonds are essential in various applications, showcasing the diversity and complexity of chemical bonding.

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Most popular questions from this chapter

Describe some characteristics of an ionic compound such as KF that would distinguish it from a covalent compound such as \(\mathrm{CO}_{2}\).

What is the difference between a Lewis dot symbol and a Lewis structure?

Give the empirical formulas and names of the compounds formed from the following pairs of ions: (a) \(\mathrm{Rb}^{+}\) and \(\mathrm{I}^{-},\) (b) \(\mathrm{Cs}^{+}\) and \(\mathrm{SO}_{4}^{2-},\) (c) \(\mathrm{Sr}^{2+}\) and \(\mathrm{N}^{3-}\), (d) \(\mathrm{Al}^{3+}\) and \(\mathrm{S}^{2-}\).

Write three resonance structures for hydrazoic acid, \(\mathrm{HN}_{3}\). The atomic arrangement is HNNN. Show formal charges.

Write Lewis structures for \(\mathrm{SeF}_{4}\) and \(\mathrm{SeF}_{6}\). Is the octet rule satisfied for Se?
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