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Chapter 7: Problem 53

Indicate whether or not molecules of the following species have a triple bond. (a) \(\mathrm{CH}_{2} \mathrm{CHCN}\) (b) \(\mathrm{HOOCCOOH}\) (c) \(\mathrm{C}_{2}^{2-}\) (d) \(\mathrm{CH}_{3} \mathrm{CHCH}_{2}\)

Short Answer

Expert verified
(a) Yes, (b) No, (c) Yes, (d) No.

Step by step solution

01

Understand Chemical Bonds

A triple bond is a covalent bond where three pairs of electrons are shared between atoms. Represented as three lines, like C鈮 in a Lewis structure, it is common in alkynes.
02

Analyze CH2CHCN

In the molecule CH2CHCN, examine the CN (cyano group) portion. Carbon and nitrogen form a triple bond in this section, represented as C鈮.
03

Analyze HOOCCOOH

The molecule HOOCCOOH (oxalic acid) consists of carbon-oxygen bonds. Oxalic acid does not contain any triple bonds because both carbon-oxygen are single or double bonds, not triples.
04

Analyze C2^(2-)

For the C2^(2-) ion, analyze the bond order. In diatomic carbon ions, triple bonds can form. The bond order calculations indicate a possible triple bond due to the presence of extra electrons.
05

Analyze CH3CHCH2

For the molecule CH3CHCH2 (propene), the structure contains a carbon-carbon double bond and no triples bonds. It is part of alkenes, which have double bonds.

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Key Concepts

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

Chemical Bond Types
Chemical bonds are the attractive forces that hold atoms together in a molecule. There are primarily three types of chemical bonds:
  • Covalent Bonds: These bonds form when atoms share electrons. This sharing can be equal, known as nonpolar covalent bonds, or unequal, known as polar covalent bonds.
  • Metallic Bonds: These are formed between metal atoms where electrons are not shared between the atoms but exist as a sea of electrons.
  • Ionic Bonds: Involves the transfer of electrons from one atom to another, typically from a metal to a non-metal.
A triple bond is a type of covalent bond, where three pairs of electrons are shared between two atoms. This results in a strong and short bond. Such bonds are often represented in chemical structures by three parallel lines, for example, C鈮.
Molecular Structure Analysis
Analyzing molecular structures is crucial for understanding the properties and behaviors of molecules. This involves determining the arrangement of atoms within a molecule and the types of bonds that hold them together. Molecules can be analyzed by examining their:
  • Lewis Structures: Illustrates the arrangement of valence electrons around atoms.
  • Bond Angles and Lengths: These measurements affect the shape and polarity of the molecule.
Understanding molecular structure helps in predicting the reactivity, stability, and physical properties of a molecule. For instance, knowing that a molecule like CH鈧僀HCH鈧� contains a double bond helps predict its participation in chemical reactions, unlike a molecule with a triple bond like C鈮 in CH鈧侰HCN, which might behave differently.
Lewis Structures
Lewis structures are diagrams that show the bonds between atoms in a molecule and the lone pairs of electrons that may exist. These structures help visualize the valence electrons involved in bond formation. Key points about Lewis structures include:
  • Bond Representation: Covalent bonds are represented as lines connecting atoms. Single bond as one line, double bond as two, and triple bond as three lines.
  • Electron Pairs: Lone pairs are shown as two dots beside an atom.
  • Formal Charges: Calculated to understand the distribution of electrons among the bonded atoms.
Using Lewis structures, one can deduce that in a molecule like C鈧偮测伝, the triple bond can be depicted as C鈮, signifying a sharing of six valence electrons between the two carbon atoms.
Covalent Bonding
Covalent bonding occurs when two atoms share electrons to attain stability, similar to noble gases. This bond type is prevalent in the formation of organic and many inorganic compounds. Two main features of covalent bonds are:
  • Bond Strength and Length: Triple bonds are stronger and shorter than double and single bonds due to the increased electron sharing.
  • Molecular Stability: Molecules with covalent bonds, particularly multiple bonds, tend to be more stable and less reactive due to the strong electron sharing.
In molecules, like CH鈧侰HCN, the presence of a C鈮 triple bond indicates a high degree of stability and strength of the bond, influencing the molecule's overall chemical reactivity and physical properties.

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Most popular questions from this chapter

The halogens form a number of interhalogen compounds. For example, chlorine pentafluoride, \(\mathrm{ClF}_{5}(g)\), can be prepared according to the following chemical equation: $$ \mathrm{KCl}(s)+3 \mathrm{~F}_{2}(g) \rightarrow \mathrm{ClF}_{5}(g)+\mathrm{KF}(s) $$ The halogen fluorides are very reactive, combining explosively with water, for example. Write the Lewis formula for each of the following halogen fluoride species: (a) \(\mathrm{ClF}_{5}\) (b) \(\mathrm{IF}_{3}\) (c) \(\mathrm{IF}_{7}\) (d) \(\mathrm{IF}_{4}^{+}\)

Use Lewis formulas and formal charge considerations to suggest that the structure of a hydrocyanic acid molecule is HCN rather than HNC.

A solution of sugar in water is a poor conductor of electricity, whereas a solution of table salt in water is a good conductor of electricity. What does this tell you about the bonding in the two substances?

Write the Lewis formula for each of the following nitrogen oxide molecules. Indicate formal charge and resonance forms. $$ \begin{array}{lll} \text { Formula } & \text { Name } & \text { Form at } 25^{\circ} \mathbf{C}, 1 \text { atm } \\ \hline \mathrm{N}_{2} \mathrm{O} & \text { dinitrogen oxide } & \text { colorless gas } \\ \mathrm{NO} & \text { nitrogen oxide } & \text { colorless gas } \\ \mathrm{N}_{2} \mathrm{O}_{3} & \text { dinitrogen trioxide } & \text { dark blue gas } \\ \mathrm{NO}_{2} & \text { nitrogen dioxide } & \text { brown gas } \\ \mathrm{N}_{2} \mathrm{O}_{4} & \text { dinitrogen tetroxide } & \text { colorless gas } \\ \mathrm{N}_{2} \mathrm{O}_{5} & \text { dinitrogen pentoxide } & \text { white solid } \end{array} $$

Write Lewis formulas for the resonance forms of the formate ion, \(\mathrm{HCOO}^{-} .\) Indicate formal charges and discuss the bonding of this ion.
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