Examples of triple bond in the following topics:
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- Alkenes and alkynes are named similarly to alkanes, based on the longest chain that contains the double or triple bond.
- Alkenes are hydrocarbons that contain one or more double bonds, while alkynes contain one or more triple bonds.
- The carbon backbone is numbered from the end that yields the lowest positioning for the double or triple bond.
- For multiple double or triple bonds, "di-," "tri-," or "tetra-" can be added prior to the "-ene" or "-yne."
- For compounds containing both double and triple bonds, the "-ene" suffix precedes the "-yne," and the compound is numbered to minimize the bond positions.
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- A triple bond involves the sharing of six electrons, with a sigma bond and two $\pi$ bonds.
- The simplest triple-bonded organic compound is acetylene, C2H2.
- Triple bonds are stronger than double bonds due to the the presence of two $\pi$ bonds rather than one.
- Similar to double bonds, no rotation around the triple bond axis is possible.
- Double bonds have shorter distances than single bonds, and triple bonds are shorter than double bonds.
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- sp2, sp hybridizations, and pi-bonding can be used to describe the chemical bonding in molecules with double and triple bonds.
- sp hybridization explains the chemical bonding in compounds with triple bonds, such as alkynes; in this model, the 2s orbital mixes with only one of the three p-orbitals, resulting in two sp orbitals and two remaining p-orbitals.
- In ethene, carbon sp2 hybridizes, because one π (pi) bond is required for the double bond between the carbons, and only three σ bonds form per carbon atom.
- The remaining, non-hybridized p-orbitals overlap for the double and triple pi bonds.
- Describe the role of hybridization in the formation of double and triple bonds.
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- Alkenes and alkynes are hydrocarbons which respectively have carbon-carbon double bond and carbon-carbon triple bond functional groups.
- The molecular formulas of these unsaturated hydrocarbons reflect the multiple bonding of the functional groups:
- This difference suggests such compounds may have a triple bond, two double bonds, a ring plus a double bond, or two rings.
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- Alkanes are relatively unreactive hydrocarbons that contain no double or triple bonds in their carbon skeletons.
- They contain no double or triple bonds in their carbon skeletons and, therefore, have the maximum number of carbon to hydrogen covalent bonds.
- This is in contrast to alkenes and alkynes, which contain double and triple bonds and are known as unsaturated hydrocarbons.
- Each carbon atom has four bonds (either C-H or C-C bonds), and each hydrogen atom is joined to a carbon atom (H-C bonds).
- Alkanes are generally less reactive than alkenes and alkynes because they lack the more reactive double and triple bonds.
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- Its biosynthesis involves breaking the triple bond of molecular nitrogen, or N2, followed by the formation of several carbon-nitrogen single and double bonds.
- One, two, or three pairs of electrons may be shared between two atoms, making single, double, and triple bonds, respectively.
- Thus, triple bonds are the strongest.
- Molecular nitrogen consists of two nitrogen atoms triple bonded to each other.
- The resulting strong triple bond makes it difficult for living systems to break apart this nitrogen in order to use it as constituents of biomolecules, such as proteins, DNA, and RNA.
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- Covalent bonding interactions include sigma-bonding (σ) and pi-bonding (π).
- Single bonds occur when two electrons are shared and are composed of one sigma bond between the two atoms.
- Double bonds occur when four electrons are shared between the two atoms and consist of one sigma bond and one pi bond.
- Triple bonds occur when six electrons are shared between the two atoms and consist of one sigma bond and two pi bonds (see later concept for more info about pi and sigma bonds).
- Unlike an ionic bond, a covalent bond is stronger between two atoms with similar electronegativity.
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- Since reactions of organic compounds involve the making and breaking of bonds, the strength of bonds, or their resistance to breaking, becomes an important consideration.
- Bond energy is the energy required to break a covalent bond homolytically (into neutral fragments).
- Bond energies are commonly given in units of kcal/mol or kJ/mol, and are generally called bond dissociation energies when given for specific bonds, or average bond energies when summarized for a given type of bond over many kinds of compounds.
- The following table is a collection of average bond energies for a variety of common bonds.
- First, a single bond between two given atoms is weaker than a double bond, which in turn is weaker than a triple bond.
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- The Lewis bonding theory can explain many properties of compounds.
- Lewis theory also accounts for bond length; the stronger the bond and the more electrons shared, the shorter the bond length is.
- According to the theory, triple bonds are stronger than double bonds, and double bonds are stronger than single bonds.
- However, the theory implies that the bond strength of double bonds is twice that of single bonds, which is not true.
- Discuss the qualitative predictions of covalent bond theory on the boiling and melting points, bond length and strength, and conductivity of molecules
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- Valence bond theory is used to explain covalent bond formation in many molecules.
- Valence bond theory is a synthesis of early understandings of how chemical bonds form.
- Lewis proposed that the basis of chemical bonding is in the ability of atoms to share two bonding electrons.
- Where bond order is concerned, single bonds are considered to be one sigma bond, double bonds are considered to contain one sigma and one pi bond, and triple bonds consist of one sigma bond and two pi bonds.
- Valence bond theory is used to explain covalent bond formation in many molecules, as it operates under the condition of maximum overlap, which leads to the formation of the strongest possible bonds.