bond order

Examples of bond order in the following topics:

• Bond Order

  • Bond order is the number of chemical bonds between a pair of atoms.
  • Bond order is the number of chemical bonds between a pair of atoms; in diatomic nitrogen (N≡N) for example, the bond order is 3, while in acetylene (H−C≡C−H), the bond order between the two carbon atoms is 3 and the C−H bond order is 1.
  • Bond order indicates the stability of a bond.
  • Bond order is also an index of bond strength, and it is used extensively in valence bond theory.
  • For a bond to be stable, the bond order must be a positive value.

• Bonding in Coordination Compounds: Valence Bond Theory

  • 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.

• Government Bonds

  • A government bond is a bond issued by a national government denominated in the country's domestic currency.
  • However, central banks may buy government bonds in order to finance government spending, thereby monetizing the debt .
  • Bonds issued by national governments in foreign currencies are normally referred to as sovereign bonds.
  • At the secondary market, each bond will be assigned with very own bond code (ISIN code).
  • Government bonds are usually referred to as risk-free bonds because the government can raise taxes or create additional currency in order to redeem the bond at maturity.

• Explanation of Valence Bond Theory

  • Valence bond theory states that overlap between two atomic orbitals forms a covalent bond between two atoms.
  • In chemistry, valence bond (VB) theory is one of two basic theories—along with molecular orbital (MO) theory—that use quantum mechanics to explain chemical bonding.
  • Both types of overlapping orbitals can be related to bond order.
  • Single bonds have one sigma bond.
  • Double bonds consist of one $\sigma$ and one $\pi$ bond, while triple bonds contain one $\sigma$ and two $\pi$ bonds.

• Corporate Bonds

  • A corporate bond is issued by a corporation seeking to raise money in order to expand its business.
  • A corporate bond is issued by a corporation seeking to raise money in order to expand the business.
  • Strictly speaking, however, the term only applies to bonds issued by corporations .
  • Corporate bonds are often listed on major exchanges (and known as listed bonds) and ECNs, and the coupon (i.e., the interest payment) is usually taxable.
  • A corporate bond is issued by a corporation seeking to raise money in order to expand its business.

• Bond Energy

  • Bond energy is the measure of bond strength.
  • In order to turn one mole of a molecule into its constituent atoms, an amount of heat equal to the bond energy needs to be put into the system.
  • The bond energy is the average of the bond dissociation energies in a molecule.
  • At internuclear distances in the order of an atomic diameter, attractive forces dominate.
  • Identify the relationship between bond energy and strength of chemical bonds

• Covalent Bonds

  • Covalent bonding requires a specific orientation between atoms in order to achieve the overlap between bonding orbitals.
  • Covalent bonding interactions include sigma-bonding (σ) and pi-bonding (π).
  • 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.

• Single Covalent Bonds

  • Single covalent bonds are sigma bonds, which occur when one pair of electrons is shared between atoms.
  • The strongest type of covalent bonds are sigma bonds, which are formed by the direct overlap of orbitals from each of the two bonded atoms.
  • A single covalent bond can be represented by a single line between the two atoms.
  • The shapes of the first five atomic orbitals are shown in order: 1s, 2s, and the three 2p orbitals.
  • Notice that the area of overlap always occurs between the nuclei of the two bonded atoms.

• Peptide Bonding between Amino Acids

  • The peptide bond is an amide bond which links amino acids together to form proteins.
  • Higher-ordered structures such as peptide chains and proteins are formed when amino acids bond to each other.
  • The bond that holds together the two amino acids is a peptide bond, or a covalent chemical bond between two compounds (in this case, two amino acids).
  • The amide bond can only be broken by amide hydrolysis, where the bonds are cleaved with the addition of a water molecule.
  • Peptide bonds are amide bonds, characterized by the presence of a carbonyl group attached to an amine.

• Covalent Bonds and Other Bonds and Interactions

  • These bonds are stronger and much more common than are ionic bonds in the molecules of living organisms.
  • Thus, triple bonds are the strongest.
  • 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.
  • Not all bonds are ionic or covalent; weaker bonds can also form between molecules.
  • Two types of weak bonds that frequently occur are hydrogen bonds and van der Waals interactions.