single bond

Examples of single bond in the following topics:

• 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.
  • Single covalent bonds occur when one pair of electrons is shared between atoms as part of a molecule or compound.
  • A single covalent bond can be represented by a single line between the two atoms.
  • For instance, the diatomic hydrogen molecule, H2, can be written as H—H to indicate the single covalent bond between the two hydrogen atoms.

• Covalent Bonds

  • Covalently sharing two electrons is also known as a "single bond."
  • Carbon will have to form four single bonds with four different fluorine atoms to fill its octet.
  • Covalently sharing two electrons is also known as a "single bond."
  • Carbon will have to form four single bonds with four different fluorine atoms to fill its octet.
  • Single bonds occur when two electrons are shared and are composed of one sigma bond between the two atoms.

• Physical Properties of Covalent Molecules

  • 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

• Bond Energy

  • 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.
  • Third, with the exception of carbon and hydrogen, single bonds between atoms of the same element are relatively weak (35 to 64 kcal).

• Double and Triple Covalent Bonds

  • The double bond between the two carbon atoms consists of a sigma bond and a π bond.
  • The three sp2 orbitals lie in a single plane at 120-degree angles.
  • Experiments have shown that double bonds are stronger than single bonds, and triple bonds are stronger than double bonds.
  • Double bonds have shorter distances than single bonds, and triple bonds are shorter than double bonds.
  • Describe the types of orbital overlap that occur in single, double, and triple bonds

• 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.
  • Valence bond structures are similar to Lewis structures, except where a single Lewis structure is insufficient, several valence bond structures can be used.
  • 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.

• Types of Bonds

  • Ionic bonds can form between nonmetals and metals, while covalent bonds form when electrons are shared between two nonmetals.
  • Pure ionic bonding cannot exist: all ionic compounds have some degree of covalent bonding.
  • Bonds with partially ionic and partially covalent character are called polar covalent bonds.
  • This difference in charge is called a dipole, and when the covalent bond results in this difference in charge, the bond is called a polar covalent bond.
  • A given nonmetal atom can form a single, double, or triple bond with another nonmetal.

• Zero-Coupon Bonds

  • A zero-coupon bond (also called a "discount bond" or "deep discount bond") is a bond bought at a price lower than its face value, with the face value repaid at the time of maturity.
  • Treasury bills, U.S. savings bonds, and long-term zero-coupon bonds.
  • Each of these investments then pays a single lump sum.
  • The bonds can be held until maturity or sold on secondary bond markets.
  • The impact of interest rate fluctuations on strip bonds is higher than for a coupon bond.

• Redeeming at Maturity

  • The journal entry to record the retirement of a bond: Debit Bonds Payable & Credit Cash.
  • A maturity date is the date when the bond issuer must pay off the bond.
  • Bonds can be classified to coupon bonds and zero coupon bonds.
  • On the balance sheet, the Bonds Payable account can be shown as different issues or consolidated into a single balance.
  • If a single balance is shown, then a schedule or note should disclose the details of the bond issues.

• Hydrogen Bonding

  • A hydrogen bond is a type of dipole-dipole interaction; it is not a true chemical bond.
  • These attractions can occur between molecules (intermolecularly) or within different parts of a single molecule (intramolecularly).
  • This hydrogen atom is a hydrogen bond donor.
  • Greater electronegativity of the hydrogen bond acceptor will create a stronger hydrogen bond.
  • Where do hydrogen bonds form?