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.

• Introduction to Bonding

  • Chemical bonds are the connections between atoms in a molecule.
  • These bonds include both strong intramolecular interactions, such as covalent and ionic bonds.
  • Hydrogen and carbon are not bonded, while in water there is a single bond between each hydrogen and oxygen.
  • Bonds, especially covalent bonds, are often represented as lines between bonded atoms.
  • Acetylene has a triple bond, a special type of covalent bond that will be discussed later.

• sp3 Hybridization

  • sp3 hybrid orbitals form when a single s and three p orbitals hybridize.
  • In a tetravalent molecule, four outer atoms are bonded to a central atom.
  • Perhaps the most common and important example of this bond type is methane, CH4.
  • To form four bonds, the atom must have four unpaired electrons; this requires that carbon's valence 2s and 2p orbitals each contain an electron for bonding.
  • The single 2s orbital is spherical, different from the dumbbell-shaped 2p orbitals.

• 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.

• 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?