covalent bond

Examples of covalent bond in the following topics:

• Covalent Bonds and Other Bonds and Interactions

  • Covalent bonds are also found in inorganic molecules such as H2O, CO2, and O2.
  • The more covalent bonds between two atoms, the stronger their connection.
  • The formation of water molecules is an example of covalent bonding.
  • There are two types of covalent bonds: polar and nonpolar.
  • Not all bonds are ionic or covalent; weaker bonds can also form between molecules.

• Dehydration Synthesis

  • In dehydration synthesis, monomers combine with each other via covalent bonds to form polymers.
  • The monomers combine with each other via covalent bonds to form larger molecules known as polymers.
  • The removal of a hydrogen from one monomer and the removal of a hydroxyl group from the other monomer allows the monomers to share electrons and form a covalent bond.
  • However, the manner by which glucose monomers join together, specifically locations of the covalent bonds between connected monomers and the orientation (stereochemistry) of the covalent bonds, results in these three different polysaccharides with varying properties and functions.
  • In the dehydration synthesis reaction between two molecules of glucose, a hydroxyl group from the first glucose is combined with a hydrogen from the second glucose, creating a covalent bond that links the two monomeric sugars (monosaccharides) together to form the dissacharide maltose.

• Hydrogen Bonding and Van der Waals Forces

  • Ionic and covalent bonds between elements require energy to break.
  • Ionic bonds are not as strong as covalent, which determines their behavior in biological systems.
  • However, not all bonds are ionic or covalent bonds.
  • When polar covalent bonds containing hydrogen form, the hydrogen in that bond has a slightly positive charge because hydrogen’s one electron is pulled more strongly toward the other element and away from the hydrogen.
  • These bonds—along with ionic, covalent, and hydrogen bonds—contribute to the three-dimensional structure of proteins that is necessary for their proper function.

• Organic Isomers

  • Structural isomers (such as butane and isobutane ) differ in the placement of their covalent bonds.
  • Geometric isomers, on the other hand, have similar placements of their covalent bonds but differ in how these bonds are made to the surrounding atoms, especially in carbon-to-carbon double bonds.
  • In the simple molecule butene (C4H8), the two methyl groups (CH3) can be on either side of the double covalent bond central to the molecule.
  • When the carbons are bound on the same side of the double bond, this is the cis configuration; if they are on opposite sides of the double bond, it is a trans configuration.
  • (a) Structural isomers have a different covalent arrangement of atoms.

• The Chemical Basis for Life

  • Carbon is the most important element to living things because it can form many different kinds of bonds and form essential compounds.
  • The carbon atom has unique properties that allow it to form covalent bonds to as many as four different atoms, making this versatile element ideal to serve as the basic structural component, or "backbone," of the macromolecules.
  • Therefore, carbon atoms can form up to four covalent bonds with other atoms to satisfy the octet rule.
  • Each of its four hydrogen atoms forms a single covalent bond with the carbon atom by sharing a pair of electrons.

• Hydrolysis

  • In dehydration synthesis reactions, a water molecule is formed as a result of generating a covalent bond between two monomeric components in a larger polymer.
  • In hydrolysis reactions, a water molecule is consumed as a result of breaking the covalent bond holding together two components of a polymer.
  • Dehydration and hydrolysis reactions are chemical reactions that are catalyzed, or "sped up," by specific enzymes; dehydration reactions involve the formation of new bonds, requiring energy, while hydrolysis reactions break bonds and release energy.
  • One glucose gets a hydroxyl group at the site of the former covalent bond, the other glucose gets a hydrogen atom.

• The Purpose and Process of Photosynthesis

  • During photosynthesis, molecules in leaves capture sunlight and energize electrons, which are then stored in the covalent bonds of carbohydrate molecules.
  • That energy within those covalent bonds will be released when they are broken during cell respiration.
  • How long lasting and stable are those covalent bonds?
  • Photosynthesis is vital because it evolved as a way to store the energy in solar radiation (the "photo-" part) as high-energy electrons in the carbon-carbon bonds of carbohydrate molecules (the "-synthesis" part).

• Hydrocarbons

  • The many covalent bonds between the atoms in hydrocarbons store a great amount of energy, which is released when these molecules are burned (oxidized).
  • Furthermore, individual carbon-to-carbon bonds may be single, double, or triple covalent bonds; each type of bond affects the geometry of the molecule in a specific way.
  • The overall geometry of the molecule is altered by the different geometries of single, double, and triple covalent bonds .
  • Double and triple bonds change the geometry of the molecule: single bonds allow rotation along the axis of the bond, whereas double bonds lead to a planar configuration and triple bonds to a linear one.
  • Single bonds, like those found in ethane, are able to rotate.

• Peptide Bonding between Amino Acids

  • The peptide bond is an amide bond which links amino acids together to form proteins.
  • 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.
  • The peptide bond (circled) links two amino acids together.
  • Peptide bonds are amide bonds, characterized by the presence of a carbonyl group attached to an amine.

• Chemical Reactions and Molecules

  • Chemical reactions occur when two or more atoms bond together to form molecules or when bonded atoms are broken apart.
  • Chemical reactions occur when two or more atoms bond together to form molecules or when bonded atoms are broken apart.
  • Two or more atoms may bond with each other to form a molecule.
  • When two hydrogens and an oxygen share electrons via covalent bonds, a water molecule is formed.
  • Explore reactions in which chemical bonds are formed and broken with this model.