covalent

(adjective)

when 2 or more nonmetallic atoms are bound together by sharing electrons.

Related Terms

  • covalent character
  • polar covalent bond
  • molecule
  • molecular geometry
  • isomer
  • electronegativity
  • compound

Examples of covalent in the following topics:

  • Ionic vs Covalent Bond Character

    • There are multiple kinds of attractive forces, including covalent, ionic, and metallic bonds.
    • Bonds that fall in between the two extremes, having both ionic and covalent character, are classified as polar covalent bonds.
    • Though ionic and covalent character represent points along a continuum, these designations are frequently useful in understanding and comparing the macroscopic properties of ionic and covalent compounds.
    • This bond is considered to have characteristics of both covalent and ionic bonds.
    • Discuss the idea that, in nature, bonds exhibit characteristics of both ionic and covalent bonds
  • Physical Properties of Covalent Molecules

    • The covalent bonding model helps predict many of the physical properties of compounds.
    • First described by Gilbert Lewis, a covalent bond occurs when electrons of different atoms are shared between the two atoms.
    • Several physical properties of molecules/compounds are related to the presence of covalent bonds:
    • Covalent compounds do not conduct electricity; this is because covalent compounds do not have charged particles capable of transporting electrons.
    • However, the Lewis theory of covalent bonding does not account for some observations of compounds in nature.
  • Covalent Bonds

    • Covalently sharing two electrons is also known as a "single bond."
    • Covalently sharing two electrons is also known as a "single bond."
    • Covalent bonding interactions include sigma-bonding (σ) and pi-bonding (π).
    • In non-polar covalent bonds, the electrons are equally shared between the two atoms.
    • Covalent compounds, on the other hand, have lower melting and boiling points.
  • Types of Bonds

    • 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.
    • A covalent bond involves electrons being shared between atoms.
    • 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 rule of thumb is that covalent compounds are more difficult to change than ionic compounds.
  • Comparison between Covalent and Ionic Compounds

    • Here, we discuss two classes of compounds based on the bond type that holds the atoms together: ionic and covalent.
    • Covalent bonds are characterized by the sharing of electrons between two or more atoms.
    • Examples of compounds that contain only covalent bonds are methane (CH4), carbon monoxide (CO), and iodine monobromide (IBr).
    • Therefore, they have higher melting and boiling points compared to covalent compounds.
    • Identify element pairs which are likely to form ionic or covalent bonds
  • Single Covalent Bonds

    • Single covalent bonds are sigma bonds, which occur when one pair of electrons is shared between atoms.
    • Covalent bonding occurs when two atomic orbitals come together in close proximity and their electron densities overlap.
    • 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.
  • Covalent Crystals

    • Atoms in covalent solids are covalently bonded with their neighbors, creating, in effect, one giant molecule.
    • A covalent bond is a chemical bond that involves the sharing of pairs of electrons between atoms.
    • Covalent solids are a class of extended-lattice compounds in which each atom is covalently bonded to its nearest neighbors.
    • They cannot be broken or abraded without breaking a large number of covalent chemical bonds.
    • It is also quite hard because of the strong covalent bonding throughout the lattice.
  • Introduction to Bonding

    • These bonds include both strong intramolecular interactions, such as covalent and ionic bonds.
    • When there is a greater electronegativity difference than between covalently bonded atoms, the pair of atoms usually forms a polar covalent bond.
    • Again, polar covalent bonds tend to occur between non-metals.
    • 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.
  • Bond Polarity

    • The terms "polar" and "nonpolar" usually refer to covalent bonds.
    • To determine the polarity of a covalent bond using numerical means, find the difference between the electronegativity of the atoms; if the result is between 0.4 and 1.7, then, generally, the bond is polar covalent.
    • The hydrogen fluoride (HF) molecule is polar by virtue of polar covalent bonds; in the covalent bond, electrons are displaced toward the more electronegative fluorine atom.
  • Introduction to Lewis Structures for Covalent Molecules

    • In covalent molecules, atoms share pairs of electrons in order to achieve a full valence level.
    • Each pair of shared electrons is a covalent bond which can be represented by a dash.
    • Since four electrons are involved in each bond, a double covalent bond is formed.
    • This is known as a 'single covalent bond.'
    • Predict and draw the Lewis structure of simple covalent molecules and compounds
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