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  2. Chemical polarity - Wikipedia

    en.wikipedia.org/wiki/Chemical_polarity

    As a quantum-mechanical description, Pauling proposed that the wave function for a polar molecule AB is a linear combination of wave functions for covalent and ionic molecules: ψ = aψ(A:B) + bψ(A + B −). The amount of covalent and ionic character depends on the values of the squared coefficients a 2 and b 2. [4]

  3. Fajans' rules - Wikipedia

    en.wikipedia.org/wiki/Fajans'_rules

    Thus sodium chloride (with a low positive charge (+1), a fairly large cation (~1 Å) and relatively small anion (0.2 Å) is ionic; but aluminium iodide (AlI 3) (with a high positive charge (+3) and a large anion) is covalent. Polarization will be increased by: high charge and small size of the cation Ionic potential Å Z+/r+ (= polarizing power)

  4. Covalent bond - Wikipedia

    en.wikipedia.org/wiki/Covalent_bond

    Covalent bonds are also affected by the electronegativity of the connected atoms which determines the chemical polarity of the bond. Two atoms with equal electronegativity will make nonpolar covalent bonds such as H–H. An unequal relationship creates a polar covalent bond such as with H−Cl.

  5. Chemical bond - Wikipedia

    en.wikipedia.org/wiki/Chemical_bond

    Molecules that are formed primarily from non-polar covalent bonds are often immiscible in water or other polar solvents, but much more soluble in non-polar solvents such as hexane. A polar covalent bond is a covalent bond with a significant ionic character. This means that the two shared electrons are closer to one of the atoms than the other ...

  6. Ionic bonding - Wikipedia

    en.wikipedia.org/wiki/Ionic_bonding

    Thus, bonding is considered ionic where the ionic character is greater than the covalent character. The larger the difference in electronegativity between the two types of atoms involved in the bonding, the more ionic (polar) it is. Bonds with partially ionic and partially covalent character are called polar covalent bonds. For example, Na–Cl ...

  7. Bonding in solids - Wikipedia

    en.wikipedia.org/wiki/Bonding_in_solids

    As noted above, covalent and ionic bonds form a continuum between shared and transferred electrons; covalent and weak bonds form a continuum between shared and unshared electrons. In addition, molecules can be polar, or have polar groups, and the resulting regions of positive and negative charge can interact to produce electrostatic bonding ...

  8. Non-covalent interaction - Wikipedia

    en.wikipedia.org/wiki/Non-covalent_interaction

    The hydrophobic effect is the desire for non-polar molecules to aggregate in aqueous solutions in order to separate from water. [22] This phenomenon leads to minimum exposed surface area of non-polar molecules to the polar water molecules (typically spherical droplets), and is commonly used in biochemistry to study protein folding and other ...

  9. Intramolecular force - Wikipedia

    en.wikipedia.org/wiki/Intramolecular_force

    Covalent bonds are generally formed between two nonmetals. There are several types of covalent bonds: in polar covalent bonds, electrons are more likely to be found around one of the two atoms, whereas in nonpolar covalent bonds, electrons are evenly shared. Homonuclear diatomic molecules are purely covalent.