Download An ionic bond is a type of chemical bond that involves a metal and a

An ionic bond is a type of chemical bond that involves a metal and a nonmetal ion
(or polyatomic ions such as ammonium) through electrostatic attraction. In short,
it is a bond formed by the attraction between two oppositely charged ions.
The metal donates one or more electrons, forming a positively charged ion or
cation with a stable electron configuration. These electrons then enter the non
metal, causing it to form a negatively charged ion or anion which also has a stable
electron configuration. The electrostatic attraction between the oppositely
charged ions causes them to come together and form a bond.
For example, in sodium chloride when sodium (Na) and chlorine (Cl) are
combined, the sodium atoms each lose an electron, forming a cation (Na+), and
the chlorine atoms each gain an electron to form an anion (Cl−). These ions are
then attracted to each other in a 1:1 ratio to form sodium chloride.
Pure ionic bonding is not known to exist. All ionic compounds have a degree of
covalent bonding. The larger the difference in electronegativity between two
atoms, the more ionic the bond. Ionic compounds conduct electricity when molten
or in solution. They generally have a high melting point and tend to be soluble in
water.
In an ionic bond, the atoms are bound by attraction of opposite ions, whereas, in a
covalent bond, atoms are bound by sharing electrons.
In reality, purely ionic bonds do not (and cannot) exist, as this would require an
infinitely large electronegativity difference, and complete charge transfer is
unfavorable from the viewpoint of raising the electronic kinetic energy. All ionic
bonds have some covalent character. For example, Na–Cl and Mg–O bonds have a
few percent covalency, while Si–O bonds are usually ~50% ionic and ~50%
covalent. Predominantly covalent bonds with partial ionic character are called
polar covalent.
Ions in crystal lattices of purely ionic compounds are spherical; however, if the
positive ion is small and/or highly charged, it will distort the electron cloud of the
negative ion. This polarization of the negative ion leads to a build-up of extra
charge density between the two nuclei, i.e., to partial covalency. Larger negative
ions are more easily polarized, but the effect is usually only important when
positive ions with charges of 3+ (e.g., Al3+) are involved. However, 2+ ions (Be2+) or
even 1+ (Li+) show some polarizing power because their sizes are so small.
Ionic Bonds
Mainly occur through attractions between opposite charges. For example,
between protonated amino (on salbutamol or quaternary ammonium (eg
acetylcholine), and the dissociated carboxylic acid group. Similarly, the
dissociated carboxylic acid group on the drug can bind with amino groups on the
receptor.
This type of bonds are very strong, and varies with
distances.
so it could act over large
Cation-π interactions can also be classified as ionic bonding. This occurs when a
cation, eg acetylcholine, interacts with the negative π bonds on an aromatic
group of the receptor.
Ion-dipole and dipole-dipole bonds have similar interactions, but are more
complicated and are weaker than ionic bonds.