Chemical bonding: what is it?
The process by which two or more atoms, molecules, or ions form a chemical bond to produce a chemical compound is known as chemical bonding. The resulting compound's atoms are held together by these chemical bonds.
The attracting force that holds the various constituents
(atoms, ions, and so forth) Chemical bonding involves bringing them together
and stabilizing them through an overall loss of energy. As a result, it is
clear that the strength of the chemical bonds that connect a chemical
compound's constituents is important; The resulting compound would be more
stable the stronger the bonds between the constituents.
Important Theories on Chemical Bonding In 1916, Albrecht
Kössel and Gilbert Lewis were the first to successfully explain how chemical
bonds form. The inertness of noble gases served as the basis for their
explanation of chemical bonding.
Lewis's Theory of Chemical Bonding • An atom can be thought
of as the outer shell and a positively charged "Kernel," which consists
of the nucleus and its inner electrons.
• There are a maximum of eight electrons that can fit inside
the outer shell.
• The "Kernel" is surrounded by a cube containing
the eight electrons that make up the outer shell.
• As a result, the atoms with an octet configuration, which
have eight electrons in their outermost shell, represent a stable
configuration.
• By forming chemical bonds with other atoms, atoms can
achieve this stable configuration. This chemical bond can be formed by either
gaining or losing an electron (NaCl, MgCl2) or by sharing an electron in some
cases (F2).
• Chemical bonds are only formed by the electrons in the
outer shell, also known as the valence electrons. These valence electrons were
represented by specific notations that Gilbert Lewis referred to as Lewis
symbols.
• In most cases, an element's valency is equal to 8 minus
the number of dots (or valence electrons) in the corresponding Lewis symbol.
The highly electropositive alkali metals and the highly
electronegative halogens are separated by noble gases according to Kossel's
theory of chemical bonding.
• By gaining an electron, halogens can form negatively
charged ions. Alkali metals, on the other hand, can lose an electron to form
positively charged ions.
• The noble gas configuration of these negatively and
positively charged ions has eight electrons in the outermost shell. ns2np6 is
the general electronic configuration of noble gases, except helium.
• As not at
all like charges draw in one another these dissimilar-to-charged particles are
kept intact by a solid power of electrostatic fascination existing between
them. Electrostatic attraction holds the magnesium ion and chlorine ions
together in MgCl2, for instance. An electrovalent bond is a type of chemical
bond between two negatively charged particles.
Also read: Paleobotany
Clarification of Kossel Lewis Approach
In 1916 Kossel and Lewis prevailed with regards to giving an
effective clarification given the idea of an electronic setup of honorable
gases about why iotas consolidate to shape particles. The atoms of noble gases
have very little if any, tendency to combine with those of other elements or
with one another. This indicates that the electronic configurations of these
atoms must be stable.
Because of the steady setup, the honorable gas iotas neither
tend to acquire nor lose electrons, thusly, their joining limit or valency is
zero. Because they are so inert, they even do not form diatomic molecules and
only exist as gaseous atoms of one type.
Types of Chemical Bonds The stability of a compound can be
determined by the type of chemical bonds it contains when substances
participate in chemical bonding and produce compounds.
The properties and strength of the chemical bonds that are created vary. When molecules or atoms join together to form compounds, there are four primary types of chemical bonds.
The following are examples of chemical bonds:
• Ionic Bonds
• Covalent Bonds
• Hydrogen Bonds
• Polar Bonds
In chemical bonding, these bonds are made when two atoms or molecules
lose, gain, or share electrons.
1. Ionic Bonding is a type of chemical bonding
that occurs when electrons are transferred between two molecules or atoms. An
electron is lost by an atom here, which is then gained by another atom. At the
point when such an electron move happens, one of the molecules fosters a
negative charge and is presently called the anion.
2. Covalent Bonding The sharing of electrons between atoms is
referred to as a covalent bond. This kind of chemical bonding is typically seen
in organic compounds, or compounds that contain carbon. The formation of a
molecule is accomplished by extending the pair of electrons that are shared by
the two atoms around the atoms' nuclei.
3. Polar and Non-Polar Covalent Bonds can be
Polar or Non-Polar. Because the more electronegative atom pulls the electron
pair closer to itself and away from the less electronegative atom, Polar
Covalent chemical bonding results in an uneven distribution of electrons. One
example of such a polar molecule is water.
Hydrogen Bonding
Hydrogen bonding is a weaker type of
chemical bonding than ionic and covalent bonding. It is a kind of polar
covalent holding among oxygen and hydrogen wherein the hydrogen fosters an
incomplete positive charge. This suggests that the more electronegative oxygen
atom is brought closer to the electrons.
Because of this, the hydrogen tends to gravitate toward any
adjacent atom's negative charges. A hydrogen bond, which is a type of chemical
bonding, is to blame for many of water's properties.
Ionic Bond: What is It?
An electrovalent or ionic bond is a bond that results from
strong electrostatic forces of attraction between positively and negatively
charged species.