Chemical bonding can occur through either ionic bonds or covalent bonds. Ionic bonds result from the electrostatic attraction between oppositely charged ions, while covalent bonds form through the sharing of electrons between atoms. The strength of these bonds can vary considerably, from strong primary bonds to weaker secondary bonds.

1. Chemical
bonding

2. A chemical bond is a lasting attraction
between atoms, ions or molecules that enables the
formation of chemical compounds. The bond may
result from the electrostatic force of attraction
between oppositely charged ions as in ionic bonds
or through the sharing of electrons as in covalent
bonds. The strength of chemical bonds varies
considerably; there are "strong bonds" or "primary
bonds" such as covalent, ionic and metallic bonds,
and "weak bonds" or "secondary bonds" such
as dipole–dipole interactions, the London dispersion
force and hydrogen bonding.
INTRODUCTION

4. a valence electron is an outer
shell electron that is associated with
an atom, and that can participate in the
formation of a chemical bond if the outer
shell is not closed; in a single covalent
bond, both atoms in the bond contribute one
valence electron in order to form a shared
pair. The presence of valence electrons can
determine
the element's chemical properties, such as
its valence—whether it may bond with other
elements and, if so, how readily and with
how many. For a main group element, a
valence electron can exist only in the
outermost electron shell; in a transition
metal, a valence electron can also be in an
inner shell.

6. LEWIS STRUCTURE
Lewis structures, also known as Lewis dot
diagrams, Lewis dot formulas, Lewis dot
structures, electron dot structures, or Lewis
electron dot structures (LEDS), are diagrams that
show the bonding between atoms of a molecule and
the lone pairs of electrons that may exist in the
molecule.[1][2][3] A Lewis structure can be drawn for
any covalentlybonded molecule, as well as coordination
compounds. The Lewis structure was named
after Gilbert N. Lewis, who introduced it in his 1916
article The Atom and the Molecule.[4]Lewis structures
extend the concept of the electron dot diagram by
adding lines between atoms to represent shared
pairs in a chemical bond.

8. OCTET RULE
The octet rule is a chemical rule of
thumb that reflects observation
that atoms of main-group elements tend
to combine in such a way that each
atom has eight electrons in its valence
shell, giving it the same electron
configuration as a noble gas. The rule is
especially applicable
to carbon, nitrogen, oxygen, and
the halogens, but also to metals such
as sodium or magnesium.

9. The valence electrons can be counted using
a Lewis electron dot diagram as shown at the
right for carbon dioxide. The electrons shared by
the two atoms in a covalent bond are counted
twice, once for each atom. In carbon dioxide
each oxygen shares four electrons with the
central carbon, two (shown in red) from the
oxygen itself and two (shown in black) from the
carbon. All four of these electrons are counted in
both the carbon octet and the oxygen octet.

10. MODES OF CHEMICAL COMBINATION
1)BY THE TRANSFER OF ELECTRONS
2)BY SHARING ELECTRONS
3)COORDINATE BONDING

11. Ionic Bonds
An ionic bond is a type of chemical bond formed
through an electrostatic attraction between two
oppositely charged ions. Ionic bonds are formed
between a cation, which is usually a metal, and an
anion, which is usually a nonmetal. Pure ionic bonding
cannot exist: all ionic compounds have some degree of
covalent bonding. Thus, an ionic bond is considered a
bond where the ionic character is greater than the
covalent character. The larger the difference in
electronegativity between the two atoms involved in the
bond, the more ionic (polar) the bond is.

14. A covalent bond, also called a molecular
bond, is a chemical bond that involves the
sharing of electron pairsbetween atoms.
These electron pairs are known as shared
pairs or bonding pairs, and the stable
balance of attractive and repulsive forces
between atoms, when they share electrons,
is known as covalent
bonding.[1][better source needed] For
many molecules, the sharing of electrons
allows each atom to attain the equivalent of
a full outer shell, corresponding to a stable
electronic configuration.
Covalent bond

16. Types of covalent bonds

18. the
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By :- abhimanyu