Atomic Bonding
Atoms can interact with each other to form molecules and other chemical compounds. This
interaction is facilitated by the valence electrons, which are the electrons in the outermost
shell of an atom. There are three primary types of chemical bonds:
1. Ionic Bonding
Definition: A type of bond formed through the transfer of electrons from one atom to
another.
How it Works:
One atom (usually a metal) loses electrons to become a positively charged ion
(cation).
Another atom (usually a non-metal) gains electrons to become a negatively
charged ion (anion).
The opposite charges attract, creating an ionic bond.
Example: Sodium chloride (NaCl), where sodium (Na) transfers an electron to chlorine
(Cl).
2. Covalent Bonding
Definition: A bond formed when two atoms share electrons.
How it Works:
Atoms come together to achieve a full outer shell of electrons, leading to stability.
This sharing can be equal (nonpolar covalent bond) or unequal (polar covalent
bond).
Examples:
Nonpolar Covalent: In diatomic molecules like O₂, the electrons are shared
equally.
Polar Covalent: In water (H₂O), the electrons are shared unequally, creating a
partial negative charge near the oxygen atom and partial positive charges near the
hydrogen atoms.
3. Metallic Bonding
Definition: A bond found in metals where electrons are delocalized and shared among
a lattice of atoms.
How it Works:
Metal atoms release some of their electrons, which move freely throughout the
structure.
This "sea of electrons" allows metals to conduct electricity and heat.
Atoms can interact with each other to form molecules and other chemical compounds. This
interaction is facilitated by the valence electrons, which are the electrons in the outermost
shell of an atom. There are three primary types of chemical bonds:
1. Ionic Bonding
Definition: A type of bond formed through the transfer of electrons from one atom to
another.
How it Works:
One atom (usually a metal) loses electrons to become a positively charged ion
(cation).
Another atom (usually a non-metal) gains electrons to become a negatively
charged ion (anion).
The opposite charges attract, creating an ionic bond.
Example: Sodium chloride (NaCl), where sodium (Na) transfers an electron to chlorine
(Cl).
2. Covalent Bonding
Definition: A bond formed when two atoms share electrons.
How it Works:
Atoms come together to achieve a full outer shell of electrons, leading to stability.
This sharing can be equal (nonpolar covalent bond) or unequal (polar covalent
bond).
Examples:
Nonpolar Covalent: In diatomic molecules like O₂, the electrons are shared
equally.
Polar Covalent: In water (H₂O), the electrons are shared unequally, creating a
partial negative charge near the oxygen atom and partial positive charges near the
hydrogen atoms.
3. Metallic Bonding
Definition: A bond found in metals where electrons are delocalized and shared among
a lattice of atoms.
How it Works:
Metal atoms release some of their electrons, which move freely throughout the
structure.
This "sea of electrons" allows metals to conduct electricity and heat.
