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“Explore the fundamentals of chemical bonding — from ionic and covalent bonds to molecular structures. Learn how atoms combine to form compounds and why chemical bonds matter.”

  • Chemical Bonding.
  • Introduction
  • Atoms are the fundamental units of matter they combine to form stable compounds.In chemical bonding atoms follow the octet and duplet rule to achieve electronic configuration of nearly noble gases to complete their octet. Hydrogen and Helium only two atoms follow the duplet rule. https://link.springer.com/subjects/chemical-bondig.
  • Chemical bonding is responsible for combining the atoms together with force which is called intermolecular forces.
  • There are following types of chemical bonding.https://alziwaq.com/ionic-bond-defination-explanation-and-diagram-and-properties/
  • Ionic bond.
  • Covalent bond
  • Polar and non polar covalent bond
  • Metallic bonding
  • Ionic bond
  • The complete transfer of electrons from one atom to another atom to form the ionic bond. Ionic bonds form between the metal and non-metal atoms to completely transfer electrons. One atom that loses electrons gets positive charge and becomes cation  and other atoms which lose electrons get negative charge and become anion and these opposite charges attract atoms to form ionic bonds. For example Nacl, and MgO.
  • Properties.
  • High melting and boiling points , electric conductivity in aqueous and molten state and crystalline solid.
  • Covalent bond. 
  • The type of chemical bond which is formed by sharing of electrons pairs between the two atoms is called covalent bond. It occurs between the non-metals. In this bonding single , double and triple bond form depending on the shared pair of electrons. For example: Water (H2O), carbon dioxide (CO2), nitrogen (N2).
  • Properties.
  • Low melting and boiling points, poor electrical conductivity.
  • Non-Polar covalent bond.
  • The covalent bond from equal sharing of electrons pairs between two identical atoms which have almost same electronegativity is called non-polar bond. For example Cl-Cl ,H-H etc.
  • Polar covalent bond
  • The bond forms unequal sharing of electrons between the two different atoms. The atom which is more electronegative attracts the shared pair of electrons more towards itself as compared to the other which is least electronegative. This creates the partial negative charges on one atom and partial positive charge on the other and these opposite charges atoms attract to form polar covalent bonds. For example H-Cl, H2O, etc.
  • Metallic bond.
  • Metallic bond forms between the metal atoms which give distinguished characteristics of metal atoms where the metals electrons delocalize over the positively charged metal ion. The sea of electrons allow the metal atoms to conduct electricity and malleable and ductile. For example iron , copper and Alluminium
  • Properties.
  • High electrical conductivity ,high  malleable and ductility , metallic luster.Metallic bond | Properties, Examples, & Explanation – Britannica
  • Other interaction.
  • Hydrogen bonding: A weaker interaction where hydrogen is electrostatically attracted to electronegative atoms like oxygen, nitrogen, or fluorine. Important in water properties, DNA stability, and protein structure.
  • Van der Waals forces: Weak interactions between molecules due to transient dipoles; significant in noble gases and large molecules like polymers.
  • Dipole dipole interaction 
  • Electrostatic attraction between the polar molecules permanent dipole.
  • London dispersion forces.
  • London dispersion forces (LDF) are a type of intermolecular force that arises due to the temporary formation of instantaneous dipoles in atoms or molecules. These forces are the weakest among the intermolecular forces and are typically observed in nonpolar molecules.
  • Chemical bonding and different types of interactions | PDF
  • Importance of chemical bonding
  • Chemical bonding helps to understand the reactivity,  properties, and structure of an atom. It underpins fields ranging from materials science and pharmaceutical chemistry to biochemistry. Understanding bonding enables chemists to predict molecular geometry, reaction tendencies, and thermodynamics of compounds.
  • Conclusion.
  • Chemical bonding is fundamental to the formation of matter as we know it. By examining ionic, covalent, and metallic bonds, along with weaker intermolecular forces like hydrogen bonding, scientists can explain  the structure and properties of compounds, opening the door to innovations in chemistry, materials, and medicine.