Chemical Bonding: Why Atoms Stick Together
Understanding atomic interactions is crucial in engineering new materials and technologies. Atoms form bonds primarily to achieve stability, which can be realized through ionic, covalent, and metallic bonding. The detailed study of these bonding types reveals how atoms interact to form the diverse structures and functions found in matter.
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What we have learnt
- Atoms bond to achieve greater stability, typically aiming for full outer electron shells.
- Ionic bonds form through the transfer of electrons between metals and non-metals.
- Covalent bonds involve the sharing of electrons between non-metal atoms.
Key Concepts
- -- Chemical Bonding
- The process of atoms joining together to form molecules, enabling stability and specific properties.
- -- Ionic Bonding
- A type of chemical bond that occurs through the transfer of electrons from one atom (usually a metal) to another (usually a non-metal), resulting in the formation of oppositely charged ions.
- -- Covalent Bonding
- A type of bond that forms when two non-metal atoms share one or more pairs of valence electrons.
- -- Metallic Bonding
- A bond formed by the attraction between delocalized electrons and positively charged metal ions, resulting in properties like conductivity and malleability.
- -- Valence Electrons
- Electrons in the outermost shell of an atom that are involved in forming chemical bonds.
- -- Octet Rule
- The principle that atoms tend to gain, lose, or share electrons to achieve a full outer electron shell, typically equating to eight electrons.
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