Chapter 3: Chemical Bonding and Structure
Chemical bonding revolves around the principle of electron stability, with atoms striving for noble gas configurations through ionic and covalent bonding. Ionic bonding involves electron transfer between metals and non-metals, resulting in the formation of cations and anions, while covalent bonding entails the sharing of electrons between non-metals. The type of bonding significantly influences the physical properties of compounds, such as melting points, electrical conductivity, and solubility.
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What we have learnt
- Atoms achieve stability by achieving noble gas configurations through bonding.
- Ionic bonding involves strong electrostatic forces between charged ions, resulting in high melting and boiling points.
- Covalent bonding results from the sharing of electron pairs between non-metals, characterized by lower melting points and poor electrical conductivity.
Key Concepts
- -- Ionic Bonding
- The electrostatic attraction between positively charged cations and negatively charged anions formed through the transfer of electrons, typically between a metal and a non-metal.
- -- Covalent Bonding
- The sharing of electron pairs between non-metal atoms, allowing them to complete their valence shell and achieve stability.
- -- Octet Rule
- The principle stating that atoms tend to gain, lose, or share electrons in order to have a full set of eight valence electrons, resembling the electron configuration of noble gases.
- -- Electronegativity
- The tendency of an atom to attract electrons in a chemical bond, influencing the type of bond that forms between atoms.
- -- Ionization Energy
- The energy required to remove an electron from an atom, playing a crucial role in the formation of cations.
- -- Electron Affinity
- The energy change that occurs when an electron is added to a neutral atom, impacting the formation of anions.
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