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Summary:Key Bonds in Materials Science
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- Universal Lab
- @universallab
Materials science involves several crucial types of bonds, including metallic bonds, covalent bonds, ionic bonds, and hydrogen bonds, along with widely discussed intermolecular forces (Van der Waals forces). While some classification debates exist, their importance is undeniable.
Intermolecular Forces vs. Hydrogen Bonds
Traditionally, intermolecular forces are defined as weak electrostatic interactions caused by permanent or instantaneous dipoles, typically referring to Van der Waals forces. Hydrogen bonds, however, can exist both between molecules and within molecules, and strong hydrogen bonds resemble covalent bonds, setting them apart from typical intermolecular forces.
1. Van der Waals Forces
Van der Waals interactions are weak intermolecular forces with no directionality or saturation, acting over 0.3–0.5 nm. They include:
Electrostatic forces (orientation forces): Attraction between permanent dipoles; decreases with temperature.
Induction forces: Interaction between a permanent dipole and an induced dipole.
Dispersion forces: Weak attraction from temporary dipoles due to electron movement.
2. Hydrogen Bonds
Formation: A hydrogen atom bonded to an electronegative atom (e.g., O, F, Cl) forms a hydrogen bond with another electronegative atom.
Properties: Hydrogen bonds are directional and saturated.
Strength: Depends on electronegativity difference and atomic radius.
Impact: Increases boiling/melting points, affects solubility, viscosity, and surface tension (e.g., water).
3. Metallic Bonds
Metallic bonds arise from electrostatic interactions between metal cations and delocalized free electrons, leading to conductivity and malleability.
4. Covalent Bonds
Covalent bonds form when atoms share electrons. Theories explaining covalent bonding include Lewis theory, valence bond theory, hybridization, VSEPR, and molecular orbital theory.
5. Ionic Bonds
Ionic bonds occur in ionic crystals due to electrostatic attraction between oppositely charged ions. Their strength is often measured by lattice energy.