Lecture Notes: Metallic Bonds

Overview

• Discussion about metallic bonds, with a humorous reference to the lecturer's past as a lead singer in a 'metallic bond' band.

Key Points

Definition and Example

• Metallic Bond: Type of chemical bond found in metals.
• Example Used: Iron (Fe) atoms.

Formation of Metallic Bonds

• Atoms: When iron atoms are together, they form a metallic bond.
• Charge: Iron atoms in metallic bonds are positively charged ions (Fe+).
• Electron Sea Model: Electrons are shared and form a 'sea of electrons' surrounding the positive ions.

Characteristics of Metallic Bonds

• Electron Sharing: Valence electrons are shared and not fixed to any one atom.
• Electrical Conductivity: Due to free-moving electrons.
• Malleability: Metals can be bent easily because of the flexible 'sea of electrons'.
• Comparison with Ionic Compounds: Unlike rigid ionic compounds (like salt), metallic bonds are more flexible and malleable.

Spectrum of Bonds

• Ionic Bonds: Electrons are transferred, e.g., salt (sodium chloride).
• Covalent Bonds: Electrons are shared equally.
• Polar Covalent Bonds: Unequal sharing of electrons.
• Metallic Bonds: Extreme sharing with a communal sea of electrons.