🔗Covalent bond vs Metallic bond🪙
Both bonds involve shared electrons, but the way electrons move sets them apart. One gives insulating molecules, the other gives shiny conductors.
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🔗Covalent bond
- ✓Electrons shared in fixed localized pairs
- ✓Forms molecules or covalent networks
- ✓Usually poor electrical conductor
- ✓Found between nonmetal atoms
- ✓Examples: O2, diamond, SiO2
🪙Metallic bond
- ✓Electrons delocalized in a shared sea
- ✓Holds a lattice of positive metal ions
- ✓Excellent conductor of heat and electricity
- ✓Malleable and ductile
- ✓Examples: iron, copper, aluminium
Verdict
Covalent bonds lock electrons between specific atoms, while metallic bonds let electrons roam freely. That mobility explains why metals conduct and bend without breaking.
Frequently asked
Why are metals malleable but covalent solids brittle?+
The electron sea lets metal layers slide, while fixed covalent bonds snap when atoms shift.
Which conducts electricity?+
Metallic bonding conducts well because delocalized electrons move freely; most covalent substances do not.
Are covalent network solids strong?+
Yes. Giant covalent structures like diamond are extremely hard and have very high melting points.
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