Covalent Bonding
Introduction
- Results from sharing of electrons between two atoms.
- It mainly exists among non-metallic elements.
Example:
The Octet Rule:
" Atoms tend to gain, lose or share electrons until they are surrounded by 8 valence electrons".
H· + H· → 
- These are called: "Lewis Structures" or "Lewis electron dot structures"
- In both structures, a covalent bond is created by sharing electrons between the two atoms, so that both atoms satisfy the octet rule
- For H2 molecule, although each H atom is surrounded by 2 electrons only, each H atom satisfy the octet rule since each H atom in the molecule resembles the nearest noble gas: He
Remark:
The number of valence electrons determines the number of covalent bonds an element will form:
If one electron ONLY is shared between the two atoms → Single Bond
If more than one electron are shared between the two atoms, implying Multiple Bonds.
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Date of last modification: 2024