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Chemical Bonding & Structure⚛️ - Coggle Diagram
Chemical Bonding & Structure⚛️
Ionic bonding
Bonding
in ionic compounds
Transfer of electrons from metals to non-metals
Metals: Lose electrons to form positive ions [Cations]
Non-metals : Gain electrons to form negative ions [Anions]
Bonding:
Strong electrostatic forces of attraction between positive and negative ions (e.g. Na⁺ and Cl⁻ ions)
Structure
of ionic compounds
Structure:
Giant Ionic Lattice Structure
(Cations & anions are arranged alternate to each other)
Properties
of ionic compounds
High melting & boiling points
Reason: Strong electrostatic forces of attractions between ions in lattice structure > large amount of energy required to overcome the forces > ionic compounds have high m.p. and b.p.
Generally
soluble in water
but
not in organic solvents
Conducts electricity only in molten state & aqueous solution
Reason: In molten or aqueous solution, the giant ionic lattice structure is broken down > ions are able to move freely to conduct electricity
Does not conduct electricity in solid state
Reason: In solid state, the ions are held by strong electrostatic forces in a giant ionic lattice structure > no free moving ions to conduct electricity
<< Covalent bonding >>
Simple Covalent Structure
Bonding
in Simple Covalent Substances
Bonding:
Weak intermolecular forces of attraction between molecules (e.g. CO₂ molecules)
Properties
of Simple Covalent Substances
Low melting & boiling points
Reason: Weak intermolecular forces of attraction between molecules > requires small amount of energy to overcome > simple covalent compounds have low m.p. & b.p.
Generally
soluble in orgnanic solvents
but
not in water
Do not conduct electricity at any state
as it is a neutral molecule [no free ions or electrons]
Giant Covalent Structure
Bonding
in Giant Covalent Substances
Bonding:
A network of strong covalent bonds between atoms
Allotropes definition:
Different structures formed by the same element
Diamond
(Allotrope of Carbon)
Bonding in Diamond:
1 C atom covalently bonded to 4 C atoms
Properties
of Diamond
Very high melting and boiling point
Reason: Network of strong covalent bonds between C atoms > large amount of energy required to overcome the bonds > thus diamond has very high m.p.
Generally
insoluble
in any solvent
Does not conduct electricity at any state
Reason: No free moving ions or electrons
Hard
(used to coat drill bits & cutting tool)
Reason: Strong covalent bonds between atoms > large amount of force required to overcome the bonds > diamond is hard
Graphite
(Allotrope of Carbon)
Bonding in Graphite:
1 C atom covalently bonded to 3 C atoms
Properties
of Graphite
Very high melting and boiling point
Reason: Network of strong covalent bonds between C atoms > large amount of energy required to overcome the bonds > thus diamond has very high m.p.
Generally
insoluble
in any solvent
Can conduct electricity at any state
Reason: 1 C atom covalently bonded to 3 other C aroms > 1 free electron per C atom not bonded > free electrons can move and conduct electricity
Soft and slippery
(used as lubricants or pencil lead)
Reason: Weak intermolecular forces of attraction between layers in graphite > small amount of energy required to overcome the forces > layers can slide over one another easily > graphite is soft and slippery
Silicon Dioxide
(SiO₂)
Similar properties as diamond
Bonding in SiO₂:
1 Si atom covalently bonded to 2 O atoms
Sharing of electrons equally between atoms of non-metals to attain the noble gas electronic configuration
Metallic bonding
Bonding
in Metals
Bonding:
Strong electrostatic forces of attraction between the positive metal ions and the 'sea of delocalised electrons'
Structure
of Metals
Structure:
Giant Metallic Lattice Structure
Metal atoms
packed closely in an orderly manner
Properties
of Metals
High melting & boiling points
Reason: Strong electrostatic forces between positive metal ions and a 'sea of delocalised electrons' > large amount of energy required to overcome the forces > metals have high m.p. and b.p.
Can conduct electricity at any state
Reason: 'sea of delocalised electrons' move freely to conduct electricity
Malleable & Ductile
Reason: Atoms are arranged in orderly layers which slide over one another easily when force is applied, without disrupting metallic bonds.