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Chemistry Unit 1 Chemical Bonding, Intermolecular Forces - Coggle Diagram
Chemistry Unit 1 Chemical Bonding
Ionic Bonding
Formation
Between a Non-metal and a metal
The non-metal loses its valence electrons to the metal atom, forming ions and achieving octet configuration in the same time.
The metal becomes a cation and the non-metal becomes an anion. They are attracted and bonded through the electrostatic force.
Examples
Sodium Chloride (NaCl, or Table Salt)
Sodium Bromide
Potassium Iodide
Properties
Usually solid at room temperature & High Boiling and Melting Point
Conduct Electricity at molten state or dissolved in water.
Brittle
Giant Lattic Structure
Covalent Bonding
Giant Covalent
High Boiling and Melting Point
Include Diamond, Graphite, Silicon Dioxide
Simple Covalent
Low Boiling and Melting Point
Include H2, O2, N2, etc.
Normally do not conduct electricity.
Formation
Between non-metals
Sharing of electrons so to achieve Octet, instead of losing electrons
More Classifications of Covalent Bonds
Single Covalent Bond
Non-Polar Covalent
Double Covalent Bond
Polar Covalent
Triple Covalent Bond
Metallic Bonding
Formation
Electrostatic force of attraction between positively charged metal cations and sea of delocolised electrons.
Between Metals
Examples
Gold
Silver
Copper
Properties
Malleable
High Boiling & Melting Points
Conducts Electricity
Lustrous
Conduct Heat
Sonorous
Ductile
Intermolecular Forces
Types
Van der Waal's Forces
London Dispersion
Dipole - Dipole
Hydrogen Bonding
Between molecules
Takes place when temporary or permanent dipoles formed within bond and molecules