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Chapter 4 (Chemical Bonding) - Coggle Diagram
Chapter 4 (Chemical Bonding)
Intermolecular (outside & weak)
Example: Van Der Waals Force
Intramolecular bond (Inside & Strong)
Ionic Bond (Metal & Non-Metal)
Properties
Have high melting and boiling point
Conducting an electric current in molten form
Sparingly soluble in organic solvent
Dissolve in water
Consisting of ions
Covalent Bond ( Non-Metal Only)
Types of Covalent Bonds
Dative Bond
A covalent bond in which both shared/bonding electrons originate from one of the joined atoms
Non-polar Covalent Bond (
There is symmetry in the distribution of electron density
Polar Covalent Bond (x < 2)
There is asymmetry in the distribution of electron density
Polar bonds are formed when one of the elements attracts the shared electrons more strongly than the second element
Ionic Bond (x >= 2)
Properties
Have low melting and boiling point
Not conducting an electric current in any form
Dissolve in most of organic solvent
Sparingly soluble in water
Consisting of atoms and molecules
Lewis Structure
Formal Charges
Formal charge = (no of valence electrons) – (no of bonds + no. of unshared electrons)
When several Lewis structures are possible, those with the smallest formal charges are the most stable and preferred
Rules To Draw
Most metallic elements are generally central
Halogens and hydrogen are generally terminal
Subtract 1 electron for each + charge for cation
Add 1 electron for each - charge for anion
Octet Rule
Exception for molecule in which the atom has less than an octet
Molecules with an odd number of valence electrons
Exception for molecule in which the atom has more than an octet