top of page
image.png
image.png
image.png
​

Bonding Diagrams

image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png

Small non metal molecules            One large structure of non metals
 

Metallic Bonding

Attraction between positive metal ions and delocalised electrons.

Properties
1.  Conduct electricity even when solid due to
   delocalised electrons.

2. Range of melting & boiling points

 

image.png

 Ionic Bonding

Electrostatic force of attraction between positive (metal) ions and negative
(non metal) ions.

Metal & Non metal





Properties of Ionic Substances

1. High Melting and Boiling points

2. Soluble in water

3.  Can not conduct electricity when solid as ions aren't free to move in lattice

        Conducts electricity when molten/in solutions as lattice is broken &
     ions are now free to move.

 

image.png
image.png

Electrolysis of Ionic Compounds

       +ve  electrode                     - electrode   

 Negative non metal ion            Positive metal ion

Using electricity to break up a molten ionic compound OR ionic solution using a 
DC supply.














DC supply needed
Allows 1 product to build up at each electrode for identification.

Carbon Electrodes
Carbon (graphite) is used as it conducts electricity as & is non reactive.

Solid ionic compounds do not undergo electrolysis as the ions are not free
to move in the lattice.

                   


 

image.png

Covalent Bonding

When 2 positive nuclei are held together by their
shared attraction for a pair of electrons.

Non metals elements/compounds.

Types of Covalent Structures

 

image.png
image.png
image.png
image.png

1 large non metal structure that ONLY contains strong covalent bonds.

5 Covalent networks

1. Boron                 4. Carbon diamond
2. Silicon                5. Carbon graphite
3. Silicon dioxide  


Properties

1.  High melting & boiling points
   (solid @ room temperature)
2.  Does not conduct electricity
3.  Does not dissolve in water



 

image.png
image.png

Graphite (delocalised electrons)



 

image.png

Small molecules that have strong covalent bonds within the molecule

 

but weak intermolecular forces BETWEEN molecules.


Properties

1.  Low melting & boiling points
   (liquid/gas @ room temperature)
2.  Does not conduct electricity
3.  Does not dissolve in water



 

image.png
image.png

Two non metal atoms joined together as a covalent molecule.


                 7 diatomic elements                 Diatomic compounds
                    Formula A2                                           Formula   AB





Iodine      Bromine     Chlorine    Fluorine    Oxygen   Nitrogen  Hydrogen





 

image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png

Shapes of Covalent bonds

Covalent molecules take on different shapes depending on how many bonds are formed around the central atom

1 bond -                                           3 bonds -





2 bonds -                                           4 bonds -       





 

image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png
image.png

2D

 

3D

 

3D

 

3D

 

2D

 

2D

 

2D

 

3D

 

image.png
image.png
image.png

Be Careful 

Carbon dioxide from its formula suggests angular BUT is actually linear due to double bonds not being able to bend.





 

image.png

Outer Electron Diagrams

Lookup the data book to work out how many outer electrons are in each element. 
                       
Group no = outer electrons
 





 

image.png
image.png

Hydrogen

1 electron

Chlorine

7 electrons

4 x Hydrogen

1 electron each

  Carbon

4 electrons

image.png
image.png
image.png
image.png
image.png
image.png

2 x Nitrogen 

5 electrons 

image.png

2 x Oxygen

6 electrons 

Summary of Conduction

image.png

Summary Table Questions

​





 

image.png
image.png
image.png
image.png
image.png
image.png
image.png
loader,gif
bottom of page