Structures Flashcards
(40 cards)
What is a giant ionic lattice
Regular arrangement of alternating positive and negative ions
Examples of giant ionic lattice
Sodium chloride
Magnesium oxide
Properties of a giant ionic lattice
Crystalline
High melting points
Conducts electricity when liquid
Doesn’t conduct electricity when solid
Soluble in water
Why is a giant ionic lattice got high melting points
Ionic bonds are strong and require a lot of energy to break therefore it has a high melting point.
Why does a giant ionic lattice conduct electricity when a liquid but not when a solid
It doesn’t conduct electricity when a solid because ions are not free to move and carry charge, the ions are free to move and carry charge when liquid therefore able to conduct electricity.
What properties does a covalent molecular have
Low melting and boiling points
Doesn’t conduct electricity,
Not soluble in water
Soft when solid
Why does a covalent molecular have low melting and boiling points
Due to weak bonds between molecules breaking easily as requires little energy to break
Why does a covalent molecular not conduct electricity
No charged particles that are free to move and carry charge
Why is a covalent molecular soft when solid
Due to the weak bond between molecules breaking easily
What is the name of the forces between the molecules in simple covalent structures
Van Der Waals
Examples of a covalent molecular
Iodine
Carbon dioxide
Water
Ammonia
Methane
What is Giant covalent DIAMOND
Extensive covalent bonding in all directions with each carbon bonded to 4 others in a tetrahedral arrangement
What might the giant covalent DIAMOND be used for
Used in drill bits
Features of the giant covalent bond DIAMOND
Very high melting and boiling points
Diamond doesn’t conduct electricity
Insoluble in water
Diamond is extremely hard
Why does the giant covalent DIAMOND have very high melting and boiling points
Due to strong covalent bonds requiring large amounts of energy to break
Why does the giant covalent DIAMOND not conduct electricity
No charged particles free to move and carry charge
Why is the giant covalent DIAMOND very hard
Due to the extensive strong covalent bonds
What is the giant covalent GRAPHITE
Layered structure with each carbon bonded to 3 others in the layer
What might the giant covalent GRAPHITE be used in
Lubricant and pencil led
There is ….. free electron per each carbon atom which becomes delocalised in the giant covalent
One
The giant covalent GRAPHITE has weak ….
Van der waals between layers
Describe the giant covalent graphite
A slippery soft solid as weak van der waals between layers allows the layers to slide over each other
Properties of the giant covalents graphite and graphene
Conducts electricity as they have delocalised electrons free to move and carry charge
Giant covalent Graphene properties
Conducts heat and electricity efficiently
Nearly transparent
100x stronger then steel
Very thin
Light
Inexpensive
