In section 1.1, we have discussed ions and bonding in I/GCSE Chemistry.

Section 1.2

Structures in atomic level are also included in I/GCSE Chemistry

• A giant ionic lattice structure

• Ionic compounds have a giant ionic lattice structure

• The ions form a closely packed regular lattice arrangement

• There are very strong electrostatic forces of attraction between the oppositely charged ions
• They all have high melting points and high boiling points --->   the strong forces as it takes a lot of energy to break them
• The solid ionic compounds cannot conduct electricity as the ions are not free to move so they cannot carry the current through the compound
• When the compound is melted, the ions are free to move in the solution, so they can conduct electricity

• Long chains of repeating units that are joined together by strong covalent bonds

• The intermolecular forces between polymer molecules are larger than between simple covalent molecules as more energy is needed to break them

• The intermolecular forces are still weaker then ionic or covalent bonds  

• All the atoms are bonded together with strong covalent bonds
• Very high melting and boiling points as there is a lot of energy required to break the strong bonds between the atoms
• They do not contain charged particles so they do not conduct electricity, except graphite
• Examples of giant covalent structures are diamond, graphite and silicon dioxide.
• These are all made from carbon atoms, though silicon dioxide also contains oxygen

• Each carbon atom has four covalent bonds
• Very hard
• The strong covalent bonds take a lot of energy to break - high melting point
• No free electrons - does not conduct electricity

• Each carbon atom has three covalent bonds.
• It has sheets of carbon atoms arranged in hexagons.
• There are no covalent bonds between the sheets so they can move over each other, making it slippery - good lubricant.
• High melting point.
• Each carbon atom has one delocalised electron - it conducts electricity.
• One sheet of graphite is called graphene.

• Fullerenes are molecules of carbon that are hollow tubes or balls.
• They can be used to cage other molecules as they can be trapped inside the hollow part, an example would be a drug.
• A large surface area so they help to make catalysts and lubricants.
• They can also form nanotubes which are incredibly small carbon cylinders.
• They can conduct electricity and are rather flexible.
• Nanotubes are often used to make technology as they are so small and have a very small mass.

Nanoparticles have a diameter between 1nm and 100nm (1nm = 1x10^-9). Nanoparticles have a large surface area to volume ratio because when particles decrease in size, their surface area increases.

• Catalysts - large surface area to volume ratio
• Drugs - absorb the drug easily
• Electric circuits - some can conduct electricity
• Surgical masks and wound dressings - antibacterial properties
• Cosmetics - reduce oil
• Sun cream - can protect the skin from UV rays and better coverage

Section 1.1 & 1.2 about Bonding, structure and properties in I/GCSE Chemistry are fully discussed.

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Written by Bryant Wong (Chemistry)

Photo reference

1. Share Education, https://shareeducatonideas.com/ionic-compound/
2. Wikipedia, https://tr.wikipedia.org/wiki/Fulleren