Bonding and Structure

• Solids are hard to compress as the particles are packed together in a regular pattern.
• Solids hace a fixed shape and cannot flow as the particles can only vibrate.
• Liquids are hard to compressas the particles are close together, with not many solids.
• Liquids can flow and move space to space.
• Gasses are easy to compress as there is a lot of spaces between the particles.
• Gasses spread out and fill the space of the container as the particles moves quickly>
• A solid to a liquid form is called melting.
• A liquid to solid is called freezing.
• A liquid to a gas is called boiling.
• A gas to liquid is called condensing.
• A full outer energy level is stable.
• Ionic bonding is when a metal and non-metal reacts together.
• Ionic compounds form giant structures and scientists casll the a giant ionic lattice.
• In a giant ionic lattice, every positive ion is surrounded by negative ions.
• Electrostatic forces of attractions hold the positive and negative ions in place. These are also called ionic bonds.
• An ionic compounds have high levels of melting anf boiling points as the strong electrostatic forces of attracted need a a lot of heat energy to break.
• An ionic compound cannot conduct electricity when they are solids as the ions are locked in place where the ions can vibrate but can't move.
• Ionic compounds can conduct electricity when they are melted of dissolved in water. Ions are free to move.
• Covalent bonding is the sharing of electrons to form a strong bond.
• Group 7 are diatomic.
• Small covalent molecules have low melting and boiling points.
• Small covalent substances have weak intermolecular forces between the molecules.
• Breaking weak intermolecular forces does not require a lot of energy.
• Giant covalent substances contain millions of strong covalent bonds.
• Diamond has 4 carbon atoms joined togeth, making it an extremely hard object, having a high melting and boiling point needing a high level of energy to break it.
• Diamond cannot conduct electricity as it has no free electron to move through the electrons.
• Silicon dioxide has a very high boiling and melting points.
• Graphite is a slippery giant covalent bond having a very high melting and boiling point, being a good conductor of electricity and heat.
• Graphite has 3 carbon atoms having hexoagonal rings, which are layers, which can slide of each other.
• Delocalised electrons allow a substance to move, being able to conduct electricity.
• Graohene is a single layer of graphite. Graphine is extremely strong, needing a high melting and boiling point, to break this bond.
• Fullerenes have hollow shapes, having hexagonal rings of carbon atoms.
• Fullerenes are used to transport drugs in the body such as pharmaceuticals.
• Fullerenes can also be usedd as lubricants between moving parts.
• Carbon nanotubes are long cylinders of fullerenes.
• Polymers are very large molecules by joining monomers.
• Monomers are alkene molecules.
• Metal is a giant structure formed in layers.
• Metalic bonding is the strong electrostatic force of attraction betweeen a positively charged ion and a sea of delocalized electrons which hilds the metal together and gives it its properties.
• Metals are malleable.