BONDING, STRUCTURE PROPERTIES OF MATTER

It can conduct electricity well It’s strong yet flexible as it has a thin structure

Drug delivery Catalysts

Each carbon is covalently bonded to 4 other carbon atoms, forming a giant covalent lattice structure. -Extremely high melting point- Is a giant covalent structure = strong covalent bonds in all directions throughout the lattice = huge amount of energy is needed to break them. -Very hard- Each carbon atom forms 4 strong covalent bonds in a rigid 3D structure. This creates a very strong, fixed lattice with no weak layers. -Does not conduct electricity- All electrons are used in covalent bonds, so there are no free electrons or ions to carry charge.

Each carbon atom is covalently bonded to 3 other carbon atoms forming hexagonal rings making up a giant covalent lattice structure -High melting and boiling point- It is a giant covalent structure, so there are strong covalent bonds throughout the layers that require a lot of energy to break. -Soft and brittle- Arranged in hexagonal layers, but there are only weak forces between the layers, so they can slide over each other easily. -Good conductor of heat and electricity- Each carbon atom forms 3 covalent bonds, leaving 1 delocalised electron per carbon atom= electrons can move through the layers and carry charge.

Carbon atoms are arranged in layers with weak forces between them mesning they don’t require a lot of energy to break, so layers slide over each other easily.

High melting and boiling points. Strong. Conducts electricity. Very light.

Each carbon atom is covalently bonded to 3 other carbon atoms, forming hexagonal rings in hollow shapes like cylinders. THEY ARE SIMPLE COVALENT MOLECULES -Good conductor of heat and electricity- Each carbon atom forms 3 covalent bonds, leaving 1 delocalised electron per carbon atom= electrons can move through the layers and carry charge.

Ionic compounds have a giant ionic lattice structure. The ions form a closely-packed regular lattice arrangement, with strong electrostatic forces of attraction between oppositely charged ions, in all directions.

High melting and boiling points- strong electrostatic forces between ions require lots of energy to overcome. Conduct electricity when molten or aqueous, but not when solid- Ions are free to move around the structure and carry electric charge but when solid they are stuck in a lattice. Often soluble in water- Water molecules can surround snd separate the ions

Ionic compounds only conduct electricity when molten or aqueous, but not when solid. This is because substances need charged particles that are free to move in order to conduct electricity. When ionic compounds are solid, their ions are in a fixed lattice, so can’t flow. However, when molten or aqueous, the ions are free to move and carry charge.

A double bond is when there are 2 covalent bonds between the same atoms, meaning there are 4 electrons being shared in total

Alloys are mixtures of a metal with one or more other elements. They are harder than pure metals because the different-sized atoms disrupt the regular layers in the metal structure, making it more difficult for the layers to slide over each other.

Low melting points- weak intermolecular forces between molecules need little energy to overcome Do NOT conduct electricity- no free electrons to carry electric charge around structure Often gases or liquids at room temperature- weak intermolecular forces so little energy is needed to overcome them = LOW mp and bp

Each silicon atom is covalently bonded to 4 oxygen atoms in a giant lattice. -Extremely high melting point– It is a giant covalent structure, so there are strong covalent bonds in all directions throughout the lattice. A huge amount of energy is needed to break them. Very hard – Each silicon atom forms 4 strong covalent bonds in a rigid 3D network, creating a strong, fixed structure with no weak layers. Does not conduct electricity – All electrons are used in covalent bonds, so there are no free electrons or ions to carry charge.

A lattice of positive metal ions surrounded by a sea of delocalised electrons. The electrostatic attraction between the positive ions and negative electrons hold the structure together.

-High melting/ boiling point- Strong electrostatic attraction between positive ions and delocalised electrons. Require a lot of energy to break this attraction. -Good thermal conductors-The delocalised electrons are free to move through the structure and transfer thermal energy quickly. -Good electrical conductors-The delocalised electrons are free to move through the structure and transfer electric charge. -Malleable and ductile- Layers of ions can slide over each other without breaking bonds.

Solid = lowest kinetic energy, Liquid = medium kinetic energy, Gas = highest kinetic energy -Solid—> liquid = melting = Particles gain energy and vibrate more. Forces between particles are partially overcome allowing them to move around each other and are not longer in a fixed position. -Liquid—> gas = evaporating/ boiling = Particles gain energy and move faster. Forces between particles are overcome, allowing the particles to move freely in all directions. Solid—> gas= sublimation = Particles gain a lot of energy. Forces between particles are completely overcome, allowing the particles to move freely in all directions.

The transfer of electrons from a metal atom to a non metals atoms in atom. The metal loses electrons becoming positive and the non metal gains these electrons becoming negative.

The sharing of one or more pairs of electrons between non metals atoms in order to achieve a full outer shell. Each shared pair forms one covalent bond.