states of matter

• Gases in a container exert a pressure as the gas molecules are constantly colliding with the wall of the container.
• Gas particles exert a pressure by constantly colliding with the walls of the container.
• Decreasing the volume of a gas causes an increased collision frequency of the gas particles with the container wall.
• Increasing the temperature of a gas causes the molecules to gain more kinetic energy, meaning the particles will move faster and collide with the container walls more frequently.
• The pressure of the gas increases as the temperature increases.
• The temperature is therefore directly proportional to the pressure at constant volume.
• A graph of temperature of gas plotted against pressure gives a straight line.
• Increasing the temperature of a gas causes an increased collision frequency of the gas particles with the container wall.
• Temperature is directly proportional to the pressure at constant volume.
• Diamond and silicon(IV) oxide are hard as it is difficult to break their 3D network of strong covalent bonds.
• Most compounds are insoluble in water and do not conduct electricity.
• Simple covalent lattices have weak intermolecular forces between the molecules and require only little energy to break the lattice.
• Metals are malleable as the layers can slide over each and reform.
• Graphite is soft as the forces between the carbon layers are weak.
• Diamond and silicon(IV) oxide do not conduct electricity as all four outer electrons on every carbon atom is involved in a covalent bond, so there are no free electrons available.
• Covalent bonding and simple covalent lattice structures have low melting and boiling points.
• Covalent bonding and giant covalent lattice structures have high melting and boiling points.
• Most compounds are insoluble with water unless they are polar or can form hydrogen bonds.
• A lot of energy is required to break the lattice of giant covalent lattices.
• Simple covalent compounds such as HCl can conduct electricity in solution.
• Giant covalent lattices have a large number of covalent bonds linking the whole structure and intermolecular forces between the molecules.
• Covalent compounds can be arranged in simple molecular or giant molecular lattices.
• An ideal gas will have a volume that is directly proportional to the temperature and inversely proportional to the pressure.
• Giant molecular lattices include silicon(IV) oxide, graphite, and diamond.
• Ideal gases have zero particle volume and no intermolecular forces of attraction or repulsion.
• The temperature in Kelvin is calculated by adding 273 to the Celsius temperature.
• The type of lattice formed depends on the sizes of the positive and negative ions which are arranged in an alternating fashion.
• An ionic bond is an electrostatic force between a positively charged metal ion and a negatively charged non-metal ion.
• The ionic lattice of MgO and NaCl are cubic.
• Ionic compounds are arranged in giant ionic lattices, also called giant ionic structures.
• Simple molecular lattices include Iodine, buckminsterfullerene (C ), and ice.
• Most ionic, metallic and covalent compounds are crystalline lattice, meaning the ions, atoms or molecules are arranged in a regular and repeating arrangement.
• Covalent bonds are bonds between nonmetals in which electrons are shared between the atoms.
• The molar mass of a gas can be calculated using the ideal gas equation.
• Real gases do not obey the kinetic theory assumptions at high temperatures and pressures due to attractive forces between molecules.
• The gas molecules do not attract or repel each other (no intermolecular forces).
• No kinetic energy is lost when the gas molecules collide with each other (elastic collisions).
• The gas molecules are moving very fast and randomly.
• Gases that follow the kinetic theory of gases are called ideal gases.
• When a gas is heated (at constant pressure), the particles gain more kinetic energy and undergo more frequent collisions with the container wall.