Chapter 4: States Of Matter

Front 1

Assumptions of the kinetic theory of an ideal gas

Back 1

1. The gas molecules move rapidly and randomly
2. The distance between the gas molecule is much greater than the diameter of the molecules so the volume of the molecules is negligible
3. There are no forces of attraction or repulsion between the molecules
4. All collisions between particles are elastic
5. The temperature of the gas is related to the average kinetic energy of the molecules

Hint 1

Distance, volume, forces, collisions, and temperature

Front 2

Conditions for a real gas to behave like an ideal gas

Back 2

High temperature
Low pressure

Front 3

Differences of a real gas to an ideal gas

Back 3

1. They do have forces of attraction and repulsion between the molecules

2. The volume of the molecules cannot be ignored

Front 4

Conditions for a real gas to behave less like an ideal gas

Back 4

Low temperature

High pressure

Front 5

Differences of a real gas to an ideal gas at high pressure and low temperature.

Back 5

1. The molecules are closer

2. The volume of the molecules is not negligible compared with the volume of the container

3. There are intermolecular forces between the molecules

4. The attractive forces pulls the molecules toward each other and away from the walls of the container

5. The pressure is lower than expected compared to an ideal gas

6. The effective volume of the gas is smaller than expected for an ideal gas

Front 6

Relationships between the volume of a gas to the temperature and pressure

Back 6

Volume is directly proportional to the temperature
Volume is inversely proportional to the pressure

Front 7

State the general gas equation

also give the units and the value for the gas constant

Back 7

pV=nRT

p is pressure in pascals, Pa

V is volume in cubic metres, m3

n is the number of moles of gas, mol

R is the gas constant, which has a value of 8.31J/Kmol

T is the temperature in kelvin, K

Front 8

Describe the liquid state, using a kinetic-molecular model

Back 8

1. Particles are close together, so the liquid has a fix volume and can be compressed slightly.

2. The particles are arranged less randomly than gas particles.

3. The particles have limited movement from place to place, in all directions

Front 9

Describe melting(when a solid is heated), using a kinetic-molecular model

Back 9

1. The energy that is transferred to the solid makes the particles vibrate more vigorously

2. The kinetic energy of the particles is overcoming the force of attraction

3. The solid changes to a liquid when its temperature is high enough

Front 10

Describe vaporisation(when a liquid is heated), using a kinetic-molecular model

Back 10

1.The energy that is transferred to the liquid makes the particles move faster

2. The kinetic energy of the particles is overcoming the force of attraction

3. The particle with the highest energy are the first to escape the attraction forces in the liquid

4. The liquid evaporates

5. Then the kinetic energy of all the particles is high enough to break free from each other in the liquid

6. The liquid boils

Front 11

Describe vapour pressure, using a kinetic-molecular model

Back 11

When a liquid evaporates, in a closed container. The molecules that escapes the liquid will become a gas molecules. These gas molecules that have escaped will collide with the walls of its container, therefore exerting a pressure.

Front 12

Describe the lattice structure of a crystalline solid of ionic lattices

Back 12

A regular arrangement of positive ions surrounded by negative ions and vice versa, attracted by the electrostatic attraction between opposite charges.

Front 13

Describe the lattice structure of a crystalline solid of simple molecular lattices

Back 13

A regular arrangement of molecules, attracted to each other by the weak intermolecular forces.

Front 14

Describe the lattice structure of a crystalline solid of giant molecular structure

Back 14

A regular arrangement of atoms, bonded covalently to each other.

Front 15

Describe the lattice structure of a crystalline solid of hydrogen-bonded solid

Back 15

A regular arrangement of molecules, attracted to each other by hydrogen bonding. The hydrogen bonds may force the molecules to be further apart in the lattice.

Front 16

Describe the lattice structure of a crystalline solid of metallic lattices

Back 16

A regular arrangement of positive ions surrounded by a sea of negative electrons. The structure are held by the electrostatic attraction that acts in all direction within the lattice.

Front 17

Describe the strength, melting point and electrical conductivity properties of ceramics.

Back 17

High strength

High melting point

Poor conductor of electricity

Front 18

Uses of ceramics

Back 18

Furnace linings, electrical insulators, glass, crockery