Topic 1.1: Introduction to the particulate nature of matter and chemical change Flashcards
Atomic Theory
All matter is composed of atoms
Law of conservation of mass
Atoms cannot be created or destroyed and are rearranged during chemical reactions.
Stoichiometry
Describes the relationship between the amounts of reactants and products during chemical reactions
Properties of matter (4)
a) Made up of particles.
b) Occupies volume.
c) Has a mass.
d) Particles are in constant motion
Properties of states of matter
a) Volume
b) Shape
c) Compression
d) Intermolecular forces
e) Particle motion
Properties of solids
a) Fixed
b) Fixed
c) Cannot be compressed
d) Strong attractive forces
e) Vibrate in a fixed position
Properties of liquids
a) Fixed
b) No fixed
c) Cannot be compressed
d) Weaker forces than in solids
e) Vibrate, rotate, and translate
Properties of gases
a) No fixed
b) No fixed
c) Can be compressed
d) Zero
e) Vibrate, rotate, and translate.
Temperature and KE
As the temperature increases the average kinetic energy of the particles increases.
SI Temperature
Kelvin
Absolute zero
Temperature at which all movement of particles stops.
Kelvin - Celsius
K = C + 273.15
Endothermic
Energy must be transferred to matter from the surroundings.
Exothermic
Energy is transferred to the surroundings from the matter.
Solid - Liquid
a) Melting
b) Freezing
Liquid - Gas
a) Boiling
b) Condensation
Gas - Solid
a) Sublimation
b) Deposition
Pure substance
Matter that has a constant composition.
Element
Contain atoms of only one type.
Compounds
Fixed proportion of elements, held together by chemical bonds.
Mixtures
Physical combination of pure substances (not chemically combined)
Homogeneous mixtures
Uniform composition and properties throughout
Heterogeneous mixtures
Non-uniform composition and varying properties
Ions
Charged atoms
