1 Prior Knowledge

• Matter:

  Matter has MASS & occupies SPACE.
• Matter:

  Three states of

  matter: solid, liquid, gas
• Pure Substance:

  one in which all the particles that make up the

  substance are the same (resulting in common

  properties).
• Element:

  a pure substance that cannot be broken

  down into simpler substances. They

  contain only one kind of atom.
• Compound:

  a pure substance that contains two or

  more different elements in a fixed

  proportion. They can be identified with a

  chemical formula.
• Molecule:

  a neutral particle that is made up of two or

  more atoms that are joined by covalent

  bonds.
• Covalent Bond:

  the force of attraction between atoms that

  share one, two, or three pairs of electrons
• Ionic Bond:

  formed between metals and non-metals,

  electrons are given up by the metals and

  received by the non-metals
• Physical Property:

  a physical characteristic of the substance.

  Example: state of matter, hardness, melting

  point, odour, solubility, colour.
• Quantitative Property:

  property that has a number associated with it.
• Physical Change:

  a change which does not affect the

  chemical properties of a substance.
• Chemical Property:

  a characteristic behaviour that occurs

  when a substance changes into a new

  substance.
• Chemical Change:

  the change of one substance into another.
• There are 5 signs that can be used as evidence

  of a chemical change:

  A permanent __UNEXPECTED___ change in colour.

  Formation of a _GAS_ or _ODOUR_.

  Formation of a __PRECIPITATE____. → When 2

  liquids combine to form a solid

  4. _ENERGY__ in the form of heat or light is either

  released or absorbed.

  5. _ELECTRICITY__ is produced.
• Reactants:

  the starting materials in a chemical

  reaction.
• Products:

  the new material(s) produced in a

  chemical reaction.
• Isotopes:

  Atoms of the same element that have different numbers of

  neutrons
• The Periodic Table:

  Elements react in order to become stable like the noble gases (have full

  outer shells) i.e. they want the same electron configuration as their closest

  noble gas neighbour. They do this by gaining or losing electrons.