Chemistry curriculum
The particulate nature of matter - State the distinguishing properties of solids liquids and gasses
liquids
no definitive shape, takes the shape of its container, has definitive volume and particles are free to move over each over
solid
Definite shape, definite volume and particles vibrate in fixed position
gas
no definite shape, no definite volume and particles can move freely
Experimental techniques
measurment
time - stopwatch
temp - thermometer
mass - digital balance
volume approx. - measuring cylinders
volume accurate - pipets/ burettes
gas - gas syringe
Criteria of purity
Chromatography
the separation of aqueous solutions by using chromatography paper and putting it in a solution
Chromatograms
a graph showing the results of chromatography
Every day life of purity
to make sure drugs have the right amount of chemicals to fix peoples ills and to make sure food wont kill you
Mixtures melt and different temperatures
mixtures change melting points due to the two clashing melting points
Methods of purification
use of a suitable solvent,
filtration, crystallisation, distillation, fractional
distillation and paper chromatography
Atoms, elements and compounds - structures and bonding
Electronic arrangement/configuration
We call the electrons on the outer shell valence electrons
On the 1st shell there are two electrons and the second and third hold 8 electrons
The period gives the number of shells while the group gives the number of electrons in the outer shell
Example
Take electrons away from positive ions and add extra for negative ions
A noble matter
They are very stable and are unreactive
Chemical vs Physical changes
Chemical changes are irreversible
Physical changes are reversible
Atomic structure
Atoms are mad of:
Neutrons: Mass = 1 charge = 0
Electrons: Mass = 0 charge = -1
Protons: Mass = 1 charge = +1
The proton number gives the number of protons or electrons and the nucleon number is the number of protons and neutrons together
Stoichiometry
Use the symbols of the elements and write the formulas of simple compounds
Deduce the formula of a simple compound from the relative numbers of atoms present
Deduce the formula of a simple compound from a module or diagramed representation
Electricity and chemistry
Chemical energetics
Chemical reactions
The Periodic Table
Periodic trends
Metallic to non metallic character across period
Relationship between group number, number of outer-shell electrons and metallic/non-metallic character
Group Properties
Group I - a collection of relatively soft metals
trend in melting point
trend in density
reaction with water
Group VII - a collection of diatomic non-metals showing a trend in colour and physical state
the reaction of chlorine, bromine, and iodine with other halide ions
predict the properties of other elements in Group VII, given the date, where appropriate
Transition elements
A collection of metals having high densities, high melting points and forming coloured compounds, and which, elements and compounds, often act as catalysts
Noble gases
Group VIII or 0, as being unreactive, monoatomic gases and explain in terms of electronic structure
Practical methods for investigating the rate of reaction which produces a gas
Suggest suitable apparatus, given information, for experiments, including collection of gases and measurement of rates of reaction
Interpret data obtained from experiments
concerned with rate of reaction
Describe the effect of concentration, particle size, catalysts and temperature on the rate of reactions
Describe and explain the effect of changing concentration in terms of frequency of collisions between reacting particles
Describe and explain the effect of changing temperature in terms of the frequency of collisions between reacting particles and more colliding particles possessing the minimum energy (activation energy) to react
Describe how concentration, temperature and surface area create a danger of explosive combustion with fine powders (e.g. flour mills) and gases (e.g. methane in mines)
Redox - Describe oxidation and reduction in chemical reactions in terms of oxygen loss/ gain (Oxidation state limited to its use to name ions, e.g. iron(II), iron(III), copper(II).)
Define redox in terms of electron transfer, and identify such reactions from given information, which could include simple equations
Define and identify an oxidising agent as a substance which oxidises another substance during a redox reaction and a reducing agent as a substance which reduces another substance during a redox reaction
Describe the meaning of an exothermic and endothermic reactions
Describe bond breaking as an endothermic process
Describe bond forming as an exothermic
process
Interpret energy level diagrams showing exothermic and endothermic reactions and the activation energy of a reaction
The densities of the Group 1 elements increase down the group
The melting point of the Group 1 elements decrease down the group
This shows that the reactivity of the alkali metals increases as you go down Group 1.
Bond-making is an exothermic process. Whether a reaction is endothermic or exothermic depends on the difference between the energy needed to break bonds and the energy released when new bonds form. If more heat energy is released when making the bonds than was taken in, the reaction is exothermic.
Energy is absorbed to break bonds. Bond-breaking is an endothermic process. Energy is released when new bonds form
Define electrolysis as the breakdown of an ionic compound when molten or in aqueous solution by the passage of electricity
Use the terms inert electrode, electrolyte, anode and cathode
Describe the electrode products and the observations made, using inert electrodes (platinum or carbon), in the electrolysis of - molten lead (II) bromide - concentrated aqueous sodium chloride - dilute sulfuric acid