Stucture and Bonding
Non-metal ions gain electrons.
Metal ions lose electrons.
Strong electrostatic forces of attraction between oppositely charged ions - This is called an IONIC BOND.
Covalent Bond = Strong bond between two non-metal atoms.
Non-metal atoms share their electrons to form COVALENT BONDS.
When two atoms share a pair of electrons they get joined together.
The covalent bond that is formed is very strong and it takes a lot of energy to break it.
Compound = Atoms of different elements join together.
Covalent bonds join atoms together to form molecules.
Stucture and Properties
These contain only a few atoms held together by STRONG COVALENT BONDS.
They have LOW MELTING and BOILING POINTS as the weak intermolecular forces break down easily.
They are NON-CONDUCTIVE - They don't have any free electrons or an overall charge.
Giant Covalent Structures - 'Macromolecules'
Contain a lot of NON-METAL ATOMS, joined by COVALENT BONDS.
The atoms are arranged into GIANT LATTICES, which are VERY STRONG structures because of the many bonds.
They have HIGH MELTING and BOILING POINTS because a lot of STRONG COVALENT BONDS must be broken.
Polymer = A large molecule formed from many identical monomers.
Thermosoftening: The forces between the chains are weak so it softens when heated and hardens when cooled.
Thermosetting: Strong covalent bonds form cross-links between the chains so they don't soften or melt when heated.
LDPE and HDPE
Low-Density Poly(Ethene) and High-Density Poly(Ethene) are made using DIFFERENT CATALYSTS and different REACTION CONDITIONS.
High-Density Poly(Ethene) = Higher softening temperature and is stronger.
Ionic Bonds form when a metal reacts with a non-metal.
Ionic compounds have giant structures in which many strong electrostatic forces of attraction hold the ions together.
They have HIGH MELTING and BOILING POINTS because of the strong bonds.
They CONDUCT ELECTRICITY when molten because the ions are free to move about and carry charge.
Metals are MALLEABLE - They can be bent or shaped.
Metals consist of LAYERS of atoms. The layers can slide over one another.
Metals are GOOD CONDUCTORS of electricity and heat. This is because the free / delocalised electrons can move through the metal, carrying charge.
Alloy: A mixture of two or more elements where at least one element is a metal.
Many alloys are mixtures of two or more metals.
Alloys contain atoms of different sizes. This makes it harder for the layers to slide over each other.
Alloys are HARDER than pure metals.
Shape Memory Alloys can return to their original shape once heated.
Uses: Dental braces.
Nanoscience = The study of small particles that are between 1 and 100 nanometres in size
One nanometre = 10^-9m
Nanoparticles have a VERY LARGE SURFACE AREAS.
They can REACT VERY QUICKLY and so make USEFUL CATALYSTS.
Nanoparticles behave differently to normal particles.
Uses: Sun screen, cosmetics, deoderants, etc.
- Particle with a very large surface area can cause damage to the lungs and breathing.
- There may be dangerous side affects.
The mass of an atom is its total number of protons and neutrons.
Isotopes are atoms of an element with different numbers of neutrons.
Isotopes have the SAME CHEMICAL PROPERTIES but DIFFERENT PHYSICAL PROPERTIES.
A atom consits of;
- a nucleus,
Relative Formula Mass (Mr) & Percentage and Formul
Relative Formula Mass
We find the Relative Formula Mass of a substance by adding up the relative atomic masses (Ar) of all the atoms in its formula.
One mole of any substance is its relative formula mass in grams.
Percentage and Formulae
The Relative Atomic Masses (Ar) of the elements in a compound and its formula can be used to work out its percentage composition.
Paper Chromotography is used to analyse colured substances.
Paper Chromatography can be used to analyse the artificial colours in food.
A spot of colour is put onto paper and solvent is allowed to move through the paper.
The colours move different distances depending on their solubility.
Instrumental methods of analysis rely on machines.
There are several different types of instrumental analysis.
Modern instrumental techniques provide fast, accurate and sensitive ways of analysing chemical substances.
Compounds in a mixture can be separated using gas chromatography:
1) The sample is dissolved in solvent and injected into one end of a column.
2) An unreactive gas, usually Nitrogen, carries the sample through a column.
3) Different substances travel through the column at different speeds and so become separated from each other.
4) The separated substances leave the column one after the other. As they leave, they are detectd by a detector.
The time taken for a substance to travel through a column is called the RETENTION TIME.
A detector produces a graph where each substance is represented by a peak:
- Number of peaks = Number of compounds present
- Position of peak = Retention time for each compound
Once separated, compounds can be identified using a mass spectrometer.
In a reversible reaction, the products of the reaction can react to form the original reactants.
Mass is NEVER LOST or GAINED in a chemical reaction. We say that mass is conserved.
Mass of products = Mass of reactants.
The Yeild of a chemical reaction describes how much product is made.
The percentage yeild of a chemical reaction tells us how much product is made compared with the maximum amount that could be made.
It is not always possible to get the entire calculated amount of product;
--> Reversible reactions ma not go to completion
--> Some product may be lost
Measuring Rates of Reaction
We can measure the changes in amounts of the chemicals taking part in the reaction by measuring their mass or volume.
For a liquid or a solid we measure the mass using a BALANCE.
For a gas we measure the volume with a GAS SYRINGE.
The rate of reaction = How quickly a reaction takes place.
There are two ways to measure the rate of a reaction:
- The rate at which a reactant is used up
- The rate at which a product is formed.
Rate of Reaction = Amount of reactant used / Amount of product formed
Factors Affecting the Rate
For a reaction to take place, particles must collide with enough energy.
This amount of energy is called the ACTIVATION ENERGY.
> Temperature: Increases the rate of reaction as the particles have more energy and collide more frequently and more energetically. At a higher temperature more particles have energy greater than the activation energy.
> Concentration: If one of the reactant chemicals is in solution the reaction rate will increase if the concentration is increased. There will be more of a chemical in a smaller volume so collisions are likely to take place more often.
> Preassure: Increasing the preassure means there are more reactant particles in a given volume. There will be more successful collisions as the particles are closer together.
> Surface Area: Increasing the S/A of a solid means that more particles are exposed to other reactants, therefore there is a greater chance of collision.
> Catalyst: Reduces the activation energy needed for a reaction to take place. (Different reactions require different catalysts.)
Exothermic and Endothermic Reactions
> Transfer energy to the surroundings - usually heat energy.
> Temperature increase can be detected using a THERMOMETER.
> Exothermic Reactions; Combustion, Oxidation reactions, Neutralisation reactions (acids and alkalis).
> Surrounding get colder.
> Examples; Electrolysis, Reactions between Ethanoic Acid and Sodium Carbonate, Thermal decomposition of Calcium Carbonate in a blast furnace.
In a reversible reaction, the reaction in one direction is Exothermic and in the other direction it's Endothermic.
In any reversible reaction, the amount of energy released when the reaction goes in one direction is exactly equal to the energy absorbed when the reaction goes in the opposite direction.
Acids and Bases
We measure the strength of acids and bases by their pH value.
Acids have a pH of less than 7.
Bases have a pH of more than 7.
Acids turn blue litmus paper red. Strong acids turn universal indicator red too.
Bases are sunstances that neutralise acids. They're usually Metal Oxides/Hydroxides.
Not all bases dissolve in water.
Alkalis are bases that dissolve in water.
Alkalis turn red litmus paper blue.
Neutral chemicals have a pH value of 7. They turn litmus paper/universal indicator green.
When we dissolve a substance in water, we make an Aqueous Solution (aq)
* Acids = H+ , Alkalis = OH-
A salt is created when an acid reacts with a base, carbonate or metal.
Acid + Base = Neutralisation - This produces salt and water.
Acid + Metal = Salt + Hydrogen
Carbon Dioxide causes bubbling during a reaction
Hydrogen can be detected with a lighted splint and burns with a squeaky pop.
Acids = HCl (aq) = H+ (aq) + Cl- (aq)
Alkalis = NaOH (aq) = Na+ (aq) + OH- (aq)
Neutralisation = H+ (aq) + OH- (aq) = H^2O (l)
To name a salt, we take the firstname of the metal in the base and the name of the acid used:
Hydrochloric Acid = Chloride
Nitric Acid = Nitrate
Sulfuric Acid = Sulfate
Insoluble salts can be made by reacting two solutions to produce a percipitate.
Percipitaion is an important way of removing some metal waste ions from industrial waste water
Making a salt from an acid and an insoluble base =
* Neutralisation --> Filtration --> Evaporation
Electrolysis = The process by which ionic substances are broken down into simpler substances using electricity.
Ionic substances form when a metal reacts with a non-metal.
The metal atoms become positive ions and the non-metal atoms become negative ions.
Electrolysis splits up a substance and elements are produced.
The ions need to be free to move about, so the substance needs to be in molten liquid state or in solution dissolved in water.
The electrolysis liquid is called the electrolyte.
Electrodes = Cathode (negative) and Anode (positive)
Cathode - Positively charged ions move to the cathode. They RECIEVE electrons and so are REDUCED.
Anode - Negatively charged ions move to the anode. They LOSE electrons so are OXIDISED.
Electrolysis - Part 2
The ions become atoms again.
The least reactive ions come out at the cathode.
If the metal we have is less reactive than Hydrogen, then it is the metal we get.
Least reactive = Product.
The Chlor-Alkali Industry & The Extraction of Alum
The Chlor-Alkali Industry
When we electrolyse Brine, we get three products, Chlorine gas (positive electrode), Hydrogen gas (negative electrode) and Sodium hydrxide solution.
The products are important reactants used in industry:
> Hydrogen - Margarine, Hydrochloric Acid
> Sodium Hydroxide - Soap, Paper, Bleach
> Chlorine - Bleach, Kill bacteria, Disinfectants
The Extraction of Aluminium
Aluminium oxide is electrolysed to manufacture aluminium.
Molten cryolite is used to reduce the temperature needed for the process.
The positive Carbon electrodes are often replaced as they gradually burn away.