Steel
Properties of Alloy: -Iron and carbon (elements) -Hard -High tensile strength
Brass
Properties of Alloy: -Copper and zinc (elements) -Lustrous gold appearance -Hard but easily machined
Solder
Properties of Alloy: -Tin and lead -Low melting point -Adheres firmly to other metals when molten
Reduction
Process: To turn a metal oxide into pure metal involves the removal of the oxygen from the metal oxide
Electrolysis
Chemical decomposition produced by passing an electric current through a liquid or solution containing ions.
Alloy
Is a mixture of more than one metal to produce a material with specific physical and chemical properties
Particle theory
All matter is made of continuously moving particles
Law of conservation
Matter can be changed from one form into another, mixtures can be separate or made, and pure substances can be decomposed but the total mass remains constant.
Delocalised Electron
An electron that has left its outer shell
Isotopes
All atoms of the same element have the same number of protons in the nucleus, however they do not necessarily have the same mass. These atoms differ in the numver of neutrons and therefore mass number
Lewis dot structure
A way of representing the valence electron configuration of an atom and show how valence electrons are arranged in compounds
Ionisation energy
The amount of energy required to remove the most losely bound electron from an atom or ion in the gaseous state
Covalent network
Properties of bond:
very high M.P and B.P
Non-conductors -Extremely hard
Solute
A substance dissolved in another substance, usually the component of solution present in the lesser amount
Solvent
A substance in which another substance is dissolved, forming a solution
Solution
A homogeneous mixture of two or more substances, which may be solids, liquids, gases, or a combination of these
Density
Mass/ volume
Fossil fuels
Are formed when dead and decaying material burns before complete decomposition
Coal
Often formed in swamps and mangroves
Petroleum
Mostly formed from the remains of buried aquatic organisms (e.g. plankton) broken down by anaerobic bacteria
Natural gas
Mostly the remains of buried aquatic organisms
Catalyst
A substance that speeds up a chemical reaction, but is not consumed by the reaction hence a catalyst can be recovered chemically unchanged at the end of the reaction
Hydrogen bonding
Occurs between hydrogen atoms and unshared pairs of electrons of N, O or F atoms- resulting in an unequal sharing of electrons leading to a partial positive charge on the H-atoms
Alkanes
Single bond
Alkenes
Double bond
Alkynes
Triple bond
Distillation
It works by evaporating tone of the liquid from the solution, it is then cooled and condensed into a separate container and the other liquid is left behind
Viscosity
The resistance of a liquid to flow- it increases with stronger intermolecular forces and decreases with higher temperatures
Saturated solution
A solution in which the maximum amount of a solvent has been dissolved. Once this is achieved an equilibrium is established
Small molecule
Properties of a type of molecule:
Low B.P
Very volatile
Flows easily
Ignites easily
Large molecule
Properties of a type of molecule:
High B.P
Not very volatile
Does not flow easily
Does not ignite easily
Isomers
Compounds with the same molecular formula but different structural arrangements are known as structural isomers
Induced intermolecular forces
When a charge on one object distorts the distribution of charge on a nearby object, producing an induction of charge and a force of attraction between the two objects e.g. rubbing a balloon on your skirt causes static in your hair
Ion-induced intermolecular forces
The result of an ion distorting the electron density of a non-polar molecule
Polarisability
The relative tendency of a charge distribution to be distorted from its normal shape by an external field
Dispersion forces
The weakest kind of intermolecular attraction and occurs between molecules- they are caused by the motion of electrions
Homologous series
Same pattern & similar formula- it is like the same molecule that is getting bigger
Oxidation
loss of electrons to become a positive ion
Bohr's model
Theory for the atom: o The nucleus is the central part of the atom that contains protons and neutrons o The electrons move through a relatively large space outside the nucleus in shells o The electrons are kept moving around the nucleus by electrostatic charges between the positively charged nucleus and negatively charged electrons
Atomic radius
-Increase down a group as each successive element has one more electron shell- due to additional energy levels -Decrease left to right as more electronegative, the charge in the nucleus increase so the electrostatic force between the nucleus and the outer electrons is stronger holding it closer to the nucleus
Electronegativity
-Increases across a period as atomic radius decreases -Decreases down a group as atomic radius increases
Ionisation energy
-Increases from left to right as more electronegative -Decreases down a group as less electronegative (electrons further away from nucleus)
Mendeleev
Developed a table of the elements based on increasing atomic weight
Gay-Lussac
"When measured at constant temperature and pressure, the volumes of gases taking part in a chemical reaction show simple whole number ratios to one another."- theory
Avogadro
"When measured at the same temperature and pressure, equal volumes of gases contain the same number of molecules." - Law
Mineral
A natural substance occurring in the Earth's crust, which is a compound (hence pure) with a definite composition and crystalline structure e.g. Al2O3
Ore
A compound or mixture of compounds (or minerals) from which it is economic to extract a substance such as a metal e.g. bauxite (contains mineral Al2O3)
Polar molecule
A molecule in which there is an uneven charge distribution
Dipole-dipole interaction
Occurs between oppositely charged ends of permanent polar
Adhesive forces
(attraction between unlike molecules) pulls the molecules inward and closer together, making the liquid surface behave like an elastic skin under tension.
Cohesive forces
(attractive forces between like molecules) cause the droplet to assume a spherical like shape to minimise the surface area.
Surface tension
Is a measure of the energy needed to increase the surface area of a liquid by a unit amount.
Precipitation
An insoluble ionic compound formed as a solid in solution from solutions of two soluble ionic compounds
Precipitation reaction
Occurs when the force of attraction between the two ions is stronger than the electrostatic attraction between the water molecules and the ions
Equilibrium
A dynamic situation in a closed system, where there is continual interchange between reactants and products in a reaction at the atomic level but with no observable change at the macroscopic level
Concentration
The amount of a given substance dissolved in a specified amount of solution
Specific heat capacity
The heat needed to raise the temperature of 1 unit mass of a substance by 1 Kelvin Degree
Exothermic dissolution
A chemical dissolves in water and heat is released causing a temperature rise
Dissolution
The action or process of dissolving
Endothermic dissolution
A chemical dissolves in water and heat is absorbed causing a drop in temperature
Thermal pollution
The discharge into a river or lake of quantities of hot water that are large enough to increase significantly the temperature of the water body
Corrosion
Metal + Oxygen --> metal oxide
Combustion
Fuel + oxygen ---> carbon dioxide + water
Respiration
Glucose + oxygen ---> carbon dioxide + water
Precipitation
Soluble salt + soluble salt ---> insoluble salt + soluble salt
Neutralisation
Acid + Base ---> salt + water
Gravimetric analysis
Is used to determine the mass and/ or percentage of different components in a sample (usually a mixture)
Desalination
the process of removing dissolved salts and minerals from seawater or brackish water. It is also called desalting or by its shortened name, desa
Copper
Can be used for electrical wires because they are generally ductile and good conductors of electricity
Liquids
The particles have more space between them and have translational and vibrational motion (vibrate slightly and fill up what its contained in)
Gases
The particles have a lot of energy, they don't interact with each other as much and have rapid translational motion
Solids
The particles are orderly arranged and closely packed- because the particles are closely packed together in solids than in liquids, solids have greater densities (with the exception of water and ice)
Mass number
protons + neutrons
Atomic weight
Protons= electrons
Ion
A charged particle formed when an atom gains or loses one or more electrons
Covalent bonds
Are formed between two of more atoms sharing electrons
Physical change
Do not involve the production of new substances, and are reversible
Chemical change
form one or more new chemical substances
Metallic bonding
Occurs between metals and involves the electrostatic attraction between delocalised electrons and the metal cations, which hold the 3D lattice together.
Ionic bonding
Involves the transfer of electrons from one atom to another. The bonding consists of electrostatic attraction between the positive and negative ions formed by this transfer of electrons, which hold the 3D lattice together.
Empirical formula
Is the simplest form of a compound and represents the simplest whole number ratio of atoms/ions in the crystal.
Ionic bonds
Properties:
High melting and boiling points. Hard. Crystalline
Good electrical conductors when molten
Good electrical conductors when in solution
Poor electrical conductors when in solid.
Covalent molecular
Properties:
Poor conductors of electricity in all states
Not hard
Covalent network
Properties:
Poor conductors electricity in all states
Hardness
Metallic bonds
Properties:
Good conductor of electricity
High melting and boiling points. Hard
Good conductor of heat
Malleable and ductile
Shiny lustre
Immiscible
When they are mixed, they do not form a homogeneous liquid, but instead stay as drops of one liquid dispersed through the other liquid
Allotropes
Are forms of the one element (in the same physical state) that have distinctly different physical properties
Volatility
The ease with which it can be converted to a vapour; it decreases as boiling point increases
Activation energy
Is the minimum amount of energy reactant molecules must possess in order to form products (kJ/mol), on an energy profile diagram, it is the space between the reactants and the peak