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| Pregunta | Respuesta |
| Definitions As | Definitions for As Chemistry |
| UNIT 1 | ...... |
| Amount Structure | ...... |
| Atomic Number | Number of protons in the nucleus of an atom |
| Mass Number | Total number of the protons and neutrons in the nucleus of one atom of an element |
| 1st Ionisation Energy | Is the energy required to remove one mole of electrons from one mole of gaseous atoms |
| 2nd Ionsation energy | The energy required to remove one mole of electrons from one mole gaseous +1ions |
| Amount of substance | .... |
| Relative atom mass | The average mass of an atom of an element compared to one-twelfth of the mass of an atom of carbon-12 |
| Relative molecular mass | The mass of one molecule of the compound relative to one-twelfth of the mass of an atom |
| Mole | The amount of substance in grams that contains as many particles (atoms, molecules, ions, electrons) as there are atoms in 12 g of carbon 12 |
| Avogadro Constant | Is the number of particles in one mole of any substance. It is equal to 6.023x10 23 |
| Molar Mass | The mass of one mole of an element or a compound |
| Molarity | The concentration of a solution with units of mol dm-3 |
| Empirical Formula | The simplest whole number ratio of atoms of each element in a compound |
| Molecular Formula | The actual number of atoms of each element in a compound |
| Bonding | ..... |
| Ionic Bonding | Electrostatic force of attraction between two oppositely charged ions in a lattice. Ions are formed by electron transfer |
| Covalent Bonding | Atoms bound by a shared pair of electrons |
| Co-ordinate Bonding | Dative covalent bonding where the shared pair of electrons in a covalent bond is donated by a single atom |
| Metallic bonding | electrostatic forces of attraction between cations in a lattice and the de-localised electrons between them |
| Dipole-Dipole | The intermolecular forces between two polar molecules |
| Van Der Waals (Induced Dipole-Dipole or London forces) | The intermolecular forces between non-polar molecules e.g. Cl-Cl |
| Hydrogen Bonding | The intermolecular bonding between Hydrogen and either Oxygen, Fluorine or Nitrogen through the electrostatic attraction between the unshielded hydrogen proton and the lone pair on each of O, F or N |
| Electronegativity | The relative attraction atoms have for the shared pair of electrons in a covalent bond |
| Intro to Organic Chem | ...... |
| Functional Group | Is an atom or group of atoms that gives the organic compound its characteristic chemical properties |
| Homologous Series | A series of compounds of similar structure in which each member differs from the next by a common repeating unit, CH2 |
| Positional Isomerism | The molecular formula and functional group are the same, but the position of the functional group is different |
| Chain Isomerism | The molecular formula and functional group are the same, but the arrangement of the carbon atoms is different |
| Functional Group Isomerism | The molecular formula is the same, but the functional group is different |
| Chain Isomerism (Branch chain isomers) | The molecular formula is the same, but the hydrocarbon chain is arranged differently |
| Structural Isomerism | The same molecular but the structural formula is different |
| Alkanes | .... |
| Saturated Hydrocarbon | A hydrocarbon that contains single bonds only |
| Unsaturated Hydrocarbon | A hydrocarbon that contains at least one carbon-carbon double bond |
| UNIT 2 | ...... |
| Energetics | ........ |
| Hess' Law | If a reaction may occur by more than one route the energy change is the same regardless of the route taken |
| Mean Bond Enthalpy | The energy required to break one mole of covalent bonds between two given atoms averaged across a range of compounds |
| Kinetics | ............ |
| Activation Energy | Activation energy is the minimum energy required for a reaction to occur |
| Catalyst | A catalyst is a substance that speeds up a chemical reaction but is itself unchanged at the end of the reaction |
| First Law of Thermodynamics | Energy can be neither created nor destroyed but it can be converted from one form to another |
| Standard Enthalpy Changes | Standard enthalpy changes refer to energy changes under conditions of constant pressure |
| The standard enthalpy of formation | The standard enthalpy of formation is the enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions |
| Standard enthalpy of combustion | The enthalpy change when 1 mole of a substance is completely burned in oxygen under standard conditions |
| Standard enthalpy of neutralisation | The enthalpy change when 1 mole of water is formed when an acid neutralises an alkali under standard conditions |
| Equilibra | ......... |
| Le Chatelier's Principle | The equilibrium position will shift to oppose any change in conditions |
| Dynamic Equilibrium | Equilibrium where the reaction is: continuous in both directions, same rate when the reaction is both forward and backwards and has relative concentrations of reactants and products that remain constant |
| Redox | .......... |
| Oxidation State | The hypothetical charge on an atom in a species when that species, irrespective of the nature of bonding, is regarded as totally ionic |
| Oxidising Agent | Electron Acceptors |
| Reducing Agents | Electron Donors |
| Oxidation | Oxidation is loss of electrons |
| Reduction | Is the gain of electrons |
| Halogens | ........ |
| Disproportionation | A reaction in which a species becomes both oxidised and reduced |
| Haloalkanes | .................... |
| Homolytic Fission | The electrons from a covalent bond are shared when the bond breaks |
| Free radical | A reactive intermediate which results from homolytic fission |
| Nucleophile | A species that can donate a lone pair of electrons on bond formation |
| Electrophile | An electron deficient species which accepts a pair of electrons on bond formation |
| Alkenes | .............. |
| Positional Isomerism | The molecular formula are the same, but the position of the double bond is different |
| Stereoisomerism | The same molecular and structural formula, but a different orientation in space |
| Geometric Isomers | The two stereoisomers have the structural formula but the bonds are arranged differently in space |
| Carbocation | A very reactive intermediate with a positive change on a carbon atom |
| Alcohols | ................ |
| Biofuel | A fuel derived or produced from renewable biological sources |
| Analytical Techniques | ...................... |
| Molecular ion | An ion formed in mass spectrometer which is the result of ionisation, but not fragmentation of the molecule |
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