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Flashcards

Chemistry As Deffinitions

20257291 Chemistry AS - Level English 67 cards

Cards in this deck (67)

  1. 1Atomic NumberThe number of protons in the nucleus of an atom.
  2. 2Mass NumberThe number of neutrons and protons in the nucleus of an atom.
  3. 3Relative atomic massThe weighted mean mass of an atom of an element compared to 1/12 the mass of an atom of C-12.
  4. 4Relative isotopic massThe mass of an atom of an isotope compared to 1/12 the mass of an atom of C-12.
  5. 5IsotopeAtoms of the same element with a different number of neutrons.
  6. 6MoleThe amount of substance containing as many particles as there are Carbon atoms in exactly 12g of C-12.
  7. 7Avogadros ConstantThe number of particles per mole of a substance. (6.02x10 23)
  8. 8Molar massThe mass in g per mole of a substance. Units gmol-1.
  9. 9Water of crystallisationThe water present in a compound giving the compound a crystalline appearance.
  10. 10AnyhydrousWhen all the water of crystallisation has been removed from a compound.
  11. 11HydratedWhen water of crystallisation is present in a compound.
  12. 12AcidReleases H+ ions in solution (proton donor).
  13. 13BaseProton Acceptor.
  14. 14AlkaliA soluble base that releases OH- ions when in solution.
  15. 15Oxidation NumberA measure of the number of electrons that an atom uses to bond with atoms of a different element.
  16. 16OxidationThe loss of electrons / increase in oxidation number (state).
  17. 17Oxidation AgentA reagent which oxidises another species but itself gets reduced.
  18. 18ReductionThe gain of electrons / decrease in oxidation number (state).
  19. 19Reduction AgentA reagent which reduces another species and itself gets oxidised.
  20. 20RedoxA reaction where both oxidation and reduction takes place.
  21. 21Displacement ReactionA reaction in which a more reactive element displaces a less reactive element from an aqueous solution of its halide ions.
  22. 22Empirical FormulaThe simplest whole number ratio of atoms of each element present in a compound.
  23. 23Molecular FormulaThe actual number of atoms of each element in a molecule.
  24. 24DisproportionationA reaction in which an element is simultaneously oxidised and reduced.
  25. 25Atomic OrbitalA region within an atom that can hold up to two electrons, with opposite spins.
  26. 26s/p/d Block ElementHighest energy sub-shell is a s/p/d sup-shell.
  27. 27Ionic BondThe electrostatic attraction between oppositely charged ions.
  28. 28Covalent BondThe sharing of a pair of electrons between two atoms.
  29. 29Dative (co-ordinate) BondThe sharing of a pair of electrons between two atoms where only one of the atoms supplies both the electrons shared.
  30. 30ElectronegativityThe ability of an atom to attract the bonding electrons towards itself in a covalent bond.
  31. 31Metallic BondingThe attraction of positive metal ions to delocalised electrons.
  32. 32PeriodicityThe repeating pattern of trends across different periods.
  33. 33Hydrogen BondA dipole-dipole attraction between a slightly positive hydrogen on one molecule and a lone pair of electrons on a highly electronegative atom (N,O,F) of another molecule.
  34. 34First Ionisation EnergyThe energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions. Units are kJmol-1.
  35. 35Successive Ionisation EnergyA measure of the energy required to remove each electron in turn.
  36. 36HydrocarbonA compound of hydrogen and carbon only.
  37. 37Homologous seriesA series of organic compounds having the same functional group but with each successive member differing by CH2.
  38. 38Functional GroupA group of atoms responsible for the characteristic reactions of the compound.
  39. 39SaturatedContaining single bonds only.
  40. 40UnsaturatedContaining at least one carbon to carbon multiple bond.
  41. 41Structural IsomersCompounds with the same molecular formula but with different structural formulae.
  42. 42StereoisomersCompounds with the same structural formula but with a different arrangement of the atoms in space.
  43. 43E/Z IsomerismAn example of stereoisomerism, in terms of restricted rotation about a double bond and the requirement for two different groups to be attached to each carbon of the C=C group.
  44. 44Cis-trans IsomerismA special case of E/Z isomerism in which two of the substituent groups are the same.
  45. 45Fractional DistillationSeparation of a liquid mixture into fractions with different boiling points
  46. 46Catalytic CrackingThe breaking down of long chained saturated hydrocarbons to form more useful alkanes ( shorter chained) and alkenes.
  47. 47BiofuelA fuel that is derived from recently living material such as plants or from the waste of animals.
  48. 48'Curly Arrow'The movement of an electron pair, showing either the breaking or formation of a covalent bond.
  49. 49Homolytic FissionThe breaking of a covalent bond where the shared pair of electrons are split equally, forming two radicals.
  50. 50Heterolytic FissionThe breaking of a covalent bond where the shared pair electrons are not equally, forming a cation and an anion.
  51. 51ElectrophileSpecies attracted to an electron rich centre where it accepts a pair of electrons to form a new covalent bond.
  52. 52NucleophileA species attracted to an electron deficient centre where is donates a pair of electrons to form a new covalent bond.
  53. 53RadicalA species with an unpaired electron.
  54. 54ExothermicHeat is given out to the surroundings (the reactants lose energy).
  55. 55EndothermicHeat is taken in from the surroundings (the reactants gain energy).
  56. 56Activation EnergyThe minimum energy required to start a reaction by the breaking of bonds.
  57. 57Standard ConditionsA pressure of 100kPa (1 atmosphere), a stated temperature, usually 298K (25'C) and a centration of 1.0moldm-3 (for ractions with aqueous solutions).
  58. 58(Standard) Enthalpy change of reactionThe enthalpy change that accompanies a reaction in the molar quantities expressed in a chemical equation (under standard conditions, all reactants and products being in the standard states).
  59. 59(Standard) Enthalpy change of formationThe enthalpy change that takes place when one mole of a compound is formed from its constituent elements (under standard conditions, all reactants and products being in their standard stateds).
  60. 60(Standard) Enthalpy change of combustionThe enthalpy change that takes place when one mole of a substance reacts completely with oxygen (under standard conditions, all reactants and products being in their standard states).
  61. 61Average bond enthalpyThe average enthalpy change that takes place when breaking, by homolytic fission, 1 mole of a given type of bond in the molecules of a gaseous species.
  62. 62CatalystSpeeds up a reaction without being consumed by the overall reaction.
  63. 63VolatilityThe ease that a liquid turns into a gas (increases as boiling point decreases).
  64. 64Dynamic EquilibirumThe equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction.
  65. 65Le Chatelier's PrincipleThen a system in dynamic equilibrium is subjected to change, the position of equilibrium will shift the minimise the change.
  66. 66Atom Economy(Molecular mass desired product / Molecular mass sum of products ) x 100
  67. 67SaltA compound produced when a H+ ion from an acid is replaced by a metal or another positive ion such as the ammonium ion NH4.

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AS - Level Chemistry Flashcards on Chemistry As Deffinitions, created by 20257291 on 02/12/2015.
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