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level: Level 1 of Definitionsd

Questions and Answers List

level questions: Level 1 of Definitionsd

QuestionAnswer
Isotopeatoms of the same element with the same number of protons and electrons but different numbers of neutrons. Isotopes of an element have different masses
Relative Isotopic massthe mass of an atom of an isotope compared with 1/12th mass of an atom of carbon-12.
Relative atomic masshe weighted mean mass of an atom compared with 1/12th mass of an atom of carbon-12.
AcidProton donor
Baseproton acceptor
AlkalineProton acceptor which Releases hydroxide ions in solution
1st ionisation energyThe energy required to remove one electron from one mole of gaseous atoms to form one mole of 1+ gaseous ions. E.g M(g) à M+(g) +e-
2nd ionisation energyThe energy required to remove one electron from one mole of gaseous atoms to form one mole of 1+ gaseous ions. E.g M(g) à M+(g) +e-
Ionic bondingthe strong electrostatic force of attraction between (positively and negatively) oppositely charged ions
Covalent bondThe electrostatic attraction between a shared pair of electrons and the nuclei on bonding atoms.
Metallic bondingThe electrostatic attraction between a shared pair of electrons and the nuclei on bonding atoms.
ElectronegativityThe ability of an atom to attract a pair of electrons in a covalent bond.
Disproportionationis a redox reaction in which the same element is both oxidised and reduced simultaneously.
Enthalpy change of combustionEnthalpy change when reacting one mole of a substance completely with oxygen under standard conditions with everything in standard state.
Enthalpy change of formationEnthalpy change when forming one mole of a substance from its constituent elements.
Enthalpy change of neutralisationReaction of acid and base to form one mole of water.
Bond enthalpyBreaking of 1 mol of bonds in gaseous molecules
CatalystSpeeds up a reaction lowers activation energy provides and alternative pathway
Activation energythe minimum amount of energy needed to start a reaction
Homologous seriesseries of organic compounds having the same functional group but with each successive member differing by CH2)
Homolytic bond fissioneach bonding atom receiving one electron from the bonded pair, forming two radicals when a covalent bond is broken
Heterolytic fissionone bonding atom receiving both electrons from the bonded pair when a covalent bond is broken
RadicalA species with an unpaired electron
Curly arrowmovement of a pair of electrons
Structural isomerMolecule with same molecular formula but different structural formula.
StereoisomerSame structural formula but different arrangement of atoms in a space
Sigma bondoverlaps of orbitals directly between the bonding atoms
Pi bondsideways overlap of adjacent p-orbitals above and below the plane of bonding atoms
ElectrophileElectron pair acceptor
Nucleophileelectron pair donor
Mole fractionmole fraction = moles of component /total moles
Partial pressurepp= mole fraction x total pressure
Difference between Monobasic acid and Dibasicm=acid which donates 1 proton d= donates 2 protons
PHph= -log[H+}
pkapka= -log[ka]
BufferSubstance which minimises and resists the change in pH formed from a weak acid and conjugate bas
Lattice enthalpyenthalpy change when forming 1 mole of ionic lattice from its gaseous ions
Enthalpy of hydrationenthalpy change when 1 mole of gaseous ion dissolves in water to form aq ions
Enthalpy of solutionenthalpy change when 1 mole of an ionic compound dissolves in water molecules
Entropydisorder in system
oxidising agentspecies which is reduced when oxidising another species
Reducing agentspecies which is oxidised when reducing another species
Standard electrodeAbility to be oxidised or reduced compared to hydrogen electrode
Transition elementsforms at least one ion with a partially filled d orbitals
Monodentate ligandDonates one pair of electrons to Forms 1 co-ordinate bond with a central metal ion
Bidentate ligandDonates two pair of electrons to Forms 2 co-ordinate bond with a central metal ion
Complex ionIon formed from a central metal ion and multiple co-ordinate bonds from ligands