AS level Chemistry OCR new Spec Definitions (Physical and Inorganic Chemistry) – Flashcards
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Relative Isotopic Mass
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mass of an isotope compared to 1/12th the mass of a carbon-12 atom
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Relative Atomic Mass
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weighted mean mass of an atom compared to 1/12th the mass of a carbon-12 atom
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1st Ionisation Energy
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energy required to remove one mole of electrons from one mole of gaseous atoms
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Common Acids
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HCl, H2SO4, HNO3, CH3COOH
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Common Alkalis
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NaOH, KOH and NH3
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Acid
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releases H+ in aqueous solution
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Alkali
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releases OH- in aqueous solution
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Strong Acids
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fully disassociated in solution
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Weak Acid
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partially disassociated in solution
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Salts
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ionic compound formed when the H+ ion in acids are replaced by metal or ammonium ions
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Amount of Substance
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means of counting the quantity of any species with unit of moles
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Mole
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amount of any substance containing as many elementary particles as there are carbon atoms in 12g of carbon-12
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Avogadro's Constant
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6.02 X 10^23 particles
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Molar Mass
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mass per mole of a substance
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Empirical Formula
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simplest whole number ratio of atoms of each element present in a compound
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Molecular Formula
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number and type of atoms of each element in a molecule
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Anhydrous
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containing no water molecules
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Hydrated
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a crystalline compound containing water molecules
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Water of Crystallisation
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water molecules that are bonded into a crystalline structure of a compound
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Ionic Bonding
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electrostatic attraction between positive and negative ions
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Covalent Bonding
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electrostatic attraction between a shared pair of electrons and the bonding nuclei
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Metallic Bonding
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strong electrostatic attraction between cations and delocalised electrons
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Electronegativity
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ability of an atom to attract the bonding electrons in a covalent bond
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Polar Bond/Permanent Dipole
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covalently bonded atoms with different electro-negativities
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Periodicity
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repeating trends in physical and chemical properties across periods
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Disproportionation
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oxidation and reduction of the same element
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Endothermic
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the ∆H is positive, as bond breaking absorbs energy from the surroundings
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Exothermic
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the ∆H is negative, as bond making releases energy into the surroundings
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Activation Energy
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the minimum energy required for a reaction to take place
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∆fH
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energy required to form one mole of a compound from its constituent elements
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∆cH
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energy required for one mole of a substance to react completely with oxygen
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∆neutH
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energy required to form one mole of water from a neutralisation reaction
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Average Bond Enthalpy
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breaking of one mole of bonds in gaseous molecules
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Homogeneous Catalyst
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same physical state as reactants
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Heterogeneous Catalyst
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different physical state to reactants
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Dynamic Equilibrium
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when the rate of the forwards reaction is the same as the rate of the reverse reaction in a closed system (concentration doesn't change)
