atoms of the same element with a different number of neutrons
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relative atomic mass
the average mass of one atom of an element compared to one twelfth of the mass of an atom of carbon-12.
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relative isotopic mass
the mass of an atom of an isotope compared to one twelfth of the mass of an atom of carbon-12.
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relative molecular mass
the average mass of one molecule compared to one twelfth of the mass of an atom of carbon-12.
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first ionisation energy
the energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions
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second ionisation energy
the energy needed to remove 1 electron from each atom in 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions
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standard solution
a solution you know the exact concentration of
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theoretical yield
the mass of product that should be formed in a chemical reaction (assumes no chemicals are lost)
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percentage yield
how wasteful a process is
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atom economy
a measure of the proportion of reactant atoms that become part of the desired product
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electrostatic attraction
holds positive and negative ions together
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electronegativity
an atoms ability to attract the electron pair in a covalent bond
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hydrogen bonding
the intermolecular force which occurs when hydrogen is covalently bonded to fluorine, nitrogen, or oxygen
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standard enthalpy change
the heat energy transferred in a reaction at constant pressurewith standard states under standard conditions (KJ/mol)
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standard enthalpy change of formation
the enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions
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standard enthalpy of combustion
the enthalpy change when 1 mole of a substance is completely burned in oxygen under standard conditions
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specific heat capacity
the amount of heat energy it takes to raise 1g of a substance by 1 Kelvin
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hess's law
the total enthalpy change is independent of the route taken
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reation rate
the change in concentration of reactant or product over time
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collision theory
a reaction won't take place unless particles collide at the correct orientation and with kinetic energy exceeding the activation energy
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activation energy
the minimum amount of kinetic energy that particles need to react
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dynamic equillibrium
the concentrations of reactants and products stay constant
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le chaelier's principle
if you change the conditions of a reversible reaction, the equilibrium position will move to counteract the change
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oxidation
reduction
disproportionation
oxidation is the loss of electron
reduction is the gain of electrons
disproportionation is when a species is both oxidised and reduced in the same reaction
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oxidation states
the total number of electrons donated or accepted
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oxidising agent
reducing agent
oxidising agent accepts electrons and is reduced
reducing agent donates electrons and is oxidised
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dative covalent bond
a covalent bond in which both electrons shard come from the same atom
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dative covalent bond
a covalent bond in which both electrons shard come from the same atom
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ligand
an atom, ion or molecule that donates a pair of electrons to the central transition metal ion to form a dative covalent bond
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a complex
a complex is a central metal atom surrounded by dative covalently bonded ligands
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Other cards in this set
Card 2
Front
the average mass of one atom of an element compared to one twelfth of the mass of an atom of carbon-12.
Back
relative atomic mass
Card 3
Front
the mass of an atom of an isotope compared to one twelfth of the mass of an atom of carbon-12.
Back
Card 4
Front
the average mass of one molecule compared to one twelfth of the mass of an atom of carbon-12.
Back
Card 5
Front
the energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions
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