A reaction that takes in heat from its surroundings.
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Exothermic
A reaction that gives out heat.
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Enthalpy Change
A heat change at constant pressure.
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Standard Enthalpy of Formation
The enthalpy change when one mole of substance is formed from its constituent elements under standard conditions, with all reactants and products in their standard states.
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Standard Enthalpy of Combustion
The enthalpy change when one mole of substance is completely burned in oxygen under standard conditions, with all reactants and products in their standard states.
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Hess's Law
This states that the enthalpy change for a chemical reaction is the same, whatever route is taken from reactants to products.
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Bond Enthalpy
The enthalpy change required to break a covalent bond with all species in the gaseous state.
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Kinetics
The study of the factors that affect rates of chemical reactants - how quickly they take place.
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Collision Theory
Most collisions between molecules or other particles do not lead to reaction. They either do not have enough energy, or they are in the wrong orientation.
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Activation Energy
The minimum energy needed to start a reaction.
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Catalyst
A substance that affects the rate of chemical reactions without being chemically changed themselves.
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Heterogeneous Catalyst
A catalyst which is in a different phase to the reactants.
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Homogeneous Catalyst
A catalyst which is in the same phase as it's reactants.
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Catalytic Converter
A honeycomb made of a ceramic material and covered with platinum and rhodium metal - the catalysts.
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Dynamic Equilibrium
A situation in which the composition of a reaction mixture does not change because both forward and backward reactions are proceeding at the same rate.
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Maxwell-Boltzmann Distribution
The distribution of energies (and therefore speeds) of the molecules in a gas or liquid.
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Equilibrium Mixture
In a reversible reaction as soon as the products are formed they react together to form the reactants again, leading to a mixture of both reactants and products. Eventually a mixture is obtained in which all three components remain constant.
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Le Châtelier's Principle
If a system at equilibrium is disturbed, the equilibrium moves in the direction that tends to reduce the disturbance.
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OILRIG
Oxidation is Loss (of electrons), Reduction is Gain (of electrons).
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Oxidation State
In an ionic compound this tells us how many electrons it has lost or gained, compared with the element in its uncombined state.
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Electronegativity
A measure of the ability of an atom to attract electrons towards itself within a covalent bond.
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Nucleophile
Reagents that attack and form bonds with positively charged carbon atoms.
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Alkene
An unsaturated hydrocarbon.
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Alkane
A saturated hydrocarbon.
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Structural Isomer
Compounds with the same molecular formula but a different structural formula.
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Positional Isomer
Two or more molecules with the same molecular formula but the functional group is in a different place. E.G CH3CH2CH2Cl and CH3CHClCH3
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Functional Group Isomer
Two or more molecules with the same molecular formula but a different functional group. E.G CH3CH2OH and CH3OCH3
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Chain Isomer
Two or more molecules with the same molecular formula but a different hydrocarbon chain.
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Other cards in this set
Card 2
Front
A reaction that gives out heat.
Back
Exothermic
Card 3
Front
A heat change at constant pressure.
Back
Card 4
Front
The enthalpy change when one mole of substance is formed from its constituent elements under standard conditions, with all reactants and products in their standard states.
Back
Card 5
Front
The enthalpy change when one mole of substance is completely burned in oxygen under standard conditions, with all reactants and products in their standard states.
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