Terms & Definitions in Advanced Subsidiary Chemistry

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  • Created by: K.T.1998
  • Created on: 07-10-16 11:25
Relative Atomic Mass
The weighted average mass of naturally occurring atoms of an element on a scale where an atom of carbon-12 has a mass of exactly twelve units.
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Relative Isotopic Mass
The mass of a particular isotope of an element on a scale where an atom of carbon-12 has a mass of exactly twelve units.
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Formula Mass
The mass of one formula unit of a compound measured on a scale on which an atom of the carbon-12 isotope has a mass of exactly twelve units.
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Empirical Formula
The formula that tells us the simplest ratio of the different atoms present in a molecule.
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Molecular Formula
The formula that tells us the actual numbers of each type of atom in a molecule.
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Mole
The amount of a substance that has the same number of specific particles as there are atoms in exactly twelve grams of the carbon-12 isotope.
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Bond Energy
The energy needed to break one mole of a particular bond in one mole of gaseous molecules.
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Bond Length
Average distance between the nuclei of two bonded atoms in a molecule.
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Enthalpy Change of Reaction
The standard enthalpy change when the amounts of reactants shown in the equation react to give products under standard conditions.
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Enthalpy Change of Formation
The standard enthalpy change when one mole of a compound is formed from its elements under standard conditions.
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Enthalpy Change of Combustion
The standard enthalpy change when one mole of a substance is burnt in excess oxygen under standard conditions.
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Enthalpy Change of Hydration of an Anhydrous Salt
The standard enthalpy change when one mole of a hydrated salt is formed from one mole of the anhydrous salt under standard conditions.
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Enthalpy Change of Solution
The standard enthalpy change when one mole of solute is dissolved in a solvent to form an infinitely dilute solution under standard conditions.
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Enthalpy Change of Neutralisation
The standard enthalpy change when one mole of water is formed by the reaction of an acid with an alkali under standard conditions.
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Enthalpy Change of Atomisation
The standard enthalpy change when one mole of gaseous atoms is formed from its element in their standard state under standard conditions.
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Reversible Reaction
A reaction in which products can be changed back to reactants by reversing the conditions.
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Dynamic Equilibrium
In an equilibrium mixture, molecules of reactants are being converted to products at the same rate as products are being converted to reactants.
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Le Chatelier's Principle
When any of the conditions affecting the position of equilibrium are changed, the position of that equilibrium shifts to minimise the change.
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Rate of Reaction
The measure of a rate at which reactants are used up or the rate at which products are formed.
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Activation Energy
The minimum energy required in order for a reaction to take place.
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Catalyst
Substance that increases the rate of a reaction but remains chemically unchanged itself at the end of a reaction.
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Other cards in this set

Card 2

Front

The mass of a particular isotope of an element on a scale where an atom of carbon-12 has a mass of exactly twelve units.

Back

Relative Isotopic Mass

Card 3

Front

The mass of one formula unit of a compound measured on a scale on which an atom of the carbon-12 isotope has a mass of exactly twelve units.

Back

Preview of the back of card 3

Card 4

Front

The formula that tells us the simplest ratio of the different atoms present in a molecule.

Back

Preview of the back of card 4

Card 5

Front

The formula that tells us the actual numbers of each type of atom in a molecule.

Back

Preview of the back of card 5
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