Chemistry C1 (Definitions)

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  • Created by: Zoe Fox
  • Created on: 09-01-13 16:50
Atomic Number
Number of PROTONS in the nucleus.
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Mass Number
Number of protons AND neutrons in the nucleus.
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Half-Life
The time taken for half of a radioactive isotope to decay
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1st Ionisation Energy
The energy required to remove 1 electron from each atom in 1 mole of GASEOUS atoms of an element to form 1 mole of GASEOUS positive ions.
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Equation of 1st ionisation energy
A(g) --------> A+(g) + E-(g)
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Reversible reaction
A reaction which will proceed both forwards and backwards according to the reaction equation.
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Dynamic Equillibrium
The equillibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the backward reaction.
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Le Chateliers Principle
If a system is at equilibrium and a change is made to any of the conditions, the equilibrium posiion will change to reduce the effect of the change.
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Acid
Proton Donor
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Base
Proton Acceptor
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Alkali
A type of base that dissolves in water forming hydroxide ions. (OH-)(aq)
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Enthalpy
The heat content which is stored in the chemical system
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Chemical System
The reactants and the products
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Surroundings
Outside the chemical system.
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Endothermic
A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants, resulting in heat being taken in from the surroundings
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Exothermic
A reaction in which the enthalpy of the products is smaller than the enthalpy of the reactants, resulting in heat loss to the surroundings
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Enthalpy Profile Diagram
It's a diagram for a reaction to compare the enthalpy of the reactants with the enthalpy of the products.
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Activation Energy
The minimum amount of energy required to start a reaction by the breaking of bonds
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Standard conditions
Pressure = 100Kpa or 1 Atmosphere. Temperature = 298K or 25 c. Concentration = 1 moldm-3
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The Standard Enthalpy Change of Reaction
The enthalpy change that accompanies a reaction in molar quantities expressedin a chemical equation under standard condicitons and being in their standard states
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The Standard Enthalpy Change of Combustion
The enthalpy change that takes place when 1 mole of a substance reacts completely with oxygen under standrad conditions and in their standard states.
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The Standard Enthalpy Change of Formation
The enthalpy change that takes place when 1 mole of a compound is formed from it's constituent elements under standard conditions in their standard states.
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Hess' Law
The enthalpy chane of a reaction is independant from the route taken from the reactants to the products.
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Enthalpy Cycle
A diagram showing the alternate routes between reactants and products which allows the indirect determination of an enthalpy change from other known enthalpy changes using Hess' law
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Rate of Reaction
The change in concentration of a reactant or a product in a given time
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Catalyst
A substance that increases the rate of a chemical reaction without being used up in the process
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Heterogeneous Catalyst
A reaction in which the catalyst is in a different physical state to the reactants
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Homogeneous Catalyst
A reaction in which the catalyst is in the same physical state as the reactants
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Boltzmann Distribution
The distribution of energies of molecules at a particular temperature, often shown as a graph
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Radical
A particle with an unpaired electron which makes it a lot more reactive
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Other cards in this set

Card 2

Front

Number of protons AND neutrons in the nucleus.

Back

Mass Number

Card 3

Front

The time taken for half of a radioactive isotope to decay

Back

Preview of the back of card 3

Card 4

Front

The energy required to remove 1 electron from each atom in 1 mole of GASEOUS atoms of an element to form 1 mole of GASEOUS positive ions.

Back

Preview of the back of card 4

Card 5

Front

A(g) --------> A+(g) + E-(g)

Back

Preview of the back of card 5
View more cards

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