Unit 1: Rate of Reactions Glossary Flashcards
What is the definition of Activation Energy?
The minimum amount of energy needed for a reaction to begin.
What is the definition of a catalyst?
A chemical which speeds up a chemical reaction without being used up itself and which can be removed chemically unchanged at the end of the reaction and can be used again.
What is the definition of concentration?
The amount of particles in a given volume.
What is the definition of products?
The substances (chemicals) at the end of a chemical reaction.
What is the definition of rate of reaction?
How quickly a reactant is used up or how quickly a product is created.
What is the definition of reactants?
The substances (chemicals) at the start of a chemical reaction.
What is the definition of surface area?
Total area of a substance which is exposed to the surroundings.
What is the definition of Covalent radius?
half the distance between the nuclei of two bonded atoms of an element.
What is the definition of electronegativity?
A measure of the attraction the nucleus of an atom involved in a bond has for the electrons of the bond.
What is the definition of the ionisation energy?
The first ionisation energy is the amount of energy required to remove one mole of electrons from one mole of atoms in the GASEOUS state.The second and subsequent ionisation energy refers to the energy required to remove a further mole of electrons from one mole of atoms in the gaseous state.
What is the definition of the screening effect?
When inner electrons shield on outer electron from the attractive effect of the nucleus and less energy is needed to remove the outer electron as a result.
What is the definition of chemical structure?
Describes the way in which atoms, ions or molecules are arranged.
What is the definition of the covalent bond?
A covalent bond is formed when two atoms share electrons in their outer shell to complete the filling of that shell.
What is the definition of delocalised?
Delocalised electrons, in metallic bonding, are free from attachment to any one metal ion and are shared amongst the entire structure.
What is the definition of D dipole
An atom or molecule in which a concentration of positive charges is separated from a concentration of negative charges.
What is the definition of the fullerenes?
Molecules of pure carbon constructed from 5 and 6-membered rings combined into hollow structures. The most stable contains 60 carbon atoms in a shape resembling a ball.
What is the definition of Hydrogen bonds?
The electrostatic forces of attraction between molecules containing a hydrogen atom bonded to an atom of a strongly electrongative element such as fluorine, oxygen or nitrogen and a highly electronegative atom on a neighbouring molecule.
What is the definition of intermolecular forces?
Forces which attract molecules together. They are weaker than chemical bonds.
What is the definition of Intramolecular forces?
Forces of attraction which exist within a molecule.
What is the definition of lattice?
A lattice is a regular 3D arrangement of particles in space. the term is applied to metal ions in a solid, and to positive and negative ions in an ionic solid.
What is the definition of London Dispersion forces?
London Dispersion Forces are the intermolecular forces of attraction which result from the electrostatic attraction between temporary dipoles and induced dipoles caused by the movement of electrons in atoms and molecules.
What is the definition of polar covalent bonding?
A covalent bond between atoms of different electronegativity, which results in an uneven distribution of electrons and a partial charge along the bond.
What is the definition of Van der Waal’s forces?
Is the general name given to all the intermolecular attraction including London dispersion forces, Permanent dipole to permanent dipole interactions and hydrogen bonding.
What is the definition of viscosity?
Viscosity id the resistance to flow that is exhibited by all liquids.
