OCR AS Chemistry

  • Created by: GemmaO29
  • Created on: 19-10-17 16:08
Activation Energy
The minimum energy required to start a chemical reaction
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Acid
A species that releases H+ ions in aqueous solution
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Empirical Formula
The simplest whole number ratio of atoms of each element present in a compound
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Avogadro's Constant
Number of Atoms in 1 mole of a compound 6.02x1023 mol-1 of Carbon 12
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Molar Mass
The mass per mole of a substance in units gmol-1
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Amount of Substance/Mole
The qwuantity whose unit is the mole. Chemists use amount of substance as a mean of counting atoms
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First Ionisation Energy
The enery required to remove one electron form one mole (each atom) of gaseous atoms of an element to form 1 mole of gaseous 1+ ions
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Water of Crystallisation
Water molecules that are bonded in a compound
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Hydrated
A compound containing water molecules
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Anhydrous
Contains no water molecules
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Salt
The product of a raction in which H+ ions are replaced by metal or ammonium ions in the acid
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Neutralisation
The reaction between and acid and a base to form a salt and water H+ + OH- makes H2O
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Alkali
A type of base that dissolves in water and releases OH- ions
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Base
A compound that neutralises an acid to form a salt
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Molecular Formula
A formula that shows the number and type of atoms of each element present in a molecule
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Disproportionation
A redox reaction in which the same element is both oxidised and reduced
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Acid
A species that release H+ ions in an aqueous solution
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Relative atomic mass
The weighted mean mass of an atom of an element compared with 1/12th 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 1/12th of the mass of an atom of Carbon 12
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Isotope
Atoms of the same element with different numbers of neutrons and different masses
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Mass Number
The sum of the number of protons and the number of neutrons in the nucleus Oxygen- 16 Nitrogen-14
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Metallic bonding
The electorstatic attraction between positive metals ions and delocalised electron
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Hydrogen Bonding
A stron dipole-dipole attraction between hydrogen atom NH,OH, or HF or a lone pair of electorns in H, N , O ,F
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Permenant dipole-dipole interactions
Attractive forces between the permenant dipoles in different molecules
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Induced Dipole-dipole interactions (London Forces)
Attractive forces between induced dipoles in different molecules
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Dipole
A seperation in electrical charge so that one atom of a polar covalent bond has a slight positive charge and the other negative
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Non-polar
With no charge seperation across a bond or in a molecule
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Polar
A molecule with a permenant dipole one ned is negative and the other is positive
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Electronegativity
A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond
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Redox Reaction
A reaction in which the reactants are both oxidised and reduced
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Dative (Coordinate) covalent bond
A shared pair of electrons in which the bonded pair of electrons has been provided by one atom only
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Covalent bond
The electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms
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Ionic bond
The electrostatic attraction between positively and negatively charged ions
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Periodicity
A repeating trend in properties of the elements across each period of the periodic table
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Reduction
Gain of electrons or a decrease in oxidation number
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Oxidation
Loss of electrons or increase in oxidation number
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Atomic number
The number of protons in the nucleus of an atom
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Thermal Decomposition
The break down of a compound under heat
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Other cards in this set

Card 2

Front

A species that releases H+ ions in aqueous solution

Back

Acid

Card 3

Front

The simplest whole number ratio of atoms of each element present in a compound

Back

Preview of the back of card 3

Card 4

Front

Number of Atoms in 1 mole of a compound 6.02x1023 mol-1 of Carbon 12

Back

Preview of the back of card 4

Card 5

Front

The mass per mole of a substance in units gmol-1

Back

Preview of the back of card 5
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