chemistry as level unit 1

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  • Created by: Anna Wood
  • Created on: 10-01-15 16:19
Ionisation energy
Energy required to remove an electron from each atom of a one mole of gaseous atoms to create one mole of gaseous ions.
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Empirical formula
The lowest whole number ration of each element present in a compound
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Molecular formula
The actual number of atoms of each element present in a compound
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Electron shielding
The repulsion of electrons in different inner shells, shielding reduces the net attraction force from the positive nucleus on the outer shell electron.
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Atomic radius
The region in which an atom can hold two electrons with opposite spins
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Ion
A positively or negative charged atom or (covalently bonded) group of atoms ( a molecular ion)
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Isotopes
Are atoms of the same element with a different number of neutrons but the same electron and proton number.
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Atomic number
The number of protons in the nucleus of an atom.
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Mass number
Number of protons and neutrons in the nucleus of an atom.
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Relative isotopic number
The mass of an atom of an isotope compared to 1/12 of the mass of carbon 12.
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Relative molecular mass
Weighed mean mass of an molecule compared to 1/12 the mass of an atom of carbon 12.
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Relative formula mass
The weighed mean mass of a formula unit compared with 1/12 of the mass of an atom of carbon 12.
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Amount of substance
Is the quantity who units is the mole. Chemist use the amount of substance as a means of counting atoms
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Avogadro constant
The number of atoms per a mole of carbon 12 = 6.02x10 23 mol-1
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Mole
Is the amount of any substance containing the amount of particles as there are carbon atoms in exactly 12g of carbon 12.
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Molar mass
Mass per a mole of substance units= g mol-1
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Molecule
A small group of atoms held together by covalent bonds.
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Molecular formula
Actual number of atoms of each element in a molecule.
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Molar volume
The volume per a mole of a gas units = dm3 mol-1 . at room temperature and pressure = 24dm3
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Concentration of a solution
Amount of solute , in mol, dissolved per 1dm3.
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Standard solution
A solution of known concentration. Normally used in titrations to determine unknown information about other substances .
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Stoichiometry
Molar relationship between the relative quantities of substances taking part in a reaction.
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Acid
A proton donor .
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Base
Proton accepter.
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Salt
Any chemical compound formed from an acid when H+ ions from the acid has been replaced by a metal ion or another positive ion such as ammonium.
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Cation
Positively charged ion.
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Anion
Negatively charged ion.
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Hydrated
Refers to a crystalline compound containing water molecules.
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Anhydrous
Substance that contains no water molecules
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Water of crystallisation
Water molecules that form an essential part of the crystalline structure of a compound.
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Oxidation number
Measure of the number of electrons that an atoms used to bond with an atoms of another element, oxidation numbers are derived from a set of rules.
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Redox reaction
Reaction in which both reduction and oxidation takes place.
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Oxidation
A loss of electrons or an increase in oxidation numbers.
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Other cards in this set

Card 2

Front

The lowest whole number ration of each element present in a compound

Back

Empirical formula

Card 3

Front

The actual number of atoms of each element present in a compound

Back

Preview of the back of card 3

Card 4

Front

The repulsion of electrons in different inner shells, shielding reduces the net attraction force from the positive nucleus on the outer shell electron.

Back

Preview of the back of card 4

Card 5

Front

The region in which an atom can hold two electrons with opposite spins

Back

Preview of the back of card 5
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