Chemistry Definitions

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The amount of solute in mol per 1dm3 of solution.
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The increase in strength of a soution.
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Standard Solution
A solution of known concentration.
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Molecular Formula
This shows the number of atoms of each element in one molecule of the substance.
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Its the ratio that reactants react in to give products an is shown by the balanced equation.
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Gas Volume
1 mol of any gas occupies 24dm3 at 20oC and 1 atomoshperic pressure.
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Atomic Number
The number of protons (and electrons) in an atom of a element.
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Relative Atomic Mass (Ar)
The mean mass of an isotope relative to 1/12 carbon-12.
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Mass Number
The number of protons and neutrons in an atom of an isotope.
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Relative Formula Mass
The mass of all of the atoms i the formula relative to 1/12 carbon-12
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Molar Mass
Mass of 1 mole of a substance g/mol.
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Relative Molecular Mass (Mr)
The mass of 1 molecule of a compound relative to 1/12 carbon-12.
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Its the amount of a substance which represents 6.02x10^23
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1 Mole
Its the number of C-12 atoms in 12g.
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Relative Atomic Mass
The mass of one atom of a particular isotope relative to 1/12 the mass of a carbon-12 atom.
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Atoms of the same element that has a different number of neutrons.
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A soluble base which gives OH- in a solution.
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Redox Reaction
A reaction in which both reduction and oxidation takes place.
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The gain of electrons or a decrease in the oxdation number.
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The loss of electrons or an increase in the oxidation number.
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The oxidation and reduction of the same element in a redox reaction.
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Covalent Bond
A bond formed by a shared pair of electrons.
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A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond.
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Lone Pair
Its an outer-shell pair of electrons that is not involved in chemical bonding.
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Octect Rule
The total number of electrons (shared and lone pairs) in the outer shell of a covalently bonded electron.
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Dative Covalent Bond
A covalent bond in which both electrons in the shared pair come from one atom.
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Chemical Bond
The attraction between 2 atoms so that they are firmly joined together.
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Ionic Compounds
They're formed between two (or more) elements of similar electronegativities sharing electrons.
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Metalic Bonds
They're formed between metal atoms.
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Ionic Bonds
They're the electrostatic attraction between oppisitely charged ions.
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A region within an atom that can hold up to two electrons with opposite spins.
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Electronic Configuration
A set of numbers, letters and symbols representing the arrangement of electrons into orbitals.
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The First Ionisation Energy
An element is the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.
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Atomic Radius
The greater the atomic radius the less the nuclear attraction.
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Nuclear Charge
The more protons the higher the nuclear charge therefore the greater the attractive force on the outer electrons.
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Electron Shielding
The repulsion between electons in different inner shells. Sheilding reduces the net attractive force from the positive nucleus on the outer-shell electrons.
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Ionisation Energy
The energy needed to form positive ions.
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Permenant Dipole
A small charge difference across the molecule resulting from the different electronegativities of the atoms.
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A molecule that has a slight charge difference.
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Van der Waals Forces
They're very weak attractive forces between induced dipoles in neighbouring molecules.
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Permenant Dipole
A small charge difference across a bond resulting from a difference in electronegativities of the bonded atoms.
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Dipole Moment
It shows the movement of the electrons in the molecule itself and which is the most polar end.
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Metallic bond
The electrostatic attraction between positive metal ions and deocalised electrons.
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Delocalised Electrons
They're shared between more than two atoms.
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Card 2




The increase in strength of a soution.

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Standard Solution


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Card 4


Molecular Formula


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