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73 Cards in this Set
- Front
- Back
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Acid |
A species that is a proton donor |
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Activation Energy |
The minimum energy required to start a reaction by the breaking of bonds |
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Alkali |
A type of base that dissolves in water forming hydroxide ions, OH- (aq) ions. |
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Amount of substance |
The quantity whose unit is the mole. Chemists use ‘amount of substance’ as a mean of counting atoms |
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Anhydrous |
A substance containing no water molecules |
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Anion |
A negatively charged ion |
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Atomic Orbital |
A region within an atom that can hold up to two electrons, with opposite spins |
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Atomic (proton) number |
The number of protons in the nucleus of an atom |
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Avogadro constant, Na |
The number of atoms per mole of the carbon-12 isotope (6.02 x 1023 mol-1) |
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Base |
A species that is a proton acceptor |
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Cation |
A positively charged ions |
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Compound |
A substance formed from two or more chemically bonded elements in a fixed ratio, usually shown by a chemical formula |
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Concentration |
The amount of solute, in mol, per dm3 (1000cm3) of solution |
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Coordinate bond |
A shared pair of electrons which has been provided by one of the bonding atoms only; also called a coordinate bond |
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Covalent bond |
A bond formed by a shared pair of electrons |
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Dative covalent bond |
A shared pair of electrons which been provided by one of the bonding atoms only; also called a coordinate bond |
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Delocalised electrons |
Electrons that are shared between more than two atoms |
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Displacement Reaction |
A reaction in which a more reactive element displaces a less reactive element from an aqueous solution of the latter’s ions |
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Disproportionation |
The oxidation and reduction of the same element in a redox reaction |
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Electron configuration |
The arrangement of electrons in an atom |
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Electronegativity |
A measure of the attraction of a bonded pair of electrons in a covalent bond |
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Electron shielding |
The repulsion between electrons in different inner shells. Shielding reduces the net attractive force from the positive nucleus on the outer shell electrons |
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Empirical formula |
The simplest whole-number ratio of atoms of each element present in a compound |
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Giant covalent lattice |
A three-dimensional structure of atoms, bonded together by strong covalent bonds |
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Giant ionic lattice |
A three-dimensional structure of oppositely charged ions, bonded together by strong ionic bonds |
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Giant metallic lattice |
A three-dimensional structure if positively charged ions and delocalised electrons, bonded together by strong metallic bonds |
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Group |
A vertical column in the periodic table. Elements in a group have similar chemical properties and their atoms have the same number of outer-shell electrons |
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Hydrated |
Crystalline and containing water molecules |
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hh |
dd |
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Intermolecular force |
An attractive force between neighbouring molecules. Intermolecular forces can be Van der Waals’ forces (including dipole-dipole forces), permanent dipole-dipole forces or hydrogen bonds |
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Hydrogen Bond |
A strong dipole-dipole attraction between an electron deficient hydrogen atom on one molecule and a lone pair of electrons on a highly electronegative atom on a different molecule |
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Intermolecular force |
An attractive force between neighbouring molecules. Intermolecular forces can be Van der Waals’ forces (including dipole-dipole forces), permanent dipole-dipole forces or hydrogen bonds |
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Ion |
A positively or negatively charged atom or (covalently bonded) group of atoms (a molecular ion) |
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Ionic bond |
The electrostatic attraction between oppositely charge ions |
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(first) Ionisation energy |
The energy required to remove one electron from each atom in mole of gaseous atoms to form one mole of gaseous 1+ ions |
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(second) Ionisation energy |
The energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions |
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(successive) Ionisation energy |
A measure of the energy required to remove each electron in turn |
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Isotopes |
Atoms of the same element with different numbers of neutrons and different masses |
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Lone pair |
An outer shell pair of electrons that is not involved in chemical bonding |
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Mass (nucleon number) |
The number of particles (protons and neutrons) in the nucleus |
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Metallic bond |
The electrostatic attraction between positive metal ions and delocalised electrons |
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Molar mass, M |
The mass per mole of a substance , g mol-1 |
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Molar volume |
The volume per mole of a gas. The units of molar volume are dm3mol-1. |
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Mole |
The amount of any substance containing as many particles as there are carbon in exactly 12g of carbon-12 isotope |
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Molecular formula |
The number of atoms of each element in a molecule |
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Molecule |
A small group of atoms held together by covalent bonds |
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Oxidation |
Loss of electrons or an increase in oxidation number |
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Oxidation number |
A measure of the number of electrons that an atoms uses to bond with atoms of another element. Oxidation numbers are derived from a set of rules |
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Oxidising agent |
A reagent that oxidises (takes electrons from) another species |
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Period |
A horizontal row of elements on the periodic table |
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Periodicity |
A regular periodic variation of properties of elements atomic number and position on the Periodic table |
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Permanent dipole |
A small charge difference across a bond resulting from a difference in electro negativities of the bonded atom |
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Permanent dipole-dipole force |
An attractive force between permanent dipoles in neighbouring molecules |
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Polar covalent bond |
A bond with a permanent dipole |
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Polar molecule |
A molecule with an overall dipole, taking into account any dipoles across bonds |
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Precipitation reaction |
The formation of a solid from a solutions during a chemical reaction. Precipitates are often formed when two aqueous solutions are mixed together |
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Principle quantum number, n |
A number representing the relative overall energy of each orbital , which increases with distance from the nucleus. The sets of orbitals with same n value are referred to as electron shells or energy levels. |
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Redox reaction |
A reaction in which reduction and oxidation take place. |
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Reducing agent |
A reagent that reduces ( adds electrons to ) another species |
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Reduction |
Gain of electrons or a decrease in oxidation number |
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Relative atomic mass, Ar |
The weighted mean mass of a formula unit compared with one-twelfth of the mass of an atoms of catbon-12 |
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Relative isotopic mass |
The mass of an atom of an isotope compared with one-twelfth of the mass of an atom of carbon-12 |
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Relative molecular mass, Mr |
The weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12 |
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Salt |
A chemical compound formed from an acid, when a H+ ion from the acid has been replaced by a metal ion or another positive ion |
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Shell |
A group of atomic orbitals with the same principal quantum number, n. Also known as a main energy level |
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Simple molecular lattice |
A three-dimensional structure of molecules, bonded together by weak intermolecular forces |
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Species |
Any type of particle that takes part in a chemical reaction |
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Standard solution |
A solution of known concentration . Standard solutions are normally used in titration to determine unknown information about another substance |
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Stoichiometry |
The molar relationship between the quantities of substances taking part in a reaction |
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Sub-shell |
A group of the same type of atomic orbitals(s, p, d or f) within a shell |
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Thermal decomposition |
The breaking up of a chemical substance with heat into at least two chemical substances |
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Van der Waals’ forces |
Very weak attractive forces between induced dipoles in neighbouring molecules |
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Water of crystallisation |
Water molecules that form an essential part of the crystalline structure of a compound |
