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| Question | Answer |
| Relative isotopic mass | The mass of an atom of the isotope, compared with one-twelfth of the mass of carbon-12. |
| Relative molecular mass | The weighted mean mass of a molecule, compared with one-twelfth of the mass of carbon-12. |
| Anhydrous | A molecule containing no water molecules |
| Simple molecular lattice | A 3-D structure of molecules, bonded together by weak intermolecular forces. |
| Shell | A group of atomic orbitals with the same principal quantum number/same main energy level. |
| Alkali | A type of base that dissolves in water, forming hydroxide ions. |
| 1st Ionisation energy | The energy required to remove one electron in each atom in one mole of gaseous atoms, to form one mole of gaseous 1+ ions. |
| Ion | A positively or negatively charged atom. |
| Acid | A proton donor |
| Intermolecular force | An attractive force between neighbouring molecules. |
| 2nd Ionisation energy | The energy required to remove an electron from each ion in one mole of gaseous 1+ ions, to form one mole of gaseous 2+ ions. |
| Successive ionisation energies | A measure of the energy required to remove each electron in turn. |
| Hydrogen bond | A strong dipole dipole set traction, between an electron deficient hydrogen atom on one molecule, and a highly electronegative molecule (O,N) on another. |
| Period | A horizontal row of elements in the periodic table, showing trends. |
| Salt | A chemical compound formed from an acid, when a H+ ion from the acid has been replaced by a metal ion or another positive ion. |
| Periodicity | A regular periodic variation of properties of elements with atomic number and position in the periodic table. |
| Hydrated | Crystalline and containing water molecules |
| Group | A vertical column in the periodic table, involving elements with the same number of electrons in their outer shell, and similar chemical properties. |
| Reduction | A gain of electrons and loss in oxidation number. |
| Oxidation | A loss in electrons and gain in oxidation number |
| Electronegativity | A measure of the attraction of a bonded atom, for the pair of electrons in a covalent bond. |
| Reducing agent | A reagent that reduces/adds electrons to another species. |
| Giant metallic lattice | A three dimensional structure of positive ions and delocalised electrons, held together by strong metallic bonds. |
| Oxidising agent | A reagent that increases/removes electrons from mother species. |
| Electron configuration | The arrangement of electrons in an atom. |
| Giant ionic lattice | A three dimensional structure of positive and negative ions held together by strong ionic bonds. |
| Redox reaction | A reaction involving both reduction and oxidation. |
| Principal quantum number | A number representing the relative overall energy level for each orbital, which increases with distance from the nucleus. |
| Thermal decomposition | The breaking up of a chemical substance, with heat into at east two different substances. |
| Oxidation number | A measure of the number of electrons that an atom uses to bond with atoms of another element. |
| Giant covalent bond | A three dimensional structure of atoms, bonded together by strong covalent bonds. |
| Van der waals forces | Very weak attractive forces between induced dipoles in neighbouring molecules. |
| Sub-shell | A group of the same type of atomic orbitals e.g. s,p,d,f |
| Molecule | A small group of atoms held together by a covalent bond |
| Empirical formulae | The simplest, whole number ratio of atoms of each element present in. Compound. |
| Polar molecule | A molecule that has an overall dipole, taking into account any dipoles across bonds. |
| Polar covalent bond | A bond with a permanent dipole. |
| Electron shielding | The repulsion between electron in different inner shells. |
| Permanent dipole-dipole force | An attractive force between permanent dipoles in neighbouring polar molecules. |
| Permanent dipole | A small charge difference across a bond resulting from a difference in electronegativities of the bonded atoms. |
| Disproportionation | The oxidation and reduction of the same element in a redox reaction. |
| Displacement reaction | A reaction in which a more active element displaces a less active element from an aqueous solution of the latter's ions. |
| Delocalised electrons | Electrons that are shared between more than two atoms |
| Dative covalent bond | A shared pair of electrons which has been provided by one of the bonding atoms only. |
| Covalent bond | A bond formed by a shared pair of electrons |
| Concentration | The amount of solute, in moles per 1000cm3 of solution. |
| Compound | A substance formed by two or more chemically bonded elements in a fixed ratio, usually shown by a chemical formula |
| Cation | A positively charged ion |
| Molecular formula | The number of atoms of each element in a molecule. |
| Mole | The amount of any substance containing as many particles as there are carbon atoms in exactly 12g of carbon-12 isotope. |
| Molar volume | The volume per mole of a gas. |
| Catalyst | A substance that increases the rate of a chemical reaction by providing a smaller activation energy and alternative reaction pathway, and is not used up in the process. |
| Molar mass (M) | The mass per mole of a substance. |
| Base | A species that is a proton acceptor |
| Metallic bond | The electrostatic attraction between fixed positive ions and a sea of delocalised electrons. |
| Mass number | The number of protons and neutrons in the nucleus. |
| Avogadro constant | The number of atoms per mole of the carbon-12 isotope 6.023x10 to the power of 23 |
| Lone pair | An outer shell pair of electrons that are not involved in chemical bonding. |
| Atomic number | The number of protons in the nucleus |
| Limiting reagent | The substance in a chemical reaction that runs out first. |
| Stoichiometry | The molar relationship between the relative quantities of substances taking part in a reaction. |
| Standard solution | A solution of known concentration. (Normally used in titrations) |
| Species | Any type of particle that takes part in a reaction. |
| Isotopes | Atoms of the same element with different mass numbers and different number of neutrons in the nucleus (but the Same proton number) |
| Orbital | A region of space within an atom that can hold up to two electrons with opposite spins. |
| Relative atomic mass | The weighted mean mass of an atom of an element, compared with one-twelfth of the mass of carbon-12 which is taken as 12 exactly |
| Spectator ions | Ions that are present, but do it take part in the chemical reaction. |
| Ionic bond | The electrostatic attraction between oppositely charged ions. |
| Relative formula mass | The weighted mean mass of a formula unit, compared with one-twelfth of the mass of carbon-12. |
| Anion | A negatively charged ion |
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