4051186
| Pregunta | Respuesta |
| Atomic Number | The number of protons in the nucleus of an atom. |
| Mass Number | The number of protons and neutrons in the nucleus of an atom. |
| Relative Isotopic Mass | The mass of an atom of an isotope compared with 1/12 of the mass of an atom of C-12. |
| Relative Atomic Mass | The weighted mean mass of an atom of an element compared with 1/12 of the mass of an atom of C-12. |
| Isotopes | Atoms of the same element with a different number of neutrons. |
| Mole | The amount of substance containing as many particles as there are carbon atoms in exactly 12g of C-12. |
| Avogadro's Constant | The number of particles per mole of a substance. (6.02 x 10^23) |
| Molar Mass | The mass, in g, per mole of a substance. Units are gmol-1. |
| Empirical Formula | The simplest whole number ratio of atoms of each element present in a compound. |
| Molecular Formula | The actual number of atoms of each element in a molecule. |
| Water of Crystallisation | The water present in a compound giving the compound a crystalline appearance. |
| Acid | Releases H+ ions in solution. (Proton donor) |
| Base | A proton acceptor. |
| Alkali | A soluble base that releases OH- ions when in solution. |
| Salt | A compound produced when a H+ ion from an acid is replaced by a metal ion or another positive ion, such as the ammonium ion. |
| Anhydrous | When all the waters of crystallisation have been removed from a compound. |
| Hydrated | When water of crystallisation is present in a crystal compound. |
| Oxidation Number | A measure of the number of electrons that an atom uses to bond with atoms of a different element. |
| Oxidation | The loss of electrons/an increase in oxidation number (state). |
| Oxidising Agent | A reagent which oxidises another species (gets reduced itself). |
| Reduction | The gain of electrons/a decrease in oxidation number (state). |
| Reducing Agent | A reagent that reduces another species (gets oxidised itself). |
| Redox | A reaction were both oxidation and reduction take place. |
| Displacement Reaction | A reaction in which a more reactive element displaces a less reactive element from aqueous solution of its halide ions. |
| Disproportionation | A reaction in which an element is simultaneously oxidised and reduced. |
| Atomic Orbital | A region within an atom that can hold up to 2 electrons, with opposite spins. |
| S/P/D Block Element | Highest energy sub–shell is an S/P/D sub-shell. |
| Ionic Bond | The electrostatic attraction between oppositely charged ions. |
| Covalent Bond | The sharing of a pair of electrons between two atoms. |
| Dative (Co-Ordinate) Bond | The sharing of a pair of electrons between two atoms where only one of the atoms supplies both the electrons shared. |
| Electronegativity | The ability of an atom to attract the bonding electrons towards itself in a covalent bond. |
| Metallic Bonding | The attraction of positive metal ions to delocalised electrons. |
| Periodicity | The repeating pattern of trends across different periods. |
| Hydrogen Bond | A dipole-dipole attraction between a slightly positive hydrogen on one molecule and a lone pair of electrons on a highly electronegative atom (N, O, F) of another molecule. |
| First Ionisation Energy | The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions. Units are kJmol-1. |
| Successive Ionisation Energy | A measure of the energy required to remove each electron in turn. |
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