4329781
Description
Flashcards by jacob gray, updated more than 1 year ago
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Created by jacob gray
over 8 years ago
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| Question | Answer |
| Isotopes | Atoms of the same element with different number of neutrons |
| Atomic / Proton number | The number of protons in the nucleus of the atom |
| Mass / Neucleon number | The number of particles (Protons and neutrons) in the nucleus of the atom |
| Ion | A positively or negatively charged atom or covalently bonded group of atoms |
| Relative isotopic mass | The mass of an atom of an isotope compared with 1/12th of the mass of an atom of carbon-12 |
| Relative atomic mass (Ar) | The weighted mean mass of an atom of an element compared to 1/12th of the mass of an atom of carbon-12 |
| Relative molecular mass (Mr) | The weighted mean mass of a molecule compared to 1/12th of the mass of an atom of carbon-12 |
| Relative formula mass | The weighted mean mass of a formula unit compared to 1/12th of the mass of an atom of carbon-12 |
| A mole | The amount of any substance containing as many particles as there are carbon atoms in 12g of carbon-12 |
| Molar mass (M) | The mass per mole of a substance |
| Empirical formula | The simplest whole-number ratio of atoms of each element present in a compound |
| A molecule | A small group of atoms held together by covalent bonds |
| Molecular formula | The actual number of atoms of each element present in a molecule |
| Molar volume | Volume per mole of gas at room temperature and pressure, 24.0 dm^3mol^-1 |
| Concentration | Amount of solute, in mol, dissolved in 1dm^3 |
| Standard solution | A solution of known concentration, used in titrations |
| Species | Any type of particle that takes part in a chemical reaction |
| Stoichiometry | The molar relationship between the relative quantities of substances taking part in a reaction |
| Acid Plus 3 to know | A species that is a proton donor H2SO4 HCl H |
| Base Plus some examples | A species that is a proton acceptor Metal oxides, MgO Metal hydroxides, NaOH Amines |
| Alkali Plus 3 to know | A type of base that dissolves in water forming hydroxide ions, OH^- Ammonia KOH NaOH |
| Salt | A chemical compound formed when a H+ ion in an acid has been replaced by a metal ion or another positive ion. |
| Cation | A positively charged ion |
| Anion | A negatively charged ion |
| Water of crystallisation | Water molecules that form an essential part of the crystalline structure of a compound |
| Hydrated | A crystalline compound containing water molecules |
| Anhydrous | A substance that contains no water molecules |
| Oxidation number | The measure of a number of electrons that an atom uses to bond with other atoms. |
| Oxidation | Loss of electrons / increase of oxidation number |
| Redox | Gain of electrons / decrease in oxidation number |
| Redox reaction | A reaction in which both reduction and oxidation occur |
| Reducing agent | A reagent that reduces another species and oxidises itself |
| Oxidising agent | A reagent that oxidises another species and reduces itself |
| First ionisation energy | The energy required to remove an electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions |
| Electron shielding | The repulsion between electrons in different shells, reducing the attraction of outer electrons to the nucleus |
| Successive ionisation energies | A measure of the energy required to remove each electron in one mole of gaseous atoms in turn. |
| Shell | A group of atomic orbitals with the same main energy level / principle quantum number |
| Principle quantum number | A number that represents the energy of each orbital |
| Atomic orbital | A region within an atom that can hold upto 2 electrons with opposite spin |
| Sub-shell | A group of the same atomic orbitals within a shell |
| Electron configuration | The arrangement of electrons on an atom |
| Compound | A substance formed from 2 or more chemically bonded elements are fixed in a ratio |
| Ionic bond | An electrostatic attraction between oppositely charged ions |
| Giant ionic lattice | A 3D structure of oppositely charged ion, held together by strong ionic bonds |
| Group | A vertical column in the periodic table, which have similar properties and same number of outer electrons |
| Covalent bond | A bond formed by a shared pair of electrons |
| Lone pair | An outer shell pair of electrons not involved in chemical bonding |
| Dative covenant / coordinate bond | A shared pair of electrons which have been provided one of the bonding atoms only |
| Electronegativity | A measure of the attraction between a bonded pair of electrons in a covalent bond |
| Permanent dipole | A small charge difference across a bond that results from a difference in the electronegativity of the bonded atoms |
| Polar covalent bond | Permanent dipole |
| Intermolecular force | An attractive force between neighbouring molecules |
| Permanent dipole-diple force | A weak attractive force between permanent dipoles in neighbouring polar molecules |
| van der Waals' forces | Attractive forces between induced dipoles in neighbouring molecules |
| Hydrogen bonding | A strong dipole-dipole attraction between a delta positive hydrogen and a lone pair of electrons on a different molecule |
| Metallic bonding | The electrostatic attraction between positive metal ions and delocalised electrons |
| Delocalised electrons | Electrons shared between more than two atoms |
| Giant metallic lattice | A 3D structure of molecules bonded together by metallic bonds |
| Simple molecular lattice | A 3D structure of molecules bonded together by weak intermolecular forces |
| Giant covalent lattice | A 3D structure of molecules bonded together by covalent bonds |
| Period | A horizontal row of elements in the periodic table that show a trend across it. |
| Periodicity | A regular periodic variation of properties of elements with atomic number and position in the periodic table |
| Thermal decomposition | Breaking up of a chemical substance with heat into at least 2 chemical substances |
| Displacement reaction | A reaction in which a more reactive element displaces a less reactive element from an aqueous solution of latter's ions |
| Disproportionation | The oxidation and reduction of the same element in a redox reaction |
| Precipitation reaction | The formation of a solid from a solution during a chemical reaction between 2 aqueous solution. |
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