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Description
Flashcards by Tali Skipper, updated more than 1 year ago
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Created by Tali Skipper
almost 10 years ago
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| Question | Answer |
| Accuracy | How close to the true value a measurement is. |
| Acid | A chemical that is a proton donor. Releases H+ (aq) in solution. |
| Activation Energy | The minimum energy required to start a reaction by breaking chemical bonds in the reactants. |
| Aim | Identifies the purpose of an investigation. What is trying to be found out. |
| Alcohol | A group of organic compounds with the functional group -OH. |
| Alicyclic Hydrocarbon. | Carbon atoms are joined in a ring structure. |
| Alkali | Soluble in water releasing OH- (aq) Ions. |
| Alkanes | Homologous series of saturated hydrocarbons. |
| Alkenes | A homologous series of unsaturated hydrocarbons. |
| Amount of Substance | The quantity whose unit is the mole. It is a way of counting atoms. |
| Aliphatic Hydrocarbons | A hydrocarbon where carbon atoms are joined together in straight or branched chains. |
| Anhydrous | A substance that contains no water molecules. |
| Anion | Negatively charged ion. |
| Anomalies/ Anomalous | Data that doesn't fit the particular trend of data and doesn't follow the general pattern. |
| Aqueous | A solution with water as the solvent. |
| Aromatic Hydrocarbons | Contain at least 1 benzene ring (ring of 6 carbons). |
| Atom | Composed of electrons and a central nucleus of protons and neutrons. |
| Atomic Number | The number of protons in the nucleus of an atom. |
| Atomic Orbital | A region of space where a maximum of 2 electrons with opposite spins in each can be found. |
| Atomic Radius | The distance from the nucleus to the boundary of the surrounding cloud of electrons. |
| Average Bond Enthalpy | The mean energy needed for 1 mole of a given type of gaseous bonds to undergo homolytic fission. |
| Avogadro Constant | The number of atoms per mole of the carbon-12 isotope = 6.02 X 10^23 mol^-1 |
| Base | A chemical that can react with acids and is a proton acceptor. |
| Biodegradable Materials | Decompose by microorganisms and environmental conditions. |
| Biological Catalysts | Enzymes - Catalyse reactions in the body. |
| Bioplastics | Materials made from a renewable source that are biodegradable. |
| Boltzmann Distribution | The distribution of energies of molecules at a particular temperature, often shown as a graph. |
| Bond Angle | The angle that is formed between to adjacent bonds on the same atom. |
| Bonded Pair | A pair of electrons that have been shared between two chemically bonded atoms. |
| Bonding Region | The space where an electron can be found in a bond. |
| Carbonyls | An organic molecule which contains the C=O functional group. |
| Carboxylic Acids | An organic acid containing a carboxyl functional group –COOH. |
| Calorimetry | The quantitative study of energy change in a chemical reaction. |
| Catalyst | A substance that increases the rate of reaction by decreasing the activation energy. It is not used up in the process. |
| Categoric Variable | A qualitative description of a variable. |
| Cation | Positively charged ion. |
| CFCs | Chlorofluorocarbons are a class of organic compounds that are non-toxic to humans but can be radicalised by UV light. |
| Chemical Energy | A special form of potential energy stored in chemical bonds. |
| Cis-Trans Isomerism | A type of E/Z isomerism where two substituent groups on each carbon are the same. |
| Collision Theory | A model to help understand and make predictions about how changing factors may change the rate of a chemical reaction. |
| Complete Combustion | The oxidising of a fuel in a plentiful supply of oxygen. |
| Compound | A substance formed from 2 or more chemically bonded elements in a fixed ratio. |
| Concentration Of A Solution | The amount of solute dissolved per 1dm^3 of solution. |
| Concordant Results | Values that are close to each other and therefore represent reliable quantitative data. |
| Continuous Variable | A measured value which could be any number. |
| Control Variable | A factor that you must keep constant between experimental runs so that you can compare results. |
| Covalent Bond | A bond formed by a shared pair of electrons between 2 atoms nuclei. |
| Curly Arrows | Model the flow of electron pairs during reaction mechanisms. |
| Dative Covalent Bond | A bond formed by a shared pair of electrons that have been provided by one of the bonding atoms only. |
| Dehydration | A chemical reaction where a water molecule is eliminated from an organic compound. |
| Delocalised Electrons | Electrons that are shared between more than 2 atoms. |
| Dependent Variable | The factor that you observe in an experiment. |
| Discrete Variables | Variables that can only be particular defined numbers. |
| Displacement Reactions | A reaction in which a more reactive element takes the place of a less-reactive element in a compound. |
| Displayed Formula | A formula which Shows the relative positioning of atoms and the bonds between them. |
| Disproportionation | The oxidation and reduction of the same element in a redox reaction. |
| Distillation | A technique used to separate miscible liquids or solutions. |
| Dot Formulae | Gives the ratio between the number of compound molecules and the number of water molecules within the crystalline structure. |
| Dynamic Equilibrium | The equilibrium that exists in a closed system when the rate of the forwards reaction is equal to the rate of the backwards reaction and all the chemicals have a constant concentration. |
| E/Z Isomerism | A type of isomerism that is caused by the restricted rotation around the C=C where 2 different substituent groups are attached to each carbon atom. |
| Electrical Conductivity | The degree to which a specified material allows charge to be carried. |
| Electron | Carries a negative charge. Has a mass of 1/2000 and the number of electrons is equal to the number of protons. |
| Electron Configuration | The arrangement of electrons in an atom or ion. |
| Electron Shielding | The repulsion between electrons in different inner shells. Shielding reduces the net attractive force form the positive nucleus on the outer-shell electrons. |
| Electronegativity | A measure of the attraction of an electron in a covalent bond. |
| Electrophile | An electron-pair acceptor. |
| Elimination | An organic chemical reaction in which one reactant forms two products. |
| Empirical Formula | The simplest whole number ratio of atoms of each element present in a compound. |
| Endothermic | A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants, resulting in heat being taken in from the surroundings. Positive DeltaH. |
| Enthalpy H | The heat content that is stored in a chemical system. |
| Enthalpy Change of Combustion | The energy change that takes place when 1 mole of a substance is completely combusted. |
| Enthalpy Change Of FormationT | The energy change that takes place when 1 mole of a compound is formed from its constituent elements in their standard states under standard conditions. |
| Enthalpy Change Of Neutralisation | The energy change associated with the formation of 1 mole of water from a neutralisation reaction. |
| Enthalpy Change Of Reaction | The energy change associated with a given reaction. |
| Enthalpy Cycle | A pictorial representation showing alternative routes between reactants and products (Hess Law). |
| Enthalpy Profile Diagrams | A diagram of a reaction that allows you to compare the enthalpy of the reactants with the enthalpy of the products. |
| Equilibrium Constant, Kc | Kc shows the position of equilibrium. It Gives the measure of where the equilibrium lays. |
| Equilibrium Law | aA+bB⇌cC+dD Kc= [C]c[D]d [A]a[B]b |
| Ester | A functional group of –COO found in some organic molecules. |
| Esterification | The chemical reaction which forms an ester. |
| Exothermic | A reaction in which the enthalpy of the products is smaller than the enthalpy of the reactants, resulting in heat loss to the surroundings. Negative DeltaH. |
| Experiment | An ordered set of practical steps which are used to test a hypothesis. |
| Extraneous Variable | A factor that is not controlled or measured in an experiment but may introduce error into the results. |
| False Positive | When a positive result is produced but not due to the desired product being formed. |
| 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. |
| Fragmentation | The process in mass spectrometry that causes a positive ion to split into pieces, one of which is a positive fragmented ion. |
| Functional Group | A group of atoms that is responsible for the characteristic chemical reactions of a compound. |
| General Formula | The simplest algebraic formula for a homologous series. |
| Giant Covalent Lattice | A 3D structure of atoms that are all bonded together by strong covalent bonds. |
| Giant Ionic Lattice | A 3D structure of oppositely charged ions held together by strong electrostatic forces of attraction. |
| Giant Metallic Lattice | A 3D structure of positive ions and delocalised electrons held together by metallic bonds. |
| Global Warming | The increased average temperature of the planet and atmosphere, thought to be caused by increase concentrations of Carbon Dioxide. |
| Group | A vertical column in the periodic table. Elements have similar chemical properties and their atoms have the same number of electrons in the outer shell. |
| Halogenation | An addition reaction where a halogen is added across the C=C. |
| Haloalkanes | A group of chemical compounds derived from alkanes, containing halogens. |
| Hess' Law | States that the enthalpy change in a chemical reaction is independent of the route it takes. |
| Heterogeneous Catalyst | A catalyst which is in a different phase from the reactant. |
| Heterolytic Fission | Happens when each bonding atom receives one electron from the bonded pair to form 2 radicals. |
| Homogeneous Catalyst | A catalyst which is in the same phase as the reactant. |
| Homologous Series | A series of organic compounds that have the same functional group with successive members differing by a CH2. |
| Homolytic Fission | Happens when one bonding atom receives both electrons from the bonding pair. |
| Hydrated | A crystalline compound containing water molecules. |
| Hydration/Hydrolysis | A reaction where water is a reactant. |
| Hydrocarbons | Compounds that contain only carbon and hydrogen atoms. |
| Hydrogen Bond | A strong permanent dipole-dipole attraction between an electron deficient H atom and a lone pair of electrons on O, N or F. |
| Hydrogenation | An addition reaction where hydrogen is added across the C=C. |
| Hypothesis | A prediction and explanation of the chemistry behind the prediction. |
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