TWChemAQAY2 1-100 A-F

A result that's really close to real answer/true value.

A molecule that cannot be superimposed on its mirror image.

A molecule formed of two identical carboxylic acid molecules, joined via an oxygen atom with the carbonyl groups either side.

• An equilibrium constant specific to weak acids that relates the acid concentration to the concentration of H+ ions.
• Ka = [H+][A-]/[HA]

A buffer with pH of less than 7 containing a mixture of a weak acid with one of its salts.

A molecule which contains the functional group COCl.

When an acyl group (-COR) is added to a molecule.

A type of polymer formed by joining small alkenes (monomers) together.

The attraction between a substance and the surface of a solid stationary phase in thin-layer chromatography and gas chromatography.

The question an experiment is trying to answer.

A substance with the general formula:

C_nH2_n+1OH

A substance with general formula:

• C_nH_2nO
• Which has a hydrogen and one alkyl group attached to a carbonyl carbon atom. (Carbonyl atom is Carbon 1).

A carboxylic acid derivative which contains the functional group: CONH₂.

The -CONH- group which is found between the monomers in a polypeptide.

A molecule where one or more of the hydrogen atoms in ammonia have been replaced with an organic functional group, such as an alykl or aromatic group.

A molecule with an amino (NH₂) and a carboxyl group (COOH).

Having both acidic and basic properties.

One you do not expect, which markedly does not fit with the pattern of the others.

A compound that contains a benzene ring.

An equation which links the rate constant k, to temperature and activation energy.

A graph where 1/temperature is plotted against ln k. (the natural log of the rate constant)

Where a reaction is catalysed by one of its products (positive feedback).

One of the four molecules (adenine, guanine, thymine, cytosine) attached to the sugar-phosphate backbone of DNA.

A buffer with a pH of more than 7 containing mixture of a weak base with one of its salts.

A ligand that can form to co-ordinate bonds to a complex ion.

Will break down naturally.

A mixture of methy esters of fatty acids which can be used as a carbon-neutral fuel.

The enthalpy change when all the bonds of the same type in 1 mole of gaseous molecules is broken.

An enthalpy cycle that allows you to calculate the lattice enthalpy change of formation for a system.

A proton donor

A proton acceptor.

A solution that resists changes in pH when small amounts of acid or alkali are added.

A graph that shows the relationship between a measurement taken in an experiment and a property of a substance. It can be used to determine and unknown value.

A ion containing a positively charged carbon atom.

An organic compound which contains a carbonyl group (C=O) as its only functional group.

A molecule that contains a carboxyl group (COOH).

A substance that increases the rate of a reaction by providing an alternative pathway with  lower activation energy. The catalyst is chemically unchanged (or regenerated) at the end of the reaction.

When impurities in a reaction mixture bind to the catalyst, blocking reactants from being adsorbed and reducing the effectiveness of the catalyst.

A chemical reaction in which hydrogen is added to an unsaturated molecule by reacting the molecule with molecular hydrogen (H₂) in the presence of a catalyst.

Data that can be sorted into categories (functional group categories for example).

A surfactant which is positively charged.

The relationship between two variables where changing one affects a change in the other.

The voltage (potential difference) between two half-cells in an electrochemical cell.

When monodentate ligands are substituted with multidentate ligands, the number of particles and the entropy of the system increases without enthalpy changing significantly. Reactions that result in an increase in entropy and little change in enthalpy are more likely to occur, so multidentate ligands form much more stable complexes than monodentate ligands.

Nuclei in different environments absorb energy of different frequencies. NMR spectroscopy measures these differences relative to a standard substance - the difference is call the chemical shift (δ).

A carbon atom that has four different groups attached.

A visual record (such a a pattern of spots on a paper) of the results of a chromatography experiment.

An analytical technique which uses a mobile phase and a stationary phase to separate out mixtures into their constituent components.

A platinum containing complex ion with a square planar shape than can be used as an anti-cancer drug.

A special type of E/Z isomerism where two of the attached groups on opposite ends of the isomer are the same.

A reaction where after a period of time there's a sudden increase in the amount of product.

An instrument for measuring how much light is absorbed by a sample.

A type of chromatography where the stationary phase is a column packed with a solid and the mobile phase is liquid solvent.

A  metal ion surrounded by co-ordinately bonded ligands.

A type of polymer formed through a series of condensation reactions.

A chemical reaction in which two molecules become joined together and a small molecule is eliminated (usually water).

A industrially used process for producing sulfuric acid.

Data which can take any value in the range.

A method of following a reaction by monitoring the formation of a product or the loss of a reactant, over the course of the reaction.

A variable that is kept constant throughout the experiment.

A covalent bond in which both electrons in the shared pair come from the same atom. Also called a dative covalent bond.

The relationship between two variables.

A substance that may cause chemical burns.

The block of elements in the middle of the periodic table.

A type of sub-level. Each can hold 10 electrons.

A device that can store readings taken at set intervals for later analysis.

A covalent bond in which both electrons are donated by the same atom (also known as a co-ordinate bond).

The variable you measure in an experiment.

A solvent which has had all of its hydrogen atoms substituted for hydrogen's heavier isotope deuterium.

A heavy isotope of hydrogen. It has an extra neutron.

Any acid with two hydrogens in each molecule (i.e. sulfuric acid).

Data which must take certain values (number of wheels on a vehicle, number of neutrons in an atom).

A method of separating liquids of different boiling points by gradually heating them and evaporating them off separately.

A covalent bond between two different sulfurs in two different -thiol groups.

An anhydrous salt, such as magnesium sulfate or calcium chloride that can be used to removed water from a product.

A type of stereroisomerism that is caused by the restricted rotation around a C=C bond. Each of the carbon atoms must have two different groups attached.

An electrical circuit made from two metal electrodes dipped in salt solutions and connected by a wire.

A list of electrode potentials written in order from most negative to most positive.

The voltage measured when a half cell is connected to a standard hydrogen electrode.

Another name for the cell potential. The voltage between two half cells in an electrochemical cell.

An electron deficient (and usually positively charged) species which is attracted to regions of high electron density (such as double bonds for example).

A reaction mechanism where an electrophile substitutes for an atom (or group of atoms) in a molecule.

A molecule that has the same structural formula as another molecule but with four groups arranged around a chiral carbon atom so that it is a non-superimposable mirror image of the other molecule.

The point during a titration at which all the acid is just neutralised - a pH curve becomes vertical at this point.

A reaction which absorbs energy (ΔH is positive).

The amount of energy needed to push an electron into a higher orbital.

The enthalpy change when one mole of a compound in its standard state is converted into its gaseous atoms.

The enthalpy change when a single mole of an element in its standard state is converted into its gaseous atoms.

The enthalpy change when 1 mole of products is made up of its constituents at their standard states and under standard conditions = room temp (298K) + pressure (100 KPa)

The enthalpy change when one mole of aqueous ions is formed from one mole of gaseous ones.

The enthalpy change when one mole of an ionic substance dissolves in enough solvent to form an infinitely dilute solution.

A measure of the amount of disorder in a system (e.g. the number of ways that particles can be rearranged and the number of ways that the energy can be shared out between those particles).

A ratio worked out from the partial pressures of the gaseous products and reactants once a reversible reaction has reached equilibrium.

A molecule that contains the functional group RCOOR.

The -COO- group which is found between monomers in a polyester.

Forming an ester by heating a carboxylic acid and an alcohol in the presence of a strong acid catalyst.

A reaction that gives out energy (ΔH is negative).

A long chain carboxylic acid which can combine with glycerol to form a fat or an oil.

A reaction that once started will carry on to completion without any energy being supplied to it.

A blue solution of copper (II) ions dissolved in sodium hydroxide which can be used to distinguish between carbonyl compounds (aldehydes and ketones).