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definitions

TermDefinition
daltons atomic theory all things are made up of small particles called atoms all atoms are indivisible
cathode rays streams of electrons
continuous spectrum many wavelengths or colours with no gaps
energy level the fixed energy value an electron in an atom may have
ground state electrons occupy the lowest energy level
excited state electrons occupy higher energy levels
heisenbergs uncertainty principle it is impossible to measure at the same time both the velocity and position of an electron
sub level a subdivision of a main energy level and consists of one or more orbitals of the same energy
orbital a region in space where there is a high possibility of finding an electron
hunds rule of maximum multiplicity when 2 or more orbitals of equal energy are available, electrons occupy them single before filling them in pairs
the pauli exclusion principle no more than 2 electrons may occupy an orbital and they must have opposite spin
element a substance that cannot be broken down into simpler substances by chemical means
triad group of 3 elements with similar chemical properties in which the atomic weight of the middle is equal to the approx equal to the average weight of the other 2
mendeleevs periodic law elements are arranged in order of increasing atomic weight, properties of elements occur periodically
modern periodic table/law arrangements of elements in order of increasing atomic number
newlands octaves arrangement of elements where the 1st and 8th element had similar properties
mass number sum of protons and neutrons in the nucleus of the atom
atomic number number of protons in the nucleus of the atom
isotope atoms of the same element which have different mass numbers due to different numbers of neutrons
relative atomic mass average mass of the element as it occurs naturally in nature compared to 1/12 of the C12 isotope
mass spectrometer vaporisation, ionisation, acceleration, separation, detection
principle of mass spectrometry charged particles moving in a magnetic field are deflected to different extents according to their masses and separated accordingly
atomic radius half the distance between the nuclei of two atoms of the same element that are joined together by a single covalent bond
first ionisation energy the minimum energy required to completely remove the most loosely bound electron from a neutral gaseous atom in it's ground state
second ionisation energy the energy required to remove an electron from an ion with one positive charge in the gaseous state
electronegativity the relative attraction that an atom in a molecule has for the shared pair of electrons in a covalent bond
radioactivity the spontaneous breaking up of unstable nuclei with the emission of one or more types of radiation
nuclear reaction the process that alters the composition, structure or energy of an atomic nucleus
transmutation the changing of one element into another
half life the time it takes for half the nuclei in any given sample to decay
radioisotope a radioactive isotope
radiocarbon dating a technique used to determine the age of an object containing carbon, based on the ratio of carbon 14 to carbon 12
compoud a substance made up of two or more different chemicals combined together
Octet Rule states that when bonding occurs, atoms tend to reach an electron arrangement with eight electrons in the outermost shell
ion charged atom or groups of atoms
transition metal forms atleast one ion with a partially filled d sublevel
electronegativity relative attraction an atom in a molecule may have for a shared pair of electrons in covalent bond
van der waals weak attractive forces between molecules resulting from the formation of temporary dipoles.
dipole dipole forces of attraction between the negative pole of one molecule and the positive pole of another.
hydrogen bonds particular types of dipole-dipole attractions between molecules in which the hydrogen atoms are bonded to nitrogen, oxygen or fluorine. The hydrogen atom carries a partial positive charge and is attracted to the electronegative atom in another molecule.
relative molecular mass the sum of the relative atomic masses of all the atoms in a molecule of the compound.
one mole 6x10^23
Conjugate acid Acid will change to a conjugate base when it donates a proton
conjugate base Base will change to a conjugate acid when it accepts a proton. The stronger the acid, the weaker the conjugate base.
conjugate acid-base pair any pair consisting of an acid and a base which differ by one proton.
neutralisation the reaction between an acid and a base to form a salt and water.
concentration the amount of solute that is dissolved ina given volume of solution
primary standard a substance which can be obtained in a stable, pure and soluble solid form
rate of reaction the change in concentration per unit time of any one reactant or product.
catalyst alters the rate of chemical reaction but is not used up in the reaction.
activation energy the minimum energy which colliding particles must have for a reaction to occur.
structural isomers compounds with the same molecular formula but different structural formulae.
aliphatic compounds an organic compound that consists of open chains of carbon atoms and closed chain compounds (rings) that resemble them in chemical properties.
aromatic compounds compounds that contain a benzene ring in their structure.
octane number a measure of its tendency to resist knocking
catalytic cracking the breaking down of long-chain hydrocarbon molecules into short chain molecules for which there is greater demand.
heat of reaction the heat change when the number of moles of reactants indicated in the balanced equation for the reaction react completely
heat of combustion the heat change when one mole of the substance is burned completely in excess oxygen.
bond energy energy required to break one mole of covalent bonds and to separate the neutral atoms completely from each other.
heat of neutralisation energy required to break one mole of covalent bonds and to separate the neutral atoms completely from each other.
hess's law if a chemical reaction takes place in a number of stages, the sum of the heat changes in the separate stages is equal to the heat change if the reaction is carried out in one stage.
law of conservation of energy that energy cannot be created or destroyed, but can only be converted from one form of energy into another.
functional group an atom or group of atoms which is responsible for the characteristic properties of a series of organic compounds.
substitution reaction a chemical reaction in which an atom or group of atoms in a molecule is replaced by another atom or group of atoms.
mechanism the detailed step by step description of how the overall reaction occurs
addition reaction one in which two substances react together to form a single substance
polymers long chain molecules made by joining together many small chain molecules
organic synthesis he process of making organic compounds from simpler starting materials.
chromatography a separation technique in which a mobile phase carrying a mixture moves in contact with a selectively adsorbent stationary phase
Afbau Principle states that when building up the electronic configuration of an atom in its ground state, the electrons occupy the lowest available energy level.
Law of conservation of mass states that the total mass of the products of a chemical reaction is the same as the total mass of the reactants.
law of conservation of matter states that in any chemical reaction, matter is neither created nor destroyed, but merely changes from one form into another. Radioactivity
Created by: katieduggan12
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