quick definitions and equations Flashcards
alicyclic
containing carbon atoms joined together in a ring that is not aromatic
aliphatic
containing carbon atoms joined together in straight or branched chains
ionic bond
the electrostatic attraction between positive and negative ions
homolytic fission
breaking of a covalent bond with one of the bonded electrons going to each atom, forming two radicals
acid
a species that releases H+ ions in an aqueous solution
activation energy
the minimum energy required to start a reaction by the breaking of bonds
alkali
a type of base that dissolves in water, forming hydroxide ions OH-
atomic orbital
a region around the nucleus that can hold up to two electrons with opposite spins
electrophile
electron deficient
attracted to an electron rich atom - nucleophile
accepts a pair of electrons to form a covalent bond
standard solution
a solution of a concentration which is accurately known
homogulous series
a family of compounds with the same chemical properties, differing by a CH2 group
heterolytic fission
breaking of a covalent bond with both of the bonded electrons going to the same atom, forming a cation and a anion
neutralisation
a chemical reaction in which an acid and a base react together to produce a salt
nucleophile
electron rich
attracted to an electron deficient atom - electrophile
donates a pair of electrons to form a covalent bond
π bond
a bond formed by the sideways overlap of two p-orbitals, with the electron density above and below the plane of the bonding atoms
curly arrow
shows the direction of movement of a pair (fully headed arrow) of electrons
relative isotopic mass
the mass of an atom of an isotope relative to 1/12 of the mass of a carbon-12 atom
oxidising agent in terms of electron transfer
accepting electrons from other species
a covalent bond
the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms
electronegativity
the attraction of a bonded atom for the pair of electrons in a covalent bond
functional group
the part of the organic molecule responsible for its chemical properties
structural isomer
compound with the same molecular formula but different structural formulas
isotopes
atoms of the same element with the same number of protons but different numbers of neutrons and different masses
dipole
the separation of opposite charges
stereoisomers
compounds with the same structural formula but a different arrangement of the atoms in space
radical
species with an unpaired electron
σ bond
a type of covalent bond which forms when atomic orbitals overlap head-on
can rotate freely
explanation for shapes of molecules
𝑥 bonding regions
𝑦 lone pairs
electrons repel
saturated hydrocarbon
only contains single bonds
unsaturated hydrocarbon
contains at least one C=C double bond
relative atomic mass
the weighted average mass of an atom of an element, taking into account its naturally occurring isotopes, relative to 1/12 of the relative atomic mass of an atom of carbon-12
relative molecular mass
the mass of that molecule compared to 1/12 of the relative atomic mass of an atom of carbon-12
atom economy equation
% atom economy = mass of desired products / total mass of reactants × 100
atom economy
how many atoms in the reactant are found in the useful products, compared to how many are wasted
first ionisation energy
the energy required to remove one mole of electrons from one mole of atoms of an element in a gaseous state to form one mole of gaseous ions
Avogadro constant
the number of atoms per mole of the carbon-12 isotope = 6.02x10^23
dative bond
a shared pair of electrons in which the bonded pair has been provided by only one of the bonded atoms
