chem definitions Flashcards
isotopes
are atoms of the same element with different numbers of neutrons and different masses
relative isotopic mass
is the mass of an isotope relative to 1/12 th of the mass of an atom of carbon - 12
relative atomic mass
is the weighted mean mass of an element relative to 1/12 th of the mass of an atom of carbon - 12
avogadro’s constant
6.02 x 10^23
molar mass
is the mass per mole of a substance (g mol^-1)
molecular formulae
the number of atoms of each element in a molecule
empirical formulae
is the simplest whole-number ration of atoms of each element in a compound
relative molecular mass
compares the mass of a molecule with the mass of an atom of carbon-12
relative formula mass
compares the mass of a formula unit with the mass of an atom of carbon-12
molar gas volume
is the volume per mole of gas molecules at a stated temperature and pressure
room temperature and pressure (RTP)
25 degrees Celsius / 298 K
101 kPa / 1 atm pressure
ideal gas equation
pV = nRT pressure (Pa) volume (m^3) amount of gas molecules (mol) R = gas constant (8.31 J mol^-1 K^-1) temperature (K)
celcius to kelvin
+ 273
kPa to Pa
x 10^3
percentage yield
= (actual yield) / (theoretical yield)
x100 for percentage
atom economy
is a measure of how well atoms have been utilised
= (sum of molar masses of desired products) / (sum of molar masses of all products)
x100 for percentage
strong acids
e.g HCL
releases all its hydrogen atoms into solution as H+ ions completely dissociates in aqueous solutions
weak acids
e.g ethanoic acid (CH3COOH)
only releases a small proportion of its available hydrogen atoms into solution as H+ ions.
partially dissociates in aqueous solution
alkali
is a base that dissolves in water releasing hydroxide ions (OH-) into the solution
acid + alkali
= salt + water
ionic bonding
is the electrostatic attraction between positive and negative ions.
it holds together cations and anions in ionic compounds
properties of ionic compounds
have high melting and boiling points
tend to dissolve in polar solvents: water
conduct electricity only in liquid state or in aqueous solution
covalent bonding
is the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms
dative covalent bond
is a covalent bond in which the shared pair of electrons has been supplied by one of the bonding atoms only.
electronegativity
the attraction of a bonded atom for the pair of electrons in a covalent bond
intermolecular forces
are weak interactions between dipoles of different molecules
split into 3 categories: induced dipole-dipole interactions, permanent dipole-dipole interactions
hydrogen bonding
induced dipole-dipole interactions (london forces)
are weak intermolecular forces that exist between all molecules
permanent dipole-dipole interactions
act between the permanent dipoles in different polar molecules
simple molecular substance
= is made up of simple molecules - small units containing a definite number of atoms with a definite molecular formula
ionisation energy
measures how easily an atom loses electrons to form positive ions
first ionisation energy
is the energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions
disproportionation
is a redox reaction in which the same element is both oxidised and reduced
enthalpy
is a measure of the heat energy in a chemical system
enthalpy change
= enthalpy of products - enthalpy of reactants
activation energy
the energy input required to break bonds acts as an energy barrier to the reaction
is the minimum energy required for a reaction to take place
standard enthalpy change of reaction
is the enthalpy change that accompanies a reaction in the molar quantities shown in a chemical equation under standard conditions, with all reactants and products in their standard states
enthalpy change of formation
is the enthalpy change that takes place when one mole of a compound is formed from its elements under standard conditions, with all reactants and products in their standard states
standard enthalpy change of combustion
is the enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, with all reactants and products in their standard states
standard enthalpy change of neutralisation
is the energy change that accompanies the reaction of an acid by a base to form one mole of h20(l), under standard conditions, with all reactants and products in their standard states
specific heat capacity
water?
is the energy required to raise the temperature of 1g of a substance by 1K
water = 4.18 J g^-1 K^-1
calculating energy change formulae
q = mcT
q = heat energy m = mass that changes temperature c = specific heat capacity T = temperature change