Headstart Flashcards
relative mass of electron
1/1836 AMU
isotopes
atoms of the same element which have different number of neutrons
why do you use the word ‘relative’ when talking about the abundance of isotopes
because we are comparing the amount of each isotope of the same element
How to calculate RAM (Relative Atomic Mass)
[mass isotope 1 (abundance%) + mass isotope 2 (abundance%) +ect]/
100
ionic bond
Strong electrostatic forces of attraction between oppositely charged ions
mole calculations
moles= mass/Mr moles= number of particles-N/avogadro's constant-Na (6.022*10^23) moles= cv - c= molarity M
atom economy
mass of useful product / total mass of reactants - percentage form
empirical formula
simplest whole number ratio of elements in a compound
concentration
the amount of solute in a given volume of solution/ number of moles of solute per litre of solution
hydrocarbon
molecule that contains only hydrogen and carbon
combustion
burning in oxygen
complete combustion and incomplete combustion of alkanes and alkenes
complete- alka/ene + oxygen –> carbon dioxide + water
incomplete- alka/ene + oxygen –> carbon (soot) + water
–> carbon monoxide + water
calculating energy release
Q = mcAT q= quantity of energy (kJ) m= mass of water (kg) c= specific heat capacity - 4.18 AT= change in temp (C)
isomers
compounds with the same molecular formulae but different structural formulae
systematic error
constant bias in a measurement that cannot be eliminated by repeating the measurement