Unit one Flashcards
relative atomic mass
the mean mass of an element compared to the mass of one twelfth of a carbon-12 atom
relative isotopic mass
the mean mass of an isotope compared to tge mass of one twelfth of carbon-12
isotopes
isotopes have the same number of electrons and protons but a different number of neutrons
spectrometer
used to measure the mass of an isotope/element
hydrochloric acid
HCl
nitric acid
HNO3
sulphuric acid
H2SO3
silver chloride
AgCl
sodium hydroxide
NaOH
calcium carbonate
CaCO
ammonium
NH4
what is the ionic charge of a magnesium ion
+2
what is the ionic charge of a fluoride ion
-
what is the ionic charge of an aluminum ion
+3
what is the ionic charge of a carbonate ion
-2
what is the ionic charge of a sulphate ion
-2
what is the ionic charge of a hydroxide ion
-
what is the ionic charge of an ammonium ion
+
what are the seven elements that exist as diatomic molecules
Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine and Iodine
moles =
mass / Mr
moles =
number of atoms / avogadros number
Avogadro’s number
6.02 x 10^23
moles =
volume (dm^3) / 24
moles =
concentration (moldm^-3) x volume (dm^3)
steps for empirical formula
calculate moles, divide by smallest, whole number ratio, empirical formula
multiple =
relative molecular mass / mass of empirical formula
% error =
[(number of readings x error) / amount] x 100
how to identify x in a salt
calculate moles of water lost, ratio of anhydrous salt to water, moles of anhydrous salt, find Mr, identify x
ideal gas equation
pressure (pa) x volume (m^3) = moles x 8.314 (Jmol^-1K^-1) x temperature (K)
how to convert C to K
K = C + 273
how to covert kPa to Pa
1kPa = 1000Pa
room temp =
298K (25C)
regular pressure =
100000Pa (100kPa)
atom economy =
(molecular mass of wanted product / molecular mass of products) x 100
percentage yield =
(actual amount / theoretical amount) x100
