Atomic Structure And The Periodic Table Flashcards
mass of an electron
1/1840
mass number
total number of particles in the nucleus
atomic number
number of protons in the nucleus
number of neutrons
mass number - atomic number
isostopes
atoms of the same type with a different number of neutrons
relative atomic mass
the average mass of an atom of an element, relative to 1/12th the mass of as carbon-12 atom
relative isotopic mass
the mass of one mole of an isotope of the element expressed on a scale on which one mole of the atoms of the C-12 isotope has a mass of exactly 12 units.
relative molecular mass
Average mass of a molecule of a substance relative to 1/12th the mass of a carbon 12 atom
determining relative atomic mass from mass spectrometer
- the sample is vaporised
- the sample is ionised
- ion is accelerated by an electric field
- ions pass through the magnetic field and are deflected
- ions are detected and recorded
the size of the peaks in mass spectra
number/abundance of each type of ion
chlorine mass spectra
chlorine has two isotopes at mass 35 and mass 37, the height of 35 trace is three times that of 37 so its three times more abundant
first ionisation energy
energy required to remove one electron from one moles of gaseous atoms to produce one mole of 1+ gaseous ions
attraction of the electron to the nucleus
· The charge on the nucleus – the higher the charge, the greater the attraction
· The distance from the nucleus - the greater the distance, the less the attraction
· Shielding from inner electrons – the more inner electrons, the less the attraction.
reasons for first ionisation energy to increase across a period
- same number of shells
- increased nuclear charge
- greater attraction to the nucleus
reasons for first ionisation energy to decrease down a group
- increasing number of shells
- greater shielding
- decreased attraction to the nucleus