topic 2 Flashcards
what are the three subatomic particles?
protons, nuetrons and electrons
what is the relative mass and charge of subatomic particles?
Relative Mass Relative Charge
Proton 1 +1
Neutron 1 0
Electron 1/1836 -1
what is an isotope?
an atom of the same element with the same number of protons and different number of neutrons
What does an ion with a +2 charge in mass spectrometry look like?
these ions appear at half their mass number on the spectrum
What are the isotopes of chlorine?
35Cl (75%) and 37Cl (25%)
what are the isotopes of bromine?
define ionisation energy?
energy required to move one mole of gaseous atom to form gaseous 1+ ions
What is the shape of the s orbital?
spherical
what is the shape of the p orbital?
dumbell-shaped
What are the factors that affect ionisation energy?
nuclear charge
atomic radius
shielding
how does nuclear charge affect ionisation energy?
more protons —> higher ionisation energy
how does atomic radius affect ionisation energy?
larger radius —> lower ionisation energy
How does shielding affect ionisation energy?
more inner shells —> lower ionisation energy
What happens to atomic raduis across and down a group?
across it decreases
down it increases
Why do large jumps of ionisation energy occur?
it occurs when electrons are removed from the inner shell
What is hunds rule?
Electrons occupy empty orbitals before pairing
what is pauli exclusion principle?
electrons in an orbital must have opposite spins
why do elements in the same group have similar properties?
because of the same valence electrons
what happens to ionisation energy down and across a periodic table?
down, it will decrease because of the increase in sheilding
across it will increase because of an increase in nuclear charge
