electron structure Flashcards
define first ionisation energy
the energy required to remove one mole of electrons from one mole of gaseous atoms
what are the 3 factors that affect ionisation energy
position of electron
proton number
shielding
how will the proton number affect ionisation energies
the more protons the greater the force of attraction so the harder it is to remove electrons.
(higher IE)
how will the amount of shielding affect the ionisation energies
the more complete inner shells (more shielding) the easier it is to remove electrons
(lower IE)
how does the distance between the electron and the nucleus affect the IE
the further the electron from the nucleus the less energy required to remove it
(lower IE)
how do electron shells affect the IE
electrons in the same shell have similar attraction to the nucleus
(similar IE)
which is easier to remove P electrons or S electrons
P electrons are easier to remove
why are P subshell electrons easier to remove that S subshell electrons
P subshell is shielded by the full S subshell and is higher in energy
how do paired electrons affect the IE
paired electrons are easier to remove as they are both negative so the repel each other
(lower IE)
why does the IE increase when moving to a PQS that is closer to the nucleus
electrons in shells closer to the nucleus experience much less shielding therefore have a greater attraction to the nucleus.