U1-2-2 - Ionisation Energy
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1st ionisation energy is the energy required to ________ from one mole of free gaseous atoms.
1st ionisation energy is the energy required to remove one mole of electrons from one mole of free gaseous atoms.
1st ionisation energy is the energy required to remove one mole of electrons from _______ of free gaseous atoms.
1st ionisation energy is the energy required to remove one mole of electrons from one mole of free gaseous atoms.
1st ionisation energy is the energy required to remove one mole of electrons from one mole of __________ atoms.
1st ionisation energy is the energy required to remove one mole of electrons from one mole of free gaseous atoms.
What is wrong with this ionisation equation?
Atoms must be free (just F, not F2)
What is wrong with this ionisation equation?
Atoms must be gaseous (g, not l)
Why does 1st IE increase going across a period? 1. ________________________________ 2. Outer e− is more strongly attracted to nucleus
Increasing nuclear charge
Why does 1st IE increase going across a period? 1. Increasing nuclear charge 2. Outer e− is ________________
more strongly attracted to the nucleus
Why does 1st IE decrease going down group 1? 1. Outer e− is ________________________ 2. Outer e− is less strongly attracted to nucleus
more screened
Why does 1st IE decrease going down group 1? 1. Outer e− is more screened 2. Outer e− is __________________________
less strongly attracted to nucleus
Sodium has the electron arrangement 2,8,1. Why is the 2nd IE greater than the 1st IE? 1. 2nd electron is removed from a 2. 2nd electron is less screened (than the 1st)
removed from a full/stable electron shell
Sodium has the electron arrangement 2,8,1. Why is the 2nd IE greater than the 1st IE? 1. 2nd electron is removed from a full/stable electron shell 2. 2nd electron is ____________ (than the 1st)
less screened