3.1 - The periodic table Flashcards
Define “first Ionisation Energy (1st I.E.)” of an element.
The energy required to remove ONE ELECTRON from ONE MOLE OF ATOMS in a GASEOUS STATE.
What are the 3 factors affecting ionisation energy
- Atomic Radius
- Nuclear Charge
- Electron shielding
Describe the trend of Atomic Radius.
The LARGER the atomic radius, the SMALLER the nuclear attraction experienced by the outer electrons.
EXPLAIN the trend of Atomic Radius.
The positive charge of the nucleus is essentially further away from the outermost electron.
Describe the trend of the Nuclear charge.
The HIGHER the nuclear charge, the LARGER the attractive force on the outer electrons.
Describe Electron Shielding.
Inner shells of electrons repel the outer-shell electrons because they are all negative.
Describe the trend of Electron Shielding.
The more inner shells there are, the larger the shielding effect and the smaller the nuclear attraction experienced by the outer electrons.
Why is each successive ionisation energy higher than th one before?
As each electron is removed, there is less repulsion between the remaining electrons and each shell will be drawn in slightly closer to the nucleus.