Ionisation Energies - OCR - Unit 1
- Created by: Eleanor
- Created on: 17-03-13 09:49
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- Ionisation Energies
- Down the periodic table
- Ionisation energy DECREASES
- An increase in the number of electron shells
- Distance of the outer electrons from nucleus increases
- Weaker force of attraction on the outer electrons
- Distance of the outer electrons from nucleus increases
- More inner shells
- Increased electron shielding
- Less attraction on the outer electrons
- Increased electron shielding
- Increased atomic radius
- Less attraction means that electrons are not pulled as close to the nucleus
- Across the periodic table
- Electrons added to the same energy level
- Ionisation energy INCREASES
- The number of protons in the nucleus increases
- A stronger nuclear attraction acting on the electrons
- The increased nuclear charge pulls the electrons towards it
- Decrease in atomic radius
- First Ionisation energy: Definition
- The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
- Affecting Factors
- Atomic Radius
- Greater the atomic radius, smaller the nuclear attraction
- Nuclear Charge
- The greater the nuclear charge, the greater the attractive force on the outer electrons
- Electron Shielding
- Inner shells of electrons repel outer shell electrons
- The more inner shells there are, the larger the shielding effect
- Inner shells of electrons repel outer shell electrons
- Atomic Radius
- First Ionisation energy equation
- X(g)----->X+(g) + e-
- Each successive ionisation energy is greater than the first
- This is due to the distance of each electron from the nucleus is decreasing
- Down the periodic table
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