Ionisation energy Flashcards
What is first ionisation energy?
The amount of energy required to remove one electron from each atom in 1 mole of gaseous atoms of an element to form 1 mole of gaseous 1+ ions
What is the equation for first ionisation energy?
X(g) —> e⁻ + X⁺(g)
How many ionisation energies can atoms have?
As many ionisation energy as as many electrons they have
Why do ionisation energies increase?
More energy is needed as each electron is removed
When is there a greater increase in ionisation energy?
When the electrons is from the next shell?
What is nuclear attraction?
The strength of the attraction between the nucleus and the outer electrons at are being removed and the greater the nuclear attraction, the greater the ionisation energy
What is nuclear charge and how does it effect nuclear attraction?
The number of protons in the nucleus and as the nuclear charge increases, the nuclear attraction increases
What are the factors that effect nuclear attraction?
Nuclear charge, size of atomic radius and shielding
What is the size of atomic radius and how does it effect nuclear attraction?
It is the distance between the nucleus and electrons and as atomic radius increases, nuclear attraction decreases
What is shielding and how does it effect nuclear attraction?
It is the number of inner shells and as shielding increases, nuclear attraction deceases
What happens to nuclear charge across a period?
The nuclear charge increases because there are more protons
What happens to atomic radius across a period?
The distance will decrease as there is greater attraction to the outer shell as there are more protons so smaller atomic radius
What happens to shielding across a period?
Shielding stays the same as electrons are added but it is to the same shell
What happens to first ionisation energy across a period?
There is a greater nuclear attraction so there is also a greater first ionisation energy
What happens to nuclear charge down a group?
As you go down, the nuclear charge increases but it has little effect
