IONISATION ENERGY ((OCR)) Flashcards
What is First Ionisation Energy?
The energy needed to remove one mole of electrons from one mole of atoms in their gaseous state to create one mole of 1+ ions that are also in a gaseous state.
What are factors that affect Ionisation Energy?
Atomic radius |Distance between nucleus and electrons |
Nuclear Charge | Protons in the nucleus |
Electron Shielding | Inner & outer shell repulsion |
What happens to the ionisation energy needed when you go across a period?
The number of protons increases so the ionisation energy you need increases
How can you predict electron arrangement from a graph?
There is usually an exponential increase of ionisation energy used after a shell’s electrons have been completely removed.
This can tell you how many electrons are in the shells.
How do successive ionisation energies work?
After the first ionisation energy, more energy is needed to remove another electron from the ion and so forth.
How many ionisation energies does Helium have?
2 | because it has two electrons.
How many ionisation energies does Neon have?
10 | because it has ten electrons
What is electron shielding?
The repulsion between inner electron shells and outer shells.
What creates the attraction between the electrons and the nucleus in a species?
Protons
Does a bigger distance between the nucleus and electron shells lower the ionisation energy needed?
Yes.
Which electron is the first to be lost and why?
The electron in the highest energy level (it experiences the least nuclear attraction.)
What is the rule for successive ionisation energies?
Successive ionisation energies are greater than the previous.
What’s the trends for ionisation energies down a group?
Decreases because atomic radius of elements (down a group) increase.
What’s the exception for the rule for ionisation energy trends?
Beryllium to Boron because it marks the filling of the 2p subshell which electrons are easier to remove.
