Electronic Structure 2.2.1 Flashcards
Define First Ionisation Energy.
The energy required to remove a mole of the first electrons form each atom in a mole in the gaseous state.
Why do successive Ionisation Energies increase?
Because after the first electron you are removing negatively charged electrons from positively charged ions.
What factors affect Ionisation energy?
Radius of the atom/ion
The charge of the atom/ion
The sub-shell of the electron
Shielding
What is the equation for the number electrons a shell can hold?
2n²
How many electrons can the 1st, 2nd, 3rd and 4th shells hold?
1st shell: 2 electrons
2nd shell: 8 electrons
3rd shell: 18 electrons
4th shell: 32 electrons
What is an Orbital?
A region of space within an atom that can hold upto two elctrons with opposite spins
What are the Sub-shells called?
s
p
d
f
what is the maximum electrons that can fit in each Sub-shell?
S sub-shell: 2 electrons
P sub-shell: 6 electrons
D sub-shell: 10 electrons
F sub-shell: 14 electrons
What shape is a S orbital?
Spherical
What shape is a P orbital?
Roughly dumbell shaped
What is the order of Orbitals?
1s 2s 2p 3s 3p 3d 4s 4p 4d 4f …
What is the order that Orbitals are filled in?
1s 2s 2p 3s 3p 4s 3d 4p 4d
What is a Positive ion called?
Cations
because as Ian says cats are positive
What is a Negative ion called
Anion
What is evidence for the advanced electronic stucture?
1st ionisation energies largely increase as atomic number increase.
However drops when a new Sub-shell is started.
