1 - Electron configuration Flashcards
Electron shells are split into __ _____
4 subshells
What are the 4 types of subshell?
s, p, d and f
How many orbitals does the s subshell contain?
1 orbital
How many electrons can the s orbital hold?
2 electrons
How many orbitals does the p subshell contain?
3 orbitals
How many electrons can the p orbital hold?
6 electrons
How many orbitals does the d subshell contain?
5 orbitals
How many electrons can the d orbital hold?
10 electrons
How many orbitals does the f subshell contain?
7 orbitals
How many electrons can the f orbital hold?
14 electrons
For transition metals Cr and Cu the 3d subshell must be…
half full (5 electrons) or full (10 electrons)
Define ‘ionisation energy’
Ionisation energy is the minimum amount of energy required to remove 1 mole of electrons from 1 mole of atoms in the gaseous state
Define ‘first ionisation energy’
The enthalpy change when 1 mole of gaseous atoms forms 1 mole of gaseous ions with a single positive charge
Define ‘second ionisation energy’
The enthalpy change when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a double positive charge
What is the 1st IE equation?
H(g) → H+(g) + e-
What is the general trend of 1st ionisation energy along a period?
1st IE increases along a period
Why does 1st IE increase along a period?
- Nuclear charge increases
- Outer electrons fill same shell so same amount of shielding
- Greater force of attraction between outer electron and nucleus
What are the exceptions for increasing ionisation energy across a period?
In period 3, aluminium and sulfur show a decrease in ionisation energy
What is the general trend of 1st ionisation energy down a group?
1st IE decreases down a group
Why does 1st IE decrease down a group?
- Shielding increases
- Increase in distance of outer electron
- Less attraction between outer electron and nucleus
How does shielding affect ionisation energy?
Shielding is when there are more electron shells between the nucleus and the outer electron
- more shielding: decreases IE as there is less attraction between nucleus and electron
- less shielding: more attraction between nucleus and electron
How does atomic size / radius affect ionisation energy?
The bigger the atom the further away the outer electrons are from the nucleus
- bigger atom: less attraction between nucleus and outer electron
- smaller atom: more attraction between nucleus and outer electron
How does nuclear charge affect ionisation energy?
The more protons in the nucleus the bigger the attraction between the nucleus and outer electrons
- greater nuclear charge: more attraction, larger IE
- smaller nuclear charge: less attraction, smaller IE
