Periodic Trends Flashcards
Define 1st Ionisation Energy
Energy required to remove one electron from each atom in a mole of GASEOUS atoms producing one mile of 1+ gaseous ions
Define 2nd Ionisation energy
Energy required to remove the second electron from each atom of one mole of gaseous atoms
What to include when describing Ionisation (x4)
Distance
Shielding
Charge
Electron affinity
General trend of Ionisation energy across a period
Ionisation energy generally increases but fluctuates at points
Why does Ionisation fluctuate across a period
Protons Subshells FoA Distance / energy level (Therefore more energy required)
General trend in Ionisation energy down a group
Ionisation energy decreases down a group
Reasons why ionisation energy decreases down a group
Electrons further from nucleus FoA is lower Shielding Higher energy level Easier to lose Less energy required
Which group has the lowest Ionisation energy in the period
Group 1
Least protons
Which group has the highest Ionisation energy in the period
Group 0
Most protons
3 types of intermolecular forces
Van Der Waals
Permanent dipole dipole
Hydrogen bonding
What is a coordinate or dative covalent bond
When one atom in the covalent bond donates the pair of electrons to share between the two of them
Occurs in CO where Oxygen donates 2
Why are noble gases the most stable
Have the most proton
Biggest FoA between the e- and nucleus
Why does atomic radius decrease across the period
Higher nuclear charge
Same shielding
Greater FoA between the e- and nucleus
E- closer to normal
Why does Ionisation energy decrease for group 3 and group 6
Group 3 Higher energy level Further from nucleus Less FoA Less energy
Group 6
E- pair repulsion in 3p orbital
Easier to remove
Less energy
Trend in period 3 metal ions
Increasing charge
Increasing ionic density
Decreasing radius
Increasing charge density
