Trends in atomic radius and ionic energy

Atomic Radius

Distance from nucleus to outermost electron.

Across a Period

Atomic radius decreases due to increased nuclear charge.

Down a Group

Atomic radius increases due to additional electron shells.

Shielding Effect

Inner electrons reduce nuclear attraction on outer electrons.

Nuclear Charge

Total positive charge from protons in nucleus.

Nuclear Attraction

Force pulling outer electrons towards the nucleus.

First Ionization Energy

Energy required to remove outermost electron.

Ionization Energy Across a Period

Generally increases due to decreasing atomic radius.

Ionization Energy Down a Group

Decreases due to increased atomic radius and shielding.

Group 3 Ionization Deviation

Higher energy p orbital requires less energy to ionize.

Group 6 Ionization Deviation

Spin pair repulsion in p orbital lowers ionization energy.

Electron Shielding

Reduction of effective nuclear charge on outer electrons.

Outermost Electrons

Electrons in the highest energy level of an atom.

Increased Distance

Greater distance reduces nuclear attraction on electrons.

Spin Pair Repulsion

Repulsion between paired electrons in the same orbital.

Effective Nuclear Charge

Net positive charge experienced by outer electrons.

Electron Configuration

Arrangement of electrons in an atom's orbitals.

Periodic Trends

Patterns in properties across periods and groups.

Energy Levels

Regions around nucleus where electrons are likely found.

Nuclear Stability

Balance between nuclear forces and repulsive forces.