Atomic Trends and Justifications

Atomic Trends and Justifications

Atomic Radius down a group: increases because the atom acquires more energy levels, putting valence electrons farther from the nucleus.

Atomic Radius across a period: decreases because effective nuclear charge increases, pulling electrons in closer.

Ionization Energy down a group: decreases because there are more core electrons creating electron shielding, placing valence electrons farther from the nucleus.

Ionization Energy across a period: increases because higher nuclear charge holds electrons tighter.

Large Ionization Energy Jump: indicates transitioning from valence electrons to inner-shell core electrons.

PES Left vs. Right Peaks: peaks farther to the left represent higher ionization energy (electrons closer to nucleus per Coulomb's Law). Peak height represents relative number of electrons.

Lattice Energy: higher ionic charges yield stronger forces of attraction; smaller atomic radius places ions closer together, increasing attraction. Charge takes priority over atomic radius.

Cations vs. Anions: cations lose electrons and become smaller due to increased effective nuclear charge; anions gain electrons and become larger due to electron-electron repulsions.