1.7: Periodic Trends

Cs

Ag

Pb

Br

Se

potassium

rubidium

francium

cesium

Na < Na⁺

Cl > Cl^-

Ti < Zn

N^3- > N

O > S

Br has a lower electronegativity

Br has a lower ionization energy

An added electron would go into a new shell for Br but not I

There is a greater attraction between an added electron and the nucleus in Br than I

The mass of the Cl atom is greater than the mass of F

The Cl nucleus contains more protons than the F nucleus

When Cl and F form bonds with other atoms, the Cl bonding electrons are more shielded from the positive nucleus than the bonding electrons of F

Because Cl is larger than F, the repulsions among electrons in the valence shell of Cl are less than the repulsions among electrons in the valence shell of F