Ch 2. Periodic Properties

Group 1 elements (excluding hydrogen)

Alkali metals

Group 2 elements

Alkaline earth metals

Groups 3-12 elements

Transition metals

Groups 13-17 elements (B, Si, Ge, As, Sb, Te, Po)

Includes metalloids, which have a combination of both metallis and non-metallic characteristics

Group 17 elements

Halogens

Group 18 elements

Noble gases

Period 6 inner transition metals

Lanthanides

Period 7 inner transition metals

Actinides

metals

Malleable, lustrous

metals

good conductors of electricity/heat

metals

form basic oxides

metals

lose electrons to form cations

metals

usually solid at room temperature, with the exception of Hg, which is liquid

metals

generally, high melting and boiling points

nonmetals

brittle, dull

nonmetals

poor conductors of electricity/heat

nonmetals

form acidic oxides

nonmetals

gain electrons to form anions

nonmetals

gas or solid at room temperature, with the exception of Br, which is liquid

nonmetals

generally, low melting and boiling points

increases right to left and down

atomic radius trend

effective nuclear charge

the amount of positive charge experienced by an electron

Zeff = Z (# protons) - S (# shielding electrons)

effective nuclear charge formula

increases left to right and up

effective nuclear charge trend

ionization energy

the energy needed to remove an electron from an atom

increases left to right and up (exceptions: groups 2 and 15 are more stable)

ionization energy trend

electron affinity

the amount of energy released when an electron is added to an atom

increases left to right and up (exceptions: groups 2 and 15 are lower, noble gases are negligible)

electron affinity trend

increases left to right and up (exception: noble gases)

electronegativity trend

increases right to left and down

metallic character trend