Group Properties of Alkali and Coinage Metals

Alkali Metals

Group I-A metals with one valence electron.

Lithium (Li)

First alkali metal, forms Li2O with oxygen.

Sodium (Na)

Alkali metal, forms Na2O2 with oxygen.

Potassium (K)

Alkali metal, reacts vigorously with water.

Rubidium (Rb)

Alkali metal, larger atomic radius than K.

Cesium (Cs)

Most active alkali metal, reacts explosively.

Francium (Fr)

Unstable radioactive alkali metal, rare.

Valence Electron

Single electron in outer shell of alkali metals.

Ionization

Process of removing a valence electron.

Reducing Agent

Substance that donates electrons in reactions.

Hydroxides

Alkali metals form strong bases, except LiOH.

Hydrides

Compounds formed with hydrogen by alkali metals.

Halides

Compounds formed with halogens by alkali metals.

Superoxides

Formed by potassium, rubidium, cesium with oxygen.

Oxygen Reaction

Alkali metals react with oxygen to form oxides.

Water Reaction

Alkali metals react with water to produce hydrogen.

Coinage Metals

Copper, silver, gold used for coins and ornaments.

Electromotive Series

Ranking of metals based on reactivity.

Complex Cations

Cations formed with ligands like NH3.

Alkaline Earth Metals

Group II-A metals with two valence electrons.

Beryllium (Be)

Least metallic alkaline earth metal, rare.

Magnesium (Mg)

Alkaline earth metal, reacts with steam.

Calcium (Ca)

Alkaline earth metal, reacts with cold water.

Strontium (Sr)

Alkaline earth metal, reacts with cold water.

Barium (Ba)

Alkaline earth metal, reacts with cold water.

Radium (Ra)

Radioactive alkaline earth metal, rare.

Amphoteric Oxide

Beryllium oxide, reacts as acid or base.

Hydration Affinity

Tendency of cations to attract water molecules.

Disproportionation

Reaction where a substance is oxidized and reduced.