Alkali Metals Overview

This collection of flashcards covers key concepts related to alkali metals, including their properties, reactivity, and reactions with water, chlorine, and oxygen.

Alkali metals

Group one elements including lithium, sodium, potassium, rubidium, cesium, and francium, characterized by being soft, low density, and low melting points.

Reactivity

How easily atoms can lose or gain electrons and react with other atoms; alkali metals are very reactive.

Electron configuration

All alkali metals have one electron in their outermost shell, which they lose to become stable.

Ionic compound

A compound formed when a metal atom donates an electron to a nonmetal, resulting in oppositely charged ions.

Sodium chloride (NaCl)

Common table salt, an example of an ionic compound formed by sodium and chlorine.

Hydrogen gas (H2)

A gas produced when alkali metals react vigorously with water.

Metal hydroxide

The product formed when an alkali metal reacts with water, along with hydrogen gas.

Metal oxides

Compounds formed when alkali metals react with oxygen.

Potassium superoxide (KO2)

A specific type of metal oxide formed by potassium reacting with oxygen.

Boiling point trend of alkali metals

Decreases as you move down the group from lithium to francium.

Melting point trend of alkali metals

Decreases as you move down the group from lithium to francium.

Electrostatic forces

The attractive forces between oppositely charged ions that hold ionic compounds together.