Ionisation Energy and Reactivity of Groups 1 & 2 Metals

These flashcards cover key vocabulary and concepts related to ionisation energy, reactivity, and chemical reactions of groups 1 and 2 metals.

Ionisation Energy

The energy required to remove an electron from an atom in its gaseous state.

Group 1 Elements

Also known as alkali metals, these elements have one electron in their outermost shell.

Group 2 Elements

Also known as alkaline earth metals, these elements have two electrons in their outermost shell.

Ionic Compounds

Compounds formed when metals donate electrons to become ions.

Reducing Agents

Substances that donate electrons in a chemical reaction, thus reducing another substance.

Reactivity Trend - Group 1

Reactivity increases down the group as outermost electron is lost more easily.

Reactivity Trend - Group 2

Reactivity also increases down the group for similar reasons as Group 1.

First Ionisation Energy

The energy needed to remove the first outer electron from an atom.

Second Ionisation Energy

The energy needed to remove the second outer electron from an atom.

Shielding Effect

The reduction of the effective nuclear charge experienced by outer electrons due to inner electron shells.

Noble Gas Configuration

The electron configuration of an atom that matches that of the nearest noble gas, resulting in stability.

Metal Oxides and Water Reaction

When alkali metals react with water, hydroxides are formed along with hydrogen gas.

Flame Test

A qualitative analysis technique used to identify the presence of certain metal ions based on flame color.

MgO Reaction with Water

Produces magnesium hydroxide, which is slightly soluble and forms an alkaline solution.

CaO Reaction with Water

Produces calcium hydroxide in a vigorous reaction which releases heat.

Sulfuric Acid Reaction

Metal oxides react with dilute sulfuric acid to form metal sulfates and water.

Hydroxides and Acids Reaction

The reaction of metal hydroxides with acids results in the formation of salts and water.

Thermal Decomposition

The breakdown of a compound into two or more different substances using heat.

Decomposition of Carbonates

Group 1 carbonates decompose when heated to yield metal oxides and carbon dioxide.

Decomposition of Nitrates

Group 1 nitrates decompose to produce nitrogen dioxide and oxygen upon heating.

Observations in Flame Tests

Different metal ions produce different flame colors when heated, which helps to identify them.

Ammonium Ions Test

Producing ammonia gas when ammonium salts react with sodium hydroxide.

Carbonate Ions Test

Producing carbon dioxide gas when carbonates react with acids, causing limewater to turn milky.

Sulfate Ions Test

Formation of white precipitate of barium sulfate when barium chloride is added to sulfate solution.

Group 2 Hydroxides

Metal hydroxides that increase in solubility down the group.

Alkaline Solutions

Solutions formed by hydroxides that have a pH greater than 7.

Hydrogen Gas Production

A byproduct of the reaction between metals and water or acids.

Oxidation of Metals

The loss of electrons from a metal during reactions with oxygen, water, or acids.

Sulfates Solubility Trend

The solubility of Group 2 sulfates decreases as you move down the group.

General Reaction of Metals with Water

M + 2H2O → 2MOH + H2, where M represents Group 1 or 2 metals.

Metal Hydroxides Reaction with Acid

Neutralization occurs when metal hydroxides react with acids to form salts.

Observations in Group 2 Reactions

Vigorous reactions observed, particularly with water, as you descend the group.