Groups 1 & 2 Edexcel International AS Chemistry

A comprehensive set of flashcards covering key concepts, terms, and definitions related to Groups 1 & 2 in Chemistry, specifically designed for review and study for exams.

Ionisation Energy

The energy required to remove an electron from an atom.

Alkali Metals

Elements in Group 1 of the periodic table, characterized by having one electron in their outermost shell.

Alkaline Earth Metals

Elements in Group 2 of the periodic table, characterized by having two electrons in their outermost shell.

Ionic Compounds

Compounds formed by the transfer of electrons from metals to nonmetals, resulting in the formation of ions.

Reducing Agents

Substances that donate electrons to others, causing the reduction of other substances and themselves being oxidized.

Reactivity Trend in Group 1

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

Shielding Effect

The phenomenon where inner shell electrons block outer shell electrons from the pull of the nucleus.

First Ionization Energy

The energy required to remove the first electron from an atom.

Second Ionization Energy

The energy required to remove the second electron from an atom.

Noble Gas Configuration

The electron configuration of noble gases, typically reached by losing or gaining electrons.

Metal Oxides

Compounds formed when metals react with oxygen.

Tarnishing

The process where metals corrode or oxidize, forming a coating that alters their appearance.

Exothermic Reaction

A chemical reaction that releases energy in the form of heat.

Hydroxides

Compounds containing the hydroxide ion (OH-), typically formed when metal oxides react with water.

Thermal Decomposition

The breakdown of a compound into smaller compounds or elements when heat is applied.

Flame Test

A qualitative analysis technique to identify metal ions based on the color of flame produced.

Qualitative Tests

Tests used to determine the presence of specific ions or compounds.

Ammonium Ions

Cations with the formula NH4+, characteristic of certain fertilizers.

Carbonate Ions

Anions with the formula CO3^2-, found in many minerals and compounds.

Sulfate Ions

Anions with the formula SO4^2-, which are common in salts.

Hydrogen Gas

A colorless, odorless gas (H2) that is produced in certain chemical reactions.

Solubility

The ability of a substance to dissolve in a solvent.

Alkaline Solutions

Solutions that have a pH greater than 7, typically containing hydroxide ions.

Oxidation

The process of losing electrons during a chemical reaction.

Reduction

The process of gaining electrons during a chemical reaction.

Neutralization Reaction

The reaction between an acid and a base to produce salt and water.

Balancing Chemical Equations

Ensuring that the number of atoms for each element is equal on both sides of the reaction.

Hydroxide Ion

The ion OH-, which contributes to the basicity of a solution.

Calcium Hydroxide

A strong base with the formula Ca(OH)2, commonly known as limewater.

Limewater

A solution of calcium hydroxide in water, used to test for carbon dioxide.

Peroxide

A compound containing an oxygen-oxygen single bond or the -O-O- group.

Alkalinity

The capacity of water to resist changes in pH that would make it more acidic.

Decomposition of Nitrates

The breakdown of nitrates (NO3-) into other products upon heating.

Test Tube Reactions

Reactions carried out in test tubes to analyze the presence of specific ions.

Barium Hydroxide

A strong base with the formula Ba(OH)2, which is highly soluble in water.

Ammonium Hydroxide

A solution of ammonia in water, often used in various chemical tests.

Chemistry of Water

The study of chemical reactions involving water and its role as a solvent.

HCl

Hydrochloric acid, a strong acid commonly used in various reactions.

Precipitate

A solid that forms from a solution during a chemical reaction.

Dilute Acid

An acid that has been mixed with water to decrease its concentration.

Chemical Reaction

A process that leads to the transformation of one set of chemical substances to another.

Metal Carbonates

Salts of carbonic acid containing metal cations and carbonate anions.

Basic Oxides

Metal oxides that can react with acids to form salts and water.

Ionic Equations

Equations that show only the reactants and products that involve ions.

pH Scale

A scale used to specify the acidity or basicity of an aqueous solution.

Chemical Identifications

Processes used to determine the chemical nature of substances.

Thermal Stability

The resistance of a chemical compound to decomposition when heated.

Testing for Gases

Analytical methods to identify gaseous products formed during reactions.

Test for Carbon Dioxide

Bubbling gas through limewater to observe a milky precipitate of calcium carbonate.

Flame Color Representation

The characteristic color emitted by a metal ion when exposed to flame.

Sodium Chloride

Common table salt, formed from the reaction of sodium ions and chloride ions.

Toxic Gases

Gases that can cause harm or death upon exposure.

Chemical Formulas

Symbolic representations of the chemical composition of a substance.

Ammonia Gas

A colorless gas with a distinctive odor, composed of nitrogen and hydrogen.