Limestone is a type of sedimentary rock that is mainly made up of a substance called calcium carbonate. Calcium carbonate has the chemical formula, CaCO 3 Because it has many uses and can be used to make other products, limestone is a valuable resource.

Basic properties of limestone The appearance of limestone can vary tremendously. Limestone is calcium carbonate and like any carbonate, it reacts with acids producing carbon dioxide gas. bubbles of CO 2 Carbon dioxide turns limewater milky. Because it reacts with acids, it is sometimes added to lakes to remove acidity caused by acid rain.

Limestone is a sedimentary rock and most of it (especially chalk) was formed from the remains of tiny sea creatures. Limestone, chalk and marble are all forms of calcium carbonate CaCO 3. LimestoneChalkMarble This process took millions of years. Limestone and chalk often contain fossils.

Where is limestone found in the British Isles? limestone areas There are also limestone cliffs on the coast in the Vale of Glamorgan

Sedimentary rocks at Llantwit Major in the Vale of Glamorgan Layers of limestone and shale fossils in the fallen limestone blocks fossils from rocks on left prepared specimen – a Jurassic oyster (180 million years old!)

More fossils found in limestone. A Jurassic ammonite from North Yorkshire. 180 million years old. A Silurian gastropod (snail) from Shropshire. 400 million years old.

Important uses of limestone As a building material 1. Limestone has been used for thousands of years for buildings and roads. However, since it is attacked by acids it is easily weathered and eroded.

2. For making glass Glass is made by heating a mixture of limestone, sand and sodium carbonate (soda).

For making cement Cement is made by heating together powdered limestone and clay in a rotary kiln. Limestone and clay Rotating kiln Gas burners Crusher Cement 3.

Cement mortar for joining bricks together concrete for buildings etc. Mix with sand and water Mix with sand and water and chippings

Summary – the uses of limestone Buildings and roads Glass ( heat with sand and sodium carbonate) Neutralise acidic soils and lakes Cement (heat with clay) Mortar (cement + water + sand) Concret e (cement + sand + gravel + water) CaCO3

Limestone Quarrying The quarrying of limestone can have major effects on the environment.

Limestone quarrying provides the raw materials for making many important substances such as glass and cement etc. It also provides employment for people and benefits the local economy. But what exactly are the disadvantages?

Limestone Quarrying – some disadvantages An ‘eyesore’ in areas of the countryside Noise from blasting Dust etc. from lorries Loss of habitat for wildlife

Evaluating the advantages and disadvantages of limestone quarrying Advantages Found naturally so easy to extract Local stone fits in with older houses. Better roads will be built. Jobs. Other related industries attracted in. Disadvantages Possible expense in explosives etc compared with other materials. Quarries destroy the landscape and wildlife habitat. Increased traffic. Noise. Health problems caused by dust. Fewer tourists.

Heating limestone When limestone is strongly heated is begins to glow (limelight!) It decomposes to form calcium oxide (quicklime) and carbon dioxide gas. We can write a word equation: calcium carbonatecalcium oxide + carbon dioxide or a symbol equation: CaCO 3 CaO + CO 2 This type of reaction, where a substance is broken down by heat is called a THERMAL DECOMPOSITION The thermal decomposition of limestone

Calcium oxide (quicklime) is produced industrially using a lime kiln Limestone in Hot air in Kiln rotates to ensure that the limestone is mixed with the hot air Air + carbon dioxide Lime out calcium carbonate heat calcium oxide + carbon dioxide A thermal decomposition reaction a lime kiln

Adding water to quicklime  Calcium hydroxide solution is limewater which turns ‘milky’ with carbon dioxide. We can write a word equation: calcium oxide + watercalcium hydroxide CaO + H 2 O Ca(OH) 2 When water is added to quicklime (calcium oxide), the reaction produces much heat and slaked lime (calcium hydroxide) is formed. A reaction that produces heat is called an exothermic reaction. or in symbols ‘slaking’ lime

Slaked lime (calcium hydroxide) also has uses:  to neutralise acidic soil  to make lime mortar (often used to restore old buildings

Heating other carbonates A number of other carbonates are decomposed in the same way as calcium carbonate when heated e.g. copper carbonate copper oxide + carbon dioxide zinc carbonate zinc oxide + carbon dioxide  Both these reactions are again examples of a thermal decomposition. heat (green)(black) CuCO 3 CuO + CO 2 (Zinc oxide is yellow when hot, white when cool) heat ZnCO 3 ZnO + CO 2