Q: Give an example of an intrusive igneous rock. Q: Give an example of an extrusive igneous rock. Q: How are igneous rocks formed? Q: What determines the size of crystals in igneous rocks? Q: Give two examples of sedimentary rocks. Q: How are sedimentary rocks formed? Q: State two features of sedimentary rocks. Q: Give an example of a metamorphic rock.

A: By the solidification of magma or lava. A: Basalt, rhyolite. A: Granite, gabbro. A: The rate of cooling. Extrusive rocks cool slowly forming large crystals. Intrusive rocks cool quickly forming small crystals. A: By the solidification of magma or lava. A: By the compaction of layers of sediment over a very long time period. A: Limestone and chalk. A: Marble. A: May contain fossils, susceptible to erosion.

Q: How are metamorphic rocks formed? Q: Which sedimentary rocks can marble be formed from? Q: Chalk, limestone and marble are all forms of which chemical? Q: State some advantages of quarrying limestone. Q: State some disadvantages of quarrying limestone. Q: What are the primary uses of limestone? Q: What happens during the thermal decomposition of calcium carbonate? Q: In order from easiest to hardest, which decomposes the most easily: calcium carbonate, copper carbonate, zinc carbonate?

A: By the action of heat and/or pressure. A: Chalk or limestone. A: By the action of heat and/or pressure. A: High demand for limestone to be used in construction; creation of jobs in the quarries, transporting the stone and at building sites; economic benefit to the local and national economies through wages and exports. A: Calcium carbonate. A: As a raw material for building, for the formation of glass, cement and concrete. A: Limestone must be blasted from the ground, creating large amounts of dust; noise pollution caused by blasting; the destruction of habitat; using large lorries to transport the limestone from the quarry damages the roads; large lorries cause congestion on local roads. A: Copper carbonate > zinc carbonate > calcium carbonate. A: When heated, calcium carbonate breaks down into calcium oxide (quicklime) and carbon dioxide.

Q: What is the Law of Conservation of Atoms? Q: What is an atom? Q: What is the Law of Conservation of Atoms? Q: What happens to calcium oxide in the presence of water? Q: What happens when you dissolve calcium hydroxide in water? Q: What happens to the total mass before and after a chemical reaction in a sealed container? Q: How can calcium oxide and calcium hydroxide be used to reduce soil acidity? Q: How can calcium carbonate be used to reduce soil acidity? Q: How can calcium carbonate can be used to remove acidic gases from coal-fired power station chimneys, reducing harmful emissions and helping to reduce acid rain?

A: It dissolves in water to form a solution called limewater. A: During chemical reactions, atoms are neither created nor destroyed; they are rearranged to make new products with different properties from the reactants. A: The smallest particles of an element that can take part in chemical reactions. A: It dissolves in water to form a solution called limewater. A: Calcium oxide reacts with water to produce calcium hydroxide. The reaction gives out heat, so the CaO hisses and expands when water is added to it. A: They neutralise the acid, forming a salt and water (pH increases). A: It remains unchanged. A: It is used in power stations chimneys to neutralise sulfur dioxide, released when coal or oil is burned, which causes acid rain. A: It neutralises the acid, forming a salt, water and carbon dioxide (the pH increases).