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We can examine the reactivity of metals by observing their reactions with oxygen, water, steam and whether it displaces other metals in. displacement reactions. This table summarises the...
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Recap the reactivity series of metals and how it's used to...
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28 lut 2020 · The first five elements are highly reactive metals that will react with cold water, hot water, and steam to form hydrogen gas and hydroxides. The next four metals (magnesium through chromium) are active metals that will react with hot water or steam to form their oxides and hydrogen gas.
displace magnesium from magnesium sulfate. (c) A reaction will happen. Copper(II) nitrate solution will form and silver will coat the copper. This is because copper is more reactive than silver, so it can displace silver from silver nitrate. copper + silver nitrate → copper(II) nitrate + copper Cu(s) + 2AgNO 3(aq) → Cu(NO 3)
Copper (II) sulfate hydrolyzes in water and makes the solution slightly acidic. Then the magnesium is reacting with the weak acid, displacing hydrogen, as well as displacing the copper. Magnesium displaces hydrogen only slowly with pure water, partly because the magnesium hydroxide product is only sparingly soluble.
Metals from magnesium to iron. These react with steam to give a metal oxide and hydrogen. Remember that the aluminium reaction is much slower than you would expect because of its stable oxide coating. Metals below hydrogen. These don't react with water under any conditions.
This page looks at the reactions of the Group 2 elements - beryllium, magnesium, calcium, strontium and barium - with water (or steam). It uses these reactions to explore the trend in reactivity in Group 2.
For example, magnesium is a reactive metal and can displace copper from copper(II)sulfate solution: Mg + CuSO 4 → MgSO 4 + Cu. The blue colour of the CuSO 4 solution fades as colourless magnesium sulfate solution is formed; Copper coats the surface of the magnesium and also forms solid metal which falls to the bottom of the beaker
