If you calculate the enthalpy change for the possible reactions between beryllium or magnesium and steam, you come up with these answers: Notice that both possible reactions are strongly exothermic, giving out almost identical amounts of heat. It definitely reacts. The explanation for the different reactivities must lie somewhere else. to form strontium hydroxide, Sr(OH) 2 and hydrogen gas (H 2). WebElements: THE periodic table on the WWW [www.webelements.com] The following reaction mechanism is applicable: Sr (s) + 2H 2 O (g) -> Sr (OH) 2 (aq) + H 2 (g) The calcium hydroxide formed shows up mainly as a white precipitate (although some does dissolve). These are necessary to convert the metal atoms into ions with a 2+ charge. Part A Write a balanced equation for the reaction of the nitrite ion with water. Identify all of the phases in your answer. Strontium reacts slowly with water. Strontium reacts with water slowly, generally to strontium hydroxide and hydrogen gas. In each case, you will get a mixture of the metal oxide and the metal nitride. This is mainly due to a decrease in ionisation energy as you go down the Group. Sr (s) + 2 H 2 O (l) Sr(OH) 2 (aq) + H 2 (g) Magnesium burns in steam to produce white magnesium oxide and hydrogen gas. Calcium, for example, reacts fairly vigorously with cold water in an exothermic reaction. Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal is exposed to an atmosphere of chlorine gas. 2Sr(s) + O 2 (g) → 2SrO(s) 3Sr(s) + N 2 (g) → Sr 3 N 2 (s) Reaction of strontium with water. This reaction takes place by heating to the temperature of no more than 500°C. Looking at the enthalpy changes for the reactions. Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal is exposed to an atmosphere of chlorine gas. These stages involve the input of: the atomisation energy of the metal. Similarly, if you calculate the enthalpy changes for the reactions between calcium, strontium or barium and cold water, you again find that the amount of heat evolved in each case is almost exactly the same - in this case, about -430 kJ mol-1. The strontium equation would look just the same. It reacts with water quicker than calcium, which is placed directly above strontium in the periodic chart, and slower than barium, placed directly below strontium. Submit Request Answer When strontium nitrite dissolves in water, the nitrite ion NO2 acts as a base. Bubbles of hydrogen gas are given off, and a white precipitate (of calcium hydroxide) is formed, together with an alkaline solution (also of calcium hydroxide - calcium hydroxide is slightly soluble). That's really all you need to know for this section! The strontium metal sinks in water and after a short while bubbles of hydrogen are evident, stuck to the surface of the metal. The reactions with air. Bubbles of hydrogen gas are given off, and a white precipitate (of calcium hydroxide) is formed, … It reacts with water to form strontium hydroxide and give off gaseous hydrogen. Calcium, for example, reacts fairly vigorously with cold water in an exothermic reaction. I apologise for my part in this. Strontium reacts slowly with water. Strontium and barium have reactivities similar to that of lithium. These all react with cold water with increasing vigour to give the metal hydroxide and hydrogen. Calcium, Strontium, and Barium. Strontium, two places below magnesium in the periodic table is more reactive with air than magnesium. These all react with cold water with increasing vigour to give the metal hydroxide and hydrogen. (b) Strontium oxide is added to water. That means that textbook (or these days, web) statements about it never get checked, and are just passed on regardless of their accuracy. (c) A fresh surface of lithium metal is exposed to oxygen gas. However, the magnesium reaction is much faster. There is an additional reason for the lack of reactivity of beryllium compared with the rest of the Group. (c) A fresh surface of lithium metal is exposed to oxygen gas. The reaction is quicker than that of calcium (immediately above strontium in the periodic table) but slower than that of barium (immediately below strontium in the periodic table). Because strontium sulfate is much less soluble in water than strontium chloride, sodium chloride, or sodium sulfate, this reaction is: Na2SO4 (aq) + SrCl2 (aq) => 2 NaCl (aq) + SrSO4 (s). This leads to lower activation energies, and therefore faster reactions. This is the energy needed to break the bonds holding the atoms together in the metallic lattice. Strontium oxide is more normally made by heating strontium carbonate. The formation of the ions from the original metal involves various stages all of which require the input of energy - contributing to the activation energy of the reaction. Sr + 2H2O --> Sr(OH)2 + H2 Strontium chloride react with water to produce strontium hydroxide and hydrogen chloride. (Equation just like the magnesium one below.). Strontium reacts slowly with water, forming strontium hydroxide, Sr(OH) 2 and hydrogen gas, H 2. The enthalpy change of a reaction is a measure of the amount of heat absorbed or evolved when the reaction takes place. The general equation … The equation is: Sr + 2H2O → Sr(OH)2 + H2(g) The resulting solution of strontium hydroxide is basic, meaning it has a pH Sr(s) + 2HCl(aq) → Sr2+(aq) + 2Cl-(aq) + H2(g). All rights reserved. You can reference the WebElements periodic table as follows:"WebElements, https://www.webelements.com, accessed November 2020. Some water-reactive substances are also pyrophoric, like organometallics and sulfuric acid, and should be kept away from moisture. 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