These alkali metals rapidly react with oxygen to produce several different ionic oxides. Oxides: O 2- , peroxides: O 2 2-, super oxide: O 2 - . This topic educates with the classification of oxides based on the nature and property of compounds. These lessons will give your learners further opportunities to make observations and to write balanced chemical equations that represent the chemical changes taking place. These compounds are usually ionic in nature.

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. Oxides of groups 1 and 2 except beryllium react with acids in order to produce salt and water as their products. For example, vanadium oxide (VO 2) is an amphoteric oxide, dissolving in acid to give the blue vanadyl ion, [VO] 2+, and in base to yield the yellow-brown hypovanadate ion, [V 4 O 9] 2−. Start studying Group 2 oxides and hydroxides. CaO (s) + H(NO3)2 (aq) -> CaNO3 (aq) + H2O (l) The Reaction Between Oxides & Sulfuric Acid 2.7:1c recall the reactions of the oxides of group 2 elements with water and dilute acid Learning outcome 10.1(b) This statement wants you to be able to describe the behaviour of the Group 2 oxides, hydroxides and carbonates with water … #1 Report Thread starter 8 years ago #1 My book states that MgO only reacts slightly with water.. What does this mean? All of the oxides react to give the hydroxide; peroxides and superoxides give other products as well. they turn red litmus blue.

MgCO3(s ) MgO(s) + CO2(g ) Thermal decomposition is defined as the use of heat to break down a reactant into more than one product Group 2 carbonates are more thermally stable as you go down the group. Such reaction is: $$MgO_{(s)} + H_{2}O_{(l)} \rightarrow Mg(OH)_{2(aq)}$$ Group 2 hydroxides. The s-metals consist of the Alkali Metals (Group 1) and the Alkaline Earth Metals (Group 2).They generally occur in compounds with oxidation states +1 and +2 respectively, though in the absence of air and water, some compounds with the metals in lower oxidation states may be prepared. Oxides are binary compounds formed by the reaction of oxygen with other elements. Are Group 2 oxides soluble in water? Group 1 hydroxides are water-soluble, group 2 oxides are sparingly soluble apart from barium hydroxide which is fairly soluble. Start studying Reactions of Group 2 Oxides and Hydroxides, and trends in solubility. Group 2 oxides with water Tertiary alcohols Reaction observation in chemistry Why do substances react in certain ways? The elements of Group 2 are beryllium, magnesium, calcium, strontium, barium, and radioactive radium. As one goes down the group, the atoms have more shells of electrons making the atom bigger and there is a decrease in ... Group 2 ionic oxides react with water to form hydroxides MgO (s) + 2 HCl (aq) MgCl2 (aq) + H2O (l) Type your answer here... oxides of group 1react with water to form alkaline hydroxides. A group 2 oxide would form water instead of hydrogen gas, and as for if it dissolves, I think it depends on is the metal hydroxide is a solid or aqeous as it could form a precipitate. The Mg would burn with a bright white flame. Start studying Group 2 oxides and hydroxides. The s-metals consist of the Alkali Metals (Group 1) and the Alkaline Earth Metals (Group 2).They generally occur in compounds with oxidation states +1 and +2 respectively, though in the absence of air and water, some compounds with the metals in lower oxidation states may be prepared.