Q. If heated Mg(s) is allowed to react with H₂O(l), the product formed other than H₂(g) will be

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Q. The pH of NaOH produced after Na(s) and H₂O(l) reaction is

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Q. Consider the reaction: Na(s) + H₂O → NaOH(aq) + H₂(g). Moles of H₂O required to balance the equation will be

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Q. If Mg(s) is allowed to react with H₂O(l), the product other than H₂(g) will be

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Q. Consider the reaction: Na(s) + H₂O(l) → NaOH(aq) + H₂(g). Moles of Na required to balance the equation are

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Q. The formula MgO shows Mg oxidation number to be

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Q. Consider the equation: Mg(s) + H₂O(l) → Mg(OH)₂(aq) + H₂(g). Moles of Mg(s) required to balance the equation will be

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Q. When allowed to react with cold water, the element that reacts vigorously to produce H₂(g) is

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Q. The element that reacts vigorously with cold water among the following is

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Q. The pH of Mg(OH)₂ produced after Mg(s) and H₂O(l) reaction is

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Q. Metal that reacts vigorously with cold water to produce a strongly alkaline solution is

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Q. Which is incorrect about the characteristics of Group II elements?

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Q. In excess water, Ca(OH)₂ produces

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Q. Consider the reaction: CaO(s) + H₂O(l) → Ca(OH)₂. The state of the product in this reaction should be

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Q. Upon reaction of metals of Group II with oxygen, electrons are lost more easily by

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Q. The alkaline solution of Ca(OH)₂ has a pH of

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Q. An increase in the nuclear charge down the Group II

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Q. Upon dissolving Ca(OH)₂ in water, the solution becomes

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Q. As we go down the Group-II, metals become

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Q. In nature, Magnesium Oxide (MgO) is

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