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Strontium and barium have reactivities similar to lithium in Group 1 of the Periodic Table. Sodium is the alkali element that reacts most violently with water. The metals at the bottom of the reactivity series will react slowly or will not react with water and dilute acids as they are less reactive Reaction with Water The table below shows how the metals from the reactivity series react with Water: $$Cl_{2\;(g)}+2H_{2}O_{(l)} \longrightarrow HOCl_{(aq)} + H^+_{(aq)} + Cl^-_{(aq)}$$, $$Li_2O_{(s)}+2H_{2}O_{(l)} \longrightarrow 2LiOH_{(aq)}$$, Trevor Landas (University of California, Davis). Reaction of Iron with water: Reaction of iron with cold water is very slow and come into notice after a long time. Calcium, for example, reacts fairly vigorously with cold water in an exothermic reaction. Phosphorus is a very reactive non-metal element.If phosphorus is kept open in air,it react with the oxygen of air and catches fire.So,in order to protect phosphorus from atmospheric air,it is stored in a bottle containing water. The hydroxide ions combine with the bicarbonate ions in the water to produce water and a carbonate ion. Oxides of Group 1 elements also react with water to create basic solutions. This solid dissolves in the water producing a metal ion (M+2) and hydroxide ions (OH-). Iron forms rust (iron oxide) when reacts with moisture present in atmosphere. Many of these chemical reactions behave in trends that can be categorized using the periodic table. In this event, the Group 1 metal is oxidized to its metal ion and water is reduced to form hydrogen gas and hydroxide ions. * But all metals do not react with water. To protect metals submerged in saltwater from corroding, remove the metal from the saltwater, thoroughly clean and rinse with fresh water. Read about our approach to external linking. Sodium carbonate precipitates out the Mg+2 and Ca+2 ions out as the respective metal carbonates and introduces Na+ ions into the solutions. The elements toward the bottom left corner of the periodic table are the metals that are the most active in the sense of being the most reactive.Lithium, sodium, and potassium all react with water, for example. The hardening species often cannot be boiled off. To protect metals submerged in saltwater from corroding, remove the metal from the saltwater, thoroughly clean and rinse with fresh water. $\ce{Br2(g) + 2H2O(l) → HBr(aq) + HOBr(aq)}$. When potassium comes in contact with water, it experiences a more severe reaction. With the exception of beryllium (Be), the alkaline metal hydrides react with water to produce the metal hydroxide and hydrogen gas. * Metals react with water and produce a metal oxide and hydrogen gas. Reaction of non-metals with water. $\ce{I2(g) + 2H2O(l) → HI(aq) + HOI(aq)}$. Once the metal is dry, use a marine paint or oil sealant to cover the metal completely. When a metal reacts with water, a metal hydroxide and hydrogen are formed. $MO_{(s)}+H_2O_{(l)} \longrightarrow M(OH)_{2(s)} \label{6}$. Examples include phosphoric acid and sulfuric acid. Magnesium (Mg) reacts with water vapor to form magnesium hydroxide and hydrogen gas. This is represented by their large, negative electrode potentials. Reaction of Metals with Water. Calcium hydroxide is slightly soluble in water so once the solution is saturated, it starts to become milky as solid calcium hydroxide appear. Group 13 elements are not very reactive with water. One of the most familiar alkaline earth metal oxides is CaO or quicklime. Alkali Metals A common characteristic of most Alkali metals is their ability to displace H2(g) from water. 2 N a (s o d i u m) + 2 H 2 O 2 N a O H + H 2 (h y d r o g e n g a s l i b e r a t e d) ↑ Less active metals react with boiling water. $\ce{Cl2(g) + 2H2O(l) → HCl(aq) + HOCl(aq)}$. For more information contact us at info@libretexts.org or check out our status page at https://status.libretexts.org. Only a little iodine dissolves in water to form a yellowish solution and hypoiodous ($$\ce{HOI}$$) acid has very weak bleaching characteristic. Group 1 elements are called alkali metals because of their ability to displace H2(g) from water and create a basic solution. These all react with cold water with increasing vigour to give the metal hydroxide and hydrogen. One notable reaction within this group is aluminum's (Al) reaction with water. 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