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Water is essentially two hydrogen atoms and one oxygen atom linked together in a liquid state. Water, despite its seeming simplicity, possesses surprising qualities. The properties of water include expanding when frozen, having high surface tension (because of the polar nature of the molecules, they tend to cling together), and many more characteristics. Without water, life on Earth may not have been able to exist, and it would almost certainly not have had the incredible complexity and diversity that we witness today.
Group 1 Consists Of Alkali Metals
An important property shared by the majority of alkali metals is their capacity to displace H2(g) from water. This is reflected in the enormous, negative electrode potentials that they have. It occurs in this situation that the Group 1 metal is oxidized to generate its metal ion, and that water is reduced to form hydrogen gas and hydroxide ions. The general reaction of an alkali metal (M) with H2O (l) is represented by the equation below:
2M(s)+2H2O(l)⟶2M+(aq)+2OH−(aq)+H2(g)
It is clear from this reaction that OH- is created, resulting in the formation of a basic or alkaline environment. Group 1 elements are referred to as alkali metals because of their propensity to displace hydrogen ions (H2(g)) from water and produce an alkaline solution.
Aside from this, alkali metals are also known to react aggressively and explosively when in contact with water. This is due to the fact that enough heat is generated during the exothermic process to induce the H2 to ignite (g).
Alkaline Earth Metals
They are classified into two groups.When treated with water, the bulk of Alkaline Earth Metals also form hydroxides as a byproduct. In spite of the fact that the hydroxides of the elements calcium, strontium, and barium are only marginally soluble in water, enough hydroxide ions are created to create a basic environment. Following is a representation of the general reaction of calcium, strontium, and barium with water; the letter M denotes the element represented by calcium, strontium, or barium:
M(s)+2H2O(l)⟶M(OH)2(aq)+H2(g)
In the presence of water vapor, magnesium (Mg) interacts with it to generate magnesium hydroxide and hydrogen gas. Beryllium (Be) is the only alkaline earth metal that does not react with water, unlike the other alkaline earth elements. In comparison to the other elements in the group, it has a small size and high ionization energy, which accounts for this.
Alkaline Earth Metal Oxides in the Presence of Water
Alkaline earth metal monoxides interact with water in a similar way to alkali metal oxides to generate metal hydroxide salts, which are toxic to humans (as illustrated in the equation below). The exception to this generalization is beryllium, whose oxide (BeO) does not react with water, contrary to the generalization.
MO(s)+H2O(l)⟶M(OH)2(s)
CaO, sometimes known as quicklime, is one of the most well-known alkaline earth metal oxides. This material is frequently employed in the treatment of water as well as the removal of hazardous SO2(g) from industrial smokestacks.
Alkali Metals Oxides and Water
Aalkali metal oxides and water oxides of Group 1 elements react with water to form basic solutions, as do other Group 1 elements. Alkali metals react with oxygen to generate monoxides, peroxides, and superoxides, depending on their composition. These organisms react in different ways to water depending on their species:
Using monoxides (M2O), alkali metal hydroxides are formed as follows: M2O(s)+2H2O(l)→2M+(aq)+2OH (aq)
Peroxides (M2O2) are responsible for the formation of metal hydroxides and hydrogen peroxide:
M2O2(s)+2H2O(l)⟶2M+(aq)+2OH−(aq)+H2O2(aq)
Superoxides (MO2) are responsible for the formation of metal hydroxides, hydrogen peroxide, and oxygen gas:
2MO2(s)+2H2O(l)⟶2M+(aq)+2OH−(aq)+H2O2(aq)+O2(g)
Earth Metal Hydrides and Water in Alkaline Earth Environments
All of the alkaline metal hydrides, with the exception of beryllium (Be), react with water to form metal hydroxide and hydrogen gas, respectively. The following is a description of the reactivity of these metal hydrides.
MH2(s)+2H2O(l)⟶M(OH)2(aq)+2H2(g)
With Boron Family
The Boron Family is the thirteenth group.
There is little reaction between Group 13 elements and water. In actuality, boron (B) does not react with water in any significant way. In this category, the reaction of aluminum (Al) with water is particularly significant. Aluminum does not appear to react with water because an exterior layer of aluminum oxide (Al2O3) solid forms and shields the rest of the metal, preventing the metal from reacting with the water.
Carbon Species (Group 14)
Group 14 elements, for the most part, do not react with water when exposed to high temperatures. Because of this, tin (Sn) is frequently sprayed on iron cans as a protective layer to prevent the can from corroding, which is an interesting side effect.
Family of Nitrogen (Group 15)
The pure elements in this family are less likely to react with water than the other elements in this family are. N2 is dissolved in water, but it does not react with the nitrogen compounds (nitrates and nitrites) or the nitrogen gas (nitrogen dioxide).
The Oxygen Family
it is the sixteenth group to be considered.For example, as previously stated, many oxides of Groups 1 and 2 combine with water to produce metallic hydroxide compounds. Oxoacids are formed when the nonmetal oxides react with water. Phosphoric acid and sulfuric acid, for example, are both acidic substances.
Halogens Family
They are classified under Group 17.In most cases, halogens react with water to form their halides and polyhalides, which are toxic. Because of their differing electronegativities, the reactions of the halogen gasses with water are diverse. It is possible for fluorine (F2) to displace oxygen gas from water because of its strong electronegative property. The oxygen gas and hydrogen fluoride that are produced as a result of this reaction Hydrohalic acids are formed when hydrogen halides react with water ( HX ). Hydrohalic acids are powerful acids in water, with the exception of HF (hydrogen peroxide). Examples of strong acids include hydrochloric acid (HCl), which is a strong base.
Cl2(g)+2H2O(l)→HCl(aq)+HOCl(aq)
Noble Gasses (Group 18)
With regard to water, no reaction occurs between noble gases and water.
Conclusion
The amount of water available has an impact on the degree of climate variability and change. It is an essential component during extreme weather events such as drought and flooding. Its availability and timely delivery are critical when it comes to meeting the needs of humans and ecosystems.
Humans use water for many things, including drinking, industrial applications, irrigating farms, hydroelectric power, waste disposal, and recreation. It is vital to conserve water supplies, both for human use and for the ecosystem’s health. Many places are running out of water as a result of population growth, pollution, and urbanization, among other factors. Climate variability and change, which affect the hydrologic cycle, have intensified these pressures even further.
