Water

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Water ( Molecular formula:H<sub>2</sub>O) constitutes of two [[Hydrogen|hydrogen]] atoms and a single [[Oxygen|oxygen]] [[Atom|atom]]. The [[Hydrogen|hydrogen]] atoms are linked to the oxygen atoms by [[Covalent bond|covalent bonds]]&nbsp;Since Oxygen has a much higher&nbsp;[[Electronegativity]]&nbsp;than Hydrogen, the distrubution of electrons is more dense towards the Oxygen molecule thus creating a slightly negative reigion.. When water [[Molecule|molecules]] interact with each other, the positively charged region ([[Hydrogen|hydrogen]] atom) of one water [[Molecule|molecule]] forms a weak [[Hydrogen bonds|hydrogen bond]] with the negatively charged region ([[Oxygen|oxygen]] atom) of a second water [[Molecule|molecule]]&nbsp;<ref>Alberts et al., Molecular Biology Of the cell, 5th edition, 2008, Garland Science, New York, pg 51</ref>. &nbsp;This is a hydrogen bond and although it isn't as strong as a covalent bond, it is highly stable and is responsible for the properties and thus abundance of water on Earth.<br>
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[[Water|Water]] (Molecular formula: H<sub>2</sub>O) consists of two [[Hydrogen|hydrogen]] atoms and a single [[Oxygen|oxygen]] [[Atom|atom]].  
  
Water is a bent molecule there the distribution of charge is assymetric. As a result of the charged regions in water, water is a [[Polarity|polar]] molecule and can conduct electricity. Water molecules react with molecules in aqueous solution through the formation of [[Hydrogen bonds|hydrogen bonds and]] via ionic interactions. These interactions mean that water is a good &nbsp;and can dissolve polar molecules and ions. Water has small molecules and maintains its physical state of bein a liquid over a large range of temperatures.It is also highly [[Cohesive|cohesive]]. Networks of [[Hydrogen bonds|hydrogen bonds hold]] the structure of ice and liquid water together. These interactions are responsible for the cohesion of water. Water is involved in many different reactions and can affect several [[Noncovalent bonds|noncovalent bonds with]] its presence. Examples of noncovalent bonds that the presence of water can affect are [[Electrostatic interactions|electrostatic interactions]], [[Hydrogen bonds|hydrogen bonds and]] [[Van der waals forces|van der Waals interactions]]. Furthermore when water cannot react with nonpolar molecules through hydrogen bonding or ionic interactions, the result is the [[Hydrophobic|hydrophobic effect that]] is accompanied by [[Hydrophobic|hydrophobic interactions]].<ref>Berg Jeremy M., Tymoczko John L., Stryer Lubert., (2007) Biochemistry, Sixth Edition, New York, W.H. Freeman and Company. P8-9</ref><br>
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[[Image:WATER MOLECULE.png|right|583x220px|WATER MOLECULE.png]]  
  
Humans contain around 40 [[Litre|litres]] of water and&nbsp;both unicellular organisms and multicellular cells live in water.<br>  
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Each [[Hydrogen|hydrogen]] atom forms a [[Covalent bond|covalent bond]] with the oxygen. [[Oxygen|Oxygen]] has a higher [[Electronegativity|electronegativity than]] hydrogen due to its two lone pairs of electrons. This causes a region of slight negativity (although not enough to create an ion) on the oxygen compared to the hydrogens. This spatial imbalance of [[Electron|electrons is]] represented by delta negative (δ-) on the oxygen and delta positive signs (δ+) on the hydrogen atoms<ref>Jim Clark (2000-Last modified February 2015) Chemguide available at http://www.chemguide.co.uk/atoms/bonding/hbond.html 19/10/15</ref>. When water [[Molecule|molecules]] interact with each other, the positively charged region ([[Hydrogen|hydrogen]] atom) of one water [[Molecule|molecule]] forms a weak [[Hydrogen bonds|hydrogen bond]] with the negatively charged region ([[Oxygen|oxygen]] atom) of a second water [[Molecule|molecule]]<ref>Alberts et al., Molecular Biology Of the cell, 5th edition, 2008, Garland Science, New York, pg 51</ref>. This is a hydrogen bond and although it isn't as strong as a covalent bond, it is highly stable and is responsible for the properties and thus abundance of water on Earth.
  
Many diseases are associated with water, for example excess water ([http://en.wikipedia.org/wiki/Hyperhydration hyperhydration]), not enough water ([[Dehydration|dehydration]]) and many&nbsp;[[Microorganisms|microorganisms]] use water as a form of transport and spread through water, e.g. [[Cholera|Cholera]].<br>  
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Water is a bent molecule there is a distribution of charge which is asymmetric. As a result of the charged regions in water, water is a [[Polarity|polar]] molecule and can conduct electricity. Water molecules react with molecules in aqueous solution through the formation of [[Hydrogen bonds|hydrogen bonds and]] via ionic interactions. These interactions mean that water is a good solvent and can dissolve polar molecules and ions. Water has small molecules and maintains its physical state of being a liquid over a large range of temperatures.It is also highly [[Cohesive|cohesive]]. Networks of [[Hydrogen bonds|hydrogen bonds hold]] the structure of ice and liquid water together. These interactions are responsible for the cohesion of water. Water is involved in many different reactions and can affect several [[Noncovalent bonds|noncovalent bonds with]] its presence. Examples of noncovalent bonds that the presence of water can affect are [[Electrostatic interactions|electrostatic interactions]], [[Hydrogen bonds|hydrogen bonds and]] [[Van der Waals forces|van der Waals interactions]] (instantaneous dipole and induced dipole effects). Furthermore when water cannot react with nonpolar molecules through hydrogen bonding or ionic interactions, the result is the [[Hydrophobic|hydrophobic effect that]] is accompanied by [[Hydrophobic|hydrophobic interactions]]<ref>Berg Jeremy M., Tymoczko John L., Stryer Lubert., (2007) Biochemistry, Sixth Edition, New York, W.H. Freeman and Company. P8-9</ref>.
  
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Humans contain around 40 [[Litre|litres]] of water and both unicellular organisms and multicellular cells live in water.
  
=== References:  ===
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Many diseases are associated with water, for example excess water ([[Hyperhydration|hyperhydration]]), not enough water ([[Dehydration|dehydration]]) and many [[Microorganisms|microorganisms]] use water as a form of transport and spread through water, e.g. [[Cholera|Cholera]].
  
<references /><br>
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Thus, water is very essential for life and is considered as the universal solvent. It helps to dissolve substances like ions in our body and partakes in many chemical reactions within the body, even to its cellular level<ref>Pohorille, Andrew &amp;amp;amp; Pratt, Lawrence. (2012). Is Water the Universal Solvent for Life?. Origins of life and evolution of the biosphere: the journal of the International Society for the Study of the Origin of Life. 42. 10.1007/s11084-012-9301-6.</ref>.
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=== References  ===
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<references />

Latest revision as of 18:07, 22 November 2018

Water (Molecular formula: H2O) consists of two hydrogen atoms and a single oxygen atom.

WATER MOLECULE.png

Each hydrogen atom forms a covalent bond with the oxygen. Oxygen has a higher electronegativity than hydrogen due to its two lone pairs of electrons. This causes a region of slight negativity (although not enough to create an ion) on the oxygen compared to the hydrogens. This spatial imbalance of electrons is represented by delta negative (δ-) on the oxygen and delta positive signs (δ+) on the hydrogen atoms[1]. When water molecules interact with each other, the positively charged region (hydrogen atom) of one water molecule forms a weak hydrogen bond with the negatively charged region (oxygen atom) of a second water molecule[2]. This is a hydrogen bond and although it isn't as strong as a covalent bond, it is highly stable and is responsible for the properties and thus abundance of water on Earth.

Water is a bent molecule there is a distribution of charge which is asymmetric. As a result of the charged regions in water, water is a polar molecule and can conduct electricity. Water molecules react with molecules in aqueous solution through the formation of hydrogen bonds and via ionic interactions. These interactions mean that water is a good solvent and can dissolve polar molecules and ions. Water has small molecules and maintains its physical state of being a liquid over a large range of temperatures.It is also highly cohesive. Networks of hydrogen bonds hold the structure of ice and liquid water together. These interactions are responsible for the cohesion of water. Water is involved in many different reactions and can affect several noncovalent bonds with its presence. Examples of noncovalent bonds that the presence of water can affect are electrostatic interactions, hydrogen bonds and van der Waals interactions (instantaneous dipole and induced dipole effects). Furthermore when water cannot react with nonpolar molecules through hydrogen bonding or ionic interactions, the result is the hydrophobic effect that is accompanied by hydrophobic interactions[3].

Humans contain around 40 litres of water and both unicellular organisms and multicellular cells live in water.

Many diseases are associated with water, for example excess water (hyperhydration), not enough water (dehydration) and many microorganisms use water as a form of transport and spread through water, e.g. Cholera.

Thus, water is very essential for life and is considered as the universal solvent. It helps to dissolve substances like ions in our body and partakes in many chemical reactions within the body, even to its cellular level[4].

References

  1. Jim Clark (2000-Last modified February 2015) Chemguide available at http://www.chemguide.co.uk/atoms/bonding/hbond.html 19/10/15
  2. Alberts et al., Molecular Biology Of the cell, 5th edition, 2008, Garland Science, New York, pg 51
  3. Berg Jeremy M., Tymoczko John L., Stryer Lubert., (2007) Biochemistry, Sixth Edition, New York, W.H. Freeman and Company. P8-9
  4. Pohorille, Andrew &amp;amp; Pratt, Lawrence. (2012). Is Water the Universal Solvent for Life?. Origins of life and evolution of the biosphere: the journal of the International Society for the Study of the Origin of Life. 42. 10.1007/s11084-012-9301-6.
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