Chemistry:Water-reactive substances
Water-reactive substances[1] are those that spontaneously undergo a chemical reaction with water, as they are highly reducing in nature.[2] Notable examples include alkali metals, lithium through caesium, and alkaline earth metals, magnesium through barium.
Some water-reactive substances are also pyrophoric, like organometallics and sulphuric acid, and should be kept away from moisture. The use of acid-resistant gloves and face shield are required and should be handled in fume hoods.[3]
Such substances are classified as R2 under the UN classification system and as Hazard 4.3 by the United States Department of Transportation. In an NFPA 704 fire diamond's white square, they are denoted as "W̶".
All chemicals that react vigorously with water or liberate toxic gas when in contact with water are recognized for their hazardous nature in the 'Approved Supply List,'[4] or the list of substances covered by the international legislation on major hazards[5] many of which are commonly used in manufacturing processes.
Alkali metals
File:Reaction of Sodium and Water.webm File:Potassium metal in water.webm The alkali metals (Li, Na, K, Rb, Cs, and Fr) are the most reactive metals in the periodic table - they all react vigorously or even explosively with cold water, resulting in the displacement of hydrogen.
The Group 1 metal (M) is oxidised to its metal ions, and water is reduced to hydrogen gas (H2) and hydroxide ion (OH−), giving a general equation of:
- 2 M(s) + 2 H2O(l) ⟶ 2 M+(aq) + 2 OH−(aq) + H2(g) [6]
The Group 1 metals or alkali metals become more reactive as their number of energy levels inceases.
Alkaline earth metals
The alkaline earth metals (Be, Mg, Ca, Sr, Ba, and Ra) are the second most reactive metals in the periodic table, and, like the Group 1 metals, have increasing reactivity with increasing numbers of energy levels. Beryllium (Be) is the only alkaline earth metal that does not react with water or steam, even if the metal is heated red hot.[7] Additionally, beryllium has a resistant outer oxide layer that lowers its reactivity at lower temperatures.
Magnesium shows insignificant reaction with water, but burns vigorously with steam or water vapor to produce white magnesium oxide and hydrogen gas:[citation needed]
- Mg(s) + H2O(g) ⟶ MgO(s) + H2(g)
Magnesium has a mild reaction with cold water. The reaction is short-lived because the magnesium hydroxide layer formed on the magnesium is almost insoluble in water and prevents further reaction.
Mg(s) + 2H2O(l) ⟶ Mg(OH)2(s) + H2(g)[8]
A metal reacting with cold water will produce metal hydroxide. However, if a metal reacts with steam, like magnesium, metal oxide is produced as a result of metal hydroxides splitting upon heating.[9]
The hydroxides of calcium, strontium and barium are only slightly water-soluble but produce sufficient hydroxide ions to make the environment basic, giving a general equation of:
- M(s) + 2 H2O(l) ⟶ M(OH)2(aq) + H2(g) [10]
Reactivity series of metals
| Order of reactivity | Metal | Reactions with water or steam |
|---|---|---|
| Most reactive | potassium (K) | Very vigorous reaction with cold water |
| Second most reactive | sodium (Na) | Vigorous reaction with cold water |
| Third most reactive | calcium (Ca) | Less vigorous reaction with cold water |
| Least reactive | magnesium (Mg) | Slow reaction with cold water, vigorous with hot water |
- If metals react with cold water, hydroxides are produced.
- If metals react with steam, oxides are formed.
Hydrogen is always produced when a metal reacts with cold water or steam.[11]
References
- ↑ "The MSDS HyperGlossary: Metal Reactive". Interactive Learning Paradigms Incorporated. http://www.ilpi.com/msds/ref/waterreactive.html.
- ↑ Raymond, Chang (2010). Chemistry (PDF) (tenth ed.). Americas, New York: McGraw-Hill. pp.897-898. ISBN:0077274318. Retrieved 27 February 2018.
- ↑ The University of Iowa. "Reactive Chemicals". https://ehs.research.uiowa.edu/108-reactive-chemicals.
- ↑ Quinn, D. J.; Davies, P. A. (2003). "MODELLING RELEASES OF WATER REACTIVE CHEMICALS". Symposium Series 149. https://www.icheme.org/communities/subject_groups/safety%20and%20loss%20prevention/resources/hazards%20archive/~/media/Documents/Subject%20Groups/Safety_Loss_Prevention/Hazards%20Archive/XVII/XVII-Paper-41.pdf. Retrieved 25 February 2018.
- ↑ Kapias, T; Griffiths, RF (2001). REACTPOOL: A new model for accidental releases of water-reactive chemicals. Crown. ISBN 0-7176-1995-8. http://www.hse.gov.uk/research/crr_pdf/2001/crr01331.pdf. Retrieved 25 February 2018.
- ↑ Landas, Trevor (2 October 2013). "Reactions of Main Group Elements with Water". https://chem.libretexts.org/Core/Inorganic_Chemistry/Descriptive_Chemistry/Main_Group_Reactions/Reactions_of_Main_Group_Elements_with_Water.
- ↑ Pilgaard, Michael. "Beryllium: Chemical Reactions". https://pilgaardelements.com/Beryllium/Reactions.htm.
- ↑ "Reactions of Group 2 Elements with Water" (in en). 2013-10-03. https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Descriptive_Chemistry/Elements_Organized_by_Block/1_s-Block_Elements/Group__2_Elements%3A_The_Alkaline_Earth_Metals/1Group_2%3A_Chemical_Reactions_of_Alkali_Earth_Metals/Reactions_of_Group_2_Elements_with_Water.
- ↑ Clark, Jim. "Reactions of the Group 2 Elements with Water". https://www.chemguide.co.uk/inorganic/group2/reacth2o.html.
- ↑ Landas, Trevor (2 October 2013). "Reactions of Main Group Elements with Water". https://chem.libretexts.org/Core/Inorganic_Chemistry/Descriptive_Chemistry/Main_Group_Reactions/Reactions_of_Main_Group_Elements_with_Water.
- ↑ Gallagher, RoseMarie; Ingram, Paul (2009). Chemistry IGCSE Revision Guide. Great Clarendon Street, Oxford OX2 6DP: Oxford University Press. pp. 114–115.
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