Sodium

Jump to: navigation, search
<tr><td>Chemical series</td><td>alkali metals</td></tr> <tr><td>Appearance</td><td>silvery white
BigNa.jpg <tr><td>Atomic radius</td><td>180pm</td></tr><tr><td>Atomic radius (calc.)</td><td>190 pm</td></tr><tr><td>Covalent radius</td><td>154 pm</td></tr><tr><td>Van der Waals radius</td><td>227 pm</td></tr> <tr><td rowspan="1" valign="top">Magnetic ordering</td><td>paramagnetic</td></tr><tr><td>Electrical resistivity</td><td>(20 °C) 47.7 nΩ·m</td></tr><tr><td>Thermal conductivity</td><td>(300 K) 142 W·m−1·K−1</td></tr><tr><td>Thermal expansion</td><td>(25 °C) 71 µm·m−1·K−1</td></tr><tr><td>Speed of sound (thin rod)</td><td>(20 °C) 3200 m/s</td></tr><tr><td>Young's modulus</td><td>10 GPa</td></tr><tr><td>Shear modulus</td><td>3.3 GPa</td></tr><tr><td>Bulk modulus</td><td>6.3 GPa</td></tr><tr><td>Mohs hardness</td><td>0.5</td></tr><tr><td>Brinell hardness</td><td>0.69 MPa</td></tr><tr><td>CAS registry number</td><td>7440-23-5</td></tr>
11 neonsodiummagnesium
Li

Na

K
Na-TableImage.png
General
Name, symbol, number sodium, Na, 11
Group, period, block 13, s
Standard atomic weight 22.98976928(2) g·mol−1
Electron configuration [Ne] 3s1
Electrons per shell 2, 8, 1
Physical properties<tr><td>Phase</td><td>solid</td></tr><tr><td>Density (near r.t.)</td><td>0.968 g·cm−3</td></tr><tr><td>Liquid density at m.p.</td><td>0.927 g·cm−3</td></tr><tr><td>Melting point</td><td>370.87 K
(97.72 °C, 207.9 °F)</td></tr><tr><td>Boiling point</td><td>1156 K
(883 °C, 1621 °F)</td></tr><tr><td>Critical point</td><td>(extrapolated)
2573 K, 35 MPa</td></tr><tr><td>Heat of fusion</td><td>2.60 kJ·mol−1</td></tr><tr><td>Heat of vaporization</td><td>97.42 kJ·mol−1</td></tr><tr><td>Heat capacity</td><td>(25 °C) 28.230 J·mol−1·K−1</td></tr>
Vapor pressure
P/Pa 1 10 100 1 k 10 k 100 k
at T/K 554 617 697 802 946 1153
Atomic properties

<tr><td>Crystal structure</td><td>cubic body centered</td></tr><tr><td>Oxidation states</td><td>1
(strongly basic oxide)</td></tr><tr><td>Electronegativity</td><td>0.93 (Pauling scale)</td></tr>

Ionization energies
(more)
1st: 495.8 kJ·mol−1
2nd: 4562 kJ·mol−1
3rd: 6910.3 kJ·mol−1
Miscellaneous
Selected isotopes
Main article: Isotopes of sodium
iso NA half-life DM DE (MeV) DP
22Na syn 2.602 y β+ 0.546 22Ne
ε - 22Ne
γ 1.2745 -
23Na 100% Na is stable with 12 neutrons
References
This box: view  talk  edit

WikiDoc Resources for

Sodium

Articles

Most recent articles on Sodium

Most cited articles on Sodium

Review articles on Sodium

Articles on Sodium in N Eng J Med, Lancet, BMJ

Media

Powerpoint slides on Sodium

Images of Sodium

Photos of Sodium

Podcasts & MP3s on Sodium

Videos on Sodium

Evidence Based Medicine

Cochrane Collaboration on Sodium

Bandolier on Sodium

TRIP on Sodium

Clinical Trials

Ongoing Trials on Sodium at Clinical Trials.gov

Trial results on Sodium

Clinical Trials on Sodium at Google

Guidelines / Policies / Govt

US National Guidelines Clearinghouse on Sodium

NICE Guidance on Sodium

NHS PRODIGY Guidance

FDA on Sodium

CDC on Sodium

Books

Books on Sodium

News

Sodium in the news

Be alerted to news on Sodium

News trends on Sodium

Commentary

Blogs on Sodium

Definitions

Definitions of Sodium

Patient Resources / Community

Patient resources on Sodium

Discussion groups on Sodium

Patient Handouts on Sodium

Directions to Hospitals Treating Sodium

Risk calculators and risk factors for Sodium

Healthcare Provider Resources

Symptoms of Sodium

Causes & Risk Factors for Sodium

Diagnostic studies for Sodium

Treatment of Sodium

Continuing Medical Education (CME)

CME Programs on Sodium

International

Sodium en Espanol

Sodium en Francais

Business

Sodium in the Marketplace

Patents on Sodium

Experimental / Informatics

List of terms related to Sodium

Editor-In-Chief: C. Michael Gibson, M.S., M.D. [1]

Associate Editor-In-Chief: Cafer Zorkun, M.D., Ph.D. [2]


Overview

Sodium (IPA: /ˈsəʊdiəm/) is a chemical element which has the symbol Na (Latin: natrium), atomic number 11, atomic mass 22.9898 g/mol, common oxidation number +1. Sodium is a soft, silvery white, highly reactive element and is a member of the alkali metals within "group 1" (formerly known as ‘group IA’). It has only one stable isotope, 23Na. Sodium was first isolated by Sir Humphry Davy in 1807 by passing an electric current through molten sodium hydroxide. Sodium quickly oxidizes in air and is violently reactive with water, so it must be stored in an inert medium, such as kerosene. Sodium is present in great quantities in the earth's oceans as sodium chloride. It is also a component of many minerals, and it is an essential element for animal life. As such, it is classified as a “dietary inorganic macro-mineral.”

Notable characteristics

The flame test for sodium displays a brilliantly bright yellow emission due to the so called "sodium D-lines" at 588.9950 and 589.5924 nanometers.

Compared with other alkali metals, sodium is generally less reactive than potassium and more so than lithium, in accordance with "periodic law": for example, their reaction in water, chlorine gas, etc.; the reactivity of their nitrates, chlorates, perchlorates, etc. The density of elements generally increase with increasing atomic number, but potassium is less dense than sodium.

Owing to its high reactivity, sodium is found in nature only as a compound and never as the free element. Sodium reacts exothermically with water: small pea-sized pieces will bounce across the surface of the water until they are consumed by it, whereas large pieces will explode. While sodium reacts with water at room temperature, the sodium piece melts with the heat of the reaction to form a sphere, if the reacting sodium piece is large enough. The reaction with water produces very caustic sodium hydroxide and highly flammable hydrogen gas. These are extreme hazards (see Precautions section below). When burned in air, sodium forms sodium peroxide Na2O2, or with limited oxygen, the oxide Na2O</sub> (unlike lithium, the nitride is not formed). If burned in oxygen under pressure, sodium superoxide NaO2 will be produced.

When sodium or its compounds are introduced into a flame it will contribute a bright yellow.

Sodium ions are necessary for regulation of blood and body fluids, transmission of nerve impulses, heart activity, and certain metabolic functions. Interestingly, sodium is needed by animals, which maintain high concentrations in their blood and extracellular fluids, but the ion is not needed by plants. A completely plant-based diet, therefore, will be very low in sodium. This requires some herbivores to obtain their sodium from salt licks and other mineral sources. The animal need for sodium is probably the reason for the highly-conserved ability to taste the sodium ion as "salty." Receptors for the pure salty taste respond best to sodium, and otherwise only to a few other small monovalent cations (Li+, NH4+, and to some extent also K+). Calcium chloride also tastes somewhat salty, but also quite bitter.

The most common sodium salt, sodium chloride (table salt), used for seasoning (for example the English word "salad" refers to salt) and warm-climate food preservation, such as pickling and making jerky (the high osmotic content of salt inhibits bacterial and fungal growth). As such, salt has been an important commodity in human activities (the English word salary refers to salarium, the perquisite ("perk") given to Roman soldiers for the purpose of buying salt). The human requirement for sodium in the diet is less than 500 mg per day, which is typically less than a tenth as much as many diets "seasoned to taste." Most people consume far more sodium than is physiologically needed. For certain people with salt-sensitive blood pressure, this extra intake may cause a negative effect on health.

Precautions

Extreme care is required in handling elemental/metallic sodium. Sodium is potentially explosive in water (depending on quantity) and is a caustic poison, since it is rapidly converted to sodium hydroxide on contact with moisture. The powdered form may combust spontaneously in air or oxygen. Sodium must be stored either in an inert (oxygen and moisture free) atmosphere (such as nitrogen or argon), or under a liquid hydrocarbon such as mineral oil or kerosene.

The reaction of sodium and water is a familiar one in chemistry labs, and is reasonably safe if amounts of sodium smaller than a pencil eraser are used and the reaction is done behind a plastic shield by people wearing eye protection. However, the sodium-water reaction does not scale up well, and is treacherous when larger amounts of sodium are used. Larger pieces of sodium melt under the heat of the reaction, and the molten ball of metal is buoyed up by hydrogen and may appear to be stably reacting with water, until splashing covers more of the reaction mass, causing thermal runaway and an explosion which scatters molten sodium, lye solution, and sometimes flame. (18.5 g explosion [3]) This behavior is unpredictable, and among the alkali metals it is usually sodium which invites this surprise phenomenon, because lithium is not reactive enough to do it, and potassium is so reactive that chemistry students are not tempted to try the reaction with larger potassium pieces.

Sodium is much more reactive than magnesium; a reactivity which can be further enhanced due to sodium's much lower melting point. When sodium catches fire in air (as opposed to just the hydrogen gas generated from water by means of its reaction with sodium) it more easily produces temperatures high enough to melt the sodium, exposing more of its surface to the air and spreading the fire.

Few common fire extinguishers work on sodium fires. Water, of course, exacerbates sodium fires, as do water-based foams. CO2 and Halon are often ineffective on sodium fires, which reignite when the extinguisher dissipates. Among the very few materials effective on a sodium fire are Pyromet and Met-L-X. Pyromet is a NaCl/(NH4)2HPO4 mix, with flow/anti-clump agents. It smothers the fire, drains away heat, and melts to form an impermeable crust. This is the standard dry-powder canister fire extinguisher for all classes of fires. Met-L-X is mostly sodium chloride, NaCl, with approximately 5% Saran plastic as a crust-former, and flow/anti-clumping agents. It is most commonly hand-applied, with a scoop. Other extreme fire extinguishing materials include [[Lith+]], a graphite based dry powder with an organophosphate flame retardant; and [[Na+]], a Na2CO3-based material.

Because of the reaction scale problems discussed above, disposing of large quantities of sodium (more than 10 to 100 grams) must be done through a licensed hazardous materials disposer. Smaller quantities may be broken up and neutralized carefully with ethanol (which has a much slower reaction than water), or even methanol (where the reaction is more rapid than ethanol's but still less than in water), but care should nevertheless be taken, as the caustic products from the ethanol or methanol reaction are just as hazardous to eyes and skin as those from water. After the alcohol reaction appears complete, and all pieces of reaction debris have been broken up or dissolved, a mixture of alcohol and water, then pure water, may then be carefully used for a final cleaning. This should be allowed to stand a few minutes until the reaction products are diluted more thoroughly and flushed down the drain. The purpose of the final water soak and wash of any reaction mass which may contain sodium is to ensure that alcohol does not carry unreacted sodium into the sink trap, where a water reaction may generate hydrogen in the trap space which can then be potentially ignited, causing a confined sink trap explosion.

Physiology and sodium ions

Main article: action potential

Sodium ions play a diverse and important role in many physiological processes. Excitable animal cells, for example, rely on the entry of Na+ to cause a depolarization. An example of this is signal transduction in the human central nervous system, which depends on sodium ion motion across the nerve cell membrane, in all nerves.

Some potent neurotoxins, such as batrachotoxin, increase the sodium ion permeability of the cell membranes in nerves and muscles, causing a massive and irreversible depolarization of the membranes, with potentially fatal consequences. However, drugs with smaller effects on sodium ion motion in nerves may have diverse pharmacological effects which range from anti-depressant to anti-seizure actions.

Sodium is the primary cation (positive ion) in extracellular fluids in animals and humans. These fluids, such as blood plasma and extracellular fluids in other tissues, bathe cells and carry out transport functions for nutrients and wastes. Sodium is also the principal cation in seawater, although the concentration there is about 3.8 times what it is normally in extracellular body fluids.

Although the system for maintaining optimal salt and water balance in the body is a complex one, one of the primary ways in which the human body keeps track of loss of body water is that osmoreceptors in the hypothalamus sense a balance of sodium and water concentration in extracellular fluids. Relative loss of body water will cause sodium concentration to rise higher than normal, a condition known as hypernatremia. This ordinarily results in thirst. Conversely, an excess of body water caused by drinking will result in too little sodium in the blood (hyponatremia), a condition which is again sensed by the hypothalamus, causing a decrease in vasopressin hormone secretion from the posterior pituitary, and a consequent loss of water in the urine, which acts to restore blood sodium concentrations to normal.

Severely dehydrated persons, such as people rescued from ocean or desert survival situations, usually have very high blood sodium concentrations. These must be very carefully and slowly returned to normal, since too-rapid correction of hypernatremia may result in brain damage from cellular swelling, as water moves suddenly into cells with high osmolar content.

Because the hypothalamus/osmoreceptor system ordinarily works well to cause drinking or urination to restore the body's sodium concentrations to normal, this system can be used in medical treatment to regulate the body's total fluid content, by first controlling the body's sodium content. Thus, when a powerful diuretic drug is given which causes the kidneys to excrete sodium, the effect is accompanied by an excretion of body water (water loss accompanies sodium loss). This happens because the kidney is unable to efficiently retain water while excreting large amounts of sodium. In addition, after sodium excretion, the osmoreceptor system may sense lowered sodium concentration in the blood, and then directs compensatory urinary loss of water, in order to correct the hyponatremia, or (low-blood-sodium) state.

See also

References

  • Rebecca J. Donatelle. Health, The Basics. 6th ed. San Francisco: Pearson Education, Inc. 2005.

External links


af:Natrium ar:صوديوم ast:Sodiu bn:সোডিয়াম zh-min-nan:Na (goân-sò͘) be:Натрый bs:Natrijum bg:Натрий ca:Sodi cs:Sodík co:Sodiu cy:Sodiwm da:Natrium de:Natrium et:Naatrium el:Νάτριοeo:Natrio eu:Sodio fa:سدیمfur:Sodi ga:Sóidiam gl:Sodio (elemento) ko:나트륨 hy:Նատրիում hi:सोडियम hr:Natrij io:Natro id:Natrium is:Natrín it:Sodio he:נתרן ht:Sodyòm ku:Sodyûm la:Natrium lv:Nātrijs lb:Natrium lt:Natris ln:Sodu jbo:sodna hu:Nátrium mk:Натриум ml:സോഡിയം mi:Konutai nl:Natriumno:Natrium nn:Natrium nov:Natrium oc:Sòdi uz:Natriy nds:Natriumqu:Natriyusq:Natriumi scn:Sodiu simple:Sodium sk:Sodík sl:Natrij sr:Натријум sh:Natrij fi:Natrium sv:Natrium ta:சோடியம் th:โซเดียมtg:Натрийuk:Натрій wa:Sodiom zh-yue:鈉


Navigation WikiDoc | WikiPatient | Up To Date Pages | Recently Edited Pages | Recently Added Pictures

Table of Contents In Alphabetical Order | By Individual Diseases | Signs and Symptoms | Physical Examination | Lab Tests | Drugs

Editor Tools Become an Editor | Editors Help Menu | Create a Page | Edit a Page | Upload a Picture or File | Printable version | Permanent link | Maintain Pages | What Pages Link Here
There is no pharmaceutical or device industry support for this site and we need your viewer supported Donations | Editorial Board | Governance | Licensing | Disclaimers | Avoid Plagiarism | Policies
Linked-in.jpg