{"id":362,"date":"2020-04-09T11:17:52","date_gmt":"2020-04-09T11:17:52","guid":{"rendered":"https:\/\/thechemicalelements.com\/?page_id=362"},"modified":"2023-08-15T10:31:28","modified_gmt":"2023-08-15T10:31:28","slug":"arsenic","status":"publish","type":"post","link":"https:\/\/thechemicalelements.com\/arsenic\/","title":{"rendered":"Arsenic (Ar)"},"content":{"rendered":"\n

Arsenic is a chemical element with an atomic number 33 in the periodic table of elements<\/a>. There\u2019s 1.5\u20132 ppm of this crystalline metalloid in the Earth\u2019s crust. Being a member of the phosphorus<\/a> family of periodic table elements, this chemical element has five valence electrons that help arsenic make numerous compounds with other substances.<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Chemical and Physical Properties of Arsenic<\/span><\/h3>\n\n\n\n
Property<\/strong><\/td>Value<\/strong><\/td><\/tr>
Symbol<\/td>As<\/td><\/tr>
Name<\/td>Arsenic<\/td><\/tr>
Atomic Number<\/td>33<\/td><\/tr>
Group<\/td>Non-Metal<\/td><\/tr>
Crystal Structure<\/td>Rhombohedral<\/td><\/tr>
Atomic Weight<\/td>74.92159<\/td><\/tr>
Shells<\/td>2,8,18,5<\/td><\/tr>
Orbitals<\/td>[Ar] 3d10 4s2 4p3<\/td><\/tr>
Valence<\/td>-3,0,3,5<\/td><\/tr>
Electronegativity<\/td>2.18<\/td><\/tr>
Covalent Radius<\/td>1.20 \u00c5<\/td><\/tr>
Ionic Radius<\/td>.58 (+3) \u00c5<\/td><\/tr>
Atomic Radius<\/td>1.33 \u00c5<\/td><\/tr>
Atomic Volume<\/td>13.1 cm\u00b3\/mol<\/td><\/tr>
Name Origin<\/td>Greek: arsenikon; Latin: arsenicum<\/td><\/tr>
Discovered By<\/td>Some mineral forms known to the ancients, but Albertus Magnus accredited with discovery<\/td><\/tr>
Year<\/td>13th Century (Albertus Magnus<\/em>)<\/td><\/tr>
Location<\/td>Unknown<\/td><\/tr>
Pronunciation<\/td>AR-s’n-ik<\/td><\/tr>
Oxidation States<\/td>(\u00b13),5<\/td><\/tr>
Density<\/td>5.72 g\/cm\u00b3<\/td><\/tr>
Uses<\/td>Weed killer, rat poison, semiconductors, paints, wallpapers, ceramics<\/td><\/tr>
Description<\/td>Soft metalloid, grey metallic to red glassy appearance<\/td><\/tr>
Color<\/td>Gray<\/td><\/tr>
Physical State<\/td>metalloid\/semimetal (brittle crystalline solid)<\/td><\/tr>
Half-life<\/td>12 days<\/td><\/tr>
Density<\/td>5.7 g.cm-3 at 14\u00b0C<\/td><\/tr>
Melting Point<\/td>814 \u00b0C (36 atm)<\/td><\/tr>
Boiling Point<\/td>615 \u00b0C (sublimation)<\/td><\/tr>
Van der Waals Radius<\/td>0.139 nm<\/td><\/tr>
Isotopes<\/td>8<\/td><\/tr>
Most Characteristic Isotope<\/td><\/td><\/tr>
The Energy of the First Ionization<\/td>947 kJ.mol -1<\/td><\/tr>
The Energy of the Second Ionization<\/td>1798 kJ.mol -1<\/td><\/tr>
The Energy of the Third Ionization<\/td>2736 kJ.mol -1<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

The chemical and physical properties of arsenic make this substance a semimetal since it displays both metal and non-metal characteristics. Having a place in the periodic table of elements under the symbol As, with an atomic number of 33, an atomic weight (mass) of 74.9216 g.mol -1, and electronic configuration <\/span>[Ar] 3d\u00b9\u2070 4s\u00b2 4p\u00b3<\/span>, arsenic is ductile and reaches its boiling point at 615 \u00b0C (sublimation), which is lower than its melting point at 814 \u00b0C (36 atm). <\/span><\/p>\n\n\n\n

When arsenic is submitted to heat treatment, it changes from a solid aggregate state into a gas aggregate state. <\/span><\/p>\n\n\n\n

The fact sheet of this member of the boron<\/a> family of elements in the periodic table also discloses that arsenic has an electronegativity of 2.0 according to Pauling. The atomic radius according to van der Waals is 0.139 nm.<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

How Was Arsenic Discovered?<\/span><\/h2>\n\n\n\n

Arsenic and its toxic properties have been known since ancient times. Even the early Egyptian, Chinese, and Greek civilizations made use of the arsenic compound. In the Middle Ages, Paracelsus was the most famous physician-alchemist who had special formulas for the preparation of metallic arsenic. During the rule of the Ming dynasty in China, the toxic arsenic compounds were used as pesticides in rice fields.  <\/span><\/p>\n\n\n\n

The ancient civilizations were also familiar with As<\/span>2<\/span>O<\/span>3   <\/span>trioxide, known under the name of \u2018white arsenic,” which has extremely high toxicity, which imposed an increased risk on human health.<\/span> This arsenic compound was made by the burning of arsenic. The arsenic metal was produced by mixing arsenic trioxide with olive oil. <\/span><\/p>\n\n\n\n

In the 1920s, the discovery of arsenic as a periodic table element was attributed to the German Catholic Dominican friar, bishop, and alchemist Albertus Magnus (before 1200 \u2013 November 15, 1280). Namely, by heating the arsenic compound orpiment (As2S3) together with a piece of soap, he managed to produce the pure form of arsenic.<\/span><\/p>\n\n\n\n

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How Did Arsenic Get Its Name?<\/span><\/h2>\n\n\n\n

The name \u201carsenic\u201d originates from the Greek expression “arsenikon”, which means “yellow orpiment”.<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Where Can You Find Arsenic?<\/span><\/h2>\n\n\n\n

Rarely found in its free form, arsenic can mostly be smelted from compounds of minerals, such as arsenopyrite (FeAsS), realgar (AsS), and orpiment (As2S3). Arsenic commonly occurs in the form of arsenic sulfide, metal arsenates, or metal arsenides.\u00a0<\/span><\/p>\n\n\n\n

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How Is Arsenic Used in Everyday Life?<\/span><\/h2>\n\n\n\n

Arsenic has a wide application in our everyday life. It is used for bronzing, pyrotechnics, and the production of a special type of glass. In the United States, arsenic is mostly used as a wood preservative.<\/span><\/p>\n\n\n\n

This member of the phosphorus family of chemical elements is also found in traditional Chinese pharmaceutical preparations for the treatment of various health problems, such as inflammation, asthma, joint pain, cough, and cancer.<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

How Dangerous Is Arsenic?<\/span><\/h2>\n\n\n\n

This substance is considered a sort of human carcinogen due to its extremely toxic effects. The most dangerous aspect of arsenic is the fact that it\u2019s odourless and colorless, which enables the unaware long-term exposure and consumption of a certain amount of arsenic. This toxic substance can contaminate the air and water via volcanic activity, metal smelting, production, and use of pesticides, wood preservatives, and underground waters.\u00a0<\/span><\/p>\n\n\n\n

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Arsenic Poisoning<\/span><\/h3>\n\n\n\n

Arsenicosis, or poisoning after exposure to arsenic, mostly occurs when even low levels are inhaled or consumed via contaminated drinking water or high arsenic concentrations in groundwater. People who work with arsenic-based pesticides, or whose work involves contact with high levels of inorganic arsenic compounds may be exposed to higher levels of arsenic. <\/span><\/p>\n\n\n\n

Some of the negative health effects that appear as a result of arsenic contamination or exposure to both higher and lower levels of arsenic include abdominal pain, skin rash, and redness, nausea, vomiting, and dysfunction of the digestive system organs, etc. Long-term exposure to high levels of arsenic and arsenates (typically via contaminated drinking water) can lead to more severe medical conditions, such as lung cancer, skin cancer, or bladder cancer.<\/span><\/p>\n\n\n\n

One such occurrence has been recorded in <\/span>Bangladesh<\/span><\/a>, where the water supply, being polluted by arsenic, imposed a great risk on the health of the population living in that area.\u00a0<\/span><\/p>\n\n\n\n

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Environmental Effects of Arsenic<\/span><\/h2>\n\n\n\n

Arsenic exposure hazard is most pronounced in industrial areas, but could also stem from the groundwater, private wells (contaminated well water), and other similar water sources contaminated with high levels of arsenic concentration. Bangladesh, Chile, the US, Argentina, Mexico, India, Taiwan, and China, comprise the list of countries with an increased risk of arsenic exposure and public health hazards related to arsenic. <\/span><\/p>\n\n\n\n

EPA or <\/span>the U.S. Environmental Protection Agency<\/span><\/a> is responsible for the protection of the environment and public health. Together with the Department of Health, the CDC – Center for Disease Control and Prevention, the <\/span>Agency for Toxic Substances and Disease Registry<\/span><\/a>, the <\/span>Food and Drug Administration<\/span><\/a> (FDA), and the U.S. <\/span>Department of Health and Human Services<\/span><\/a> (DHHS), EPA has classified inorganic arsenic as a human carcinogen. <\/span><\/p>\n\n\n\n

In collaboration with the International Agency for Research on Cancer (IARC), the <\/span>World Health Organization<\/span><\/a> published a scientific paper confirming the toxic effects of arsenic and supporting the claim that exposure to soluble inorganic arsenic presents a major public health concern. <\/span><\/p>\n\n\n\n

Additionally, the <\/span>Occupational Safety & Health Administration<\/span><\/a> provides all the needed information on arsenic health hazards, as well as means of precaution and protection after arsenic poisoning.\u00a0<\/span><\/p>\n\n\n\n

<\/div>\n\n\n\n

Isotopes of Arsenic<\/span><\/h2>\n\n\n\n

This chemical element counts 33 known isotopes, among which there\u2019s only one stable isotope (<\/span>75<\/span>As).<\/span><\/p>\n\n\n\n

The following is a chart representation of the arsenic isotopes.<\/span><\/p>\n\n\n\n

Nuclide<\/b>\n

[n 1]<\/span><\/p>\n<\/td>

Z<\/i><\/b><\/td>N<\/i><\/b><\/td>Isotopic mass <\/b>(Da)<\/span>\n

[n 2]<\/span>[n 3]<\/span><\/p>\n<\/td>

Half-life<\/b><\/td>Decay<\/b>\n

mode<\/b><\/p>\n

[n 4]<\/span><\/p>\n<\/td>

Daughter<\/b>\n

isotope<\/b><\/p>\n

[n 5][n 6]<\/span><\/p>\n<\/td>

Spin and<\/b>\n

parity<\/b><\/p>\n

[n 7][n 8]<\/span><\/p>\n<\/td>

Natural abundance <\/b>(mole fraction)<\/span><\/td><\/tr>
Excitation energy<\/b>[n 8]<\/span><\/td>Normal proportion<\/b><\/td>Range of variation<\/b><\/td><\/tr>
60<\/span>As<\/span><\/td>33<\/span><\/td>27<\/span><\/td>59.99313(64)#<\/span><\/td> <\/td>p<\/span><\/a><\/td>59<\/span>Ge<\/span><\/td>5+#<\/span><\/td> <\/td> <\/td><\/tr>
61<\/span>As<\/span><\/td>33<\/span><\/td>28<\/span><\/td>60.98062(64)#<\/span><\/td> <\/td>p<\/span><\/td>60<\/span>Ge<\/span><\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
62<\/span>As<\/span><\/td>33<\/span><\/td>29<\/span><\/td>61.97320(32)#<\/span><\/td> <\/td>p<\/span><\/td>61<\/span>Ge<\/span><\/td>1+#<\/span><\/td> <\/td> <\/td><\/tr>
63<\/span>As<\/span><\/td>33<\/span><\/td>30<\/span><\/td>62.96369(54)#<\/span><\/td> <\/td>p<\/span><\/td>62<\/span>Ge<\/span><\/td>(3\/2\u2212)#<\/span><\/td> <\/td> <\/td><\/tr>
64<\/span>As<\/span><\/td>33<\/span><\/td>31<\/span><\/td>63.95757(38)#<\/span><\/td>40(30) ms<\/span>\n

[18(+43-7) ms]<\/span><\/p>\n<\/td>

\u03b2<\/span>+<\/span><\/a><\/td>64<\/span>Ge<\/span><\/td>0+#<\/span><\/td> <\/td> <\/td><\/tr>
65<\/span>As<\/span><\/td>33<\/span><\/td>32<\/span><\/td>64.94956(32)#<\/span><\/td>170(30) ms<\/span><\/td>\u03b2<\/span>+<\/span><\/td>65<\/span>Ge<\/span><\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
66<\/span>As<\/span><\/td>33<\/span><\/td>33<\/span><\/td>65.94471(73)<\/span><\/td>95.77(23) ms<\/span><\/td>\u03b2<\/span>+<\/span><\/td>66<\/span>Ge<\/span><\/td>(0+)<\/span><\/td> <\/td> <\/td><\/tr>
66m1<\/span>As<\/span><\/td>1356.70(17) keV<\/span><\/td>1.1(1) \u00b5s<\/span><\/td> <\/td> <\/td>(5+)<\/span><\/td> <\/td> <\/td><\/tr>
66m2<\/span>As<\/span><\/td>3023.9(3) keV<\/span><\/td>8.2(5) \u00b5s<\/span><\/td> <\/td> <\/td>(9+)<\/span><\/td> <\/td> <\/td><\/tr>
67<\/span>As<\/span><\/td>33<\/span><\/td>34<\/span><\/td>66.93919(11)<\/span><\/td>42.5(12) s<\/span><\/td>\u03b2<\/span>+<\/span><\/td>67<\/span>Ge<\/span><\/td>(5\/2\u2212)<\/span><\/td> <\/td> <\/td><\/tr>
68<\/span>As<\/span><\/td>33<\/span><\/td>35<\/span><\/td>67.93677(5)<\/span><\/td>151.6(8) s<\/span><\/td>\u03b2<\/span>+<\/span><\/td>68<\/span>Ge<\/span><\/td>3+<\/span><\/td> <\/td> <\/td><\/tr>
68m<\/span>As<\/span><\/td>425.21(16) keV<\/span><\/td>111(20) ns<\/span>\n

[?107(+23-16) ns]<\/span><\/p>\n<\/td>

 <\/td> <\/td>1+<\/span><\/td> <\/td> <\/td><\/tr>
69<\/span>As<\/span><\/td>33<\/span><\/td>36<\/span><\/td>68.93227(3)<\/span><\/td>15.2(2) min<\/span><\/td>\u03b2<\/span>+<\/span><\/td>69<\/span>Ge<\/span><\/td>5\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
70<\/span>As<\/span><\/td>33<\/span><\/td>37<\/span><\/td>69.93092(5)<\/span><\/td>52.6(3) min<\/span><\/td>\u03b2<\/span>+<\/span><\/td>70<\/b>Ge<\/b><\/td>4(+#)<\/span><\/td> <\/td> <\/td><\/tr>
70m<\/span>As<\/span><\/td>32.008(23) keV<\/span><\/td>96(3) \u00b5s<\/span><\/td> <\/td> <\/td>2(+)<\/span><\/td> <\/td> <\/td><\/tr>
71<\/span>As<\/span><\/td>33<\/span><\/td>38<\/span><\/td>70.927112(5)<\/span><\/td>65.28(15) h<\/span><\/td>\u03b2<\/span>+<\/span><\/td>71<\/span>Ge<\/span><\/td>5\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
72<\/span>As<\/span><\/td>33<\/span><\/td>39<\/span><\/td>71.926752(5)<\/span><\/td>26.0(1) h<\/span><\/td>\u03b2<\/span>+<\/span><\/td>72<\/b>Ge<\/b><\/td>2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
73<\/span>As<\/span><\/td>33<\/span><\/td>40<\/span><\/td>72.923825(4)<\/span><\/td>80.30(6) d<\/span><\/td>EC<\/span><\/a><\/td>73<\/b>Ge<\/b><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
74<\/span>As<\/span><\/td>33<\/span><\/td>41<\/span><\/td>73.9239287(25)<\/span><\/td>17.77(2) d<\/span><\/td>\u03b2<\/span>+<\/span> (66%)<\/span><\/td>74<\/b>Ge<\/b><\/td>2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span> (34%)<\/span><\/td>74<\/b>Se<\/b><\/td><\/tr>
75<\/span>As<\/span><\/td>33<\/span><\/td>42<\/span><\/td>74.9215965(20)<\/span><\/td>Stable<\/b><\/td>3\/2\u2212<\/span><\/td>1.0000<\/span><\/td> <\/td><\/tr>
75m<\/span>As<\/span><\/td>303.9241(7) keV<\/span><\/td>17.62(23) ms<\/span><\/td> <\/td> <\/td>9\/2+<\/span><\/td> <\/td> <\/td><\/tr>
76<\/span>As<\/span><\/td>33<\/span><\/td>43<\/span><\/td>75.922394(2)<\/span><\/td>1.0942(7) d<\/span><\/td>\u03b2<\/span>\u2212<\/span> (99.98%)<\/span><\/td>76<\/b>Se<\/b><\/td>2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
EC (.02%)<\/span><\/td>76<\/i><\/b>Ge<\/i><\/b><\/td><\/tr>
76m<\/span>As<\/span><\/td>44.425(1) keV<\/span><\/td>1.84(6) \u00b5s<\/span><\/td> <\/td> <\/td>(1)+<\/span><\/td> <\/td> <\/td><\/tr>
77<\/span>As<\/span><\/td>33<\/span><\/td>44<\/span><\/td>76.9206473(25)<\/span><\/td>38.83(5) h<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>77m<\/span>Se<\/span><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
77m<\/span>As<\/span><\/td>475.443(16) keV<\/span><\/td>114.0(25) \u00b5s<\/span><\/td> <\/td> <\/td>9\/2+<\/span><\/td> <\/td> <\/td><\/tr>
78<\/span>As<\/span><\/td>33<\/span><\/td>45<\/span><\/td>77.921827(11)<\/span><\/td>90.7(2) min<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>78<\/b>Se<\/b><\/td>2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
79<\/span>As<\/span><\/td>33<\/span><\/td>46<\/span><\/td>78.920948(6)<\/span><\/td>9.01(15) min<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>79m<\/span>Se<\/span><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
79m<\/span>As<\/span><\/td>772.81(6) keV<\/span><\/td>1.21(1) \u00b5s<\/span><\/td> <\/td> <\/td>(9\/2)+<\/span><\/td> <\/td> <\/td><\/tr>
80<\/span>As<\/span><\/td>33<\/span><\/td>47<\/span><\/td>79.922534(25)<\/span><\/td>15.2(2) s<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>80<\/b>Se<\/b><\/td>1+<\/span><\/td> <\/td> <\/td><\/tr>
81<\/span>As<\/span><\/td>33<\/span><\/td>48<\/span><\/td>80.922132(6)<\/span><\/td>33.3(8) s<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>81m<\/span>Se<\/span><\/td>3\/2\u2212<\/span><\/td> <\/td> <\/td><\/tr>
82<\/span>As<\/span><\/td>33<\/span><\/td>49<\/span><\/td>81.92450(21)<\/span><\/td>19.1(5) s<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>82<\/i><\/b>Se<\/i><\/b><\/td>(1+)<\/span><\/td> <\/td> <\/td><\/tr>
82m<\/span>As<\/span><\/td>250(200) keV<\/span><\/td>13.6(4) s<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>82<\/i><\/b>Se<\/i><\/b><\/td>(5-)<\/span><\/td> <\/td> <\/td><\/tr>
83<\/span>As<\/span><\/td>33<\/span><\/td>50<\/span><\/td>82.92498(24)<\/span><\/td>13.4(3) s<\/span><\/td>\u03b2<\/span>\u2212<\/span><\/td>83m<\/span>Se<\/span><\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
84<\/span>As<\/span><\/td>33<\/span><\/td>51<\/span><\/td>83.92906(32)#<\/span><\/td>4.02(3) s<\/span><\/td>\u03b2<\/span>\u2212<\/span> (99.721%)<\/span><\/td>84<\/span>Se<\/span><\/td>(3)(+#)<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, <\/span>n<\/span><\/a> (.279%)<\/span><\/td>83<\/span>Se<\/span><\/td><\/tr>
84m<\/span>As<\/span><\/td>0(100)# keV<\/span><\/td>650(150) ms<\/span><\/td> <\/td> <\/td> <\/td> <\/td> <\/td><\/tr>
85<\/span>As<\/span><\/td>33<\/span><\/td>52<\/span><\/td>84.93202(21)#<\/span><\/td>2.021(10) s<\/span><\/td>\u03b2<\/span>\u2212<\/span>, n (59.4%)<\/span><\/td>84<\/span>Se<\/span><\/td>(3\/2\u2212)#<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span> (40.6%)<\/span><\/td>85<\/span>Se<\/span><\/td><\/tr>
86<\/span>As<\/span><\/td>33<\/span><\/td>53<\/span><\/td>85.93650(32)#<\/span><\/td>0.945(8) s<\/span><\/td>\u03b2<\/span>\u2212<\/span> (67%)<\/span><\/td>86<\/span>Se<\/span><\/td> <\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (33%)<\/span><\/td>85<\/span>Se<\/span><\/td><\/tr>
87<\/span>As<\/span><\/td>33<\/span><\/td>54<\/span><\/td>86.93990(32)#<\/span><\/td>0.56(8) s<\/span><\/td>\u03b2<\/span>\u2212<\/span> (84.6%)<\/span><\/td>87<\/span>Se<\/span><\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n (15.4%)<\/span><\/td>86<\/span>Se<\/span><\/td><\/tr>
88<\/span>As<\/span><\/td>33<\/span><\/td>55<\/span><\/td>87.94494(54)#<\/span><\/td>300# ms<\/span>\n

[>300 ns]<\/span><\/p>\n<\/td>

\u03b2<\/span>\u2212<\/span><\/td>88<\/span>Se<\/span><\/td> <\/td> <\/td> <\/td><\/tr>
\u03b2<\/span>\u2212<\/span>, n<\/span><\/td>87<\/span>Se<\/span><\/td><\/tr>
89<\/span>As<\/span><\/td>33<\/span><\/td>56<\/span><\/td>88.94939(54)#<\/span><\/td>200# ms<\/span>\n

[>300 ns]<\/span><\/p>\n<\/td>

\u03b2<\/span>\u2212<\/span><\/td>89<\/span>Se<\/span><\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
90<\/span>As<\/span><\/td>33<\/span><\/td>57<\/span><\/td>89.95550(86)#<\/span><\/td>80# ms<\/span>\n

[>300 ns]<\/span><\/p>\n<\/td>

 <\/td> <\/td> <\/td> <\/td> <\/td><\/tr>
91<\/span>As<\/span><\/td>33<\/span><\/td>58<\/span><\/td>90.96043(97)#<\/span><\/td>50# ms<\/span>\n

[>300 ns]<\/span><\/p>\n<\/td>

 <\/td> <\/td>3\/2\u2212#<\/span><\/td> <\/td> <\/td><\/tr>
92<\/span>As<\/span><\/td>33<\/span><\/td>59<\/span><\/td>91.96680(97)#<\/span><\/td>30# ms<\/span>\n

[>300 ns]<\/span><\/p>\n<\/td>

 <\/td> <\/td> <\/td> <\/td> <\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

Source: Wikipedia<\/span><\/p>\n\n\n\n

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Arsenic Compounds <\/span><\/h2>\n\n\n\n

Arsenic compounds exhibit both metallic and nonmetallic properties. The most common oxidation states are the trivalent and pentavalent forms. The inorganic forms of arsenic are considered as the most toxic substances. After ingestion, the inorganic arsenic compounds are methylated to dimethylarsinic acid (DMA) and monomethylarsonic acid (MMA). These two compounds of arsenic are less toxic, and can be easily excreted via urine.\u00a0<\/span><\/p>\n\n\n\n

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Forms of Arsenic Compounds<\/span><\/h3>\n\n\n\n

Regarding their biological and toxicological properties, the arsenic compounds can be classified into three major groups:<\/span><\/p>\n\n\n\n