| ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
Standard atomic weight Ar°(Hg) | ||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||||
---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
There are seven stable isotopes of mercury (80Hg) with 202Hg being the most abundant (29.86%). The longest-lived radioisotopes are 194Hg with a half-life of 444 years, and 203Hg with a half-life of 46.612 days. Most of the remaining 40 radioisotopes have half-lives that are less than a day. 199Hg and 201Hg are the most often studied NMR-active nuclei, having spin quantum numbers of 1/2 and 3/2 respectively. All isotopes of mercury are either radioactive or observationally stable, meaning that they are predicted to be radioactive but no actual decay has been observed. These isotopes are predicted to undergo either alpha decay or double beta decay.
180Hg, producible from 180Tl, was found in 2010 to be capable of an unusual form of spontaneous fission. [4] The fission products are 80Kr and 100Ru.
Nuclide [n 1] | Z | N | Isotopic mass (Da) [n 2] [n 3] | Half-life [n 4] | Decay mode [n 5] | Daughter isotope [n 6] | Spin and parity [n 7] [n 4] | Natural abundance (mole fraction) | |||||||||||
---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
Excitation energy [n 4] | Normal proportion | Range of variation | |||||||||||||||||
170Hg [5] | 80 | 90 | 80(+400-40) μs | α | 166Pt | 0+ | |||||||||||||
171Hg | 80 | 91 | 171.00376(32)# | 80(30) μs [59(+36−16) μs] | α | 167Pt | 3/2−# | ||||||||||||
172Hg | 80 | 92 | 171.99883(22) | 420(240) μs [0.25(+35−9) ms] | α | 168Pt | 0+ | ||||||||||||
173Hg | 80 | 93 | 172.99724(22)# | 1.1(4) ms [0.6(+5−2) ms] | α | 169Pt | 3/2−# | ||||||||||||
174Hg | 80 | 94 | 173.992864(21) | 2.0(4) ms [2.1(+18−7) ms] | α | 170Pt | 0+ | ||||||||||||
175Hg | 80 | 95 | 174.99142(11) | 10.8(4) ms | α | 171Pt | 5/2−# | ||||||||||||
176Hg | 80 | 96 | 175.987355(15) | 20.4(15) ms | α (98.6%) | 172Pt | 0+ | ||||||||||||
β+ (1.4%) | 176Au | ||||||||||||||||||
177Hg | 80 | 97 | 176.98628(8) | 127.3(18) ms | α (85%) | 173Pt | 5/2−# | ||||||||||||
β+ (15%) | 177Au | ||||||||||||||||||
178Hg | 80 | 98 | 177.982483(14) | 0.269(3) s | α (70%) | 174Pt | 0+ | ||||||||||||
β+ (30%) | 178Au | ||||||||||||||||||
179Hg | 80 | 99 | 178.981834(29) | 1.09(4) s | α (53%) | 175Pt | 5/2−# | ||||||||||||
β+ (47%) | 179Au | ||||||||||||||||||
β+, p (.15%) | 178Pt | ||||||||||||||||||
180Hg [n 8] | 80 | 100 | 179.978266(15) | 2.58(1) s | β+ (52%) | 180Au | 0+ | ||||||||||||
α (48%) | 176Pt | ||||||||||||||||||
SF | 100Ru, 80Kr | ||||||||||||||||||
181Hg | 80 | 101 | 180.977819(17) | 3.6(1) s | β+ (64%) | 181Au | 1/2(−) | ||||||||||||
α (36%) | 177Pt | ||||||||||||||||||
β+, p (.014%) | 180Pt | ||||||||||||||||||
β+, α (9×10−6%) | 177Ir | ||||||||||||||||||
181mHg | 210(40)# keV | 13/2+ | |||||||||||||||||
182Hg | 80 | 102 | 181.97469(1) | 10.83(6) s | β+ (84.8%) | 182Au | 0+ | ||||||||||||
α (15.2%) | 178Pt | ||||||||||||||||||
β+, p (10−5%) | 181Pt | ||||||||||||||||||
183Hg | 80 | 103 | 182.974450(9) | 9.4(7) s | β+ (74.5%) | 183Au | 1/2− | ||||||||||||
α (25.5%) | 179Pt | ||||||||||||||||||
β+, p (5.6×10−4%) | 182Pt | ||||||||||||||||||
183m1Hg | 198(14) keV | 13/2+# | |||||||||||||||||
183m2Hg | 240(40)# keV | 5# s | β+ | 183Au | 13/2+# | ||||||||||||||
184Hg | 80 | 104 | 183.971713(11) | 30.6(3) s | β+ (98.89%) | 184Au | 0+ | ||||||||||||
α (1.11%) | 180Pt | ||||||||||||||||||
185Hg | 80 | 105 | 184.971899(17) | 49.1(10) s | β+ (94%) | 185Au | 1/2− | ||||||||||||
α (6%) | 181Pt | ||||||||||||||||||
185mHg | 99.3(5) keV | 21.6(15) s | IT (54%) | 185Hg | 13/2+ | ||||||||||||||
β+ (46%) | 185Au | ||||||||||||||||||
α (.03%) | 181Pt | ||||||||||||||||||
186Hg | 80 | 106 | 185.969362(12) | 1.38(6) min | β+ (99.92%) | 186Au | 0+ | ||||||||||||
α (.016%) | 182Pt | ||||||||||||||||||
186mHg | 2217.3(4) keV | 82(5) μs | (8−) | ||||||||||||||||
187Hg | 80 | 107 | 186.969814(15) | 1.9(3) min | β+ | 187Au | 3/2− | ||||||||||||
α (1.2×10−4%) | 183Pt | ||||||||||||||||||
187mHg | 59(16) keV | 2.4(3) min | β+ | 187Au | 13/2+ | ||||||||||||||
α (2.5×10−4%) | 183Pt | ||||||||||||||||||
188Hg | 80 | 108 | 187.967577(12) | 3.25(15) min | β+ | 188Au | 0+ | ||||||||||||
α (3.7×10−5%) | 184Pt | ||||||||||||||||||
188mHg | 2724.3(4) keV | 134(15) ns | (12+) | ||||||||||||||||
189Hg | 80 | 109 | 188.96819(4) | 7.6(1) min | β+ | 189Au | 3/2− | ||||||||||||
α (3×10−5%) | 185Pt | ||||||||||||||||||
189mHg | 80(30) keV | 8.6(1) min | β+ | 189Au | 13/2+ | ||||||||||||||
α (3×10−5%) | 185Pt | ||||||||||||||||||
190Hg | 80 | 110 | 189.966322(17) | 20.0(5) min | β+ [n 9] | 190Au | 0+ | ||||||||||||
191Hg | 80 | 111 | 190.967157(24) | 49(10) min | β+ | 191Au | 3/2(−) | ||||||||||||
191mHg | 128(22) keV | 50.8(15) min | β+ | 191Au | 13/2+ | ||||||||||||||
192Hg | 80 | 112 | 191.965634(17) | 4.85(20) h | EC [n 10] | 192Au | 0+ | ||||||||||||
193Hg | 80 | 113 | 192.966665(17) | 3.80(15) h | β+ | 193Au | 3/2− | ||||||||||||
193mHg | 140.76(5) keV | 11.8(2) h | β+ (92.9%) | 193Au | 13/2+ | ||||||||||||||
IT (7.1%) | 193Hg | ||||||||||||||||||
194Hg | 80 | 114 | 193.965439(13) | 444(77) y | EC | 194Au | 0+ | ||||||||||||
195Hg | 80 | 115 | 194.966720(25) | 10.53(3) h | β+ | 195Au | 1/2− | ||||||||||||
195mHg | 176.07(4) keV | 41.6(8) h | IT (54.2%) | 195Hg | 13/2+ | ||||||||||||||
β+ (45.8%) | 195Au | ||||||||||||||||||
196Hg | 80 | 116 | 195.965833(3) | Observationally Stable [n 11] | 0+ | 0.0015(1) | |||||||||||||
197Hg | 80 | 117 | 196.967213(3) | 64.14(5) h | EC | 197Au | 1/2− | ||||||||||||
197mHg | 298.93(8) keV | 23.8(1) h | IT (91.4%) | 197Hg | 13/2+ | ||||||||||||||
EC (8.6%) | 197Au | ||||||||||||||||||
198Hg | 80 | 118 | 197.9667690(4) | Observationally Stable [n 12] | 0+ | 0.0997(20) | |||||||||||||
199Hg | 80 | 119 | 198.9682799(4) | Observationally Stable [n 13] | 1/2− | 0.1687(22) | |||||||||||||
199mHg | 532.48(10) keV | 42.66(8) min | IT | 199Hg | 13/2+ | ||||||||||||||
200Hg | 80 | 120 | 199.9683260(4) | Observationally Stable [n 14] | 0+ | 0.2310(19) | |||||||||||||
201Hg | 80 | 121 | 200.9703023(6) | Observationally Stable [n 15] | 3/2− | 0.1318(9) | |||||||||||||
201mHg | 766.22(15) keV | 94(3) μs | 13/2+ | ||||||||||||||||
202Hg | 80 | 122 | 201.9706430(6) | Observationally Stable [n 16] | 0+ | 0.2986(26) | |||||||||||||
203Hg | 80 | 123 | 202.9728725(18) | 46.595(6) d | β− | 203Tl | 5/2− | ||||||||||||
203mHg | 933.14(23) keV | 24(4) μs | (13/2+) | ||||||||||||||||
204Hg | 80 | 124 | 203.9734939(4) | Observationally Stable [n 17] | 0+ | 0.0687(15) | |||||||||||||
205Hg | 80 | 125 | 204.976073(4) | 5.14(9) min | β− | 205Tl | 1/2− | ||||||||||||
205mHg | 1556.40(17) keV | 1.09(4) ms | IT | 205Hg | 13/2+ | ||||||||||||||
206Hg | 80 | 126 | 205.977514(22) | 8.15(10) min | β− | 206Tl | 0+ | Trace [n 18] | |||||||||||
207Hg | 80 | 127 | 206.98259(16) | 2.9(2) min | β− | 207Tl | (9/2+) | ||||||||||||
208Hg | 80 | 128 | 207.98594(32)# | 42(5) min [41(+5−4) min] | β− | 208Tl | 0+ | ||||||||||||
209Hg | 80 | 129 | 208.99104(21)# | 37(8) s | 9/2+# | ||||||||||||||
210Hg | 80 | 130 | 209.99451(32)# | 10# min [>300 ns] | 0+ | ||||||||||||||
211Hg | 80 | 131 | 210.99380(200)# | 26(8) s | 9/2+# | ||||||||||||||
212Hg | 80 | 132 | 212.02760(300)# | 1# min [>300 ns] | 0+ | ||||||||||||||
213Hg | 80 | 133 | 213.07670(300)# | 1# s [>300 ns] | 5/2+# | ||||||||||||||
214Hg | 80 | 134 | 214.11180(400)# | 1# s [>300 ns] | 0+ | ||||||||||||||
215Hg | 80 | 135 | 215.16210(400)# | 1# s [>300 ns] | 3/2+# | ||||||||||||||
216Hg | 80 | 136 | 216.19860(400)# | 100# ms [>300 ns] | 0+ | ||||||||||||||
This table header & footer: |
EC: | Electron capture |
IT: | Isomeric transition |
SF: | Spontaneous fission |
Actinium (89Ac) has no stable isotopes and no characteristic terrestrial isotopic composition, thus a standard atomic weight cannot be given. There are 33 known isotopes, from 204Ac to 236Ac, and 7 isomers. Three isotopes are found in nature, 225Ac, 227Ac and 228Ac, as intermediate decay products of, respectively, 237Np, 235U, and 232Th. 228Ac and 225Ac are extremely rare, so almost all natural actinium is 227Ac.
Astatine (85At) has 41 known isotopes, all of which are radioactive; their mass numbers range from 188 to 229. There are also 24 known metastable excited states. The longest-lived isotope is 210At, which has a half-life of 8.1 hours; the longest-lived isotope existing in naturally occurring decay chains is 219At with a half-life of 56 seconds.
There are 42 isotopes of polonium (84Po). They range in size from 186 to 227 nucleons. They are all radioactive. 210Po with a half-life of 138.376 days has the longest half-life of any naturally-occurring isotope of polonium and is the most common isotope of polonium. It is also the most easily synthesized polonium isotope. 209Po, which does not occur naturally, has the longest half-life of all isotopes of polonium at 124 years. 209Po can be made by using a cyclotron to bombard bismuth with protons, as can 208Po.
Lead (82Pb) has four observationally stable isotopes: 204Pb, 206Pb, 207Pb, 208Pb. Lead-204 is entirely a primordial nuclide and is not a radiogenic nuclide. The three isotopes lead-206, lead-207, and lead-208 represent the ends of three decay chains: the uranium series, the actinium series, and the thorium series, respectively; a fourth decay chain, the neptunium series, terminates with the thallium isotope 205Tl. The three series terminating in lead represent the decay chain products of long-lived primordial 238U, 235U, and 232Th. Each isotope also occurs, to some extent, as primordial isotopes that were made in supernovae, rather than radiogenically as daughter products. The fixed ratio of lead-204 to the primordial amounts of the other lead isotopes may be used as the baseline to estimate the extra amounts of radiogenic lead present in rocks as a result of decay from uranium and thorium.
Thallium (81Tl) has 41 isotopes with atomic masses that range from 176 to 216. 203Tl and 205Tl are the only stable isotopes and 204Tl is the most stable radioisotope with a half-life of 3.78 years. 207Tl, with a half-life of 4.77 minutes, has the longest half-life of naturally occurring Tl radioisotopes. All isotopes of thallium are either radioactive or observationally stable, meaning that they are predicted to be radioactive but no actual decay has been observed.
Naturally occurring platinum (78Pt) consists of five stable isotopes (192Pt, 194Pt, 195Pt, 196Pt, 198Pt) and one very long-lived (half-life 4.83×1011 years) radioisotope (190Pt). There are also 34 known synthetic radioisotopes, the longest-lived of which is 193Pt with a half-life of 50 years. All other isotopes have half-lives under a year, most under a day. All isotopes of platinum are either radioactive or observationally stable, meaning that they are predicted to be radioactive but no actual decay has been observed. Platinum-195 is the most abundant isotope.
There are two natural isotopes of iridium (77Ir), and 37 radioisotopes, the most stable radioisotope being 192Ir with a half-life of 73.83 days, and many nuclear isomers, the most stable of which is 192m2Ir with a half-life of 241 years. All other isomers have half-lives under a year, most under a day. All isotopes of iridium are either radioactive or observationally stable, meaning that they are predicted to be radioactive but no actual decay has been observed.
Natural hafnium (72Hf) consists of five observationally stable isotopes (176Hf, 177Hf, 178Hf, 179Hf, and 180Hf) and one very long-lived radioisotope, 174Hf, with a half-life of 7.0×1016 years. In addition, there are 34 known synthetic radioisotopes, the most stable of which is 182Hf with a half-life of 8.9×106 years. This extinct radionuclide is used in hafnium–tungsten dating to study the chronology of planetary differentiation.
Naturally occurring ytterbium (70Yb) is composed of seven stable isotopes: 168Yb, 170Yb–174Yb, and 176Yb, with 174Yb being the most abundant. 30 radioisotopes have been characterized, with the most stable being 169Yb with a half-life of 32.014 days, 175Yb with a half-life of 4.185 days, and 166Yb with a half-life of 56.7 hours. All of the remaining radioactive isotopes have half-lives that are less than 2 hours, and the majority of these have half-lives that are less than 20 minutes. This element also has 18 meta states, with the most stable being 169mYb.
Naturally occurring erbium (68Er) is composed of 6 stable isotopes, with 166Er being the most abundant. 39 radioisotopes have been characterized with between 74 and 112 neutrons, or 142 to 180 nucleons, with the most stable being 169Er with a half-life of 9.4 days, 172Er with a half-life of 49.3 hours, 160Er with a half-life of 28.58 hours, 165Er with a half-life of 10.36 hours, and 171Er with a half-life of 7.516 hours. All of the remaining radioactive isotopes have half-lives that are less than 3.5 hours, and the majority of these have half-lives that are less than 4 minutes. This element also has numerous meta states, with the most stable being 167mEr.
Naturally occurring dysprosium (66Dy) is composed of 7 stable isotopes, 156Dy, 158Dy, 160Dy, 161Dy, 162Dy, 163Dy and 164Dy, with 164Dy being the most abundant. Twenty-nine radioisotopes have been characterized, with the most stable being 154Dy with a half-life of 1.4 million years, 159Dy with a half-life of 144.4 days, and 166Dy with a half-life of 81.6 hours. All of the remaining radioactive isotopes have half-lives that are less than 10 hours, and the majority of these have half-lives that are less than 30 seconds. This element also has 12 meta states, with the most stable being 165mDy, 147mDy and 145mDy.
Naturally occurring neodymium (60Nd) is composed of 5 stable isotopes, 142Nd, 143Nd, 145Nd, 146Nd and 148Nd, with 142Nd being the most abundant (27.2% natural abundance), and 2 long-lived radioisotopes, 144Nd and 150Nd. In all, 33 radioisotopes of neodymium have been characterized up to now, with the most stable being naturally occurring isotopes 144Nd (alpha decay, a half-life (t1/2) of 2.29×1015 years) and 150Nd (double beta decay, t1/2 of 7×1018 years). All of the remaining radioactive isotopes have half-lives that are less than 12 days, and the majority of these have half-lives that are less than 70 seconds; the most stable artificial isotope is 147Nd with a half-life of 10.98 days. This element also has 13 known meta states with the most stable being 139mNd (t1/2 5.5 hours), 135mNd (t1/2 5.5 minutes) and 133m1Nd (t1/2 ~70 seconds).
Naturally occurring cerium (58Ce) is composed of 4 stable isotopes: 136Ce, 138Ce, 140Ce, and 142Ce, with 140Ce being the most abundant and the only one theoretically stable; 136Ce, 138Ce, and 142Ce are predicted to undergo double beta decay but this process has never been observed. There are 35 radioisotopes that have been characterized, with the most stable being 144Ce, with a half-life of 284.893 days; 139Ce, with a half-life of 137.640 days and 141Ce, with a half-life of 32.501 days. All of the remaining radioactive isotopes have half-lives that are less than 4 days and the majority of these have half-lives that are less than 10 minutes. This element also has 10 meta states.
Naturally occurring barium (56Ba) is a mix of six stable isotopes and one very long-lived radioactive primordial isotope, barium-130, identified as being unstable by geochemical means (from analysis of the presence of its daughter xenon-130 in rocks) in 2001. This nuclide decays by double electron capture (absorbing two electrons and emitting two neutrinos), with a half-life of (0.5–2.7)×1021 years (about 1011 times the age of the universe).
There are 39 known isotopes and 17 nuclear isomers of tellurium (52Te), with atomic masses that range from 104 to 142. These are listed in the table below.
Tin (50Sn) is the element with the greatest number of stable isotopes. Moreover, tin is not only the element with the greatest number of observationally stable isotopes, but also the element with the greatest number of theoretically stable isotopes. This is probably related to the fact that 50 is a "magic number" of protons. In addition, twenty-nine unstable tin isotopes are known, including tin-100 (100Sn) and tin-132 (132Sn), which are both "doubly magic". The longest-lived tin radioisotope is tin-126 (126Sn), with a half-life of 230,000 years. The other 28 radioisotopes have half-lives of less than a year.
Bromine (35Br) has two stable isotopes, 79Br and 81Br, and 32 known radioisotopes, the most stable of which is 77Br, with a half-life of 57.036 hours.
Aluminium or aluminum (13Al) has 22 known isotopes from 22Al to 43Al and 4 known isomers. Only 27Al (stable isotope) and 26Al (radioactive isotope, t1/2 = 7.2×105 y) occur naturally, however 27Al comprises nearly all natural aluminium. Other than 26Al, all radioisotopes have half-lives under 7 minutes, most under a second. The standard atomic weight is 26.9815385(7). 26Al is produced from argon in the atmosphere by spallation caused by cosmic-ray protons. Aluminium isotopes have found practical application in dating marine sediments, manganese nodules, glacial ice, quartz in rock exposures, and meteorites. The ratio of 26Al to 10Be has been used to study the role of sediment transport, deposition, and storage, as well as burial times, and erosion, on 105 to 106 year time scales. 26Al has also played a significant role in the study of meteorites.
Californium (98Cf) is an artificial element, and thus a standard atomic weight cannot be given. Like all artificial elements, it has no stable isotopes. The first isotope to be synthesized was 245Cf in 1950. There are 20 known radioisotopes ranging from 237Cf to 256Cf and one nuclear isomer, 249mCf. The longest-lived isotope is 251Cf with a half-life of 898 years.
Einsteinium (99Es) is a synthetic element, and thus a standard atomic weight cannot be given. Like all synthetic elements, it has no stable isotopes. The first isotope to be discovered was 253Es in 1952. There are 18 known radioisotopes from 240Es to 257Es, and 3 nuclear isomers. The longest-lived isotope is 252Es with a half-life of 471.7 days, or around 1.293 years.