Isotopes Of Cadmium

Information about Isotopes Of Cadmium

Naturally occurring Cadmium (Cd) is composed of 8 isotopes. For two of them, natural radioactivity was observed, and three others are predicted to be radioactive but their decays were never observed, due to extremely long half-life times. The two natural radioactive isotopes are ¹¹³Cd (beta decay, half-life is 7.7 Ã— 10¹⁵ years) and ¹¹⁶Cd (two-neutrino double beta decay, half-life is 2.9 Ã— 10¹⁹ years). The other three are ¹⁰⁶Cd, ¹⁰⁸Cd (double electron capture), and ¹¹⁴Cd (double beta decay); only lower limits on their half-life times have been set. At least three isotopes - ¹¹⁰Cd, ¹¹¹Cd, and ¹¹²Cd - are absolutely stable. Among the isotopes absent in the natural cadmium, the most long-lived are ¹⁰⁹Cd with a half-life of 462.6 days, and ¹¹⁵Cd with a half-life of 53.46 hours. All of the remaining radioactive isotopes have half-lives that are less than 2.5 hours and the majority of these have half-lives that are less than 5 minutes. This element also has 8 known meta states with the most stable being ^113mCd (t_Â½ 14.1 years), ^115mCd (t_Â½ 44.6 days) and ^117mCd (t_Â½ 3.36 hours).

The known isotopes of cadmium range in atomic mass from 94.950 u (⁹⁵Cd) to 131.946 u (¹³²Cd). The primary decay mode before the second most abundant stable isotope, ¹¹²Cd, is electron capture and the primary modes after are beta emission and electron capture. The primary decay product before ¹¹²Cd is element 47 (silver) and the primary product after is element 49 (indium).
Standard atomic mass: 112.411(8) u

Table

nuclide symbol	Z(p)	N(n)	isotopic mass (u)	half-life	nuclear spin	representative isotopic composition (mole fraction)	range of natural variation (mole fraction)
nuclide symbol	excitation energy			half-life	nuclear spin	representative isotopic composition (mole fraction)	range of natural variation (mole fraction)
⁹⁵Cd	48	47	94.94987(64)#	5# ms	9/2+#
⁹⁶Cd	48	48	95.93977(54)#	1# s	0+
⁹⁷Cd	48	49	96.93494(43)#	2.8(6) s	9/2+#
⁹⁸Cd	48	50	97.92740(8)	9.2(3) s	0+
^98mCd	2427.5(6) keV			190(20) ns	8+#
⁹⁹Cd	48	51	98.92501(22)#	16(3) s	(5/2+)
¹⁰⁰Cd	48	52	99.92029(10)	49.1(5) s	0+
¹⁰¹Cd	48	53	100.91868(16)	1.36(5) min	(5/2+)
¹⁰²Cd	48	54	101.91446(3)	5.5(5) min	0+
¹⁰³Cd	48	55	102.913419(17)	7.3(1) min	5/2+
¹⁰⁴Cd	48	56	103.909849(10)	57.7(10) min	0+
¹⁰⁵Cd	48	57	104.909468(12)	55.5(4) min	5/2+
¹⁰⁶Cd	48	58	105.906459(6)	STABLE [>410E+18 a]	0+	0.0125(6)
¹⁰⁷Cd	48	59	106.906618(6)	6.50(2) h	5/2+
¹⁰⁸Cd	48	60	107.904184(6)	STABLE [>410E+15 a]	0+	0.0089(3)
¹⁰⁹Cd	48	61	108.904982(4)	461.4(12) d	5/2+
^109m1Cd	59.6(4) keV			12(2) Âµs	1/2+
^109m2Cd	463.0(5) keV			10.9(5) Âµs	11/2-
¹¹⁰Cd	48	62	109.9030021(29)	STABLE	0+	0.1249(18)
¹¹¹Cd	48	63	110.9041781(29)	STABLE	1/2+	0.1280(12)
^111mCd	396.214(21) keV			48.50(9) min	11/2-
¹¹²Cd	48	64	111.9027578(29)	STABLE	0+	0.2413(21)
¹¹³Cd	48	65	112.9044017(29)	7.7(3)E+15 a	1/2+	0.1222(12)
^113mCd	263.54(3) keV			14.1(5) a	11/2-
¹¹⁴Cd	48	66	113.9033585(29)	STABLE [>6.4E+18 a]	0+	0.2873(42)
¹¹⁵Cd	48	67	114.9054310(29)	53.46(5) h	1/2+
^115mCd	181.0(5) keV			44.56(24) d	(11/2)-
¹¹⁶Cd	48	68	115.904756(3)	3.1(4)E+19 a	0+	0.0749(18)
¹¹⁷Cd	48	69	116.907219(4)	2.49(4) h	1/2+
^117mCd	136.4(2) keV			3.36(5) h	(11/2)-
¹¹⁸Cd	48	70	117.906915(22)	50.3(2) min	0+
¹¹⁹Cd	48	71	118.90992(9)	2.69(2) min	(3/2+)
^119mCd	146.54(11) keV			2.20(2) min	(11/2-)#
¹²⁰Cd	48	72	119.90985(2)	50.80(21) s	0+
¹²¹Cd	48	73	120.91298(9)	13.5(3) s	(3/2+)
^121mCd	214.86(15) keV			8.3(8) s	(11/2-)
¹²²Cd	48	74	121.91333(5)	5.24(3) s	0+
¹²³Cd	48	75	122.91700(4)	2.10(2) s	(3/2)+
^123mCd	316.52(23) keV			1.82(3) s	(11/2-)
¹²⁴Cd	48	76	123.91765(7)	1.25(2) s	0+
¹²⁵Cd	48	77	124.92125(7)	0.65(2) s	(3/2+)#
^125mCd	50(70) keV			570(90) ms	11/2-#
¹²⁶Cd	48	78	125.92235(6)	0.515(17) s	0+
¹²⁷Cd	48	79	126.92644(8)	0.37(7) s	(3/2+)
¹²⁸Cd	48	80	127.92776(32)	0.28(4) s	0+
¹²⁹Cd	48	81	128.93215(32)#	242(8) ms	3/2+#
^129mCd	0(200)# keV			104(6) ms	11/2-#
¹³⁰Cd	48	82	129.9339(3)	162(7) ms	0+
¹³¹Cd	48	83	130.94067(32)#	68(3) ms	7/2-#
¹³²Cd	48	84	131.94555(54)#	97(10) ms	0+

Notes

The precision of the isotope abundances and atomic mass is limited through variations. The given ranges should be applicable to any normal terrestrial material.
Geologically exceptional samples are known in which the isotopic composition lies outside the reported range. The uncertainty in the atomic mass may exceed the stated value for such specimens.
Values marked # are not purely derived from experimental data, but at least partly from systematic trends. Spins with weak assignment arguments are enclosed in parentheses.
Uncertainties are given in concise form in parentheses after the corresponding last digits. Uncertainty values denote one standard deviation, except isotopic composition and standard atomic mass from IUPAC which use expanded uncertainties.

References

Isotope masses from Ame2003 Atomic Mass Evaluation by G. Audi, A.H. Wapstra, C. Thibault, J. Blachot and O. Bersillon in Nuclear Physics A729 (2003).
Isotopic compositions and standard atomic masses from Atomic weights of the elements. Review 2000 (IUPAC Technical Report). Pure Appl. Chem. Vol. 75, No. 6, pp. 683-800, (2003) and Atomic Weights Revised (2005).
Half-life, spin, and isomer data selected from these sources. Editing notes on this article's talk page.
Audi, Bersillon, Blachot, Wapstra. The Nubase2003 evaluation of nuclear and decay properties, Nuc. Phys. A 729, pp. 3-128 (2003).
National Nuclear Data Center, Brookhaven National Laboratory. Information extracted from the NuDat 2.1 database (retrieved Sept. 2005).
David R. Lide (ed.), Norman E. Holden in CRC Handbook of Chemistry and Physics, 85th Edition, online version. CRC Press. Boca Raton, Florida (2005). Section 11, Table of the Isotopes.

Isotopes of silver	Isotopes of cadmium	Isotopes of indium
Index to isotope pages

Cadmium (IPA: /ˈkÃ¦dmiəm/) is a chemical element in the periodic table that has the symbol Cd and atomic number 48.
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Isotopes are any of the several different forms of an element each having different atomic mass (mass number). Isotopes of an element have nuclei with the same number of protons (the same atomic number) but different numbers of neutrons.
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Radioactive decay is the process in which an unstable atomic nucleus loses energy by emitting radiation in the form of particles or electromagnetic waves. This decay, or loss of energy, results in an atom of one type, called the parent nuclide
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For , see .

The half-life of a quantity, subject to exponential decay, is the time required for the quantity to decay to half of its initial value.
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beta decay is a type of radioactive decay in which a beta particle (an electron or a positron) is emitted. In the case of electron emission, it is referred to as "beta minus" (β⁻), while in the case of a positron emission as "beta plus" (β⁺).
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For , see .

The half-life of a quantity, subject to exponential decay, is the time required for the quantity to decay to half of its initial value.
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Emission processes: Neutron emission Positron emission Proton emission
Capturing: Electron capture Neutron capture
Stellar nucleosynthesis pp-Chain CNO cycle α process Triple-α Carbon burning Ne burning O burning Si burning R-process S-process P-process
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For , see .

The half-life of a quantity, subject to exponential decay, is the time required for the quantity to decay to half of its initial value.
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Double electron capture is a decay mode of atomic nucleus. For a nuclide (A, Z) with number of nucleons A and atomic number Z, double electron capture is only possible if the mass of the nuclide of (A, Z-2) is lower.
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For , see .

The half-life of a quantity, subject to exponential decay, is the time required for the quantity to decay to half of its initial value.
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A nuclear isomer is a metastable state of an atomic nucleus caused by the excitation of one or more of its nucleons. A nuclear isomer occupies a higher energy state than the corresponding non-excited nucleus, called the ground state.
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atomic mass (m_a) is the mass of an atom at rest, most often expressed in unified atomic mass units.^[1] The atomic mass may be considered to be the total mass of protons, neutrons and electrons in a single atom (when the atom is motionless).
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The unified atomic mass unit (u), or dalton (Da), is a small unit of mass used to express atomic and molecular masses. It is defined to be one twelfth of the mass of an unbound atom of the carbon-12 nuclide, at rest and in its ground state.
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Electron capture (sometimes called Inverse Beta Decay) is a decay mode for isotopes that will occur when there are too many protons in the nucleus of an atom and insufficient energy to emit a positron; however, it continues to be an inviable decay mode for radioactive
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In nuclear physics, a decay product, also known as a daughter product, daughter isotope or daughter nuclide, is a nuclide resulting from the radioactive decay of a parent isotope or precursor nuclide.
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Silver (IPA: /ˈsɪlvə(ɹ)/) is a chemical element with the symbol Ag (Latin: argentum) and atomic number 47.
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Indium (IPA: /ˈɪndiəm/) is a chemical element with chemical symbol In and atomic number 49. This rare, soft, malleable and easily fusible poor metal is chemically similar to aluminium or gallium but more
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Proton

The quark structure of the proton.
Composition: 2 up, 1 down
Family: Fermion
Group: Quark
Interaction: Gravity, Electromagnetic, Weak, Strong
Antiparticle: Antiproton
Discovered: Ernest Rutherford (1919)
Symbol: p+
Mass: 1.
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Neutron

The quark structure of the neutron.
Composition: one up, two down
Family: Fermion
Group: Quark
Interaction: Gravity, Electromagnetic, Weak, Strong
Antiparticle: Antineutron
Discovered: James Chadwick^[1]
Symbol: n
Mass: 1.
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FPs / 10⁶ thermal ²³⁵U
Nuclide Halflife Yield
¹⁵⁵Eu 4.76 < 330
⁸⁵Kr 10.76 2717
^113mCd 14.1 < 3
⁹⁰Sr 28.9 57518
¹³⁷Cs 30.23 60899
^121mSn 43.
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Naturally occurring Silver (Ag) is composed of the two stable isotopes ¹⁰⁷Ag and ¹⁰⁹Ag with ¹⁰⁷Ag being the more abundant (51.839% natural abundance). Standard atomic mass: 107.8682(2) u.
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Indium (In)
Standard atomic mass: 114.818(3) u

Table

nuclide
symbol Z(p) N(n)
isotopic mass (u)
half-life nuclear
spin representative
isotopic
composition
(mole fraction) range of natural
variation
(mole fraction)
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Index to the isotopes of <element> pages
1
H 2
He
3
Li 4
Be 5
B 6
C 7
N 8
O 9
F 10
Ne
11
Na 12
Mg 13
Al 14
Si 15
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Isotopes Of Cadmium

Information about Isotopes Of Cadmium

Table

Notes

References

Table