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Isotopes of titanium (22Ti)
Main isotopes[1] Decay
Isotope abun­dance half-life (t1/2) mode pro­duct
44Ti synth 59.1 y ε 44Sc
45Ti synth 3.08 h β+ 45Sc
46Ti 8.25% stable
47Ti 7.44% stable
48Ti 73.7% stable
49Ti 5.41% stable
50Ti 5.18% stable
Standard atomic weight Ar°(Ti)

Naturally occurring titanium (22Ti) is composed of five stable isotopes; 46Ti, 47Ti, 48Ti, 49Ti and 50Ti with 48Ti being the most abundant (73.8% natural abundance). Twenty-three radioisotopes have been characterized, with the most stable being 44Ti with a half-life of 59.1 years and 45Ti with a half-life of 184.8 minutes. All of the remaining radioactive isotopes have half-lives that are less than 10 minutes, and the majority of these have half-lives that are less than one second.

The isotopes of titanium range from 39Ti to 64Ti. The primary decay mode for isotopes lighter than the stable isotopes is β+ and the primary mode for the heavier ones is β−; the decay products are respectively scandium isotopes and vanadium isotopes.

There are two stable isotopes of titanium with an odd number of nucleons, 47Ti and 49Ti, which thus have non-zero nuclear spin of 5/2− and 7/2− (respectively) and are NMR-active.[4]

List of isotopes

[edit]


Nuclide
[n 1] 		Z N Isotopic mass (Da)[5]
[n 2][n 3] 		Half-life[1]
[n 4] 		Decay
mode[1]
[n 5] 		Daughter
isotope
[n 6] 		Spin and
parity[1]
[n 7][n 4] 		Natural abundance (mole fraction)
Excitation energy Normal proportion[1] Range of variation
39Ti 22 17 39.00268(22)# 28.5(9) ms β+, p (93.7%) 38Ca 3/2+#
β+ (~6.3%) 39Sc
β+, 2p (?%) 37K
40Ti 22 18 39.990345(73) 52.4(3) ms β+, p (95.8%) 39Ca 0+
β+ (4.2%) 40Sc
41Ti 22 19 40.983148(30) 81.9(5) ms β+, p (91.1%) 40Ca 3/2+
β+ (8.9%) 41Sc
42Ti 22 20 41.97304937(29) 208.3(4) ms β+ 42Sc 0+
43Ti 22 21 42.9685284(61) 509(5) ms β+ 43Sc 7/2−
43m1Ti 313.0(10) keV 11.9(3) μs IT 43Ti (3/2+)
43m2Ti 3066.4(10) keV 556(6) ns IT 43Ti (19/2−)
44Ti 22 22 43.95968994(75) 59.1(3) y EC 44Sc 0+
45Ti 22 23 44.95812076(90) 184.8(5) min β+ 45Sc 7/2−
45mTi 36.53(15) keV 3.0(2) μs IT 45Ti 3/2−
46Ti 22 24 45.952626356(97) Stable 0+ 0.0825(3)
47Ti 22 25 46.951757491(85) Stable 5/2− 0.0744(2)
48Ti 22 26 47.947940677(79) Stable 0+ 0.7372(3)
49Ti 22 27 48.947864391(84) Stable 7/2− 0.0541(2)
50Ti 22 28 49.944785622(88) Stable 0+ 0.0518(2)
51Ti 22 29 50.94660947(52) 5.76(1) min β− 51V 3/2−
52Ti 22 30 51.9468835(29) 1.7(1) min β− 52V 0+
53Ti 22 31 52.9496707(31) 32.7(9) s β− 53V (3/2)−
54Ti 22 32 53.950892(17) 2.1(10) s β− 54V 0+
55Ti 22 33 54.955091(31) 1.3(1) s β− 55V (1/2)−
56Ti 22 34 55.95768(11) 200(5) ms β− 56V 0+
57Ti 22 35 56.96307(22) 95(8) ms β− 57V 5/2−#
58Ti 22 36 57.96681(20) 55(6) ms β− 58V 0+
59Ti 22 37 58.97222(32)# 28.5(19) ms β− 59V 5/2−#
59mTi 108.5(5) keV 615(11) ns IT 59Ti 1/2−#
60Ti 22 38 59.97628(26) 22.2(16) ms β− 60V 0+
61Ti 22 39 60.98243(32)# 15(4) ms β− 61V 1/2−#
61m1Ti 125.0(5) keV 200(28) ns IT 61Ti 5/2−#
61m2Ti 700.1(7) keV 354(69) ns IT 61Ti 9/2+#
62Ti 22 40 61.98690(43)# 9# ms
[>620 ns] 		0+
63Ti 22 41 62.99371(54)# 10# ms
[>620 ns] 		1/2−#
64Ti 22 42 63.99841(64)# 5# ms
[>620 ns] 		0+
65Ti[6] 22 43 65.00559(75)# 1# ms 1/2−#
66Ti[6] 22 44 0+
This table header & footer:
  1. ^ mTi – Excited nuclear isomer.
  2. ^ ( ) – Uncertainty (1σ) is given in concise form in parentheses after the corresponding last digits.
  3. ^ # – Atomic mass marked #: value and uncertainty derived not from purely experimental data, but at least partly from trends from the Mass Surface (TMS).
  4. ^ a b # – Values marked # are not purely derived from experimental data, but at least partly from trends of neighboring nuclides (TNN).
  5. ^ Modes of decay:
    EC: Electron capture



    n: Neutron emission
    p: Proton emission
  6. ^ Bold symbol as daughter – Daughter product is stable.
  7. ^ ( ) spin value – Indicates spin with weak assignment arguments.

Titanium-44

[edit]

Titanium-44 (44Ti) is a radioactive isotope of titanium that undergoes electron capture with a half-life of 59.1 years to an excited state of scandium-44, before reaching the ground state of 44Sc and ultimately of 44Ca.[7] Because titanium-44 can decay only through electron capture, its half-life increases slowly with its ionization state and it becomes stable in its fully ionized state (that is, having a charge of +22),[8] though as astrophysical environments never lack electrons completely, it will always decay.

Titanium-44 is produced in relative abundance in the alpha process in stellar nucleosynthesis and the early stages of supernova explosions.[9] It is produced when stable calcium-40 adds an alpha particle (helium-4), as nickel-56 is the result of adding three more. The age of supernova remnants (even though nickel-56 has died away to iron) may be determined through measurements of gamma-ray emissions from the relatively long-lived titanium-44 and of its abundance.[8] It was observed in the Cassiopeia A supernova remnant and SN 1987A at a relatively high concentration, enhanced by the delayed decay in the ionizing conditions.[7]

See also

[edit]

Daughter products other than titanium

References

[edit]
Revisions and contributorsEdit on WikipediaRead on Wikipedia

Isotopes of titanium

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(atomic number 22) has five stable isotopes—⁴⁶Ti, ⁴⁷Ti, ⁴⁸Ti, ⁴⁹Ti, and ⁵⁰Ti—that constitute its natural isotopic composition on , with ⁴⁸Ti being the most abundant at 73.72%. These isotopes have relative atomic masses of 45.95263(4) u, 46.95176(4) u, 47.94794(4) u, 48.94787(4) u, and 49.94479(4) u, respectively, resulting in a of 47.867(1) for the element. In addition to these stable nuclides, titanium has numerous radioactive isotopes, with over two dozen characterized to date and mass numbers spanning approximately 40 to 66. The longest-lived radioisotope is ⁴⁴Ti, which decays primarily by to ⁴⁴Sc with a of 60 years and is significant in astrophysical studies of . Other notable short-lived isotopes include ⁴⁵Ti, with a of 3.08 hours, which is used in (PET) for applications due to its β⁺ decay. Titanium isotopes, both stable and radioactive, are employed in , cosmology, and to trace processes such as planetary formation and .

Overview

Natural occurrence and abundance

Naturally occurring titanium consists of five stable isotopes: ^{46}Ti, ^{47}Ti, ^{48}Ti, ^{49}Ti, and ^{50}Ti. These isotopes have relative abundances of 8.25% for ^{46}Ti, 7.44% for ^{47}Ti, 73.72% for ^{48}Ti, 5.41% for ^{49}Ti, and 5.18% for ^{50}Ti, resulting in a standard atomic weight of 47.867(1). ^{48}Ti is the most abundant, comprising over 73% of natural titanium. Titanium is primarily sourced from minerals such as (FeTiO_3) and (TiO_2), which are found in igneous rocks, sediments, and placer deposits worldwide. Unlike elements with long-lived radioactive isotopes, natural titanium contains no primordial radionuclides, as all its naturally occurring isotopes are stable. Slight variations in titanium isotopic ratios have been observed in meteorites and lunar samples, attributed to early solar system processes such as nucleosynthetic anomalies or mixing of presolar materials. For instance, calcium-aluminum-rich inclusions in chondritic meteorites show mass-independent fractionation in titanium isotopes, reflecting heterogeneous distribution in the solar nebula. Precise determination of these abundances relies on mass spectrometry techniques, such as multiple-collector (MC-ICP-MS), which achieve high-resolution separation and quantification of isotopic ratios in geological samples.

Synthetic isotopes and production

Synthetic isotopes of titanium encompass a wide range of artificially produced nuclides beyond the five stable natural ones (⁴⁶Ti, ⁴⁷Ti, ⁴⁸Ti, ⁴⁹Ti, and ⁵⁰Ti), spanning mass numbers from ³⁹Ti to ⁶⁶Ti, with 25 known radioactive isotopes, all of which are unstable. Recent observations include ⁶⁵Ti and ⁶⁶Ti reported in 2025. These synthetic isotopes are created exclusively in laboratory settings, as they do not occur naturally in significant quantities, and their production has enabled studies in , , and medical applications. The earliest discoveries of titanium isotopes, including initial synthetic efforts, date back to the 1930s, when F.W. used and deuteron bombardment techniques to identify both stable and early radioactive variants at the in . Production of synthetic titanium isotopes primarily relies on nuclear reactions induced by particle accelerators, reactors, and high-energy collisions. , often performed in nuclear reactors, involves capturing neutrons on stable targets to form heavier isotopes, such as ⁵¹Ti produced via on ⁵⁰Ti at facilities like in the 1940s. Proton bombardment in cyclotrons targets lighter elements to yield titanium nuclides through reactions like (p,n) or (p,2n); for instance, ⁴⁵Ti is generated by irradiating natural with 13 MeV protons, followed by chemical separation. Similarly, ⁴⁴Ti is produced via proton irradiation of scandium targets in cyclotrons, such as the RFT-30, enabling its use as a generator for scandium-44 in . Spallation reactions and projectile fragmentation at high-energy accelerators, like those simulating conditions, create lighter isotopes through the breakup of heavier targets; ⁴⁴Ti, for example, has been observed in such fragmentation of calcium or iron nuclei. These methods produce isotopes with half-lives ranging from extremely short, such as ~10⁻²¹ seconds for ⁶⁶Ti formed in heavy-ion collisions, to relatively longer ones like 3.08 hours for ⁴⁵Ti. Stable natural isotopes serve as enriched starting materials for many of these syntheses to optimize yields.

Nuclear properties

Isotopic masses and binding energies

The atomic masses of isotopes are precisely determined through experimental measurements and evaluated in the Atomic Mass Evaluation (AME2020), providing essential data for understanding nuclear structure and stability. These masses, expressed in atomic mass units (u), along with their mass excesses (the difference between the atomic mass and the mass number A, in energy units), reveal deviations from integer masses due to binding effects. For (Z=22), the stable isotopes exhibit masses clustered around A=46 to 50, with uncertainties typically on the order of 0.000001 u. The total binding energy B of a nucleus is calculated using the in units: B=[ZmH+Nmn−M]c2B = \left[ Z m_{\mathrm{H}} + N m_{\mathrm{n}} - M \right] c^2 where Z is the , N = A - Z is the neutron number, m_H is the atomic mass of (1.007825 u), m_n is the mass (1.008665 u), M is the of the , and c is the . This quantifies the stability arising from the strong overcoming Coulomb repulsion. The binding per nucleon, B/A, serves as a key metric for comparing isotopic stability, typically reaching 8.5–8.7 MeV for mid-mass titanium isotopes. Representative data for the stable titanium isotopes from AME2020 are summarized below, including atomic masses, mass excesses, binding energies per nucleon, and nuclear spin-parity values from associated nuclear data evaluations. Uncertainties are included in parentheses.
IsotopeAtomic Mass (u)Mass Excess (keV)Binding Energy per Nucleon (MeV)Spin-Parity
⁴⁶Ti45.952626(1)-44 128(1)8.6590⁺
⁴⁷Ti46.951758(1)-44 938(1)8.6655/2⁻
⁴⁸Ti47.947941(1)-48 493(1)8.7290⁺
⁴⁹Ti48.947864(1)-48 564(1)8.7167/2⁻
⁵⁰Ti49.944786(1)-51 432(1)8.7610⁺
For ⁴⁸Ti, the binding energy per nucleon is approximately 8.73 MeV, exemplifying the calculation: with Z=22, N=26, and M=47.947941 u, the mass defect yields a total B ≈ 418.8 MeV, or B/A ≈ 8.73 MeV. Lighter titanium isotopes, such as ⁴⁴Ti (mass 43.959690(8) u, mass excess -37 549(1) keV, B/A ≈ 8.53 MeV), show lower binding energies per nucleon, while heavier ones like ⁵⁰Ti peak near the stability maximum. This trend—increasing B/A from lighter to mid-mass isotopes, peaking around ⁵⁰Ti—defines the stability window for titanium, where the semi-magic neutron number N=28 enhances binding due to shell effects. The even-even isotopes (⁴⁶Ti, ⁴⁸Ti, ⁵⁰Ti) consistently exhibit spin-parity 0⁺, reflecting paired nucleons, whereas odd-neutron isotopes like ⁴⁷Ti (5/2⁻) and ⁴⁹Ti (7/2⁻) show half-integer spins from the unpaired neutron's orbital angular momentum.

Decay modes and half-lives

The unstable isotopes of display decay modes that follow typical patterns for neutron-deficient and neutron-rich nuclides relative to the stable isotopes ^{46}Ti through ^{50}Ti. Neutron-deficient isotopes below ^{48}Ti predominantly undergo (EC) or β⁺ decay, as exemplified by ^{44}Ti and ^{45}Ti, while neutron-rich isotopes above ^{50}Ti favor beta minus (β⁻) decay, such as ^{51}Ti and ^{52}Ti. is exceedingly rare and not a dominant pathway for any titanium isotope due to unfavorable Q-values and nuclear structure effects. Half-lives of titanium radioisotopes span several orders of magnitude, reflecting their proximity to the line of stability. The longest-lived is ^{44}, with a half-life of 60.0 ± 0.9 years, decaying solely by EC. Another relatively long-lived example is ^{45}, with a half-life of 184.8 ± 0.5 minutes, primarily via β⁺ decay. In contrast, most other unstable titanium isotopes are short-lived, with half-lives under 1 hour; for instance, ^{51} has a half-life of 5.76 ± 0.05 minutes through β⁻ decay, and ^{52} decays in 1.7 ± 0.1 minutes via β⁻. These short half-lives for the majority of isotopes (from ^{39} to ^{63}, excluding the noted exceptions) arise from high decay energies and allowed transitions. Specific decay chains highlight the processes involved. For ^{44}Ti, EC occurs 100% to excited states in ^{44}Sc, primarily the 78 keV level (branching ratio ~86%) and the 68 keV level (~14%), followed by the daughter ^{44}Sc decaying via β⁺ or EC to stable ^{44}Ca with prominent γ emission at 1157.0 keV (intensity 99.6%). The Q-value for the EC branch of ^{44}Ti to the ground state of ^{44}Sc is 267.8 ± 1.9 keV, limiting decay to low-lying excited states and prohibiting β⁺ emission. Similarly, ^{51}Ti undergoes β⁻ decay (Q-value 983 ± 5 keV) to excited states in ^{51}V, often followed by γ de-excitation. These chains underscore how binding energies influence decay feasibility, with β⁺/EC favored when Q-values exceed ~1022 keV for positron emission.
IsotopeDecay ModeHalf-LifeQ-Value (keV)Notes
^{44}TiEC (100%)60.0 ± 0.9 y267.8 ± 1.9 (to ^{44}Sc g.s.)Decays to excited ^{44}Sc; prominent γ at 1157 keV from daughter
^{45}Tiβ⁺ (85%) + EC (15%)184.8 ± 0.5 min4395 ± 2 (to ^{45}Sc g.s.)Used in PET due to
^{51}Tiβ⁻ (100%)5.76 ± 0.05 min983 ± 5To excited ^{51} states
This table illustrates representative examples across the mass range, emphasizing the transition from EC/β⁺ to β⁻ dominance.

Notable isotopes

Titanium-44

Titanium-44 (44^{44}Ti) is the longest-lived radioactive isotope of titanium, possessing an atomic mass of 43.959690 u. It undergoes electron capture decay exclusively to scandium-44 (44^{44}Sc) with a branching ratio of 100%, exhibiting a half-life of 60 years. The daughter 44^{44}Sc nucleus de-excites primarily through the emission of characteristic gamma rays, including a prominent line at 1157 keV. In astrophysical environments, 44^{44}Ti is synthesized via the alpha-particle capture reaction 40^{40}Ca(α\alpha,γ\gamma)44^{44}Ti during the alpha-rich freeze-out phase in massive stars and subsequent core-collapse supernovae. Theoretical models predict yields of 44^{44}Ti constituting approximately 0.1-1% of the total mass of material ejected in these events, serving as a key diagnostic for . Detection of 44^{44}Ti in supernova remnants relies on observing its decay gamma-ray signature at 1157 keV, which has been identified in the remnant (Cas A) using the COMPTEL instrument aboard the . Similarly, the 67.9 keV and 78.4 keV lines from 44^{44}Ti decay were detected in the remnant of () by the satellite, providing direct evidence of recent . More recently, in 2025, the reported the detection of the 44^{44}Sc emission line at 4.09 keV in the central region of at ~3σ significance, further validating the 44^{44}Ti models. Laboratory production of 44^{44}Ti occurs through nuclear reactions such as 48^{48}Ca(p,α\alpha)44^{44}Ti or 49^{49}Ti(γ\gamma,n)44^{44}Ti in particle accelerators, achieving yields on the order of 101010^{10} atoms per irradiation. These methods enable the study of 44^{44}Ti for applications in generators and experiments.

Titanium-48

Titanium-48 (⁴⁸Ti) is the most abundant isotope of , constituting approximately 73.72% of naturally occurring . Its is 47.947947 u, and as an even-even nucleus with 22 protons and 26 neutrons, it possesses a nuclear spin of 0⁺, contributing to its exceptional stability. Due to this high natural abundance and stability, ⁴⁸Ti serves as a primary reference isotope in for analysis, enabling precise normalization of isotopic ratios in geological and material science studies. In terms of nuclear properties, ⁴⁸Ti exhibits a high total of approximately 418.7 MeV, corresponding to an average per of about 8.723 MeV, which underscores its role as one of the most tightly bound isotopes in the titanium series. This isotope is primarily produced through silicon burning processes in massive stars, where explosive in the silicon-burning phase generates significant yields of ⁴⁸Ti during the late stages of . Enriched forms of ⁴⁸Ti, with purities exceeding 99%, are commercially available in metallic powder or oxide forms, facilitating specialized applications. Notably, highly enriched ⁴⁸Ti targets are used in the production of vanadium-48 (⁴⁸V) through neutron capture reactions (⁴⁸Ti(n,γ)⁴⁸V), yielding a positron-emitting radionuclide with a half-life of 15.97 days suitable for positron emission tomography (PET) imaging in medical diagnostics. As an even-even nucleus, ⁴⁸Ti experiences minimal mass-dependent isotopic in geochemical processes, owing to its symmetric nuclear structure and lack of odd-nucleon effects that could enhance separation in or equilibrium reactions. This stability ensures that ⁴⁸Ti remains a consistent component in Earth's geochemical cycles, with negligible variations in natural samples beyond those induced by planetary formation processes.

Titanium-50

Titanium-50 (⁵⁰Ti) is the heaviest stable of , with a natural abundance of 5.18%. Its is 49.944791(2) u, and as an even-even nucleus (22 protons and 28 neutrons), it possesses a nuclear spin of 0⁺. The per in ⁵⁰Ti is approximately 8.756 MeV, reflecting the slight odd-even staggering characteristic of the titanium isotopic chain, where even-even isotopes like ⁵⁰Ti exhibit enhanced stability relative to adjacent odd-mass neighbors due to effects. Given its low natural yield compared to the dominant ⁴⁸Ti isotope (73.72% abundance), ⁵⁰Ti is typically produced and enriched to levels exceeding 99% purity using techniques such as gas centrifugation of titanium compounds or laser isotope separation methods. These processes exploit differences in mass or spectroscopic properties to separate , enabling the production of high-purity material in forms like metal powder or crystal bars for specialized uses. In , enriched ⁵⁰Ti plays a key role as a in hot fusion reactions aimed at synthesizing superheavy elements, particularly at facilities like the GSI Helmholtz Centre for Heavy Ion Research. For instance, intense ⁵⁰Ti beams have been accelerated to fuse with heavy targets such as lead or , probing pathways to elements with atomic numbers beyond 118 and exploring the predicted . Geochemically, ⁵⁰Ti shows enrichments in calcium-aluminum-rich inclusions (CAIs) within primitive carbonaceous chondrites, which formed as the first solids to condense from the solar nebula around 4.567 billion years ago. These anomalies indicate inheritance from presolar nucleosynthetic processes and provide evidence for the high-temperature conditions and early compositional gradients in the .

Applications and significance

Astrophysical and cosmochemical roles

Titanium isotopes play a crucial role in tracing nucleosynthetic processes in stellar environments. The stable isotopes of titanium, such as ⁴⁶Ti, ⁴⁷Ti, ⁴⁸Ti, ⁴⁹Ti, and ⁵⁰Ti, are primarily synthesized during the hydrostatic oxygen and silicon burning stages in the cores of massive stars, where nuclear reactions build heavier nuclei from lighter elements like carbon and oxygen. These processes occur in the late evolutionary phases of stars with initial masses exceeding 8 solar masses, contributing significantly to the solar system's titanium inventory through subsequent supernova explosions that eject the material into the interstellar medium. In contrast, the radioactive isotope ⁴⁴Ti is produced via the alpha-process during explosive nucleosynthesis in core-collapse supernovae, particularly in the alpha-rich freezeout phase following the collapse, where high temperatures and neutron-poor conditions favor the buildup of proton-rich nuclei from nuclear statistical equilibrium. In cosmochemistry, titanium isotope ratios serve as powerful tracers of heterogeneity in the early solar nebula, reflecting inherited nucleosynthetic variations from . Measurements of ratios such as ⁴⁶Ti/⁴⁷Ti and ⁵⁰Ti/⁴⁷Ti reveal systematic differences between carbonaceous chondrites, which formed beyond approximately 2.5 AU, and non-carbonaceous meteorites from the inner solar system, including ordinary chondrites, eucrites, and samples from , , and Mars; carbonaceous materials show enrichments in ⁴⁶Ti and ⁵⁰Ti relative to ⁴⁷Ti, indicating a radial isotopic established during solar system formation. (Fractionated with Unknown Nuclear) anomalies in primitive meteorites, particularly in calcium-aluminum-rich inclusions (CAIs), exhibit extreme deviations in titanium isotopes—up to ±40‰ in ⁵⁰Ti/⁴⁷Ti—arising from incomplete mixing of distinct nucleosynthetic components, such as those from stars or supernovae, and highlighting small-scale isotopic diversity on the order of millimeters in the . The decay of ⁴⁴Ti provides a direct probe for dating young remnants through its gamma-ray emission lines at 1157 keV and associated lines from daughter products. With a of about 60 years, the observed from ⁴⁴Ti decay allows estimation of the remnant's age by modeling the initial production and exponential decline; for instance, /SPI and observations of yield a ⁴⁴Ti mass of (1.4 ± 0.2) × 10⁻⁴ M⊙, consistent with an explosion age of approximately 340 years. In stellar , titanium absorption lines in the optical spectra of cool stars reveal abundance patterns that track galactic chemical evolution. , as an alpha-element, shows enhancements relative to iron ([Ti/Fe] > 0) in metal-poor stars formed from gas enriched by core-collapse supernovae, but absolute titanium abundances decrease with decreasing metallicity ([Ti/H] < 0 for [Fe/H] < -2). In very metal-poor giants, neutral titanium (Ti I) lines yield abundances 0.3–0.5 dex lower than ionized titanium (Ti II) lines due to non-local effects, such as over-ionization in the low-density atmospheres, necessitating corrections to accurately determine depletions and variations across populations.

Industrial and research uses

Enrichment of stable isotopes, such as ⁴⁶Ti through ⁵⁰Ti, is achieved primarily through and methods, enabling production to purities exceeding 99.9% atomic percent. These techniques are employed by specialized facilities to supply isotopically tailored materials for various applications, with natural abundances influencing the cost and feasibility of enrichment—higher-abundance isotopes like ⁴⁸Ti (73.7%) being less expensive to process than rarer ones like ⁵⁰Ti (5.2%). In medical applications, enriched ⁴⁸Ti serves as a target material for cyclotron production of ⁴⁸V via the ⁴⁸Ti(p,n)⁴⁸V reaction, yielding the positron-emitting isotope used in PET imaging for cancer detection and monitoring. This approach enhances production efficiency compared to natural targets, supporting the development of ⁴⁸V-labeled compounds like VO(acac)₂ as novel radiotracers for tumor uptake visualization. Stable titanium isotopes also function as tracers in biological studies, for instance, ⁴⁹Ti to assess the and of nanoparticles in environmental and organismal contexts, such as uptake in aquatic species. Enriched ⁵⁰Ti has been proposed for incorporation into to tailor nuclear properties, reducing products and improving for structural components in fusion reactors. In geochemical applications, ratios like ⁴⁷Ti/⁴⁹Ti serve as tracers for and environmental processes, enabling monitoring of , , and transport in systems. Research on titanium isotopes includes searches for neutrinoless double beta decay, where ⁴⁸Ti appears as the daughter nucleus in ⁴⁸Ca decays, with experiments setting half-life limits exceeding 10²² years and no evidence observed. Additionally, precise measurements of neutron cross-sections for titanium isotopes, including (n,2n), (n,p), and (n,α) reactions, inform the design of nuclear reactors by predicting material behavior under neutron irradiation.

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