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Titanium dioxide

Titanium dioxide
Titanium(IV) oxide
The unit cell of rutile
IUPAC names
Titanium dioxide
Titanium(IV) oxide
Other names
ChemSpider  Y
Jmol-3D images Image
RTECS number XR2775000
Molar mass 79.866 g/mol
Appearance White solid
Odor odorless
Density 4.23 g/cm3 (Rutile)

3.78 g/cm3 (Anatase)

Melting point 1,843 °C (3,349 °F; 2,116 K)
Boiling point 2,972 °C (5,382 °F; 3,245 K)
Band gap 3.05 eV (rutile)[1]
2.488 (anatase)
2.583 (brookite)
2.609 (rutile)
50 J·mol−1·K−1[2]
−945 kJ·mol−1[2]
Safety data sheet ICSC 0338
Not listed
NFPA 704
Flash point Non-flammable
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 15 mg/m3[3]
REL (Recommended)
Ca [5000 mg/m3][3]
Related compounds
Other cations
Zirconium dioxide
Hafnium dioxide
Related titanium oxides
Titanium(II) oxide
Titanium(III) oxide
Titanium(III,IV) oxide
Related compounds
Titanic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 N  (: Y/N?)

Titanium dioxide, also known as titanium(IV) oxide or titania, is the naturally occurring oxide of titanium, chemical formula TiO
. When used as a pigment, it is called titanium white, Pigment White 6 (PW6), or CI 77891. Generally it is sourced from ilmenite, rutile and anatase. It has a wide range of applications, from paint to sunscreen to food colouring. When used as a food colouring, it has E number E171.


  • Occurrence 1
  • Production 2
    • Nanotubes 2.1
  • Applications 3
    • Pigment 3.1
      • Sunscreen and UV blocking pigments in the industry 3.1.1
    • Photocatalyst 3.2
    • Other applications 3.3
  • Health and safety 4
  • See also 5
  • References 6
  • External links 7


Titanium dioxide occurs in nature as the well-known minerals rutile, anatase and brookite, and additionally as two high pressure forms, a monoclinic baddeleyite-like form and an orthorhombic α-PbO2-like form, both found recently at the Ries crater in Bavaria.[4][5] It is mainly sourced from ilmenite ore. This is the most widespread form of titanium dioxide-bearing ore around the world. Rutile is the next most abundant and contains around 98% titanium dioxide in the ore. The metastable anatase and brookite phases convert irreversibly to the equilibrium rutile phase upon heating above temperatures in the range 600–800 °C (1,112–1,472 °F).[6]

Titanium dioxide has eight modifications – in addition to rutile, anatase, and brookite, three metastable phases can be produced synthetically (monoclinic, tetragonal and orthorombic), and five high-pressure forms (α-PbO2-like, baddeleyite-like, cotunnite-like, orthorhombic OI, and cubic phases) also exist:

Form Crystal system Synthesis
rutile tetragonal
anatase tetragonal
brookite orthorhombic
TiO2(B)[7] monoclinic Hydrolysis of K2Ti4O9 followed by heating
TiO2(H), hollandite-like form[8] tetragonal Oxidation of the related potassium titanate bronze, K0.25TiO2
TiO2(R), ramsdellite-like form[9] orthorhombic Oxidation of the related lithium titanate bronze Li0.5TiO2
TiO2(II)-(α-PbO2-like form)[10] orthorhombic
baddeleyite-like form, (7 coordinated Ti)[11] monoclinic
TiO2 -OI[12] orthorhombic
cubic form[13] cubic P > 40 GPa, T > 1600 °C
TiO2 -OII, cotunnite(PbCl2)-like[14] orthorhombic P > 40 GPa, T > 700 °C

The cotunnite-type phase was claimed by L. Dubrovinsky and co-authors to be the hardest known oxide with the Vickers hardness of 38 GPa and the bulk modulus of 431 GPa (i.e. close to diamond's value of 446 GPa) at atmospheric pressure.[14] However, later studies came to different conclusions with much lower values for both the hardness (7–20 GPa, which makes it softer than common oxides like corundum Al2O3 and rutile TiO2)[15] and bulk modulus (~300 GPa).[16][17]

The oxides are commercially important ores of titanium. The metal can also be mined from other minerals such as ilmenite or leucoxene ores, or one of the purest forms, rutile beach sand. Star sapphires and rubies get their asterism from rutile impurities present in them.[18]

Titanium dioxide (B) is found as a mineral in magmatic rocks and hydrothermal veins, as well as weathering rims on perovskite. TiO2 also forms lamellae in other minerals.[19]

Spectral lines from titanium oxide are prominent in class M stars, which are cool enough to allow molecules of this chemical to form.


The production method depends on the feedstock. The most common method for the production of titanium dioxide utilizes the mineral ilmenite. Ilmenite is mixed with sulfuric acid. This reacts to remove the iron oxide group in the ilmenite. The by-product iron(II) sulfate is crystallized and filtered-off to yield only the titanium salt in the digestion solution. This product is called synthetic rutile. This is further processed in a similar way to rutile to give the titanium dioxide product. Synthetic rutile and titanium slags are made especially for titanium dioxide production.[20] The use of ilminite ore usually only produces pigment grade titanium dioxide. Another method for the production of synthetic rutile from ilmenite utilizes the Becher Process.

Rutile is the second most abundant mineral sand. Rutile found in primary rock cannot be extracted hence the deposits containing rutile sand can be mined meaning a reduced availability to the high concentration ore. Crude titanium dioxide (in the form of rutile or synthetic rutile) is purified via converting to titanium tetrachloride in the chloride process. In this process, the crude ore (containing at least 70% TiO2) is reduced with carbon, oxidized with chlorine to give titanium tetrachloride; i.e., carbothermal chlorination. This titanium tetrachloride is distilled, and re-oxidized in a pure oxygen flame or plasma at 1500–2000 K to give pure titanium dioxide while also regenerating chlorine.[21] Aluminium chloride is often added to the process as a rutile promotor; the product is mostly anatase in its absence. The preferred raw material for the chloride process is natural rutile because of its high titanium dioxide content.[22]

One method for the production of titanium dioxide with relevance to nanotechnology is solvothermal Synthesis of titanium dioxide.

Titanium oxide nanotubes, SEM image.


Anatase can be converted by

  • International Chemical Safety Card 0338
  • "2"Nano-Oxides, Inc. – Nano Powders, LEGIT information on Titanium Dioxide TiO (PDF). Retrieved November 2008. 
  • NIOSH Pocket Guide to Chemical Hazards
  • Distributor in China Interview with Chairman Yang Tao by ICOAT.CC.2The Largest TiO
  • , 30 July"Fresh doubt over America map",
  • Titanium Dioxide Classified as Possibly Carcinogenic to Humans, 2007 (if inhaled as a powder)
  • photocatalysis2A description of TiO
  • 2Crystal structures of the three forms of TiO
  • , November 22, 2006International Herald Tribune"Architecture in Italy goes green", Elisabetta Povoledo,
  • , November 8,"A Concrete Step Toward Cleaner Air", Bruno Giussani,
  • "Titanium Dioxide Classified as Possibly Carcinogenic to Humans", Canadian Centre for Occupational Health and Safety, August, 2006
  • Sunscreen in the Sky? Reflective Particles May Combat Warming
  • Titanium and titanium dioxide production data (US and World)

External links

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  2. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23.  
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  4. ^ El, Goresy; Chen, M; Dubrovinsky, L; Gillet, P; Graup, G (2001). "An ultradense polymorph of rutile with seven-coordinated titanium from the Ries crater.". Science 293 (5534): 1467–70.  
  5. ^ El Goresy, Ahmed; Chen, Ming; Gillet, Philippe; Dubrovinsky, Leonid; Graup, GüNther; Ahuja, Rajeev (2001). "A natural shock-induced dense polymorph of rutile with α-PbO2 structure in the suevite from the Ries crater in Germany". Earth and Planetary Science Letters 192 (4): 485.  
  6. ^  
  7. ^ Marchand R., Brohan L., Tournoux M. (1980). "A new form of titanium dioxide and the potassium octatitanate K2Ti8O17". Materials Research Bulletin 15 (8): 1129–1133.  
  8. ^ Latroche, M; Brohan, L; Marchand, R; Tournoux, (1989). "New hollandite oxides: TiO2(H) and K0.06TiO2". Journal of Solid State Chemistry 81 (1): 78–82.  
  9. ^ Akimoto, J.; Gotoh, Y.; Oosawa, Y.; Nonose, N.; Kumagai, T.; Aoki, K.; Takei, H. (1994). "Topotactic Oxidation of Ramsdellite-Type Li0.5TiO2, a New Polymorph of Titanium Dioxide: TiO2(R)". Journal of Solid State Chemistry 113 (1): 27–36.  
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  12. ^ Dubrovinskaia N A, Dubrovinsky L S., Ahuja R, Prokopenko V B., Dmitriev V., Weber H.-P., Osorio-Guillen J. M., Johansson B (2001). "Experimental and Theoretical Identification of a New High-Pressure TiO2 Polymorph". Phys. Rev. Lett. 87 (27 Pt 1): 275501.  
  13. ^ Mattesini M, de Almeida J. S., Dubrovinsky L., Dubrovinskaia L, Johansson B., Ahuja R. (2004). "High-pressure and high-temperature synthesis of the  
  14. ^ a b Dubrovinsky, LS; Dubrovinskaia, NA; Swamy, V; Muscat, J; Harrison, NM; Ahuja, R; Holm, B; Johansson, B (2001). "Materials science: The hardest known oxide". Nature 410 (6829): 653–654.  
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  16. ^ Al-Khatatbeh, Y.; Lee, K. K. M. and Kiefer, B. (2009). "High-pressure behavior of TiO2 as determined by experiment and theory". Phys. Rev. B 79 (13): 134114.  
  17. ^ Nishio-Hamane D., Shimizu A., Nakahira R., Niwa K., Sano-Furukawa A., Okada T., Yagi T., Kikegawa T. (2010). "The stability and equation of state for the cotunnite phase of TiO2 up to 70 GPa". Phys. Chem. Minerals 37 (3): 129–136.  
  18. ^ Emsley, John (2001). Nature's Building Blocks: An A–Z Guide to the Elements. Oxford:  
  19. ^ Banfield, J. F., Veblen, D. R., and Smith, D. J. (1991). (B) by structure determination using high-resolution electron microscopy, image simulation, and distance–least–squares refinement"2"The identification of naturally occurring TiO (PDF). American Mineralogist 76: 343. 
  20. ^ Winkler, Jochen (2003). Titanium Dioxide. Hannover: Vincentz Network. pp.  30–31.  
  21. ^ "Titanium Dioxide Manufacturing Processes". Millennium Inorganic Chemicals. Archived from the original on 14 August 2007. Retrieved 5 September 2007. 
  22. ^ Winkler, Jochen (2003). Titanium Dioxide. Hannover: Vincentz Network. p. 32.  
  23. ^ Mogilevsky, Gregory; Chen, Qiang; Kleinhammes, Alfred; Wu, Yue (2008). "The structure of multilayered titania nanotubes based on delaminated anatase". Chemical Physics Letters 460 (4–6): 517–520.  
  24. ^ Armstrong, Graham; Armstrong, A. Robert; Canales, Jesús and Bruce, Peter G. (2005). "Nanotubes with the TiO2-B structure". Chemical Communications (19): 2454–6.  
  25. ^ Gong, Dawei; Grimes, Craig A.; Varghese, Oomman K.; Hu, Wenchong; Singh, R. S.; Chen, Zhi; Dickey, Elizabeth C. (2001). "Titanium oxide nanotube arrays prepared by anodic oxidation". Journal of Materials Research 16 (12): 3331.  
  26. ^ a b Wang, Cui. "Hard-templating of chiral TiO2 nanofibres with electron transition-based optical activity". Science and Technology of Advanced Materials 16 (5): 054206.  
  27. ^ "Market Study: Titanium Dioxide". Ceresana. Retrieved 21 May 2013. 
  28. ^ a b Winkler, Jochen (2003). Titanium Dioxide. Hannover: Vincentz Network. pp.  5.  
  29. ^ Koleske, J. V. (1995). Paint and Coating Testing Manual. ASTM International. p. 232.  
  30. ^ Koleske, J. V. (1995). Paint and Coating Testing Manual. ASTM International. p. 229.  
  31. ^ Pearlescence with Iriodin.
  32. ^ Phillips, Lance G. and Barbano, David M. (1997). "The Influence of Fat Substitutes Based on Protein and Titanium Dioxide on the Sensory Properties of Lowfat Milk". Journal of Dairy Science 80 (11): 2726.  
  33. ^ Les, Caren B. (November 2008) Light spells doom for bacteria.
  34. ^ 2Polymers, Light and the Science of TiO, DuPont, pp. 1–2
  35. ^ Fibre Cement Coating.
  36. ^ Kurtoglu M. E., Longenbach T., Gogotsi Y. (2011). "Preventing Sodium Poisoning of Photocatalytic TiO2 Films on Glass by Metal Doping". International Journal of Applied Glass Science 2 (2): 108–116.  
  37. ^ a b c "Discovery and applications of photocatalysis — Creating a comfortable future by making use of light energy". Japan Nanonet Bulletin Issue 44, 12 May 2005.
  38. ^ Fujishima, Akira; Honda, Kenichi (1972). "Electrochemical Photolysis of Water at a Semiconductor Electrode". Nature 238 (5358): 37–8.  
  39. ^ "Carbon-doped titanium dioxide is an effective photocatalyst". Advanced Ceramics Report. 1 December 2003. This carbon-doped titanium dioxide is highly efficient; under artificial visible light, it breaks down chlorophenol five times more efficiently than the nitrogen-doped version. 
  40. ^ Cheap, Clean Ways to Produce Hydrogen for Use in Fuel Cells? A Dash of Disorder Yields a Very Efficient Photocatalyst. Sciencedaily (28 January 2011)
  41. ^ Advanced Concrete Pavement materials, National Concrete Pavement Technology Center, Iowa State University, p. 435.
  42. ^ Hogan, Jenny (4 February 2004) "Smog-busting paint soaks up noxious gases". New Scientist.
  43. ^ TIME's Best Inventions of 2008. (31 October 2008).
  44. ^ Winkler, Jochen (2003). Titanium Dioxide. Hannover: Vincentz Network. pp.  115–116.  
  45. ^ Konstantinou, Ioannis K; Albanis, Triantafyllos A (2004). "TiO2-assisted photocatalytic degradation of azo dyes in aqueous solution: Kinetic and mechanistic investigations". Applied Catalysis B: Environmental 49: 1.  
  46. ^ Hanaor, Dorian A. H.; Sorrell, Charles C. (2014). "Sand Supported Mixed-Phase TiO2 Photocatalysts for Water Decontamination Applications". Advanced Engineering Materials 16 (2): 248–254.  
  47. ^ Jones, BJ; Vergne, MJ; Bunk, DM; Locascio, LE; Hayes, MA (2007). "Cleavage of Peptides and Proteins Using Light-Generated Radicals from Titanium Dioxide".  
  48. ^ Lewis, Nathan. "2"Nanocrystalline TiO. Research. California Institute of Technology. Retrieved 9 October 2009. 
  49. ^ Earle, M. D. (1942). "The Electrical Conductivity of Titanium Dioxide".  
  50. ^ Paschotta, Rüdiger. "Bragg Mirrors". Encyclopedia of Laser Physics and Technology. RP Photonics. Retrieved 1 May 2009. 
  51. ^ Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press.  
  52. ^ Occupational Health Services, Inc. (31 May 1988). "Hazardline" (Electronic Bulletin). New York: Occupational Health Services, Inc. 
  53. ^ Sax, N.I.; Lewis, Richard J., Sr. (2000). Dangerous Properties of Industrial Materials III (10th ed.). New York: Van Nostrand Reinhold. p. 3279.  
  54. ^ "Nano-tech sunscreen presents potential health risk". ABC News. 18 December 2008. Retrieved 12 April 2010. 
  55. ^ Sadrieh N, Wokovich AM, Gopee NV; et al. (May 2010). particles"2"Lack of significant dermal penetration of titanium dioxide from sunscreen formulations containing nano- and submicron-size TiO. Toxicol. Sci. 115 (1): 156–66.  
  56. ^ "Nano World: Nanoparticle toxicity tests". 5 April 2006. Retrieved 12 April 2010. 
  57. ^ Shaw T, Simpson B, Wilson B, Oostman H, Rainey D, Storrs F (August 2010). "True photoallergy to sunscreens is rare despite popular belief". Dermatitis 21 (4): 185–98.  
  58. ^ "Titanium dioxide" (PDF) 93. International Agency for Research on Cancer. 2006. 
  59. ^ Serpone, Nick; Kutal, Charles (1993). Photosensitive metal-organic systems: mechanistic principles and applications. Columbus, OH: American Chemical Society.  
  60. ^ "Suncream may be linked to Alzheimer's disease, say experts". Daily Mail (London). 24 August 2009. Retrieved 25 August 2009. 
  61. ^ "Nanoparticles Used in Common Household Items Cause Genetic Damage in Mice". 17 November 2009. Retrieved 17 November 2009. 
  62. ^ Yazdi AS, Guarda G, Riteau N; et al. (November 2010). "Nanoparticles activate the NLR pyrin domain containing 3 (Nlrp3) inflammasome and cause pulmonary inflammation through release of IL-1α and IL-1β". Proc. Natl. Acad. Sci. U.S.A. 107 (45): 19449–54.  
  63. ^ Zhu Y, Eaton JW, Li C (2012). "Titanium Dioxide (TiO(2)) Nanoparticles Preferentially Induce Cell Death in Transformed Cells in a Bak/Bax-Independent Fashion". PLoS ONE 7 (11): e50607.  
  64. ^ National Institute for Occupational Safety and Health. "Current Intelligence Bulletin 63: Occupational Exposure to Titanium Dioxide (NIOSH Publication No. 2011-160)" (PDF). National Institute for Occupational Safety and Health. 
  65. ^ Berglund F, Carlmark B (October 2011). "Titanium, sinusitis, and the yellow nail syndrome". Biol Trace Elem Res 143 (1): 1–7.  
  66. ^ "Dunkin' Donuts to remove titanium dioxide from donuts". CNN Money. March 2015. 
  67. ^ "Dunkin' Donuts Nixing Controversial Ingredient From Its Doughnuts". Eater. March 2015. 
  68. ^ "Dunkin' to stop using whitening agent". USA TODAY. March 2015. 
  69. ^ Dunkin' Donuts ditches titanium dioxide – but is it actually harmful? The Conversation. March 12, 2015


See also

Dunkin' Donuts in the United States is dropping titanium dioxide from its powdered sugar donuts after public pressure.[66][67][68] However, Andrew Maynard, director of Risk Science Centre at the University of Michigan disregarded extreme danger from use of titanium dioxide in food. He says that the titanium dioxide used by Dunkin’ Brands and many other food producers is not a new material, and it is not a nanomaterial either. Nanoparticles are typically smaller than 100 nanometers in diameter. Yet most of the particles in food grade titanium dioxide are much larger.[69]

There is some evidence the rare disease yellow nail syndrome may be caused by titanium, either implanted for medical reasons or through eating various foods containing titanium dioxide.[65]

The body of research regarding the carcinogenicity of different particle sizes of titanium dioxide has led the US National Institute for Occupational Safety and Health to recommend two separate exposure limits. NIOSH recommends that fine TiO
particles be set at an exposure limit of 2.4 mg/m3, while ultrafine TiO
be set at an exposure limit of 0.3 mg/m3, as time-weighted average concentrations up to 10 hours a day for a 40-hour work week.[64] These recommendations reflect the findings in the research literature that show smaller titanium dioxide particles are more likely to pose carcinogenic risk than the larger titanium dioxide particles.

[63] signalling pathways.apoptotic, independently of the known compartment lysosomal nanoparticles and the TiO
results from the interaction between TiO
due to cytotoxicity may cause cancer is unclear. Molecular research suggests that cell TiO
The mechanism by which [62][61] Studies have also found that titanium dioxide nanoparticles cause inflammatory response and genetic damage in mice.[60] Titanium dioxide dust, when inhaled, has been classified by the

Many sunscreens use nanoparticle titanium dioxide (along with nanoparticle zinc oxide) which, despite reports of potential health risks,[54] is not actually absorbed through the skin.[55] Other effects of titanium dioxide nanoparticles on human health are not well understood.[56] Nevertheless, allergy to topical application has been confirmed.[57]

Titanium dioxide accounts for 70% of the total production volume of pigments worldwide. It is widely used to provide whiteness and opacity to products such as paints, plastics, papers, inks, foods, and toothpastes. It is also used in cosmetic and skin care products, and it is present in almost every sunblock, where it helps protect the skin from ultraviolet light.

Titanium dioxide is incompatible with strong reducing agents and strong acids.[52] Violent or incandescent reactions occur with molten metals that are very electropositive, e.g. aluminium, calcium, magnesium, potassium, sodium, zinc and lithium.[53]

Health and safety

Synthetic single crystals of TiO2, ca. 2–3 mm in size, cut from a larger plate.

Other applications

  1. The process uses natural oxygen and sunlight and thus occurs under ambient conditions; it is wavelength selective and is accelerated by UV light.
  2. The photocatalyst is inexpensive, readily available, non-toxic, chemically and mechanically stable, and has a high turnover.
  3. The formation of photocyclized intermediate products, unlike direct photolysis techniques, is avoided.
  4. Oxidation of the substrates to CO2 is complete.
  5. TiO2 can be supported as thin films on suitable reactor substrates, which can be readily separated from treated water.[46]

Attempts have been made to photocatalytically mineralize pollutants (to convert into CO2 and H2O) in waste water.[44] TiO2 offers great potential as an industrial technology for detoxification or remediation of wastewater due to several factors:[45]

A photocatalytic cement that uses titanium dioxide as a primary component, produced by Italcementi Group, was included in Time's Top 50 Inventions of 2008.[43]

TiO2 incorporated into outdoor building materials, such as paving stones in nitrogen oxides.[42]

In 1995 Fujishima and his group discovered the superhydrophilicity phenomenon for titanium dioxide coated glass exposed to sun light.[37] This resulted in the development of self-cleaning glass and anti-fogging coatings.

The photocatalytic properties of titanium dioxide were discovered by Akira Fujishima in 1967[37] and published in 1972.[38] The process on the surface of the titanium dioxide was called the Honda-Fujishima effect (本多-藤嶋効果).[37] Titanium dioxide, in thin film and nanoparticle form has potential for use in energy production: as a photocatalyst, it can carry out hydrolysis; i.e., break water into hydrogen and oxygen. With the hydrogen collected, it could be used as a fuel. The efficiency of this process can be greatly improved by doping the oxide with carbon.[39] Further efficiency and durability has been obtained by introducing disorder to the lattice structure of the surface layer of titanium dioxide nanocrystals, permitting infrared absorption.[40]

Titanium dioxide, particularly in the anatase form, is a hydrolysis catalyst. It is also used in dye-sensitized solar cells, which are a type of chemical solar cell (also known as a Graetzel cell).

TiO2 fibers and spirals.


This pigment is used extensively in plastics and other applications not only as a white pigment or an opacifier but also for its UV resistant properties where the powder disperses the light – unlike organic UV absorbers – and reduces UV damage, due mostly to the extremely high refractive index of the particles.[34] Certain polymers used in coatings for concrete[35] or those used to impregnate concrete as a reinforcement are sometimes charged with titanium white pigment for UV shielding in the construction industry, but it only delays the oxidative photodegradation of the polymer in question, which is said to "chalk" as it flakes off due to lowered impact strength and may crumble after years of exposure in direct sunlight if UV stabilizers have not been included.

Titanium dioxide is found in the majority of physical sunscreens because of its high refractive index, its strong UV light absorbing capabilities and its resistance to discolouration under ultraviolet light. This advantage enhances its stability and ability to protect the skin from ultraviolet light. Nano-scaled titanium dioxide particles are primarily used in sun screen lotion because they scatter visible light less than titanium dioxide pigments while still providing UV protection.[28] Sunscreens designed for infants or people with sensitive skin are often based on titanium dioxide and/or zinc oxide, as these mineral UV blockers are believed to cause less skin irritation than other UV absorbing chemicals.

In cosmetic and skin care products, titanium dioxide is used as a pigment, sunscreen and a thickener. It is also used as a tattoo pigment and in styptic pencils. Titanium dioxide is produced in varying particle sizes, oil and water dispersible, and in certain grades for the cosmetic industry.

Sunscreen and UV blocking pigments in the industry

The exterior of the Saturn V rocket was painted with titanium dioxide; this later allowed astronomers to determine that J002E3 was the S-IVB stage from Apollo 12 and not an asteroid.

Titanium dioxide is used to mark the white lines of some tennis courts.[33]

Titanium dioxide has been shown statistically to increase skimmed milk's whiteness, increasing skimmed milk's sensory acceptance score.[32]

In ceramic glazes titanium dioxide acts as an opacifier and seeds crystal formation.

Titanium dioxide is the most widely used white pigment because of its brightness and very high refractive index, in which it is surpassed only by a few other materials. Approximately 4.6 million tons of pigmentary TiO2 are used annually worldwide, and this number is expected to increase as utilization continues to rise.[28] When deposited as a thin film, its refractive index and colour make it an excellent reflective optical coating for dielectric mirrors and some gemstones like "mystic fire topaz". TiO2 is also an effective opacifier in powder form, where it is employed as a pigment to provide whiteness and opacity to products such as paints, coatings, plastics, papers, inks, foods, medicines (i.e. pills and tablets) as well as most toothpastes. In paint, it is often referred to offhandedly as "the perfect white", "the whitest white", or other similar terms. Opacity is improved by optimal sizing of the titanium dioxide particles. Some grades of titanium based pigments as used in sparkly paints, plastics, finishes and pearlescent cosmetics are man-made pigments whose particles have two or more layers of various oxides – often titanium dioxide, iron oxide or alumina – in order to have glittering, iridescent and or pearlescent effects similar to crushed mica or guanine-based products. In addition to these effects a limited colour change is possible in certain formulations depending on how and at which angle the finished product is illuminated and the thickness of the oxide layer in the pigment particle; one or more colours appear by reflection while the other tones appear due to interference of the transparent titanium dioxide layers.[29] In some products, the layer of titanium dioxide is grown in conjunction with iron oxide by calcination of titanium salts (sulfates, chlorates) around 800 °C[30] or other industrial deposition methods such as chemical vapour deposition on substrates such as mica platelets or even silicon dioxide crystal platelets of no more than 50 µm in diameter.[31] The iridescent effect in these titanium oxide particles (which are only partly natural) is unlike the opaque effect obtained with usual ground titanium oxide pigment obtained by mining, in which case only a certain diameter of the particle is considered and the effect is due only to scattering.


The most important application areas are paints and varnishes as well as paper and plastics, which account for about 80% of the world's titanium dioxide consumption. Other pigment applications such as printing inks, fibers, rubber, cosmetic products and foodstuffs account for another 8%. The rest is used in other applications, for instance the production of technical pure titanium, glass and glass ceramics, electrical ceramics, catalysts, electric conductors and chemical intermediates.[27] It also is in most red-coloured candy.


[26] nanofibers can be also prepared by coating 2 Hollow TiO

SEM (top) and TEM (bottom) images of chiral TiO2 nanofibers.[26]

Another process for synthesizing TiO
nanotubes is through anodization in an electrolytic solution. When anodized in a 0.5 weight percent HF solution for 20 minutes, well-aligned titanium oxide nanotube arrays can be fabricated with an average tube diameter of 60 nm and length of 250 nm. Based on X-ray Diffraction, nanotubes grown through anodization are amorphous.[25]

[24]. A higher reaction temperature (170 °C) and less reaction volume gives the corresponding nanowires.μm and an inner diameter of 5 to 8 nm and have a length of 1 nm and heated at 400 °C for another 15 hours. The yield of nanotubes is quantitative and the tubes have an outer diameter of 10 to 20 hydrochloric acid and heated at 130 °C for 72 hours. The reaction product is washed with dilute sodium hydroxide M. In the synthesis, anatase is mixed with 10 photocatalysts which are of potential interest as catalytic supports and nanoribbons titanate and [23]

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