Solid heterogeneous catalysts such as in automobile catalytic converters are plated on structures designed to maximize their surface area.

A low-temperature oxidation catalyst used to convert carbon monoxide to less toxic carbon dioxide at room temperature. It can also remove formaldehyde from the air.

Catalysis is the change in rate of a chemical reaction due to the participation of a substance called a catalyst. Unlike other reagents that participate in the chemical reaction, a catalyst is not consumed by the reaction itself. A catalyst may participate in multiple chemical transformations. Catalysts that speed the reaction are called positive catalysts. Substances that slow a catalyst's effect in a chemical reaction are called inhibitors. Substances that increase the activity of catalysts are called promoters, and substances that deactivate catalysts are called catalytic poisons.

Catalytic reactions have a lower rate-limiting free energy of activation than the corresponding uncatalyzed reaction, resulting in higher reaction rate at the same temperature. However, the mechanistic explanation of catalysis is complex. Catalysts may affect the reaction environment favorably, or bind to the reagents to polarize bonds, e.g. acid catalysts for reactions of carbonyl compounds, or form specific intermediates that are not produced naturally, such as osmate esters in osmium tetroxide-catalyzed dihydroxylation of alkenes, or cause lysis of reagents to reactive forms, such as atomic hydrogen in catalytic hydrogenation.

Kinetically, catalytic reactions are typical chemical reactions; i.e. the reaction rate depends on the frequency of contact of the reactants in the rate-determining step. Usually, the catalyst participates in this slowest step, and rates are limited by amount of catalyst and its "activity". In heterogeneous catalysis, the diffusion of reagents to the surface and diffusion of products from the surface can be rate determining. A Nanomaterial-based catalyst is an example of a heterogeneous catalyst. Analogous events associated with substrate binding and product dissociation apply to homogeneous catalysts.

Although catalysts are not consumed by the reaction itself, they may be inhibited, deactivated, or destroyed by secondary processes. In heterogeneous catalysis, typical secondary processes include coking where the catalyst becomes covered by polymeric side products. Additionally, heterogeneous catalysts can dissolve into the solution in a solid–liquid system or evaporate in a solid–gas system.

Background[link]

The production of most industrially important chemicals involves catalysis. Similarly, most biochemically significant processes are catalysed. Research into catalysis is a major field in applied science and involves many areas of chemistry, notably in organometallic chemistry and materials science. Catalysis is relevant to many aspects of environmental science, e.g. the catalytic converter in automobiles and the dynamics of the ozone hole. Catalytic reactions are preferred in environmentally friendly green chemistry due to the reduced amount of waste generated,^[1] as opposed to stoichiometric reactions in which all reactants are consumed and more side products are formed. The most common catalyst is the hydrogen ion (H⁺). Many transition metals and transition metal complexes are used in catalysis as well. Catalysts called enzymes are important in biology.

A catalyst works by providing an alternative reaction pathway to the reaction product. The rate of the reaction is increased as this alternative route has a lower activation energy than the reaction route not mediated by the catalyst. The disproportionation of hydrogen peroxide creates water and oxygen, as shown below.

2 H₂O₂ → 2 H₂O + O₂

This reaction is preferable in the sense that the reaction products are more stable than the starting material, though the uncatalysed reaction is slow. In fact, the decomposition of hydrogen peroxide is so slow that hydrogen peroxide solutions are commercially available. This reaction is strongly affected by catalysts such as manganese dioxide, or the enzyme peroxidase in organisms. Upon the addition of a small amount of manganese dioxide, the hydrogen peroxide reacts rapidly. This effect is readily seen by the effervescence of oxygen.^[2] The manganese dioxide is not consumed in the reaction, and thus may be recovered unchanged, and re-used indefinitely. Accordingly, manganese dioxide catalyses this reaction.^[3]

General principles of catalysis[link]

Typical mechanism[link]

Catalysts generally react with one or more reactants to form intermediates that subsequently give the final reaction product, in the process regenerating the catalyst. The following is a typical reaction scheme, where C represents the catalyst, X and Y are reactants, and Z is the product of the reaction of X and Y:

X + C → XC (1)

Y + XC → XYC (2)

XYC → CZ (3)

CZ → C + Z (4)

Although the catalyst is consumed by reaction 1, it is subsequently produced by reaction 4, so for the overall reaction:

X + Y → Z

As a catalyst is regenerated in a reaction, often only small amounts are needed to increase the rate of the reaction. In practice, however, catalysts are sometimes consumed in secondary processes.

As an example of this process, in 2008 Danish researchers first revealed the sequence of events when oxygen and hydrogen combine on the surface of titanium dioxide (TiO₂, or titania) to produce water. With a time-lapse series of scanning tunneling microscopy images, they determined the molecules undergo adsorption, dissociation and diffusion before reacting. The intermediate reaction states were: HO₂, H₂O₂, then H₃O₂ and the final reaction product (water molecule dimers), after which the water molecule desorbs from the catalyst surface.^[4][5]

Catalysis and reaction energetics[link]

Generic potential energy diagram showing the effect of a catalyst in a hypothetical exothermic chemical reaction X + Y to give Z. The presence of the catalyst opens a different reaction pathway (shown in red) with a lower activation energy. The final result and the overall thermodynamics are the same.

Catalysts work by providing an (alternative) mechanism involving a different transition state and lower activation energy. Consequently, more molecular collisions have the energy needed to reach the transition state. Hence, catalysts can enable reactions that would otherwise be blocked or slowed by a kinetic barrier. The catalyst may increase reaction rate or selectivity, or enable the reaction at lower temperatures. This effect can be illustrated with a Boltzmann distribution and energy profile diagram.

In the catalyzed elementary reaction, catalysts do not change the extent of a reaction: they have no effect on the chemical equilibrium of a reaction because the rate of both the forward and the reverse reaction are both affected (see also thermodynamics). The fact that a catalyst does not change the equilibrium is a consequence of the second law of thermodynamics. Suppose there was such a catalyst that shifted an equilibrium. Introducing the catalyst to the system would result in reaction to move to the new equilibrium, producing energy. Production of energy is a necessary result since reactions are spontaneous if and only if Gibbs free energy is produced, and if there is no energy barrier, there is no need for a catalyst. Then, removing the catalyst would also result in reaction, producing energy; i.e. the addition and its reverse process, removal, would both produce energy. Thus, a catalyst that could change the equilibrium would be a perpetual motion machine, a contradiction to the laws of thermodynamics.^[6]

If a catalyst does change the equilibrium, then it must be consumed as the reaction proceeds, and thus it is also a reactant. Illustrative is the base-catalysed hydrolysis of esters, where the produced carboxylic acid immediately reacts with the base catalyst and thus the reaction equilibrium is shifted towards hydrolysis.

The SI derived unit for measuring the catalytic activity of a catalyst is the katal, which is moles per second. The productivity of a catalyst can be described by the turn over number (or TON) and the catalytic activity by the turn over frequency (TOF), which is the TON per time unit. The biochemical equivalent is the enzyme unit. For more information on the efficiency of enzymatic catalysis, see the article on Enzymes.

The catalyst stabilizes the transition state more than it stabilizes the starting material. It decreases the kinetic barrier by decreasing the difference in energy between starting material and transition state. It does not change the energy difference between starting materials and products (thermodynamic barrier), or the available energy (this is provided by the environment as heat or light).

Typical catalytic materials[link]

The chemical nature of catalysts is as diverse as catalysis itself, although some generalizations can be made. Proton acids are probably the most widely used catalysts, especially for the many reactions involving water, including hydrolysis and its reverse. Multifunctional solids often are catalytically active, e.g. zeolites, alumina, higher-order oxides, graphitic carbon, nanoparticles, nanodots, and facets of bulk materials. Transition metals are often used to catalyze redox reactions (oxidation, hydrogenation). Examples are nickel, such as Raney nickel for hydrogenation, and vanadium(V) oxide for oxidation of sulfur dioxide into sulfur trioxide. Many catalytic processes, especially those used in organic synthesis, require so called "late transition metals", which include palladium, platinum, gold, ruthenium, rhodium, and iridium.

Some so-called catalysts are really precatalysts. Precatalysts convert to catalysts in the reaction. For example, Wilkinson's catalyst RhCl(PPh₃)₃ loses one triphenylphosphine ligand before entering the true catalytic cycle. Precatalysts are easier to store but are easily activated in situ. Because of this preactivation step, many catalytic reactions involve an induction period.

Chemical species that improve catalytic activity are called co-catalysts (cocatalysts) or promotors in cooperative catalysis.

Types of catalysis[link]

Catalysts can be either heterogeneous or homogeneous, depending on whether a catalyst exists in the same phase as the substrate. Biocatalysts (enzymes) are often seen as a separate group.

Heterogeneous catalysts[link]

The microporous molecular structure of the zeolite ZSM-5 is exploited in catalysts used in refineries

Zeolites are extruded as pellets for easy handling in catalytic reactors.

Heterogeneous catalysts act in a different phase than the reactants. Most heterogeneous catalysts are solids that act on substrates in a liquid or gaseous reaction mixture. Diverse mechanisms for reactions on surfaces are known, depending on how the adsorption takes place (Langmuir-Hinshelwood, Eley-Rideal, and Mars-van Krevelen).^[7] The total surface area of solid has an important effect on the reaction rate. The smaller the catalyst particle size, the larger the surface area for a given mass of particles.

For example, in the Haber process, finely divided iron serves as a catalyst for the synthesis of ammonia from nitrogen and hydrogen. The reacting gases adsorb onto "active sites" on the iron particles. Once adsorbed, the bonds within the reacting molecules are weakened, and new bonds between the resulting fragments form in part due to their close proximity. In this way the particularly strong triple bond in nitrogen is weakened and the hydrogen and nitrogen atoms combine faster than would be the case in the gas phase, so the rate of reaction increases.^{[citation needed]} Another place where a heterogeneous catalyst is applied is in the contact process (oxidation of sulfur dioxide on vanadium(V) oxide for the production of sulfuric acid).

Heterogeneous catalysts are typically “supported,” which means that the catalyst is dispersed on a second material that enhances the effectiveness or minimizes their cost. Sometimes the support is merely a surface on which the catalyst is spread to increase the surface area. More often, the support and the catalyst interact, affecting the catalytic reaction. Supports are porous materials with a high surface area, most commonly alumina or various kinds of activated carbon. Specialized supports include silicon dioxide, titanium dioxide, calcium carbonate, and barium sulfate.

Homogeneous catalysts[link]

Homogeneous catalysts function in the same phase as the reactants, but the mechanistic principles invoked in heterogeneous catalysis are generally applicable. Typically homogeneous catalysts are dissolved in a solvent with the substrates. One example of homogeneous catalysis involves the influence of H⁺ on the esterification of esters, e.g. methyl acetate from acetic acid and methanol.^[8] For inorganic chemists, homogeneous catalysis is often synonymous with organometallic catalysts.^[9]

Electrocatalysts[link]

In the context of electrochemistry, specifically in fuel cell engineering, various metal-containing catalysts are used to enhance the rates of the half reactions that comprise the fuel cell. One common type of fuel cell electrocatalyst is based upon nanoparticles of platinum that are supported on slightly larger carbon particles. When in contact with one of the electrodes in a fuel cell, this platinum increases the rate of oxygen reduction to water, either to hydroxide or hydrogen peroxide.

Organocatalysis[link]

Whereas transition metals sometimes attract most of the attention in the study of catalysis, small organic molecules without metals can also exhibit catalytic properties, as is apparent from the fact that many enzymes lack transition metals. Typically, organic catalysts require a higher loading (amount of catalyst per unit amount of reactant, expressed in mol% amount of substance) than transition metal(-ion)-based catalysts, but these catalysts are usually commercially available in bulk, helping to reduce costs. In the early 2000s, these organocatalysts were considered "new generation" and are competitive to traditional metal(-ion)-containing catalysts. Organocatalysts are supposed to operate akin to metal-free enzymes utilizing, e.g., non-covalent interactions such as hydrogen bonding. The discipline organocatalysis is divided in the application of covalent (e.g., proline, DMAP) and non-covalent (e.g., thiourea organocatalysis) organocatalysts referring to the preferred catalyst-substrate binding and interaction, respectively.

Significance of catalysis[link]

left: Partially caramelised cube sugar, right: burning cube sugar with ash as catalyst

Estimates are that 90% of all commercially produced chemical products involve catalysts at some stage in the process of their manufacture.^[10] In 2005, catalytic processes generated about $900 billion in products worldwide.^[11] Catalysis is so pervasive that subareas are not readily classified. Some areas of particular concentration are surveyed below.

Energy processing[link]

Petroleum refining makes intensive use of catalysis for alkylation, catalytic cracking (breaking long-chain hydrocarbons into smaller pieces), naphtha reforming and steam reforming (conversion of hydrocarbons into synthesis gas). Even the exhaust from the burning of fossil fuels is treated via catalysis: Catalytic converters, typically composed of platinum and rhodium, break down some of the more harmful byproducts of automobile exhaust.

2 CO + 2 NO → 2 CO₂ + N₂

With regard to synthetic fuels, an old but still important process is the Fischer-Tropsch synthesis of hydrocarbons from synthesis gas, which itself is processed via water-gas shift reactions, catalysed by iron. Biodiesel and related biofuels require processing via both inorganic and biocatalysts.

Fuel cells rely on catalysts for both the anodic and cathodic reactions.

Catalytic heaters generate flameless heat from a supply of combustible fuel.

Bulk chemicals[link]

Some of the largest-scale chemicals are produced via catalytic oxidation, often using oxygen. Examples include nitric acid (from ammonia), sulfuric acid (from sulfur dioxide to sulfur trioxide by the chamber process), terephthalic acid from p-xylene, and acrylonitrile from propane and ammonia.

Many other chemical products are generated by large-scale reduction, often via hydrogenation. The largest-scale example is ammonia, which is prepared via the Haber process from nitrogen. Methanol is prepared from carbon monoxide.

Bulk polymers derived from ethylene and propylene are often prepared via Ziegler-Natta catalysis. Polyesters, polyamides, and isocyanates are derived via acid-base catalysis.

Most carbonylation processes require metal catalysts, examples include the Monsanto acetic acid process and hydroformylation.

Fine chemicals[link]

Many fine chemicals are prepared via catalysis; methods include those of heavy industry as well as more specialized processes that would be prohibitively expensive on a large scale. Examples include olefin metathesis using Grubbs' catalyst, the Heck reaction, and Friedel-Crafts reactions.

Because most bioactive compounds are chiral, many pharmaceuticals are produced by enantioselective catalysis (catalytic asymmetric synthesis).

Food processing[link]

One of the most obvious applications of catalysis is the hydrogenation (reaction with hydrogen gas) of fats using nickel catalyst to produce margarine.^[12] Many other foodstuffs are prepared via biocatalysis (see below).

Biology[link]

In nature, enzymes are catalysts in metabolism and catabolism. Most biocatalysts are protein-based, i.e. enzymes, but other classes of biomolecules also exhibit catalytic properties including ribozymes, and synthetic deoxyribozymes.^[13]

Biocatalysts can be thought of as intermediate between homogenous and heterogeneous catalysts, although strictly speaking soluble enzymes are homogeneous catalysts and membrane-bound enzymes are heterogeneous. Several factors affect the activity of enzymes (and other catalysts) including temperature, pH, concentration of enzyme, substrate, and products. A particularly important reagent in enzymatic reactions is water, which is the product of many bond-forming reactions and a reactant in many bond-breaking processes.

Enzymes are employed to prepare many commodity chemicals including high-fructose corn syrup and acrylamide.

In the environment[link]

Catalysis impacts the environment by increasing the efficiency of industrial processes, but catalysis also plays a direct role in the environment. A notable example is the catalytic role of chlorine free radicals in the breakdown of ozone. These radicals are formed by the action of ultraviolet radiation on chlorofluorocarbons (CFCs).

Cl^· + O₃ → ClO^· + O₂

ClO^· + O^· → Cl^· + O₂

History[link]

In a general sense, anything that increases the rate of a process is a "catalyst", a term derived from Greek καταλύειν, meaning "to annul," or "to untie," or "to pick up." The phrase catalysed processes was coined by Jöns Jakob Berzelius in 1836^[14] to describe reactions that are accelerated by substances that remain unchanged after the reaction. Other early chemists involved in catalysis were Alexander Mitscherlich who referred to contact processes and Johann Wolfgang Döbereiner who spoke of contact action and whose lighter based on hydrogen and a platinum sponge became a huge commercial success in the 1820s. Humphry Davy discovered the use of platinum in catalysis. In the 1880s, Wilhelm Ostwald at Leipzig University started a systematic investigation into reactions that were catalyzed by the presence of acids and bases, and found that chemical reactions occur at finite rates and that these rates can be used to determine the strengths of acids and bases. For this work, Ostwald was awarded the 1909 Nobel Prize in Chemistry.^[15]

Inhibitors, poisons and promoters[link]

Substances that reduce the action of catalysts are called catalyst inhibitors if reversible, and catalyst poisons if irreversible. Promoters are substances that increase the catalytic activity, even though they are not catalysts by themselves.

Inhibitors are sometimes referred to as "negative catalysts" since they decrease the reaction rate.^[16] However the term inhibitor is preferred since they do not work by introducing a reaction path with higher activation energy; this would not reduce the rate since the reaction would continue to occur by the non-catalyzed path. Instead they act either by deactivating catalysts, or by removing reaction intermediates such as free radicals.^[16][17]

The inhibitor may modify selectivity in addition to rate. For instance, in the reduction of ethyne to ethene, the catalyst is palladium (Pd) partly "poisoned" with lead(II) acetate (Pb(CH₃COO)₂). Without the deactivation of the catalyst, the ethene produced will be further reduced to ethane.^[18][19]

The inhibitor can produce this effect by e.g. selectively poisoning only certain types of active sites. Another mechanism is the modification of surface geometry. For instance, in hydrogenation operations, large planes of metal surface function as sites of hydrogenolysis catalysis while sites catalyzing hydrogenation of unsaturates are smaller. Thus, a poison that covers surface randomly will tend to reduce the number of uncontaminated large planes but leave proportionally more smaller sites free, thus changing the hydrogenation vs. hydrogenolysis selectivity. Many other mechanisms are also possible.

Promoters can cover up surface to prevent production of a mat of coke, or even actively remove such material (e.g. rhenium on platinum in platforming). They can aid the dispersion of the catalytic material or bind to reagents.

Current market[link]

The global demand on catalysts in 2010 was estimated at approximately 29.5 billions USD. With the rapid recovery in automotive and chemical industry overall, the global catalyst market is expected to experience fast growth in the next years.^[20]

See also[link]

	Chemistry portal
	Biology portal

• Autocatalysis
• BIG-NSE (Berlin Graduate School of Natural Sciences and Engineering)
• Catalysis Science & Technology (a chemistry journal)
• Environmental triggers
• Enzyme catalysis
• Industrial catalysts
• Kelvin probe force microscope
• Pharmaceutic adjuvant
• Phase Boundary Catalysis
• Phase transfer catalyst
• Photocatalysis
• Ribozyme (RNA Biocatalysis)
• SUMO enzymes
• Temperature-programmed reduction
• Thermal desorption spectroscopy

References[link]

• Nic, M.; Jirat, J.; Kosata, B., eds. (2006–). "catalyst". IUPAC Compendium of Chemical Terminology (Online ed.). DOI:10.1351/goldbook.C00876. ISBN 0-9678550-9-8. http://goldbook.iupac.org/C00876.html. 

1. ^ "The 12 Principles of Green Chemistry". United States Environmental Protection Agency. http://www.epa.gov/sciencematters/june2011/principles.htm. Retrieved 2012-04-30. 
2. ^ "Genie in a Bottle". University of Minnesota. 2005-03-02. http://www.chem.umn.edu/services/lecturedemo/info/genie.htm. 
3. ^ Masel, Richard I. “Chemical Kinetics and Catalysis” Wiley-Interscience, New York, 2001. ISBN 0-471-24197-0.
4. ^ Jacoby, Mitch (16 February 2009). "Making Water Step by Step". Chemical & Engineering News: p. 10. http://pubs.acs.org/cen/news/87/i07/8707notw6.html. 
5. ^ Matthiesen J, Wendt S, Hansen JØ, Madsen GK, Lira E, Galliker P, Vestergaard EK, Schaub R, Laegsgaard E, Hammer B, Besenbacher F (2009). "Observation of All the Intermediate Steps of a Chemical Reaction on an Oxide Surface by Scanning Tunneling Microscopy". ACS Nano 3 (3): 517–526. DOI:10.1021/nn8008245. ISSN 1520-605X. PMID 19309169. http://pubs.acs.org/doi/abs/10.1021/nn8008245. 
6. ^ Robertson, A.J.B. Catalysis of Gas Reactions by Metals. Logos Press, London, 1970.
7. ^ Helmut Knözinger, Karl Kochloefl “Heterogeneous Catalysis and Solid Catalysts” in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a05_313. Article Online Posting Date: January 15, 2003
8. ^ Arno Behr “Organometallic Compounds and Homogeneous Catalysis” Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a18_215. Article Online Posting Date: June 15, 2000
9. ^ Elschenbroich, C. ”Organometallics” (2006) Wiley-VCH: Weinheim. ISBN 978-3-527-29390-2
10. ^ "Recognizing the Best in Innovation: Breakthrough Catalyst". R&D Magazine, September 2005, pg 20.
11. ^ http://www.climatetechnology.gov/library/2005/tech-options/tor2005-143.pdf
12. ^ "Types of catalysis". Chemguide. http://www.chemguide.co.uk/physical/catalysis/introduction.html. Retrieved 2008-07-09. 
13. ^ Nelson, D. L.; Cox, M. M. "Lehninger, Principles of Biochemistry" 3rd Ed. Worth Publishing: New York, 2000. ISBN 1-57259-153-6.
14. ^ Keith J. Laidler and J.H. Meiser, Physical Chemistry, Benjamin/Cummings (1982), p.423
15. ^ M.W. Roberts (2000). "Birth of the catalytic concept (1800–1900)". Catalysis Letters 67 (1): 1–4. DOI:10.1023/A:1016622806065. http://www.springerlink.com/content/qm3732u7x7577224/fulltext.pdf. 
16. ^ ^{a b} K.J. Laidler Physical Chemistry with Biological Applications, Benjamin/Cummings 1978, p.415-417
17. ^ K.J. Laidler and J.H. Meiser, Physical Chemistry, Benjamin/Cummings (1982), p.425
18. ^ W.P. Jencks, “Catalysis in Chemistry and Enzymology” McGraw-Hill, New York, 1969. ISBN 0-07-032305-4
19. ^ Myron L Bender, Makoto Komiyama, Raymond J Bergeron “The Bioorganic Chemistry of Enzymatic Catalysis” Wiley-Interscience, Hoboken, U.S., 1984 ISBN 0-471-05991-9
20. ^ "Market Report: Global Catalyst Market, 2nd Edition". Acmite Market Intelligence. http://www.acmite.com/market-reports/chemicals/global-catalyst-market-report.html. 

External links[link]

Look up catalysis in Wiktionary, the free dictionary.

• Science Aid: Catalysts Page for high school level science
• W.A. Herrmann Technische Universität presentation
• Alumite Catalyst, Kameyama-Sakurai Laboratory, Japan
• Inorganic Chemistry and Catalysis Group, Utrecht University, The Netherlands
• Centre for Surface Chemistry and Catalysis
• Carbons & Catalysts Group, University of Concepcion, Chile
• Center for Enabling New Technologies Through Catalysis, An NSF Center for Chemical Innovation, USA
• "Bubbles turn on chemical catalysts", Science News magazine online, April 6, 2009.

Bluehamzzorz

Anna Nalick
Anna Nalick, 20 June 2011
Background information
Birth name	Anna Christine Nalick
Born	(1984-03-30) March 30, 1984 (age 28)[1]
Origin	Glendora, California, United States
Genres	Pop
Occupations	Singer-songwriter
Instruments	Vocals, Guitar, Piano
Years active	2003–present
Labels	Columbia Epic
Website	www.annanalick.com
Notable instruments
Vocals, Guitar, Piano

Anna Christine Nalick (born March 30, 1984) is an American singer-songwriter. Her debut album, Wreck of the Day, featuring her first radio hit, "Breathe (2 AM)", was released on April 19, 2005. Nalick left her label under Sony in 2009 after a falling-out surrounding the release of her second album. On March 2, 2011, Nalick announced her new album "Broken Doll and Odds and Ends" to be released May 2011, but after several delays, the album was released on June 5.

Biography[link]

A key memory of her childhood is the fifth grade math class where she would stop paying attention and instead rewrite the lyrics to a Cranberries song.^[2] She grew up in a family where two of the grandparents had performed on Broadway, and where her parents exposed her to a number of different artists, including Elvis Presley and Led Zeppelin. Nalick also considers Billie Holiday, Jeff Buckley, John Mayer, U2, and Fiona Apple to be some of her early influences and inspirations. She also cited other influences as Tori Amos, Blind Melon, and Stevie Ray Vaughan, in a 2005 interview.^[2]

In another interview, Nalick recalls showing off her talents to her third grade teacher, who then remarked that she'd end up "one day on The Tonight Show with Jay Leno." Nalick did perform in 2005 on the Tonight Show, making sure to invite the teacher to the audience.^[3]

Nalick initially decided to go to college before pursuing her dream of music, continuing to record her songs on a Rainbow Brite cassette recorder.^[2] But she soon met a photography^[2] professor, who had a student with parents in the music business. Nalick agreed to pass along a low-fidelity six-song demo tape, and soon enough, was introduced to Christopher Thorn and Brad Smith, the founding members of Blind Melon now turned production team, as well as Eric Rosse, best known for his production work for Tori Amos. In October 2003, putting her college plans on hold, she signed on with Columbia Records. Nalick went into the studio with Thorn, Smith and Rosse as producers, together with mix-engineer Mark Endert (Fiona Apple, Maroon 5, and Gavin DeGraw). She recorded with a group of musicians that included Smith on bass, Thorn on guitar, Rosse and Zak Rae on keyboards, Lyle Workman and Stuart Mathis on guitar, Joey Waronker and Matt Chamberlain on drums. The result was her album Wreck of the Day, released two years later.^[2]

[edit] 2004-2006: Wreck of the Day

This section needs additional citations for verification. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. (November 2009)

Anna Nalick's first single from her Wreck of the Day album was "Breathe (2 AM)", which peaked at #45 U.S. and went 3x Platinum on the Billboard Hot 100, and went huge on Adult Contemporary and Adult Top 40. It was heavily played on AAA and Hot AC stations across the U.S., along with light airplay on Pop stations, and Nalick became one of 2005's biggest newcomers. Her video for the track got very heavy airplay on VH1 and some MTV airplay as well. At the time of the writing, Wreck of the Day has sold over 615,000 copies with a gold certification from the RIAA, and a #20 peak on the Billboard 200. In New Zealand, Wreck of The Day reached the Top 15 albums on the Top 40 Albums Chart.

In the fall of 2005, Nalick released "In the Rough". The single was moderately successful, charting on the Billboard Hot Adult Top 40 Tracks at #15. Her album sales only slightly increased after the release of "In the Rough", perhaps because the previous single had been released almost a full year before.

Her first single from Wreck of the Day, "Breathe (2 AM)", experienced a resurgence on worldwide charts following a highly prominent appearance in a Grey's Anatomy episode (As We Know It), aired February 12, 2006. Other episodes of the show have featured the acoustic songs 'Catalyst' and 'Wreck of the Day' from the same album. The title track has also been featured on the show One Tree Hill.

In 2006, the album was re-released with three new songs and re-recording of the title track that was released as the album's third and final single. With little promotion and no video, the song only managed to chart on the Adult Top 40 spending two weeks at number 39 and one week at number 40 before falling off the chart.^[4]

In a September 2006 Q magazine interview, Britney Spears said she wished she had written Nalick's "Breathe (2 AM)". Two months later, Nalick took honors as "AC Female Artist of the Year" at the New Music Awards, beating out Sheryl Crow. According to her official website, Nalick was so convinced that Crow would win the award that she kicked back and relaxed, removing her shoes. When her name was called, she ran to the stage shoeless to make sure that she was able to have enough time for her acceptance speech.

A clip from the single, "Satellite" from Wreck of the Day is often played on the Satellite Sisters radio show. Wreck of the Day was also featured during Season 2, Episode 20 of the television show Joan of Arcadia.

[edit] 2007-current: Shine - EP, Interruption, Comeback, Broken Doll & Odds and Ends

This section needs additional citations for verification. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. (November 2009)

Anna Nalick performing at Hotel Cafe, Hollywood, California, USA on 5 October 2010

On May 11, 2007, the first indication of Nalick writing her second album appeared on her website. Few updates were given after that.^[5] The only other song to be released during this "era" was a track on the Desperate Housewives compilation CD entitled "Band of Gold".

On January 28, 2008, Nalick premiered her first single off the new album, "Shine", on AOL music's page.^[6] The EP "Shine" was released March 25, 2008.^[7] It featured the title single, a cover of Red Hot Chili Peppers' song "Breaking the Girl", and acoustic renditions of Nalick's best-known tracks.

On July 12, 2008, it was reported that Broken Doll was to be the title of Nalick's second album. The album was originally scheduled for release in the summer of 2008; however, a falling-out with Epic Records resulted in the album being scrapped. Little was heard from Nalick until the summer of 2010.

In August 2010, Nalick made a comeback announcement on her Facebook profile, accompanied by new photographs revealing a bold new look; it was revealed that she had left Sony in 2009 to be a free agent. She is currently independently making a record with producer Nathan Chapman (Taylor Swift, Jewel), with an expected release date in 2011. On August 25, 2010, Nalick premiered a new song, "The Lullaby Singer", on her official website.^[8] Nalick held five live performances - Hotel Café in Hollywood, California, for August 31, September 21, September 28, and October 5, 2010, and 3rd & Lindsley in Nashville, Tennessee, for September 9, 2010 ^[9] - to accompany the comeback announcement.

Nalick continues to announce new shows and further developments of her new album, via her Facebook and Twitter feeds. She previewed two additional songs on her website as well: "Words" in November 2010, and "Break Me Open" on January 5, 2011. Nalick expects to have this album out in Spring 2012.

To make up for lost time, Nalick is set to release two albums in 2011. The first is a semi-acoustic album featuring some new songs, revisited tracks from her debut and unreleased "Broken Doll" album, and covers. Later in the year, her fully produced album of brand new material, featuring songs like "The Lullaby Singer", "Break Me Open", "Words", and "Walk Away" will be released.

On 2 March 2011, Nalick announced on her Facebook page the official name for the first upcoming album: Broken Doll & Odds and Ends, a little variation from the one she announced before. It had been set for release in May 2011, but several unforeseen difficulties resulted in delays. Broken Doll & Odds and Ends was released on iTunes on 5 June 2011, with physical CD release happening at her Hotel Café show on 3 August 2011.^[10]

Nalick performed on Good Day Sacramento, singing "Walk Away" in honor of the people who died in 9/11.

Discography[link]

Studio albums[link]

Singles[link]

References[link]

External links[link]

• Anna Nalick's official site