Illustration of a redox reaction

Redox (reduction-oxidation) reactions include all chemical reactions in which atoms have their oxidation state changed. This can be either a simple redox process, such as the oxidation of carbon to yield carbon dioxide (CO₂) or the reduction of carbon by hydrogen to yield methane (CH₄), or a complex process such as the oxidation of glucose (C₆H₁₂O₆) in the human body through a series of complex electron transfer processes.

Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid-base reactions. Fundamentally, redox reactions are a family of reactions that are concerned with the transfer of electrons between species.

The term comes from the two concepts of reduction and oxidation.^[1] It can be explained in simple terms:

• Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion.
• Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.

Like acid-base reactions, redox reactions are a matched set, that is, there cannot be an oxidation reaction without a reduction reaction happening simultaneously. The oxidation alone and the reduction alone are each called a half-reaction, because two half-reactions always occur together to form a whole reaction. When writing half-reactions, the gained or lost electrons are typically included explicitly in order that the half-reaction be balanced with respect to electric charge.

Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation state — the actual transfer of electrons may never occur. Thus, oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always cause a change in oxidation state, but there are many reactions that are classed as "redox" even though no electron transfer occurs (such as those involving covalent bonds).

Non-redox reactions which do not involve changes in formal charge are known as metathesis reactions.^{[citation needed]}

The two parts of a redox reaction

Rusting iron

A bonfire. Combustion consists of redox reactions involving free radicals.

Etymology[link]

"Redox" is a portmanteau of "reduction" and "oxidation."

The word oxidation originally implied reaction with oxygen to form an oxide, since (di)oxygen was historically the first recognized oxidizing agent. Later, the meaning was generalized to include all processes involving loss of electrons.

The word reduction originally referred to the loss in weight upon heating a metallic ore such as a metal oxide to extract the metal. Lavoisier showed that this loss of weight was due to the loss of oxygen as a gas. Later, scientists realized that the metal atom gains electrons in this process. The meaning of reduction was then generalized to include all processes involving gain of electrons.

The electrochemist John Bockris has used the words electronation and deelectronation to describe reduction and oxidation processes respectively when they occur at electrodes^[2]. These words are analogous to protonation and deprotonation, but they have not been widely adopted by chemists.

Oxidizing and reducing agents[link]

In redox processes, the reductant transfers electrons to the oxidant. Thus, in the reaction, the reductant or reducing agent loses electrons and is oxidized, and the oxidant or oxidizing agent gains electrons and is reduced. The pair of an oxidizing and reducing agent that are involved in a particular reaction is called a redox pair. A redox couple is a reducing species and its corresponding oxidized form, e.g., Fe²⁺/Fe³⁺.

Oxidizers[link]

Substances that have the ability to oxidize other substances are said to be oxidative or oxidizing and are known as oxidizing agents, oxidants, or oxidizers. That is, the oxidant (oxidizing agent) removes electrons from another substance; i.e., it oxidizes other substances, and is thus itself reduced. And, because it "accepts" electrons, it is also called an electron acceptor.

Oxidants are usually chemical substances with elements in high oxidation states (e.g., H₂O₂, MnO−
4, CrO₃, Cr₂O2−
7, OsO₄), or else highly electronegative elements (O₂, F₂, Cl₂, Br₂) that can gain extra electrons by oxidizing another substance.

Reducers[link]

Substances that have the ability to reduce other substances are said to be reductive or reducing and are known as reducing agents, reductants, or reducers. The reductant (reducing agent) transfers electrons to another substance; i.e., it reduces others, and is thus itself oxidized. And, because it "donates" electrons, it is also called an electron donor. Electron donors can also form charge transfer complexes with electron acceptors.

Reductants in chemistry are very diverse. Electropositive elemental metals, such as lithium, sodium, magnesium, iron, zinc, and aluminium, are good reducing agents. These metals donate or give away electrons readily. Hydride transfer reagents, such as NaBH₄ and LiAlH₄, are widely used in organic chemistry,^[3][4] primarily in the reduction of carbonyl compounds to alcohols. Another method of reduction involves the use of hydrogen gas (H₂) with a palladium, platinum, or nickel catalyst. These catalytic reductions are used primarily in the reduction of carbon-carbon double or triple bonds.

Standard electrode potentials (reduction potentials)[link]

Each half-reaction has a standard electrode potential (E⁰_cell), which is equal to the potential difference (or voltage) (E⁰_cell) at equilibrium under standard conditions of an electrochemical cell in which the cathode reaction is the half-reaction considered, and the anode is a standard hydrogen electrode where hydrogen is oxidized: ½ H₂ → H⁺ + e^-.

The electrode potential of each half-reaction is also known as its reduction potential E⁰_red, or potential when the half-reaction takes place at a cathode. The reduction potential is a measure of the tendency of the oxidizing agent to be reduced. Its value is zero for H⁺ + e⁻ → ½ H₂ by definition, positive for oxidizing agents stronger than H⁺ (e.g., +2.866 V for F₂) and negative for oxidizing agents which are weaker than H⁺ (e.g. –0.763 V for Zn²⁺).^[5]

For a redox reaction which takes place in a cell, the potential difference E⁰_cell = E⁰_cathode – E⁰_anode

Historically, however, the potential of the reaction at the anode was sometimes expressed as an oxidation potential, E⁰_ox = – E⁰. The oxidation potential is a measure of the tendency of the reducing agent to be oxidized, but does not represent the physical potential at an electrode. With this notation, the cell voltage equation is written with a plus sign E⁰_cell = E⁰_cathode + E⁰_{ox (anode)}

Examples of redox reactions[link]

A good example is the reaction between hydrogen and fluorine in which hydrogen is being oxidized and fluorine is being reduced:

H₂ + F₂ → 2 HF

We can write this overall reaction as two half-reactions:

the oxidation reaction:

H₂ → 2 H⁺ + 2 e⁻

and the reduction reaction:

F₂ + 2 e⁻ → 2 F⁻

Analyzing each half-reaction in isolation can often make the overall chemical process clearer. Because there is no net change in charge during a redox reaction, the number of electrons in excess in the oxidation reaction must equal the number consumed by the reduction reaction (as shown above).

Elements, even in molecular form, always have an oxidation state of zero. In the first half-reaction, hydrogen is oxidized from an oxidation state of zero to an oxidation state of +1. In the second half-reaction, fluorine is reduced from an oxidation state of zero to an oxidation state of −1.

When adding the reactions together the electrons are canceled:

H2	→	2 H+ + 2 e−
F2 + 2 e−	→	2 F−
H2 + F2	→	2 H+ + 2 F−

And the ions combine to form hydrogen fluoride:

2 H⁺ + 2 F⁻ → 2 HF

The overall reaction is:

H₂ + F₂ → 2 HF

Displacement reactions[link]

Redox occurs in single displacement reactions or substitution reactions. The redox component of these types of reactions is the change of oxidation state (charge) on certain atoms, not the actual exchange of atoms in the compounds.

For example, in the reaction between iron and copper(II) sulfate solution:

Fe + CuSO₄ → FeSO₄ + Cu

The ionic equation for this reaction is:

Fe + Cu²⁺ → Fe²⁺ + Cu

As two half-equations, it is seen that the iron is oxidized:

Fe → Fe²⁺ + 2 e−

And the copper is reduced:

Cu²⁺ + 2 e−
→ Cu

Other examples[link]

• The oxidation of iron(II) to iron(III) by hydrogen peroxide in the presence of an acid:

Fe²⁺ → Fe³⁺ + e⁻

H₂O₂ + 2 e⁻ → 2 OH⁻

Overall equation:

2 Fe²⁺ + H₂O₂ + 2 H⁺ → 2 Fe³⁺ + 2 H₂O

• The reduction of nitrate to nitrogen in the presence of an acid (denitrification):

2 NO₃⁻ + 10 e⁻ + 12 H⁺ → N₂ + 6 H₂O

Iron rusting in pyrite cubes

• Oxidation of elemental iron to iron(III) oxide by oxygen (commonly known as rusting, which is similar to tarnishing):

4 Fe + 3 O₂ → 2 Fe₂O₃

• The combustion of hydrocarbons, such as in an internal combustion engine, which produces water, carbon dioxide, some partially oxidized forms such as carbon monoxide, and heat energy. Complete oxidation of materials containing carbon produces carbon dioxide.

• In organic chemistry, the stepwise oxidation of a hydrocarbon by oxygen produces water and, successively, an alcohol, an aldehyde or a ketone, a carboxylic acid, and then a peroxide.

Redox reactions in industry[link]

The primary process of reducing ore to produce metals is discussed in the article on Smelting.

Oxidation is used in a wide variety of industries such as in the production of cleaning products and oxidizing ammonia to produce nitric acid, which is used in most fertilizers.

Redox reactions are the foundation of electrochemical cells.

The process of electroplating uses redox reactions to coat objects with a thin layer of a material, as in chrome-plated automotive parts, silver plating cutlery, and gold-plated jewelry.

The production of compact discs depends on a redox reaction, which coats the disc with a thin layer of metal film.^{[clarification needed]}

Redox reactions in biology[link]

Top: ascorbic acid (reduced form of Vitamin C)
Bottom: dehydroascorbic acid (oxidized form of Vitamin C)

Many important biological processes involve redox reactions.

Cellular respiration, for instance, is the oxidation of glucose (C₆H₁₂O₆) to CO₂ and the reduction of oxygen to water. The summary equation for cell respiration is:

C₆H₁₂O₆ + 6 O₂ → 6 CO₂ + 6 H₂O

The process of cell respiration also depends heavily on the reduction of NAD⁺ to NADH and the reverse reaction (the oxidation of NADH to NAD⁺). Photosynthesis and Cellular respiration are complementary but photosynthesis is not the reverse of the redox reaction in cell respiration:

6 CO₂ + 6 H₂O + light energy → C₆H₁₂O₆ + 6 O₂

Biological energy is frequently stored and released by means of redox reactions. Photosynthesis involves the reduction of carbon dioxide into sugars and the oxidation of water into molecular oxygen. The reverse reaction, respiration, oxidizes sugars to produce carbon dioxide and water. As intermediate steps, the reduced carbon compounds are used to reduce nicotinamide adenine dinucleotide (NAD⁺), which then contributes to the creation of a proton gradient, which drives the synthesis of adenosine triphosphate (ATP) and is maintained by the reduction of oxygen. In animal cells, mitochondria perform similar functions. See Membrane potential article.

Free radical reactions are redox reactions that occur as a part of homeostasis and killing microorganisms, where an electron detaches from a molecule and then reattaches almost instantaneously. Free radicals are a part of redox molecules and can become harmful to the human body if they do not reattach to the redox molecule or an antioxidant. Unsatisfied free radicals can spur the mutation of cells they encounter and are thus causes of cancer.

The term redox state is often used to describe the balance of NAD⁺/NADH and NADP⁺/NADPH in a biological system such as a cell or organ. The redox state is reflected in the balance of several sets of metabolites (e.g., lactate and pyruvate, beta-hydroxybutyrate and acetoacetate), whose interconversion is dependent on these ratios. An abnormal redox state can develop in a variety of deleterious situations, such as hypoxia, shock, and sepsis. Redox signaling involves the control of cellular processes by redox processes.

Redox proteins and their genes must be co-located for redox regulation according to the CoRR hypothesis for the function of DNA in mitochondria and chloroplasts.

Redox cycling[link]

A wide variety of aromatic compounds are enzymatically reduced to form free radicals that contain one more electron than their parent compounds. In general, the electron donor is any of a wide variety of flavoenzymes and their coenzymes. Once formed, these anion free radicals reduce molecular oxygen to superoxide, and regenerate the unchanged parent compound. The net reaction is the oxidation of the flavoenzyme's coenzymes and the reduction of molecular oxygen to form superoxide. This catalytic behavior has been described as futile cycle or redox cycling.

Examples of redox cycling-inducing molecules are the herbicide paraquat and other viologens and quinones such as menadione.^[6]

Redox reactions in geology[link]

A uranium mine, near Moab, Utah. Note alternating red and white/green sandstone. This corresponds to oxidized and reduced conditions in groundwater redox chemistry. The rock forms in oxidizing conditions, and is then "bleached" to the white/green state when a reducing fluid passes through the rock. The reduced fluid can also carry uranium-bearing minerals.

In geology, redox is important to both the formation of minerals, mobilization of minerals, and in some depositional environments. In general, the redox state of most rocks can be seen in the color of the rock. Red is associated with oxidizing conditions of formation, and green is typically associated with reducing conditions. White (bleached rock) can also be associated with reducing conditions. Famous examples of redox conditions affecting geological processes include uranium deposits and Moqui marbles.

Balancing redox reactions[link]

Describing the overall electrochemical reaction for a redox process requires a balancing of the component half-reactions for oxidation and reduction. In general, for reactions in aqueous solution, this involves adding H⁺, OH⁻, H₂O, and electrons to compensate for the oxidation changes.

Acidic media[link]

In acidic media, H⁺ ions and water are added to half reactions to balance the overall reaction.

For example, when manganese(II) reacts with sodium bismuthate:

Unbalanced reaction:	Mn2+(aq) + NaBiO3(s) → Bi3+(aq) + MnO4− (aq)
Oxidation:	4 H2O(l) + Mn2+(aq) → MnO− 4(aq) + 8 H+(aq) + 5 e−
Reduction:	2 e− + 6 H+ + BiO− 3(s) → Bi3+(aq) + 3 H2O(l)

The reaction is balanced by scaling the two half-cell reactions to involve the same number of electrons (multiplying the oxidation reaction by the number of electrons in the reduction step and vice versa):

8 H₂O(l) + 2 Mn²⁺(aq) → 2 MnO−
4(aq) + 16 H⁺(aq) + 10 e−

10 e−
+ 30 H⁺ + 5 BiO−
3(s) → 5 Bi³⁺(aq) + 15 H₂O(l)

Adding these two reactions eliminates the electrons terms and yields the balanced reaction:

14 H⁺(aq) + 2 Mn²⁺(aq) + 5 NaBiO₃(s) → 7 H₂O(l) + 2 MnO−
4(aq) + 5 Bi³⁺(aq) + 5 Na⁺(aq)

Basic media[link]

In basic media, OH⁻ ions and water are added to half reactions to balance the overall reaction.

For example, in the reaction between potassium permanganate and sodium sulfite:

Unbalanced reaction:	KMnO4 + Na2SO3 + H2O → MnO2 + Na2SO4 + KOH
Reduction:	3 e− + 2 H2O + MnO4− → MnO2 + 4 OH−
Oxidation:	2 OH− + SO32− → SO42− + H2O + 2 e−

Balancing the number of electrons in the two half-cell reactions gives:

6 e−
+ 4 H₂O + 2 MnO₄⁻ → 2 MnO₂ + 8 OH⁻

6 OH⁻ + 3 SO₃²⁻ → 3 SO₄²⁻ + 3 H₂O + 6 e−

Adding these two half-cell reactions together gives the balanced equation:

2 KMnO₄ + 3 Na₂SO₃ + H₂O → 2 MnO₂ + 3 Na₂SO₄ + 2 KOH

Memory aids[link]

The key terms involved in redox are often confusing to students.^[7][8] For example, an element that is oxidized loses electrons; however, that element is referred to as the reducing agent. Likewise, an element that is reduced gains electrons and is referred to as the oxidizing agent.^[9] Acronyms or mnemonics are commonly used^[10] to help remember what is happening:

• "OIL RIG"—Oxidation Is Loss of electrons, Reduction Is Gain of electrons.^{[7][8][10][9]}

• "LEO the lion says GER" — Loss of Electrons is Oxidation, Gain of Electrons is Reduction.^{[7][8][10][9]}

• "LEORA says GEROA" — Loss of Electrons is Oxidation (Reducing Agent) and Gain of Electrons is Reduced (Oxidizing Agent).^[9]

See also[link]

References[link]

External links[link]

Wikimedia Commons has media related to: Redox reactions

• Chemical Equation Balancer - An open source chemical equation balancer that handles redox reactions.
• Video - Synthesis of Copper(II) Acetate 20 Feb. 2009
• Redox reactions calculator
• Redox reactions at Chemguide
• Online redox reaction equation balancer, balances equations of any half-cell and full reactions

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Jacob "Jake" Black is a fictional character in the Twilight series by Stephenie Meyer. He is described as a Native American of the Quileute tribe in La Push, near Forks, Washington. In the second book of the series, he undergoes a transformation that allows him to morph into a wolf. For the majority of the series, Jacob competes with Edward Cullen for Bella Swan's love. In the films Twilight, New Moon, Eclipse, and Breaking Dawn, Jacob is played by Taylor Lautner.

Concept and creation[link]

According to Stephenie Meyer, Jacob was originally meant to be a device through which Bella could learn Edward's secret in Twilight. Meyer, her agent, and her editor all liked the character so much that they decided to give him a larger role in the following book, New Moon, with Meyer calling the character, "my favorite gift that New Moon gave to me."^[1]

"Jacob was my first experience with a character taking over—a minor character developing such roundness and life that I couldn't keep him locked inside a tiny role....From the very beginning, even when Jacob only appeared in chapter six of Twilight, he was so alive. I liked him. More than I should for such a small part."

Meyer has said that after Jacob started emerging as a prominent character in New Moon, she went back to Twilight, which she was editing at the time, to "weave Jacob and [his father Billy] throughout Twilight more centrally."^[1]

Role in the books[link]

[edit] Twilight

Jacob is given a small role in the first book of the series. He is introduced as the son of Billy Black, an old Swan family friend. When Bella uses him to get information on Edward Cullen and his family, Jacob tells her Quileute legends and introduces her to the idea that Edward is a vampire. Bella comes to like Jacob, and he develops a crush on her.^[2]

[edit] New Moon

In New Moon, Jacob's character is used as a device to help Bella emerge from her months-long depression, brought on by her distress over Edward's departure. The friendship between the two characters grows strong, but Jacob also develops romantic feelings for Bella that she does not reciprocate. It is revealed that, as a member of the Quileute tribe, Jacob is descended from an ancient line of "shape-shifters" that assume wolf form. In their backstory, the Quileutes are vampires' mortal enemies. When Jacob undergoes his first transformation into a wolf, it is in response to a new vampire threat. Soon, the character becomes busy patrolling the forest with his pack, searching for vampires in the area. When Bella is caught by the vampire Laurent alone in a clearing, she is saved by Jacob and the wolf pack, who chase and kill Laurent.

Jacob serves as a rescue for Bella and a foil to Edward on multiple occasions in the narrative. When Bella, whose character has taken increasingly dangerous risks to feel closer to Edward, impulsively jumps off a cliff and almost drowns, Jacob saves her life. After Edward mistakenly believes she has died and plans to kill himself, Bella and Edward's sister, Alice Cullen, rush to Italy to stop his suicide, leaving Jacob hurt and angry. Jacob is disgusted by Edward's return and by Bella's willingness to take him back after he left her. Jacob reminds Edward of his tribe's treaty with the Cullen family, which states that the Cullens are not allowed to bite humans.^[3]

[edit] Eclipse

In Eclipse, Jacob, enraged by the fact that Bella plans to become a vampire, attempts to distance himself by not returning her phone calls and refusing to see her. Later, during the scene when Jacob visits Bella and Edward to discuss the vampire Victoria's return, he tells Bella that he misses her and wishes that they could remain friends. With Edward's approval, Bella begins to visit Jacob on a regular basis. On one of these visits, Jacob tells Bella that he is in love with her and that he wants her to choose him over Edward. Bella is caught off guard by his confession and tells him she only thinks of him as a friend. He forcibly kisses her, much to her displeasure, and she reacts by punching him in the face, breaking her hand and not leaving a scratch on him.

Jacob's werewolf pack and the Cullen family join forces to defeat Victoria and the army of newborn vampires she has created. Before the battle, Jacob overhears Edward and Bella discussing their engagement, which angers him greatly. Jacob threatens suicide and Bella, in an attempt to stop him, kisses him passionately. Afterward, she comes to the realization that she loves Jacob, but her love for Edward is greater. The epilogue is written from Jacob's point-of-view; angry, heartbroken, and hurt at Bella's decision to become a vampire, he runs away in his wolf form to escape his pain.^[4]

[edit] Breaking Dawn

Jacob returns after an absence of several weeks to attend Bella and Edward's wedding in Breaking Dawn. Though described as being still visibly pained by her decision, he tells Bella that he wants her to be happy. However, when Bella inadvertently informs him that she and Edward plan to have sex before she becomes a vampire, Jacob becomes enraged because he is said to know that Edward's strength could kill her. When Bella and Edward return from their honeymoon, Jacob becomes the narrator of the story for several chapters, during which he learns that she is pregnant with Edward's half-vampire, half-human child and has become desperately weak. When Jacob informs the pack of Bella's pregnancy, their leader Sam Uley plans an attack on the Cullens in order to kill Bella and, thereby, her unborn child because of the threat he believes the child presents. Jacob, who feels that the Cullens are innocent, disobeys Sam's command and separates himself from the pack. Fulfilling his birthright as an Alpha wolf, he is joined in a new pack by Seth and Leah Clearwater, who aid Jacob and the Cullens in protecting Bella. After the birth of Renesmee Carlie Cullen, Bella and Edward's daughter, Jacob immediately "imprints"— an involuntary response in which a shape-shifter finds his soul mate—on Renesmee. As a result, his affections are shifted and the romantic conflict between Jacob and Bella's characters is resolved. They remain close friends. The enmity between Jacob and the Cullens is also dispelled, and he and Edward come to view each other as brothers.^[5]

Characterization[link]

This unreferenced section requires citations to ensure verifiability.

Physical appearance[link]

Jacob is characterized as having primarily dark features by his "dark russet skin", "dark eyes", and "black hair". In Twilight, he is described as a lanky 6' 2" fifteen-year-old with hair down to his shoulders. By Breaking Dawn, Jacob's growing character stands at 7 feet and has a muscular build. In New Moon, after discovering that he can turn into a wolf, he cuts off his long hair. He later grows it out in Eclipse, thinking that Bella prefers it long. This makes his fur as a wolf shaggier and longer than that of the other wolves. He is said to be quite handsome, as Bella once mentions her jealousy of his features and describes him as "sort of beautiful". He tends to wear only cut-off style jeans or shorts with no shirt, since clothes are often ruined during his transformations into a wolf. As a wolf, Jacob has fur that is described as reddish-brown. In the films, the members of the pack all have the same tattoo on their right shoulder.

Personality and abilities[link]

Bella describes Jacob as a "happy person" who extends this happiness to the people around him. As Jacob's character emerges in New Moon, he is shown to be cheery, passionate, and adventurous, but hot-headed. Jacob is also able to shape-shift at will into a giant wolf, and sometimes when angered he will involuntarily phase. His body temperature is warmer than a human's body should be, reaching about 108.9 °F (42.7 °C), which allows him to withstand very cold weather. In human form, his body heals within seconds, he possesses superhuman strength and speed, has a high durability rate, sharp senses and free running abilities. In werewolf form he can communicate with his werewolf pack telepathically, has enhanced superhuman strength and speed and a substantial size increase. Werewolves teeth can cut through the hard bodies of a vampire with ease. Werewolves do not age if they regularly turn into their wolf form, with Jacob's body physically grown to the equivalent of a 25-year-old in Breaking Dawn. Jacob is the strongest of the pack. Once they begin phasing, a werewolf may "imprint"—a method of finding one's soulmate—on someone, and will act as whatever the imprintee needs, whether it be a protector, a lover, or an older sibling. Jacob imprints on Edward and Bella's daughter Renesmee in Breaking Dawn.

While treating Jacob in Eclipse, Carlisle takes a blood sample and runs some tests on it. He discovers that he has 24 pairs of chromosomes, one more than a human. A distinction is made in Breaking Dawn between the Children of the Moon ("true werewolves") and this shape-shifting tribe. The former are held to be a more ferocious type, with a transformative venomous bite and who involuntary phase as do traditional werewolves on the full moon.

Film portrayal[link]

Taylor Lautner played the part of Jacob Black in the film adaptation of Twilight.^[6] Due to major physical changes in the character of Jacob between Twilight and New Moon, director Chris Weitz considered replacing Lautner in the sequel with an actor who could more accurately portray "the new, larger Jacob Black."^[7] In an attempt to keep the role, Lautner stated, "I have been working out. I've been working out since the day we finished filming Twilight. I just weighed myself today; I've put on 19 pounds... [and] I'm guaranteeing Weitz 10 more [pounds] by filming."^[8] In January 2009, Weitz and Summit Entertainment announced that Lautner would continue to play the role of Jacob in New Moon.^[9]

Team Jacob[link]

Many fans of the Twilight franchise, particularly teenagers, like to debate whether Edward or Jacob is the better match for Bella. Both sides of the debate have coalesced around informal "teams" of followers, whether "Team Jacob" or "Team Edward." In a poll done by Novel Novice Twilight and appearing on NNT News in 2008, Team Jacob got 2,641 votes and Team Edward got 5,130 votes. A poll done by Top7 with over 43,000 votes had Jacob trailing Edward by around 3,000 votes.^[10]

Saturday Night Live lampooned these overzealous teenage fans in a sketch on December 12, 2009, with host Taylor Lautner portraying a diehard Edward supporter.^[11]

References[link]

External links[link]

Twilight portal

• Stephenie Meyer Official Website

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