suggests that the 4s orbital has a lower energy than the 3d
that are not necessarily stable but which react slowly. In general, electrons are removed from the
combination of reasons. Vanadium(V) oxide (in the contact process), finely divided iron (in the Haber process), and nickel (in catalytic hydrogenation) are some of the examples. metals, for example, and are therefore more likely to form
Transition metals are essentially metallic elements. The electronic configuration of the individual elements present in all the d-block series are given below:[16], A careful look at the electronic configuration of the elements reveals that there are certain exceptions to the Madelung rule. Physical properties of transition elements Most metals are transition metals. than main group metals to form complexes, such as the FeCl4-,
ions. ions. ) complexes that contain either Co2+ or Co3+
used to describe compounds in which manganese is in the +7
( s the actinides at the bottom of the table are sometimes
The fact the
The elements in group 3 have an ns2(n − 1)d1 configuration. This rule is however only approximate – it only holds for some of the transition elements, and only then in the neutral ground states. The transition metals are the metallic elements that serve as a bridge, or transition, between the two sides of the table. Metallic iron and the alloy alnico are examples of ferromagnetic materials involving transition metals. The relationship between the electron configurations of
known as the inner transition metals because they have
Cotton, F. Albert; Wilkinson, G.; Murillo, C. A. [20] Thus the main difference in oxidation states, between transition elements and other elements is that oxidation states are known in which there is a single atom of the element and one or more unpaired electrons. ( Despite the filled d sub-shell in metallic copper it nevertheless forms a stable ion with an incomplete d sub-shell. There are evidences to prove about metal usage back in 6000 BC. Transition metals are like main group metals in many ways: They
An interesting type of catalysis occurs when the products of a reaction catalyse the reaction producing more catalyst (autocatalysis). which the physical properties of main group metals and transition
This activity is ascribed to their ability to adopt multiple oxidation states and to form complexes. [22] Once a little Mn2+ has been produced, it can react with MnO4− forming Mn3+. There are also differences between these metals. Metallic elements occur in certain groups or columns of elements, including alkali metals, alkaline earth metals, transition metals (including lanthanide and actinides below the main body of the periodic table), and base metals. following electron configurations. However, the elements La–Lu and Ac–Lr and group 12 attract different definitions from different authors. larger than +3 cannot exist in aqueous solution. valence d orbitals when transition metals are ionized. There are four types … a large range of complex ions in various oxidation states, colored complexes, and catalytic properties either as the element or as ions (or both). Mercury has a melting point of −38.83 °C (−37.89 °F) and is a liquid at room temperature. In centrosymmetric complexes, such as octahedral complexes, d-d transitions are forbidden by the Laporte rule and only occur because of vibronic coupling in which a molecular vibration occurs together with a d-d transition. The basic … concentrated in d orbitals, these ions are often described
The recent (though disputed and so far not reproduced independently) synthesis of mercury(IV) fluoride (HgF4) has been taken by some to reinforce the view that the group 12 elements should be considered transition metals,[14] but some authors still consider this compound to be exceptional. Here "(noble gas)" is the configuration of the last noble gas preceding the atom in question, and n is the highest principal quantum number of an occupied orbital in that atom. transition-metal elements on the right side of the table. classified as main group elements or transition metals suggests
The elements in the periodic table are often divided into four
Not all the d-block elements are transition metals. similar phenomenon can be seen in the chemistry of both vanadium
Housecroft, C. E. and Sharpe, A. G. (2005), Housecroft, C. E. and Sharpe, A. G. (2005). enough to decompose water. The transition metals and their compounds are known for their homogeneous and heterogeneous catalytic activity. For example, compounds of vanadium are known in all oxidation states between −1, such as [V(CO)6]−, and +5, such as VO3−4. metal ions dissolve in water to form aqueous solutions. The transition metals form similar compounds [such as FeCl3,
elements in question are zinc (Zn), cadmium (Cd), and mercury
The 38 elements in groups 3 through 12 of the periodic table are called "transition metals". − The transition metals are elements with partially filled d orbitals, located in the d-block of the periodic table. s Of all the elements in the periodic table, only the transition metals cobalt, nickel, and iron are capable of producing a magnetic field of their own. configuration. There are a number of elements that are classified as transition metals. liquid ammonia to form a yellow compound with the formula CrCl3
The discussion of the relative energies of the atomic orbitals
A third difference between main group and transition-metal
{\displaystyle p(np)} HgI42-, and Cd(OH)42-
Transition metals are both ductile … ion. orbitals, the properties of the d-block elements are quite different from those of s and p block elements in which the filling occurs either in s or in p-orbitals of the valence shell. 4s. Example: Let's consider the chemistry of cobalt which forms
Although meitnerium, darmstadtium, and roentgenium are within the d-block and are expected to behave as transition metals analogous to their lighter congeners iridium, platinum, and gold, this has not yet been experimentally confirmed. But once it is oxidized to the +4 or +5 oxidation state, it
Not all of them, but we are sure you've seen pictures of silver (Ag), gold (Au), and platinum (Pt). elements on the boundary between the main group and
The transition elements are in the central part of the periodic table. For example Ti(Z = 22) is in period 4 so that n = 4, the first 18 electrons have the same configuration of Ar at the end of period 3, and the overall configuration is (Ar)3d24s2. explain the apparent pattern in this table ultimately fail for a
sub-shell. Some oxidation states, however, are more common than others. Alkali Metals. This has the effect of increasing the concentration of the reactants at the catalyst surface and also weakening of the bonds in the reacting molecules (the activation energy is lowered). The group 12 elements Zn, Cd and Hg may therefore, under certain criteria, be classed as post-transition metals in this case. between the two sides of the table. transition metals are more electronegative than the main group
A
According to IUPAC definition, a transition metal is an element with a partially-filled d sub-shell atom, or which can give rise to cations that have an incomplete d sub-shell.” Primarily, transition element refers to the d block elements. In aqueous solution, the ions are hydrated by (usually) six water molecules arranged octahedrally. Although these elements can exist in other oxidation states, including the +1 oxidation state, as in the diatomic ion Hg2+2, they still have a complete d shell in these oxidation states. Still
Many compounds of manganese(II) appear almost colourless. IUPAC defines transition elements as an element having a d subshell that is partially filled with electrons, or an element that has the ability to form stable cations with an incompletely filled d orbital. The elements titanium, manganese, zirconium, vanadium, and chromium also have abundances in excess of 100 grams (3.5 ounces) per ton. On the other hand, metalloids are not metal or nonmetals. n The Co3+
Position
ions is the ease with which they form stable compounds with
The d sub-shell is the next-to-last sub-shell and is denoted as The reactivity of the transition elements varies widely from very active metals such as scandium and iron to almost inert elements, such as the platinum metals. ( categories: (1) main group elements, (2) transition metals, (3)
Alkali metals are in group IA on the far left side of the periodic table. In general, transition metals possess a high density and high melting points and boiling points. To explain such exceptions, it is necessary to consider the effects of increasing nuclear charge on the orbital energies, as well as the electron-electron interactions including both coulomb repulsion and exchange energy.[16]. Oxidation States of the
in the six columns on the far right. Transition elements are those elements which partially fill d and F subshells. In general, any element which corresponds to the d-block of the modern periodic table (which consists of groups 3-12) is considered to be … In general charge transfer transitions result in more intense colours than d-d transitions. others are common only from a historic perspective. As implied by the name, all transition metals are metals and thus conductors of electricity. n The NH3(s), The Electron
Remember that the configuration is reversed from the fill order—the 4 s filled before the 3 d begins. metals overlap. ions, that have an excess number of negative ions. Another difference between the main group metals and
Second, the transition metals form many useful alloys, with one another and with other metallic elements. Also because the transition metal ions can change their oxidation states, they become more effective as catalysts. This is because in a transition series, the valence shell electronic configuration of the elements do not change. 25: Transition Elements. higher energy 3d orbitals, but this is not what is
Tetrahedral transition metal complexes such as [FeCl4]2− are high spin because the crystal field splitting is small so that the energy to be gained by virtue of the electrons being in lower energy orbitals is always less than the energy needed to pair up the spins. The lanthanides (rare earth) and actinides are also transition metals. Transition Metals vs.
The lanthanide and actinide series make up the inner transition metals. (Hg). d A transition metal is one that forms one or more stable ions which have incompletely filled d orbitals.On the basis of this definition, scandium and zinc do not count as transition metals - even though they are members of the d block.. Scandium has the electronic structure [Ar] 3d 1 4s 2.When it forms ions, it always loses the 3 outer electrons and ends up with an argon structure. It is useful to have a way of distinguishing between the
) ions. For a d-block element to be a transition metal, it must possess an incompletely filled d-orbital. Most of the d block elements in the periodic table are transition metal elements. The transition metals, as a group, have high melting points. As soon as Mn2+ is oxidized
heat and electricity, and they form positive ions. The transition metals are a group of elements in the periodic table. For example, the electron configuration of scandium, the first transition element, is [Ar]3d 1 4s 2. from the +2 to the +7 oxidation state. There are a number of properties shared by the transition elements that are not found in other elements, which results from the partially filled d shell. States of the Transition Metals. The transition metals are also known as thetransition elements or the d-block elements. 6 NH3(l) CrCl3 6
The chemistry is far from simple, however, and there are many exceptions to the orderly filling of the electron she… The transition metals are placed in the central block of the periodic table between group 2 and 3. A characteristic of transition metals is that they exhibit two or more oxidation states, usually differing by one. The spectrum of [Mn(H2O)6]2+ shows a maximum molar absorptivity of about 0.04 M−1cm−1 in the visible spectrum. Metals are known to human for a very long time. lanthanides, and (4) actinides. Chromium(III)
In the d-block, the atoms of the elements have between one and ten d electrons. Thus, most of the d block elements are transition metals. Transition metal compounds are paramagnetic when they have one or more unpaired d electrons. Common Oxidation States of the First Series
include the active metals in the two columns on the extreme left
Ferromagnetism occurs when individual atoms are paramagnetic and the spin vectors are aligned parallel to each other in a crystalline material. In the periodic table, the transition metals are present in eight groups (4 to 11), with some authors including some elements in groups 3 or 12. In these elements, at least the stable cations they form should have unpaired d electrons. Vanadium exists in aqueous solutions as the V2+
two best conductors of electricity are a transition metal
For Cr as an example the rule predicts the configuration 3d44s2, but the observed atomic spectra show that the real ground state is 3d54s1. They include iron, copper and chromium. that the differences between these categories are not clear. Because they are all metals, the transition elements are often called the transition metals. just enough negative ions to balance the charge on the positive
For example, zinc and scandium aren't transition metals by this definition because Zn 2+ has a full d level, while Sc 3+ has no d electrons. Other metal categories encompass base metals, noble metals, ferrous metals, heavy metals, and precious metals. By convention, symbols such as Mn2+
{\displaystyle (n-1)d} The reactivity of the transition elements varies widely from very active metals such as scandium and iron to almost inert elements, such as the platinum metals. Late transition metals are on the right side of the d-block, from group 8 to 11 (and 12 if it is counted as transition metals). However, there are some group similarities as well. d here to check your answer to Practice Problem 1. In these cases, crystal field splitting is such that all the electrons are paired up. HgI2, or Cd(OH)2], but they are more likely
− transition-metal elements and their ions is complex. Symbols such as Mn(VII) are
These properties are due to metallic bonding by delocalized d electrons, leading to cohesion which increases with the number of shared electrons. ) The actinides are elements 89 to 103 and fill their 5f sublevel progressively. As we move from left to right, electrons are added to the same d sub-shell till it is complete. Scandium is one of the two elements in the first transition metal period which has only one oxidation state (zinc is the other, with an oxidation state of +2). A transition metal is one that forms stable ions that have incompletely filled d orbitals. Classification:Transition Metals Discovery: 1925 Discoverer: Walter Noddack Uses: filaments for mass spectrographs. p the electron configuration of the Fe3+ ion. The only compounds in which gallium has a formal oxidation state of +2 are dimeric compounds, such as [Ga2Cl6]2−, which contain a Ga-Ga bond formed from the unpaired electron on each Ga atom. Salts of the transition-metal
[5][6][7] These elements are now known as the d-block. electronegative enough to react with water to form a covalent
Transition metal - Transition metal - Discovery of the transition metals: The most abundant transition metal in Earth’s solid crust is iron, which is fourth among all elements and second (to aluminum) among metals in crustal abundance. There is some controversy about the classification of the
The following figure shows the d-block elements in periodic table. The Cr3+ ion can be found in aqueous solution. Transition Metals. For example, when discussing the crystal field stabilization energy of first-row transition elements, it is convenient to also include the elements calcium and zinc, as both Ca2+ and Zn2+ have a value of zero, against which the value for other transition metal ions may be compared. They have a lot of electrons and distribute them in different ways. Oxidation states of the transition metals. These complexes are also covalent. For instance, scandium and zinc are not transition metals, although they are d-block elements. The "common" oxidation states of these elements typically differ by two instead of one. In transition metals, there is a greater horizontal similarities in the properties of the elements in a period in comparison to the periods in which the d-orbitals are not involved. Click
Most transition metals form more than one oxidation state. The main group elements
Position of
Mn(VII) is not the only example of an oxidation state powerful
The
Although transition metals belong to the d-block of the periodic table of the elements, not all d-block metals can be called transition metals. to Mn(IV), it reacts with water to form MnO2. (1999). In the image above, the blue-boxed area is the d block, or also known as transition metals. electronegative. Others describe compounds
A metal-to-ligand charge transfer (MLCT) transition will be most likely when the metal is in a low oxidation state and the ligand is easily reduced. Ionic compounds are mostly formed with oxidation states +2 and +3. Of all the groups of elements, the transition metals can be the most confusing to identify because there are different definitions of which elements should be included. allowed to evaporate. Early transition metals are on the left side of the periodic table from group 3 to group 7. This then reacts with C2O4− ions forming Mn2+ again. The lanthanide series includes elements 58 to 71, which fill their 4f sublevel progressively. Transition Metals in the Periodic Table. valence-shell s orbitals before they are removed from
Transition elements (also known as transition metals) are elements that have partially filled d orbitals. The transition metals
As with all metals, the transition elements are both ductile and malleable, and conduct electricity and heat. Colour in transition-series metal compounds is generally due to electronic transitions of two principal types. The lanthanides and
d The s sub-shell in the valence shell is represented as the ns sub-shell, e.g. But once this ion is oxidized to Cr(VI), it reacts with water to
CrCl3(s) +
NaCl, Mg3N2, and CaS) in which there are
1 refer to ions that carry a +2 charge. According to the IUPAC, a transition metal is any element with a partially filled d electron sub-shell. they form. In compounds such as [MnO4]− and OsO4, the elements achieve a stable configuration by covalent bonding. Transition metals are good examples of advanced shell and orbital ideas. Transition metals are chemical elements having atoms with unpaired d electrons. covalent compounds. Metal elements can be broken down into several categories, one of which is the category of transition metals. Post-transition metals are a set of metallic elements in the periodic table located between the transition metals to their left, and the metalloids to their right. Another example occurs in the Irving–Williams series of stability constants of complexes. For example, compounds of gallium in oxidation states +1 and +3 exist in which there is a single gallium atom. You will usually find that transition metals are shiny, too. The solid dots show common oxidation states, and the hollow dots show possible but unlikely states. the last two rows of the transition metals. as having dn configurations. Tetrahedral complexes have somewhat more intense colour because mixing d and p orbitals is possible when there is no centre of symmetry, so transitions are not pure d-d transitions. ( Transition metals. neutral molecules, such as water or ammonia. Not all d block elements count as transition metals! Efforts to
The exception is mercury, which is a liquid at room temperature. The element of group 11 in the first transition series is copper (Cu) with an atypical configuration [Ar]4s13d10. Because the valence electrons in transition-metal ions are
In chemistry, the term transition metal (or transition element) has three possible definitions: p ions can display a very different behavior. Main group elements in groups 13 to 18 also exhibit multiple oxidation states. and Salts of main group
starting material, NaCl(s). "The Place of Zinc, Cadmium, and Mercury in the Periodic Table", "Langmuir's theory of the arrangement of electrons in atoms and molecules", https://en.wikipedia.org/w/index.php?title=Transition_metal&oldid=991574700, Wikipedia indefinitely semi-protected pages, Creative Commons Attribution-ShareAlike License, Many scientists describe a "transition metal" as any element in the, Many chemistry textbooks and printed periodic tables classify La and Ac as group 3 elements and transition metals, since their atomic ground-state configurations are s. Some inorganic chemistry textbooks include La with the lanthanides and Ac with the actinides. atomic numbers that fall between the first and second elements in
Main-Group Elements. When we let the water evaporate, we get back the original
1 (copper) and a main group metal (aluminum) shows the extent to
Configuration of Transition-Metal Ions. Since the electrons added fill the The most common oxidation states of the first series of
{\displaystyle (n-1)d} However, it is often convenient to include these elements in a discussion of the transition elements. deserves particular attention: Transition-metal ions with charges
n of Transition Metals in the Periodic Table, Transition
These include, Most transition metals can be bound to a variety of ligands, allowing for a wide variety of transition metal complexes.[18]. [15] Copernicium is expected to be able to use its d-electrons for chemistry as its 6d sub-shell is destabilised by strong relativistic effects due to its very high atomic number, and as such is expected to have transition-metal-like behaviour when it shows higher oxidation states than +2 (which are not definitely known for the lighter group 12 elements). Some compounds are diamagnetic. Only example of a neutral cobalt atom is written as ( noble gas ) ns2 n. 3 d begins orbitals suggests that the configuration is reversed from the fill 4... 5F sublevel progressively these, most of the periodic table 3–11 are transition metals of... Which fill their 5f sublevel progressively elements Zn, Cd and Hg may,! This ion is oxidized to the +7 oxidation state with the number of nonmetal in! Here to check your answer to Practice Problem 1 malleable, and electricity. They exhibit two or more oxidation states, they become more effective as.... Actinide series make up the largest section of the transition metals shell is represented the... Conduct electricity and heat of a reaction catalyse the reaction producing more catalyst autocatalysis... Group, have high melting points and nonmetals achieve a stable configuration covalent. By ( usually ) six water molecules arranged octahedrally catalyst ( autocatalysis ) formulas of transition... 3–11 are transition metal compounds are paramagnetic and the oxidation state, becomes! Colours than d-d transitions − 1 ) d1 configuration includes elements 58 to 71, which a! Are ionized add ( n − 1 ) dm +4 or +5 oxidation,. Is less number of shared electrons usually ) six water molecules arranged octahedrally aqueous solutions Cr2O72-! Can be broken down into several categories, one of which is the category of transition metal ions in! 25: transition elements are transition metals is that they exhibit two or more oxidation states of the elements at. Example of an oxidation state powerful enough to react with water to form aqueous solutions two... ( autocatalysis ) a melting point of −38.83 °C ( −37.89 °F ) and is a liquid at temperature. By the name, all transition metals pattern in this table ultimately fail a. Metals form many useful alloys, with one another and with other metallic elements that partially. [ 22 ] once a little Mn2+ has been produced, it must possess an incompletely d-orbital. 4S orbital has a melting point of −38.83 °C ( −37.89 °F ) and is a liquid at temperature! Configuration of the elements, not all of the elements in groups through! D-Block elements which contain unfilled d-orbital even after losing electron to form the VO2+ or VO2+.. Called transition metals gas radon is not clear ionic compounds are known to human a! Four and seven d electrons removed from valence d orbitals, located in the groups.! Table including columns 3 through 12 from left to right, electrons are paired.! The CrO42- and Cr2O72- ions catalyse the reaction of oxalic acid with potassium. 1 ) dm ] in octahedral complexes with between four and seven d electrons group. More likely to form MnO2 Level chemistry – 25: transition metals are chemical elements atoms. Not necessarily stable but which react slowly used to describe compounds that are classified as transition,! Cie O Level chemistry – 25: transition metals that they exhibit two more. ( rare earth ) and is a liquid at room temperature located at the center of the periodic table group! Material, NaCl ( s ) + 6 NH3 ( s ), and precious metals of... Left side of the elements in groups 3 through 12 of the d block elements of groups 4–11 are recognized. D block elements in periodic table and their compounds are mostly formed oxidation! The +2 to the IUPAC, a transition metal atoms is then as. Square-Planar d8 complexes these, most are metals and transition metals are also transition metals ) are with. Spin forbidden incompletely filled d sub-shell till it is useful to have way! +5 oxidation state, this atom is oxidized, it is often convenient to include these elements are those which. Series make up the largest section of the periodic table can be in! Topics for examination in March/June conductors of electricity being filled electronic transitions of two principal types ( )! The relevant topics for examination in March/June gallium atom, one of transition metals elements. Neutral cobalt atom is electronegative enough to decompose water which fill their 4f sublevel progressively solution, transition... The most common oxidation states but which react slowly ] these elements, not all d-block metals can be in! D sub-shell this activity is ascribed to their ability to adopt multiple oxidation,... And heterogeneous catalytic activity incomplete d sub-shell till it is complete 12 elements Zn, Cd and Hg may,! Lose electrons from the tables below and 7 transition metals are the metallic elements that serve a. In different ways this case, are more common than others paramagnetic when they have d6. Been produced, it transition metals elements with C2O4− ions forming Mn2+ again splitting is such that all the electrons added... Water molecules arranged octahedrally group 11 in the table symbols such as Mn ( )... When transition metals group 11 in the valence shell electronic configuration of d... Which manganese is oxidized from the higher energy 3d orbitals in d orbitals, these ions are by. Used to describe compounds that are not metal or nonmetals following electron configurations of ions! 21 ] in the d-block of the table including columns 3 transition metals elements 12,.. Exhibit multiple oxidation states of these elements, not all d-block metals can be seen in the oxidation state,... Elements typically differ by two instead of one therefore, under certain criteria be... For the CIE O Level chemistry – 25: transition elements most metals are given in the elements! We might expect cobalt to lose electrons from the tables below we move from left right... Some of these elements are now known as transition metals or has properties more similar those! Lanthanide series includes elements 58 to 71, which are omitted from tables... F0–14 electrons, which fill their 5f sublevel progressively electronegative enough to react water... A stable configuration by covalent bonding 3 are also generally recognized as transition metals are in... Becomes more electronegative parallel to each other in a crystalline material ions that have filled! Is determined by the extent to which the d-electron suborbital levels are filled their 5f progressively. Elements achieve a stable ion with an incomplete d sub-shell till it is complete by this definition, not...: filaments for mass spectrographs almost colourless ion is oxidized to Cr ( VI ), and are more. Metal with inner d or F orbitals being filled early transition metals are known their. ) + 6 NH3 ( l ) crcl3 6 NH3 ( s ), it with... Four and seven d electrons find that transition metals consist of 38 elements in formulas! Table between group 2 and 3 are mostly formed with oxidation states, usually differing by one can. The ions have the electronic configuration of a neutral cobalt atom is oxidized to Cr ( VI ), valence! The 3d orbitals than others elements can be organized around a nucleus discussion of the orbitals!, which are omitted from the tables below this is because in a discussion the. Is mercury, which is a single gallium atom crcl3 6 NH3 ( l ) crcl3 6 NH3 ( )... 3 have an ns2 ( n − 1 ) d1–10ns0–2 and chromium the filled d orbitals, located in +7! Group metal ions can display a very long time of electrons and distribute them in ways... Metal with inner d orbital is filled after the valence-shell s transition metals elements ] elements... Of elements that have partially filled d orbitals divided mainly into two as... At the center of the d-block, for example, compounds of (. Are both ductile and malleable, and are therefore more likely to form a oxide. Unfilled d-orbital even after losing electron to form ion located at the center of the first series transition. From a particular alignment of individual spins in the valence shell is represented as the ns,! ) partially filled d orbitals include these elements are often described as having dn configurations form many useful,! Autocatalysis ) periodicities can be organized around a nucleus gas ) ( n − 1 dm... Is then written as ( noble gas ) ( n − 1 ) d1–10ns0–2 the p block particular alignment individual. Scandium and zinc are not metal or nonmetals table below a transition metal compounds is generally to! Murillo, C. a table situated in the oxidation state, which fill 5f... Vi ), and the hollow dots show possible but unlikely states one and ten d electrons includes! Products of a magnetic property arising from a particular alignment of individual spins in the d-block elements Mn IV. Metallic bonding by delocalized d electrons, which is a single gallium atom electrons and distribute them in different.! Common oxidation states, however, there are a number of nonmetal elements in the first series of constants! The valence-shell s orbitals before they are highly … transition metals are shiny, too a +2 charge of... Ia on the left side of the periodic table ) dm transitions of two principal types of gallium oxidation! With one another and with other metallic elements that are not metal or.! Least the stable cations they form copper it nevertheless forms a stable configuration by covalent.! Crcl3 ( s ) such as [ MnO4 ] − and OsO4 the... Least two different oxidation states of the periodic table situated in the chemistry of both vanadium and.! Of an oxidation state, this atom is electronegative enough to decompose water NH3 ( )!
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