Hybridization of atoms in ethene molecue can be found from lewis structure. In the lewis structure of The more resonance forms a molecule has makes the molecule more stable. [47], Like all hydrocarbons, ethylene is a combustible asphyxiant. ), { "8.01:_Chemical_Bonds_Lewis_Symbols_and_the_Octet_Rule" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.02:_Ionic_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.03:_Covalent_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.04:_Bond_Polarity_and_Electronegativity" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.05:_Drawing_Lewis_Structures" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.06:_Resonance_Structures" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.07:_Exceptions_to_the_Octet_Rule" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.08:_Strength_of_Covalent_Bonds" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.E:_Basic_Concepts_of_Chemical_Bonding_(Exercises)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.S:_Basic_Concepts_of_Chemical_Bonding_(Summary)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "01:_Introduction_-_Matter_and_Measurement" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "02:_Atoms_Molecules_and_Ions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "03:_Stoichiometry-_Chemical_Formulas_and_Equations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "04:_Reactions_in_Aqueous_Solution" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "05:_Thermochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "06:_Electronic_Structure_of_Atoms" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "07:_Periodic_Properties_of_the_Elements" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "08:_Basic_Concepts_of_Chemical_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "09:_Molecular_Geometry_and_Bonding_Theories" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "10:_Gases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "11:_Liquids_and_Intermolecular_Forces" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "12:_Solids_and_Modern_Materials" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "13:_Properties_of_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "14:_Chemical_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "15:_Chemical_Equilibrium" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "16:_AcidBase_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "17:_Additional_Aspects_of_Aqueous_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "18:_Chemistry_of_the_Environment" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "19:_Chemical_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "20:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "21:_Nuclear_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "22:_Chemistry_of_the_Nonmetals" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "23:_Chemistry_of_Coordination_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "24:_Chemistry_of_Life-_Organic_and_Biological_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "Valence Bond Theory", "formal charge", "resonance structure", "showtoc:no", "license:ccbyncsa", "licenseversion:30" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FMap%253A_Chemistry_-_The_Central_Science_(Brown_et_al. Fill in any lone pair electrons and identify any pi bond electrons. Q.6 Elements of group 16 have lower ionization enthalpy values compared to those of group 15 elements. Products of these intermediates include polystyrene, unsaturated polyesters and ethylene-propylene terpolymers. @1IXtGZk6C;q:V/d?>NmmQT Of%~fP:Ghud`9]3;$,7RG]c}X6Dr";~s|`Cr8DS4{5zlE\?O9Ul Zas,0yu F9>G:_|RCC8"qp>P`. At this point, both terminal oxygen atoms have octets of electrons. [28], Although of great value industrially, ethylene is rarely synthesized in the laboratory and is ordinarily purchased. Six electrons are used to form three bonding pairs between the oxygen atoms and the carbon: 4. chlorine itself is not used. If you are good at lewis structure drawing and. Resonance Structures for NH3 (Ammonia) Wayne Breslyn 614K subscribers Subscribe 81 Share 12K views 2 years ago There is really only one way to draw the Lewis structure for Ammonia (NH3). The electron dot structure, widely known as Lewis Structure, is a skeletal diagrammatic representation of a molecule taking into account the constituent atoms and the valence shell electrons. One of the first organometallic compounds, Zeise's salt is a complex of ethylene. If we place three lone pairs of electrons on each terminal oxygen, we obtain. Some products derived from this group are polyvinyl chloride, trichloroethylene, perchloroethylene, methyl chloroform, polyvinylidene chloride and copolymers, and ethyl bromide. Resonance structures are a set of two or more Lewis Structures that collectively describe the electronic bonding of a single polyatomic species including fractional bonds and fractional charges. A teacher walks into the Classroom and says If only Yesterday was Tomorrow Today would have been a Saturday Which Day did the Teacher make this Statement? Approach: There is only one bond in this example, and no any lone pairs, so only the electrons can be moved around. Attached it what I have so far. Questionsif(typeof ez_ad_units!='undefined'){ez_ad_units.push([[468,60],'chemistryscl_com-leader-1','ezslot_12',151,'0','0'])};__ez_fad_position('div-gpt-ad-chemistryscl_com-leader-1-0'); To know whether resonance structures can be drawn for C2H4, you should understand the structure of lewis structure of C2H4. There are some requirements to be the center atom. B) Resonance structures are not isomers. What are the Physical devices used to construct memories? C2H4 Lewis Structure Steps The Lewis Structure of any molecule can be easily done if we follow certain given procedures. between atoms. At this point, the carbon atom has only 6 valence electrons, so we must take one lone pair from an oxygen and use it to form a carbonoxygen double bond. Ethylene is also an important natural plant hormone and is used in agriculture to force the ripening of fruits. of ethene. ethene molecule, Total number of pairs of electrons are 6. Count up the valence electrons: (1*5) + (3*6) + 1 (ion) = 24 electrons. Now let's draw all of the structural isomers that have the molecular formula C3H8O. We could name it 2-butene, but there are . Use resonance structures to describe the bonding in benzene. compound in alkene compound series. VSEPR stands for Valence Shell Electron Pair Repulsion model or theory. Therefore, we should try to find charges if Some resonance structures are more favorable than others. Atomic orbitals combine together to form hybrid orbitals and the process is known as hybridization. [citation needed], In the mid-19th century, the suffix -ene (an Ancient Greek root added to the end of female names meaning "daughter of") was widely used to refer to a molecule or part thereof that contained one fewer hydrogen atoms than the molecule being modified. Well, C2H4 is a simple straight-chain hydrocarbon that bears a sweet aroma and has a colorless form. This is due to the fact that each carbon surrounds a planar triangle. structure. It is listed as an IARC class 3 carcinogen, since there is no current evidence that it causes cancer in humans.[48]. So, what we can do is, we can take those electrons from the bottom and place them in the center between the two C atoms. stream [36] The properties of ethylene were studied in 1795 by four Dutch chemists, Johann Rudolph Deimann, Adrien Paets van Troostwyck, Anthoni Lauwerenburgh and Nicolas Bondt, who found that it differed from hydrogen gas and that it contained both carbon and hydrogen. No. Ethylene is widely used in the chemical industry, and its worldwide production (over 150 million tonnes in 2016[7]) exceeds that of any other organic compound. The Resonance Plugin generates all resonance structures of a molecule. [33], Ethylene appears to have been discovered by Johann Joachim Becher, who obtained it by heating ethanol with sulfuric acid;[34] he mentioned the gas in his Physica Subterranea (1669). Resonance structures are not in equilibrium with each other. C2H2, and C2H4. The other sp2 hybrid orbitals form sigma bonds between C and H, therefore, leading to C-H single bonding structure. 2003-2023 Chegg Inc. All rights reserved. This can help us determine the molecular geometry, how the molecule might react with other molecules, and some of the physical properties of the molecule (like boiling point and surface tension).Chemistry help at https://www.Breslyn.org The tail of the arrow begins at the electron source and the head points to where the electron will be. Sometimes, even when formal charges are considered, the bonding in some molecules or ions cannot be described by a single Lewis structure. My aim is to uncover unknown scientific facts and sharing my findings with everyone who has an interest in Science. In the United States and Europe, approximately 90% of ethylene is used to produce ethylene oxide, ethylene dichloride, ethylbenzene and polyethylene. Map: Chemistry - The Central Science (Brown et al. This is important because neither resonance structure actually exists, instead there is a hybrid. There are several things that should be checked before and after drawing the resonance forms. If we see the last group, we can find out that all the elements are inert gases having eight electrons in their valence shells (except He which has two). Then calculate the number of valence electrons used in this drawing. The placement of atoms and single bonds always stays the same. When we draw the Lewis Structure of C2H4, we find a linear 2-D representation. Ethylene (IUPAC name: ethene) is a hydrocarbon which has the formula C 2 H 4 or H 2 C=CH 2.It is a colourless, flammable gas with a faint "sweet and musky" odour when pure. We therefore place the last 2 electrons on the central atom: 6. For resonance structures there must be a double or triple bond present, which is not the case with CH4.When we draw resonance structures for molecules, like CH4, we start with a valid Lewis structure and then follow these general rules.- Resonance forms must be valid Lewis structures.- Maintain the same number of valence electrons. The name ethylene was used in this sense as early as 1852.[39]. Step 3: Now, that we have drawn the atoms by their symbols, let us denote the valence electrons by dots. 1 Calculated resonance structures of . They are used when there is more than one way to place double bonds and lone pairs on atoms. There is a carbocation beside the . C2H4 is also called Ethene.For the Electron Dot Structure for ethene, C2H4, the key to understanding how to distribute the valence electrons is to recognize the need for a double bond between the two carbon atoms.----- Steps to Write Lewis Structure for compounds like C2H4 -----1. The position of the atoms is the same in the various resonance structures of a compound, but the position of the electrons is different. If you are a beginner to lewis structure drawing, follow these sections slowly and properly to understand So, it is important for us to learn about C2H4 in detail to understand the nature of straight-chain hydrocarbons in a better manner. In a single bond, we have a sigma bond. This gives 4 + (3 6) + 2 = 24 valence electrons. [12][22], Global ethylene production was 107 million tonnes in 2005,[8] 109 million tonnes in 2006,[23] 138 million tonnes in 2010, and 141 million tonnes in 2011. For, Find the total valence electrons for the C2H4 molecule.2. Now, we should try to minimize charges by converting a lone pair or pairs to a bond. Formal charges are used in Chemistry to determine the location of a charge in a molecule and determine how good of a Lewis structure it will be. If so, the resonance structure is not valid. If so, the resonance structure is not valid. B If the 6 remaining electrons are uniformly distributed pairwise on alternate carbon atoms, we obtain the following: Three carbon atoms now have an octet configuration and a formal charge of 1, while three carbon atoms have only 6 electrons and a formal charge of +1. Draw the bond connectivities: The three oxygens are drawn in the shape of a triangle with the nitrogen at the center of the triangle. Sigma orbital overlap: This signifies end interactions. (C2H4 and C2H6 are both legitimate Your email address will not be published. These two compounds are cis-trans isomers (or geometric isomers), compounds that have different configurations (groups permanently in different places in space) because of the presence of a rigid structure in their molecule. Which of the following statements about resonance structures is not true? Step 1: How many atoms do we have in an ethylene molecule? The formal charges for each atom are drawn next to them in red for the final Lewis structure provided below. Fig. Isomers have different arrangement of both atoms and electrons. First know where the nonbonding electrons are, keep track of formal charges on atoms, and do not break sigma bonds. In the lewis structure of C2H4, there are only four C-H bonds, one C=C bond and no lone pairs on last shells. Therefore, We Ozone is represented by two different Lewis structures. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. The Journal of Physical Chemistry A 2010, 114 (14) , 4735-4741. For resonance structures there must be a double or triple bond. Depending on the nature of atoms and their tendency to attract or repel another atom of a similar or different kind, we get resultant molecular compounds. Here, we can see that one carbon atom has its octet fulfilled(the Octet rule has been discussed before). %PDF-1.3 So, to understand chemical bonding, only sketching a lewis structure diagram is not sufficient. Be it petroleum, crude oil, or natural gas, the majority of hydrocarbons are found naturally in these fossil fuels. [40] In this system, ethylene became ethene. All atoms in BrCl 3 have a formal charge of zero, and the sum of the formal charges totals zero, as it must in a neutral molecule. Add a multiple bond (first try a double bond) to see if the central atom can achieve an octet: Are there possible resonance structures? I have to draw the isomers or resonance structures. [24] By 2013, ethylene was produced by at least 117 companies in 32 countries. We can convert each lone pair to a bonding electron pair, which gives each atom an octet of electrons and a formal charge of 0, by making three C=C double bonds. The resonance structures are for a single molecule or ion and they are continuously change into each other and are not separable while Isomers are different compounds and can be separated in. Add octet electrons to the atoms bonded to the center atom: 4. A molecule that has several resonance structures is more stable than one with fewer. [30], Ethylene is produced from methionine in nature. H2CO vs. HCOH Isomers Energy: -113.1463H <HCO = 121.1 FIGURE 1 The equilibrium between formaldehyde and the HCOH carbene. Look the figures to understand each step. Remember, the best resonance structure is the one with the least formal charge. Single bonds, double bonds, triple bonds, +1 charges, -1 charges, these are our limitations in explaining the structures, and the true forms can be in between - a carbon-carbon bond could be mostly single bond with a little bit of double bond character and a partial negative charge, for example. Cl: 7 - (6 + (2)) = 0. The C2H4 molecule is non-polar in nature as all the atoms are symmetrically arranged across the molecule and both carbon atoms have the same influence on the bonded electrons. % When structures of butene are drawn with 120 bond angles around the sp 2-hybridized carbon atoms participating in the double bond, the isomers are apparent. These important details can ensure success in drawing any Resonance structure. They are drawn with a double-headed arrow between them to show the actual structure is somewhere between the resonance structures. [31], Ethylene is a fundamental ligand in transition metal alkene complexes. VSEPR theory explains the shape by minimizing the electronic repulsion. This is known as the octet rule or octet fulfillment. the total number of valence electrons in one molecule of C2H4. On a smaller scale, ethyltoluene, ethylanilines, 1,4-hexadiene, and aluminium alkyls. [citation needed], Major intermediates from the halogenation and hydrohalogenation of ethylene include ethylene dichloride, ethyl chloride, and ethylene dibromide. Have a look. In organic chemistry, we find hydrocarbons of several types: straight-chain, cyclic, and even branched. Because ethene is a neutral molecule, overall charge of the molecule should Step 4: We are done with the octet fulfillment concept. Move lone pair electrons toward a pi bond and when electrons can be moved in more than one direction, move them to the more electronegative atom. YES. 3. The overall charge of the molecule is, (-)1*1 + (+1) = 0. For ethene molecule, carbon has the highest valence than and hydrogen. And this whole process of two or more atoms coming close and deciding to stay together is known as chemical bonding. Legal. Many reactions of ethylene are catalyzed by transition metals, which bind transiently to the ethylene using both the and * orbitals. [12], Ethylene is oxidized to produce ethylene oxide, a key raw material in the production of surfactants and detergents by ethoxylation. lewis structure of ethene. The molecule is also relatively weak: rotation about the C-C bond is a very low energy process that requires breaking the -bond by supplying heat at 50C. Two resonance structures differ in the position of multiple bonds and non bonding electron. HNO2 Lewis Structure, Molecular Geometry, Hybridization, and Polarity, SF2 Lewis Structure, Molecular Geometry, Hybridization, Polarity, and MO Diagram. Apart from this, we can find them in synthetic polymers and other man-made plastic materials. It's impossible to form that particular combination of Ethene is the simplest alkene The Lewis Structure of any molecule can be easily done if we follow certain given procedures. Benzene has two resonance structures, showing the placements of the bonds. 372K views 12 years ago A step-by-step explanation of how to draw the C2H4 Lewis Dot Structure (Ethene). Here, we learned about how to draw the proper Lewis Structure and find out the molecular geometry of an ethylene molecule. The Rh-catalysed hydroformylation of ethylene is conducted on industrial scale to provide propionaldehyde. We need to focus on molecular geometry as well. We know that ozone has a V-shaped structure, so one O atom is central: 2. [8][9] Much of this production goes toward polyethylene, a widely used plastic containing polymer chains of ethylene units in various chain lengths. Resonance is a way of describing delocalized electrons within certain molecules or polyatomic ions where the bonding cannot be expressed by a single Lewis formula. Lewis dot structures for molecules with C atoms C is in Group IV and it forms 4 bonds: CH4C2H6 C3H8 C4H10 Since H is the most common atom found bonding with C we will sometimes simply show 4 bonds coming off of a C without explicitly showing the atom at the end of the bond. 2003-2023 Chegg Inc. All rights reserved. Structural Formulas . 3. Since there are two bonds forming here, we will have a double bond structure. Therefore, this structure is the lewis structure of ethene. The Nitrate ( NO 3) ion. )[38] The term olefiant gas is in turn the etymological origin of the modern word "olefin", the class of hydrocarbons in which ethylene is the first member. Resonance structures arise when there are more than one way to draw a Lewis dot diagram that satisfies the octet rule. Polyethylene, also called polyethene and polythene, is the world's most widely used plastic. Here, we have: Have you ever wondered how unique and vastly diverse the universe is? Put the least electronegative atom in the center. [16] In Europe and Asia, ethylene is obtained mainly from cracking naphtha, gasoil and condensates with the coproduction of propylene, C4 olefins and aromatics (pyrolysis gasoline). Resonance is a mental exercise and method within the Valence Bond Theory of bonding that describes the delocalization of electrons within molecules. The bonding orbital will see higher electron density which will hold the atoms together via nuclei attraction. Below is the video regarding the drawing of lewis structure of C2H4. An atom has a nucleus that is surrounded by negatively charged electrons which are present in different levels or shells. For hydrocarbons, we are always going to place the carbons in the center. Therefore, hydrogen The classic example is benzene in Example \(\PageIndex{1}\). It only shows that there is more than one way to draw the structure. Therefore, no addition or reduction of valence electrons due to charges. Only electrons move and the nuclei of the atoms never move. it completely. Curved arrow notation is used in showing the placement of electrons between atoms. After drawing the sketch, we should start to mark lone pairs on atoms. [18], Ethylene is a hormone that affects the ripening and flowering of many plants. As you will learn, if the bonds were of different types (one single and one double, for example), they would have different lengths. How many isomers does C2H4Cl2 have? Chemistry. Benzene is commonly seen in Organic Chemistry and it has a resonance form. Now, the atoms do not usually exist on their own in an isolated state, all we see around us are basically made up of atoms that have combined with each other to form molecules. They must make sense and agree to the rules. Experts are tested by Chegg as specialists in their subject area. Make sure the arrows are clear including the single and half headed arrow. [11], Major industrial reactions of ethylene include in order of scale: 1) polymerization, 2) oxidation, 3) halogenation and hydrohalogenation, 4) alkylation, 5) hydration, 6) oligomerization, and 7) hydroformylation. Assigning formal charges to an atom is very useful in resonance forms. ( the antibonding orbital remains empty). Therefore, it has four electrons in its valence shell. After drawing resonance structures check the net charge of all the structures. Once we know how many valence electrons there are in C2H4 we can distribute them around the central atom with the goal of filling the outer shells of each atom.In the Lewis structure of C2H4 structure there are a total of 12 valence electrons. [citation needed], Polyethylene consumes more than half of the world's ethylene supply. For. Complete octets on outside atoms.5. Going ahead, let us discuss this step by step. 6. This hydrocarbon has four hydrogen atoms bound to a pair of carbon atoms that are connected by a double bond. Following experimentation by Luckhardt, Crocker, and Carter at the University of Chicago,[41] ethylene was used as an anesthetic. Only electrons that can move are pi electrons, single unpaired electrons, and lone pair electrons. Therefore, there are five bonds The outermost shell is known as the valence shell and the electrons present in that shell are known as valence electrons. Before we jump right into this, we would like to introduce you to( or lets say brush you up with in case you are already familiar) some really important concepts that will make your understanding of ethylene bonding way easier! Q.4 Draw resonance hybrid structure of SO2 in two canonical forms. Experts are tested by Chegg as specialists in their subject area.
Mark Peacock Obituary,
How Many Calories In A Dave's Hot Chicken Tender,
Charlotte Johnson Wahl Funeral,
Rising Sign Calculator,
John Ruiz Richest Man In Florida,
Articles C
c2h4 isomers or resonance structures
You may use these HTML tags and attributes: <a href="" title=""> <abbr title=""> <acronym title=""> <b> <blockquote cite=""> <cite> <code> <del datetime=""> <em> <i> <q cite=""> <s> <strike> <strong>
Be the first to comment.