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Hydrogen chloride
The compound hydrogen chloride has the formula HCl. At room temperature, it is a colorless gas, which forms white fumes of hydrochloric acid upon contact with atmospheric humidity. Hydrogen chloride gas and hydrochloric acid are important in technology and industry. The formula HCl is often used to refer, somewhat misleadingly, to hydrochloric acid, an aqueous solution that can be derived from hydrogen chloride which has the formula HClaq.
Chemistry
Hydrogen chloride is composed of diatomic molecules, each consisting of a hydrogen atom H and a chlorine atom Cl connected by a covalent single bond. Since the chlorine atom is much more electronegative than the hydrogen atom, the covalent bond between the two atoms is quite polar. Consequently, the molecule has a large dipole moment with a negative partial charge δ− at the chlorine atom and a positive partial charge δ+ at the hydrogen atom. In part due to its high polarity, HCl is very soluble in water (and in other polar solvents).
Upon contact, H2O and HCl combine to form hydronium cations H3O+ and chloride anions Cl− through a reversible chemical reaction:
HCl + H2O → H3O+ + Cl−
The resulting solution is called hydrochloric acid and is a strong acid. The acid dissociation or ionization constant, Ka, is large, which means HCl dissociates or ionizes practically completely in water. Even in the absence of water, hydrogen chloride can still act as an acid. For example, hydrogen chloride can dissolve in certain other solvents such as methanol, protonate molecules or ions, and serve as an acid-catalyst for chemical reactions where anhydrous (water-free) conditions are desired.
HCl + CH3OH → CH3O+H2 + Cl−
Because of its acidic nature, hydrogen chloride is a corrosive gas, particularly in the presence of any moisture.
Structure and properties
The infrared spectrum of gaseous hydrogen chloride consists of a number of sharp absorption lines grouped around 2886 cm−1 (wavelength ~3.47 µm). The HCl molecule absorbs photons, and converts it to kinetic energy in the form of rotation and vibration, that becomes heat in collective behavior.
A chemical bond may be viewed simply as a spring with a certain Hooke's constant. However, due to quantum mechanical rules, only certain vibrational modes are permitted. The energy within this spring can be written thus:
E(v) = hνe(v + 1/2)
At room temperature, almost all molecules in the ground state v = 0. To promote an HCl molecule to the v = 1 state, we would expect to see an infrared absorption about 2880 cm−1. This absorption corresponding to the Q-branch is not observed due to it being forbidden due to symmetry. Instead, two sets of signals (P- and R-branches) are seen due to rotation of the molecules.
Due to quantum mechanical rules, only certain rotational modes are permitted. They are characterized by the rotational quantum number J = 0, 1, 2, 3, ... ΔJ can only take values of ± 1.
E(J) = h·B·J(J+1)
The value of B is much smaller than ν e, such that a much smaller amount of energy is required to rotate the molecule; for a typical molecule, this lies within the microwave region. However, due to the vibrational energy of this molecule, the set of absorptions lie within the infrared region, allowing a spectrum showing the rovibrational modes of this molecule to be easily collected using an ordinary infrared spectrometer with a conventional gas cell.
Plotting the assigned rotational quantum numbers (of fundamental transitions) of the R branch and P branch (J+1 and −J respectively) versus their energies (usually in cm−1) and taking a third order regression of the data allows for the calculation of the centrifugal distortion constant, moment of inertia, average bond length, the coupling constant, and other useful information.
Ptain, j'arrive pas à croire que t'es en train de lire ça, ta connerie dépasse donc largement la mienne... (bon je ne mets pas de smil ici, ça serait trop facile...)
One doublet due to isotopic composition of Chlorine.
Naturally abundant chlorine consists of two isotopes, 35Cl and 37Cl, in a ratio of approximately 3:1. While the spring constants are very similar, the reduced masses are different causing significant differences in the rotational energy, thus doublets are observed on close inspection of each absorption line, weighted in the same ratio of 3:1.
Production
Most hydrogen chloride produced on an industrial scale is used for hydrochloric acid production.
Direct synthesis
In the chlor-alkali industry, salt solution is electrolyzed producing chlorine (Cl2), sodium hydroxide, and hydrogen (H2). The pure chlorine gas can be re-combined in an HCl forming hydrogen chloride gas.
Cl2 + H2 → 2HCl
As the reaction is exothermic, the installation is called an HCl oven or HCl Burner. The resulting hydrogen chloride gas is absorbed in deionized water, resulting in chemically pure hydrochloric acid. This reaction can give a very pure product, e.g. for use in the food industry.
[edit]Organic synthesis
The largest production of hydrochloric acid is integrated with the formation of chlorinated and fluorinated organic compounds, e.g., Teflon, Freon, and other CFCs, as well as chloroacetic acid, and PVC. Often this production of hydrochloric acid is integrated with captive use of it on-site. In the chemical reactions, hydrogen atoms on the hydrocarbon are replaced by chlorine atoms, whereupon the released hydrogen atom recombines with the spare atom from the chlorine molecule, forming hydrogen chloride. Fluorination is a subsequent chlorine-replacement reaction, producing again hydrogen chloride.
R-H + Cl2 → R-Cl + HCl
R-Cl + HF → R-F + HCl
The resulting hydrogen chloride gas is either reused directly, or absorbed in water, resulting in hydrochloric acid of technical or industrial grade.
Laboratory methods
Small amounts of HCl gas for laboratory use can be generated in a HCl generator by dehydrating hydrochloric acid with either sulfuric acid or anhydrous calcium chloride. Alternatively, HCl can be generated by the reaction of sulfuric acid with sodium chloride:[1]
2NaCl + H2SO4 → Na2SO4 + 2HCl↑
HCl can also be prepared by the hydrolysis of certain reactive chloride compounds such as phosphorus chlorides, thionyl chloride (SOCl2), and acyl chlorides. Adding more water would absorb the HCl gas forming hydrochloric acid. For example, cold water can be gradually dripped onto phosphorus pentachloride (PCl5) to give HCl in this reaction:
PCl5 + H2O → POCl3 + 2HCl
Hot water could liberate more HCl by hydrolyzing PCl5 all the way to ortho-phosphoric acid. Reaction of water with phosphorus trichloride (PCl3) also yields HCl. Reaction of thionyl chloride with water would give sulfur dioxide (SO2) gas as well as HCl. For the reactions of thionyl chloride or acyl chlorides with water, see thionyl chloride or acyl halide.
Applications
Most hydrogen chloride is used in the production of hydrochloric acid. It is also an important reagent in other industrial chemical transformations, e.g.:
Hydrochlorination of rubber
Production of vinyl and alkyl chlorides
In the semiconductor industry, it is used to both etch semiconductor crystals and to purify silicon via SiHCl3.
It may also be used to treat cotton to delint it, and to separate it from wool.[citation needed]
Where anhydrous hydrogen chloride is desired for small scale laboratory work, the gas is available in cylinders.
History
Alchemists of the Middle Ages recognized that hydrochloric acid (then known as spirit of salt or acidum salis) released vaporous hydrogen chloride, which was called marine acid air. In the 17th century, Johann Rudolf Glauber used salt (sodium chloride) and sulfuric acid for the preparation of sodium sulfate, releasing hydrogen chloride gas (see production, below). In 1772, Carl Wilhelm Scheele also reported this reaction and is sometimes credited with its discovery. Joseph Priestley prepared hydrogen chloride in 1772, and in 1810 Humphry Davy established that it is composed of hydrogen and chlorine.[2]
During the Industrial Revolution, demand for alkaline substances such as soda ash increased, and Nicolas Leblanc developed a new industrial-scale process for producing the soda ash. In the Leblanc process, salt was converted to soda ash, using sulfuric acid, limestone, and coal, giving hydrogen chloride as by-product. Initially, this gas was vented to air, but the Alkali Act of 1863 prohibited such release, so then soda ash producers absorbed the HCl waste gas in water, producing hydrochloric acid on an industrial scale. Later, the Hargreaves process was developed, which is similar to the Leblanc process except sulfur dioxide, water, and air are used instead of sulfuric acid in a reaction which is exothermic overall. In the early 20th century the Leblanc process was effectively replaced by the Solvay process, which did not produce HCl. However, hydrogen chloride production continued as a step in hydrochloric acid production.
Historical uses of hydrogen chloride in the 20th century include hydrochlorinations of alkynes in producing the chlorinated monomers chloroprene and vinyl chloride, which are subsequently polymerized to make polychloroprene (Neoprene) and polyvinyl chloride (PVC), respectively. In the production of vinyl chloride, acetylene (C2H2) is hydrochlorinated by adding the HCl across the triple bond of the C2H2 molecule, turning the triple into a double bond, yielding vinyl chloride.
The "acetylene process", used until the 1960s for making chloroprene, starts out by joining two acetylene molecules, and then adds HCl to the joined intermediate across the triple bond to convert it to chloroprene as shown here:
This "acetylene process" has been replaced by a process which adds Cl2 to one of the double bonds in 1,3-butadiene instead, and subsequent elimination produces HCl instead, as well as chloroprene.
Safety
Hydrogen chloride forms corrosive hydrochloric acid on contact with water found in body tissue. Inhalation of the fumes can cause coughing, choking, inflammation of the nose, throat, and upper respiratory tract, and in severe cases, pulmonary edema, circulatory system failure, and death. Skin contact can cause redness, pain, and severe skin burns. Hydrogen chloride may cause severe burns to the eye and permanent eye damage.
The compound hydrogen chloride has the formula HCl. At room temperature, it is a colorless gas, which forms white fumes of hydrochloric acid upon contact with atmospheric humidity. Hydrogen chloride gas and hydrochloric acid are important in technology and industry. The formula HCl is often used to refer, somewhat misleadingly, to hydrochloric acid, an aqueous solution that can be derived from hydrogen chloride which has the formula HClaq.
Chemistry
Hydrogen chloride is composed of diatomic molecules, each consisting of a hydrogen atom H and a chlorine atom Cl connected by a covalent single bond. Since the chlorine atom is much more electronegative than the hydrogen atom, the covalent bond between the two atoms is quite polar. Consequently, the molecule has a large dipole moment with a negative partial charge δ− at the chlorine atom and a positive partial charge δ+ at the hydrogen atom. In part due to its high polarity, HCl is very soluble in water (and in other polar solvents).
Upon contact, H2O and HCl combine to form hydronium cations H3O+ and chloride anions Cl− through a reversible chemical reaction:
HCl + H2O → H3O+ + Cl−
The resulting solution is called hydrochloric acid and is a strong acid. The acid dissociation or ionization constant, Ka, is large, which means HCl dissociates or ionizes practically completely in water. Even in the absence of water, hydrogen chloride can still act as an acid. For example, hydrogen chloride can dissolve in certain other solvents such as methanol, protonate molecules or ions, and serve as an acid-catalyst for chemical reactions where anhydrous (water-free) conditions are desired.
HCl + CH3OH → CH3O+H2 + Cl−
Because of its acidic nature, hydrogen chloride is a corrosive gas, particularly in the presence of any moisture.
Structure and properties
The infrared spectrum of gaseous hydrogen chloride consists of a number of sharp absorption lines grouped around 2886 cm−1 (wavelength ~3.47 µm). The HCl molecule absorbs photons, and converts it to kinetic energy in the form of rotation and vibration, that becomes heat in collective behavior.
A chemical bond may be viewed simply as a spring with a certain Hooke's constant. However, due to quantum mechanical rules, only certain vibrational modes are permitted. The energy within this spring can be written thus:
E(v) = hνe(v + 1/2)
At room temperature, almost all molecules in the ground state v = 0. To promote an HCl molecule to the v = 1 state, we would expect to see an infrared absorption about 2880 cm−1. This absorption corresponding to the Q-branch is not observed due to it being forbidden due to symmetry. Instead, two sets of signals (P- and R-branches) are seen due to rotation of the molecules.
Due to quantum mechanical rules, only certain rotational modes are permitted. They are characterized by the rotational quantum number J = 0, 1, 2, 3, ... ΔJ can only take values of ± 1.
E(J) = h·B·J(J+1)
The value of B is much smaller than ν e, such that a much smaller amount of energy is required to rotate the molecule; for a typical molecule, this lies within the microwave region. However, due to the vibrational energy of this molecule, the set of absorptions lie within the infrared region, allowing a spectrum showing the rovibrational modes of this molecule to be easily collected using an ordinary infrared spectrometer with a conventional gas cell.
Plotting the assigned rotational quantum numbers (of fundamental transitions) of the R branch and P branch (J+1 and −J respectively) versus their energies (usually in cm−1) and taking a third order regression of the data allows for the calculation of the centrifugal distortion constant, moment of inertia, average bond length, the coupling constant, and other useful information.
Ptain, j'arrive pas à croire que t'es en train de lire ça, ta connerie dépasse donc largement la mienne... (bon je ne mets pas de smil ici, ça serait trop facile...)
One doublet due to isotopic composition of Chlorine.
Naturally abundant chlorine consists of two isotopes, 35Cl and 37Cl, in a ratio of approximately 3:1. While the spring constants are very similar, the reduced masses are different causing significant differences in the rotational energy, thus doublets are observed on close inspection of each absorption line, weighted in the same ratio of 3:1.
Production
Most hydrogen chloride produced on an industrial scale is used for hydrochloric acid production.
Direct synthesis
In the chlor-alkali industry, salt solution is electrolyzed producing chlorine (Cl2), sodium hydroxide, and hydrogen (H2). The pure chlorine gas can be re-combined in an HCl forming hydrogen chloride gas.
Cl2 + H2 → 2HCl
As the reaction is exothermic, the installation is called an HCl oven or HCl Burner. The resulting hydrogen chloride gas is absorbed in deionized water, resulting in chemically pure hydrochloric acid. This reaction can give a very pure product, e.g. for use in the food industry.
[edit]Organic synthesis
The largest production of hydrochloric acid is integrated with the formation of chlorinated and fluorinated organic compounds, e.g., Teflon, Freon, and other CFCs, as well as chloroacetic acid, and PVC. Often this production of hydrochloric acid is integrated with captive use of it on-site. In the chemical reactions, hydrogen atoms on the hydrocarbon are replaced by chlorine atoms, whereupon the released hydrogen atom recombines with the spare atom from the chlorine molecule, forming hydrogen chloride. Fluorination is a subsequent chlorine-replacement reaction, producing again hydrogen chloride.
R-H + Cl2 → R-Cl + HCl
R-Cl + HF → R-F + HCl
The resulting hydrogen chloride gas is either reused directly, or absorbed in water, resulting in hydrochloric acid of technical or industrial grade.
Laboratory methods
Small amounts of HCl gas for laboratory use can be generated in a HCl generator by dehydrating hydrochloric acid with either sulfuric acid or anhydrous calcium chloride. Alternatively, HCl can be generated by the reaction of sulfuric acid with sodium chloride:[1]
2NaCl + H2SO4 → Na2SO4 + 2HCl↑
HCl can also be prepared by the hydrolysis of certain reactive chloride compounds such as phosphorus chlorides, thionyl chloride (SOCl2), and acyl chlorides. Adding more water would absorb the HCl gas forming hydrochloric acid. For example, cold water can be gradually dripped onto phosphorus pentachloride (PCl5) to give HCl in this reaction:
PCl5 + H2O → POCl3 + 2HCl
Hot water could liberate more HCl by hydrolyzing PCl5 all the way to ortho-phosphoric acid. Reaction of water with phosphorus trichloride (PCl3) also yields HCl. Reaction of thionyl chloride with water would give sulfur dioxide (SO2) gas as well as HCl. For the reactions of thionyl chloride or acyl chlorides with water, see thionyl chloride or acyl halide.
Applications
Most hydrogen chloride is used in the production of hydrochloric acid. It is also an important reagent in other industrial chemical transformations, e.g.:
Hydrochlorination of rubber
Production of vinyl and alkyl chlorides
In the semiconductor industry, it is used to both etch semiconductor crystals and to purify silicon via SiHCl3.
It may also be used to treat cotton to delint it, and to separate it from wool.[citation needed]
Where anhydrous hydrogen chloride is desired for small scale laboratory work, the gas is available in cylinders.
History
Alchemists of the Middle Ages recognized that hydrochloric acid (then known as spirit of salt or acidum salis) released vaporous hydrogen chloride, which was called marine acid air. In the 17th century, Johann Rudolf Glauber used salt (sodium chloride) and sulfuric acid for the preparation of sodium sulfate, releasing hydrogen chloride gas (see production, below). In 1772, Carl Wilhelm Scheele also reported this reaction and is sometimes credited with its discovery. Joseph Priestley prepared hydrogen chloride in 1772, and in 1810 Humphry Davy established that it is composed of hydrogen and chlorine.[2]
During the Industrial Revolution, demand for alkaline substances such as soda ash increased, and Nicolas Leblanc developed a new industrial-scale process for producing the soda ash. In the Leblanc process, salt was converted to soda ash, using sulfuric acid, limestone, and coal, giving hydrogen chloride as by-product. Initially, this gas was vented to air, but the Alkali Act of 1863 prohibited such release, so then soda ash producers absorbed the HCl waste gas in water, producing hydrochloric acid on an industrial scale. Later, the Hargreaves process was developed, which is similar to the Leblanc process except sulfur dioxide, water, and air are used instead of sulfuric acid in a reaction which is exothermic overall. In the early 20th century the Leblanc process was effectively replaced by the Solvay process, which did not produce HCl. However, hydrogen chloride production continued as a step in hydrochloric acid production.
Historical uses of hydrogen chloride in the 20th century include hydrochlorinations of alkynes in producing the chlorinated monomers chloroprene and vinyl chloride, which are subsequently polymerized to make polychloroprene (Neoprene) and polyvinyl chloride (PVC), respectively. In the production of vinyl chloride, acetylene (C2H2) is hydrochlorinated by adding the HCl across the triple bond of the C2H2 molecule, turning the triple into a double bond, yielding vinyl chloride.
The "acetylene process", used until the 1960s for making chloroprene, starts out by joining two acetylene molecules, and then adds HCl to the joined intermediate across the triple bond to convert it to chloroprene as shown here:
This "acetylene process" has been replaced by a process which adds Cl2 to one of the double bonds in 1,3-butadiene instead, and subsequent elimination produces HCl instead, as well as chloroprene.
Safety
Hydrogen chloride forms corrosive hydrochloric acid on contact with water found in body tissue. Inhalation of the fumes can cause coughing, choking, inflammation of the nose, throat, and upper respiratory tract, and in severe cases, pulmonary edema, circulatory system failure, and death. Skin contact can cause redness, pain, and severe skin burns. Hydrogen chloride may cause severe burns to the eye and permanent eye damage.
ppfffllllllllll... j" ai un petit boulet minable a mes pieds, une curiosité.
![[Vezøul]Numerø41](/data/avatars/m/29/29556.jpg?1125588453){kind=avatar}
Un organe est un ensemble de tissus concourant à la réalisation d'une fonction physiologique. Le niveau d'organisation supérieur à l'organe est le système, qui remplit un ensemble de fonctions complémentaires et le niveau d'organisation inférieur à l'organe est le tissu.
Sommaire
* 1 Organes humains par région
o 1.1 Région de la tête et du cou
o 1.2 Région dorsale et moelle
o 1.3 Thorax
o 1.4 Abdomen
o 1.5 Bassin
o 1.6 Membres
* 2 Organes humains par fonction
o 2.1 Les Fonctions physiologiques
o 2.2 Organes d'approvisionnement
o 2.3 Organes de consommation
o 2.4 Organes d'élimination
o 2.5 Organes non-classés
* 3 Organes des végétaux
* 4 Organe artificiel
* 5 Organes virtuels
* 6 Niveau des organes
* 7 Notes et références
* 8 Voir aussi
o 8.1 Articles connexes
o 8.2 Liens externes
Organes humains par région
Région de la tête et du cou
Un il humain
* os du crâne,
* face (anatomie),
* orbite,
* il,
* bouche,
* langue,
* dents,
* nez,
* oreilles,
* scalp,
* larynx,
* pharynx,
* glandes salivaires,
* méninges,
* cerveau,
* glande thyroïde,
* glandes parathyroïdes.
Région dorsale et moelle
* vertèbre,
* moelle épinière.
Thorax
* glande mammaire,
* côtes,
* poumons,
* cur,
* médiastin,
* sophage,
* diaphragme.
Abdomen
* Parois du corps,
* péritoine,
* estomac,
* duodénum,
* intestin,
* côlon,
* foie,
* vésicule biliaire
* rate,
* pancréas,
* reins,
* glandes surrénales.
Bassin
* bassin osseux,
* sacrum,
* coccyx,
* ovaires,
* trompe de Fallope,
* utérus,
* vagin,
* vulve,
* clitoris,
* périnée,
* vessie,
* testicules,
* verge,
* rectum,
* pénis.
Membres
* muscle,
* Squelette humain,
* nerfs,
* main,
* poignet,
* coude,
* épaule,
* hanche,
* genou,
* cheville.
Organes humains par fonction
Les Fonctions physiologiques
Les fonctions physiologiques sont :
* Digestion
* Goût
* Irrigation sanguine
* Odorat
* Ouïe
* Régulation de la glycémie
* Respiration
* Toucher
* Vue
Organes d'approvisionnement
* Poumons
Organes de consommation
* Cerveau
* Muscles
Organes d'élimination
* Foie
* Reins
* Peau
* Intestin
* Vessie urinaire
Organes non-classés
* Cur
* il
* Oreille
* Estomac
* Pénis
* Testicules
* Pancréas
Organes des végétaux
* Racines
* Rhizome
* Tronc
* Tige
* Branche
* Feuille
* Fleur
* Pistil
* Pétale
* Fruit
* Graine
Organe artificiel
Fabriqué par l'homme
* Appareil destiné à remplacer un organe chez un être vivant.
* Sous-ensemble d'un appareillage, composé de plusieurs pièces assemblées, destiné à effectuer une opération particulière ou un travail spécifique.
o Mécanique (« transmission », organe de mécanique automobile)
o Électrique (organe de commande) interrupteur, régulateur.
Organes virtuels
Par extension, on parlera d'organe dans le cadre des organisations humaines (exemple : organe de presse).
Niveau des organes
La structure des organismes biologiques qui constituent la biosphère peut être décomposée en plusieurs niveaux d'organisation : atomique, moléculaire, cellulaire, tissulaire, des organes, des systèmes, et enfin celui de l'organisme dans sa totalité fonctionnelle.
L'étude scientifique du vivant se fait par des recherches sur les éléments de chacun de ces niveaux, puis par la compréhension des interactions entre ces différents niveaux (voir l'article Méthode scientifique).
L'étude du niveau des organes permet de comprendre la structure, la fonction et le fonctionnement des organes, qui constituent les différents systèmes fonctionnels de l'organisme (système nerveux, système digestif, système immunitaire ).
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Mais casse toi on te dit !
C'est pas comme si c'était la première fois qu'on te le disait, en plus.
Tu aimes tant que ça passer pour un con ?
C'est dingue quand même…
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L' oubli de la situation, il est face a un cercueuil, on le prend en photo, et il sourit, oubliant littéralement que ce n' est pas l' endroit vraiment approprié .
Quand a machin katrol, je me fous totalement de tout ce que tu peux dire.
J'ai compris. C'est par ce que le gros, en plus d'être gros, il rigole devant le mort. Et le mort, comme il est mort, il voit pas que le gros morceau se fout d'sa gueule, à ce mort sot.
C'est complètement diabolique !
Reste maintenant à établir le rôle des fleurs là-dedans.
Edit. Merci de l'esplication, Patlek. Faut avouer que c'était patleklair. :zen:
C'est complètement diabolique !
Reste maintenant à établir le rôle des fleurs là-dedans.
Edit. Merci de l'esplication, Patlek. Faut avouer que c'était patleklair. :zen:
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Ouais.
OK.
Quand on a la tête à l'envers, pas sûr qu'on puisse trop réfléchir à ce qui serait "approprié", on agit par réflexe, par habitude, on sourit pour la photo.
Et puis, cette notion d'attitude "appropriée"...
'fin, bref, le côté "marrant" m'avait complètement échappé.
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Tant mieux, connard.
Tant mieux. Ça me ferait chier d'imaginer que tu puisses m'apprécier.
Maintenant que tu as compris que tout le monde te prend pour un crétin, faut faire quoi ?
Demander ta démission dès que tu seras passé au 20 heures pour démentir ?
Allez. Ouste, tu nous fatigues la patience.
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.....mais ne voit-on pas ses yeux rougis par les larmes?
..ce qui prouve qu'en fait cette photo prise est la démonstration d'un attachement affectif très fort et que c'est en somme une sorte d'ultime geste d'amitié.
Ce sourire, loin d'être inepte, est plutôt l'expression d'un sentiment sincère.
D'ailleurs, traditionnellement, à l'époque où la photo ne servait pas qu'à dire bonjour madame, photographier les morts sur leur catafalque était pour la famille le dernier souvenir de la présence du défunt dans leur vie....plus tard on y introduisit les petits gâteaux, les vins fins et la cérémonie funéraire devenait l'occasion d'une fête familiale, où le souvenir du disparu n'était qu'un prétexte à une beuverie mondaine.
Chose que Brel à très bien rendu dans son hommage à l'Émile"
Par ailleurs, des études sérieuses ont prouvées que ce type de réunion exacerbait le désir sexuel, une certaine promiscuité avec le cadavre renvoyait les convives à leur propre impermanence, provoquant le besoin quasi irrépressible de se sentir eux mêmes en vie. Et quelle meilleure façon d'y parvenir que le sexe. La prochaine fois que vous assisterez donc à une veillée mortuaire, ne culpabilisez donc plus d'avoir une grosse envie de défourailer bobonne dans la voiture, en lui mettant sa race et en lâchant tout sur sa voilette de deuil. Mon Doc que ça fait du bien et qu'on se sent viiiiivre !
En conclusion, je ne qualifierai donc pas cette image de pathétique, ni de comique.
J'y vois tout simplement un ami heureux de pouvoir garder un souvenir. Et le sourire affiché est un pied de nez à la mocheté de la mort présente, laissant en plus filtrer l'espoir de ce jeune homme de pouvoir enfin tirer un coup.
:zen:
..ce qui prouve qu'en fait cette photo prise est la démonstration d'un attachement affectif très fort et que c'est en somme une sorte d'ultime geste d'amitié.
Ce sourire, loin d'être inepte, est plutôt l'expression d'un sentiment sincère.
D'ailleurs, traditionnellement, à l'époque où la photo ne servait pas qu'à dire bonjour madame, photographier les morts sur leur catafalque était pour la famille le dernier souvenir de la présence du défunt dans leur vie....plus tard on y introduisit les petits gâteaux, les vins fins et la cérémonie funéraire devenait l'occasion d'une fête familiale, où le souvenir du disparu n'était qu'un prétexte à une beuverie mondaine.
Chose que Brel à très bien rendu dans son hommage à l'Émile"
Par ailleurs, des études sérieuses ont prouvées que ce type de réunion exacerbait le désir sexuel, une certaine promiscuité avec le cadavre renvoyait les convives à leur propre impermanence, provoquant le besoin quasi irrépressible de se sentir eux mêmes en vie. Et quelle meilleure façon d'y parvenir que le sexe. La prochaine fois que vous assisterez donc à une veillée mortuaire, ne culpabilisez donc plus d'avoir une grosse envie de défourailer bobonne dans la voiture, en lui mettant sa race et en lâchant tout sur sa voilette de deuil. Mon Doc que ça fait du bien et qu'on se sent viiiiivre !
En conclusion, je ne qualifierai donc pas cette image de pathétique, ni de comique.
J'y vois tout simplement un ami heureux de pouvoir garder un souvenir. Et le sourire affiché est un pied de nez à la mocheté de la mort présente, laissant en plus filtrer l'espoir de ce jeune homme de pouvoir enfin tirer un coup.
:zen:
Ha, mais çà colle pire que du chewing gum ce truc là.
Je vais finir par penser que ce machin est amoureux de moi (!!, le drame!!!)
Allez, pour info, la photo: c' est moi a l' enterrement de blackcat, les yeux rougis par les larmes de crocodile.
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