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lgbasallote

  • 2 years ago

Which of the following is NOT soluble in water? A) NaCl B) KBr C) CH3CH2OH D) HCl E) C6H6 and how do i know?

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  1. lgbasallote
    • 2 years ago
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    i know for sure it's not A

  2. cwrw238
    • 2 years ago
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    its C6H6 (benzene)

  3. lgbasallote
    • 2 years ago
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    since when did you go green o.O

  4. lgbasallote
    • 2 years ago
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    and why do you say so/

  5. cwrw238
    • 2 years ago
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    yesterday

  6. cwrw238
    • 2 years ago
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    why do i say its benzene?

  7. lgbasallote
    • 2 years ago
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    yes...how would you know?

  8. lgbasallote
    • 2 years ago
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    im thinking it would have something to do with adhesion and cohesion? or no?

  9. cwrw238
    • 2 years ago
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    ok KBr is a soluble salt - an ionic compound ch3ch2oh is alcohol - it mixes well with my whisky benzene is a liquid which if you add to water forms a separate layer its an aromatic organic compound

  10. lgbasallote
    • 2 years ago
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    ok...assuming i have no idea what you just said and i lack the experience to think like that...how else can i know?

  11. cwrw238
    • 2 years ago
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    hmm - well all i can say its a hydrocarbon which are not usually soluble in water.

  12. lgbasallote
    • 2 years ago
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    im thinking it has something to do with cohesion-adhesion or hydrogen bonding or IMFA or something >.<

  13. lgbasallote
    • 2 years ago
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    im so confused

  14. cwrw238
    • 2 years ago
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    yes - benzene would not take part in hydrogen bonding - that might be it - the molecule is hexagonal and very stable. sorry i can't be of more help

  15. lgbasallote
    • 2 years ago
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    why do you say stable? and what does stability have anything to do with h-bonding?

  16. cwrw238
    • 2 years ago
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    benzene does not react with water at room temperature and only reacts with strong reagents at elevated temperatures the hexagonal arrangement makes for strong bonding.

  17. lgbasallote
    • 2 years ago
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    well im gonna need a more general answer :(

  18. lgbasallote
    • 2 years ago
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    what makes a compound not react with water

  19. cwrw238
    • 2 years ago
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    in alcohol for instance the hydrogen in OH bit is partially charge and attacks the H3O ion in the water. this can't happen with benzene

  20. cwrw238
    • 2 years ago
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    *attracts not attacks

  21. cwrw238
    • 2 years ago
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    gotta go now - my chemistry knowledge is pretty rusty I'm afraid

  22. lgbasallote
    • 2 years ago
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    aww ok

  23. SanjanaP
    • 2 years ago
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    I think It is C6H6 I think that is right :O

  24. lgbasallote
    • 2 years ago
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    HOW to know which it is? im not really interested what the answer is

  25. NotTim
    • 2 years ago
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    why not just use a solubility table? most textbooks are provided witt one in the appendix...

  26. lgbasallote
    • 2 years ago
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    this is for a quiz...we dont have books in quizzes...i need to know HOW

  27. NotTim
    • 2 years ago
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    ...

  28. NotTim
    • 2 years ago
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    am i allowed answering this?

  29. lgbasallote
    • 2 years ago
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    what do you mean?

  30. NotTim
    • 2 years ago
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    am i allowed answerign things related to marked papers?

  31. lgbasallote
    • 2 years ago
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    this isnt a marked paper

  32. lgbasallote
    • 2 years ago
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    im trying to review for my quiz in a few hours

  33. lgbasallote
    • 2 years ago
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    what i was saying was that in our quiz we dont have books with solubilty table thingies so i shouldnt rely on it

  34. lgbasallote
    • 2 years ago
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    anyway my question is just "HOW TO KNOW WHICH COMPUOUND IS SOLUBLE AND WHICH IS NOT"

  35. GOODMAN
    • 2 years ago
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    Wow.

  36. lgbasallote
    • 2 years ago
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    ?

  37. GOODMAN
    • 2 years ago
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    Goodluck :D

  38. lgbasallote
    • 2 years ago
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    lol :p

  39. NotTim
    • 2 years ago
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    I was provided a solubility charts eh, for my examination.... http://en.wikipedia.org/wiki/Solubility_chart

  40. lgbasallote
    • 2 years ago
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    but without a solubility chart...how to know?

  41. NotTim
    • 2 years ago
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    i think it was related to the ions and charges tho. to figure it out

  42. lgbasallote
    • 2 years ago
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    im assuming it has something to do with hydrogen bonding or something

  43. lgbasallote
    • 2 years ago
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    but none of the elements are ions o.O

  44. NotTim
    • 2 years ago
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    Ahem. Wikipedia is my source. Please do not quote me on this.

  45. NotTim
    • 2 years ago
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    Solubility of ionic compounds in water Main article: Solubility chart Main article: Solubility table Some ionic compounds (salts) dissolve in water, which arises because of the attraction between positive and negative charges (see: solvation). For example, the salt's positive ions (e.g. Ag+) attract the partially negative oxygens in H2O. Likewise, the salt's negative ions (e.g. Cl−) attract the partially positive hydrogens in H2O. Note: oxygen is partially negative because it is more electronegative than hydrogen, and vice-versa (see: chemical polarity). AgCl(s) Ag+(aq) + Cl−(aq) However, there is a limit to how much salt can be dissolved in a given volume of water. This amount is given by the solubility product, Ksp. This value depends on the type of salt (AgCl vs. NaCl, for example), temperature, and the common ion effect. One can calculate the amount of AgCl that will dissolve in 1 liter of water, some algebra is required. Ksp = [Ag+] × [Cl−] (definition of solubility product) Ksp = 1.8 × 10−10 (from a table of solubility products) [Ag+] = [Cl−], in the absence of other silver or chloride salts, [Ag+]2 = 1.8 × 10−10 [Ag+] = 1.34 × 10−5 The result: 1 liter of water can dissolve 1.34 × 10−5 moles of AgCl(s) at room temperature. Compared with other types of salts, AgCl is poorly soluble in water. In contrast, table salt (NaCl) has a higher Ksp and is, therefore, more soluble. Soluble Insoluble Group I and NH4+ compounds Carbonates (Except Group I, NH4+ and uranyl compounds) Nitrates Sulfites (Except Group I and NH4+ compounds) Acetates (Ethanoates) (Except Ag+ compounds) Phosphates (Except Group I and NH4+ compounds) Chlorides (Chlorates and Perchlorates), bromides and iodides (Except Ag+, Pb2+, Cu+ and Hg22+) Hydroxides and oxides (Except Group I, NH4+, Ba2+, Sr2+ and Tl+) Sulfates (Except Ag+, Pb2+, Ba2+, Sr2+ and Ca2+) Sulfides (Except Group I, Group II and NH4+ compounds) Hydroxides (Only with (aq) Ba2+, Li+, Na+, K+, Rb+, Cs+, Fr+ )

  46. NotTim
    • 2 years ago
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    http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water

  47. lgbasallote
    • 2 years ago
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    hmm so it's ion induced dipole huh

  48. lgbasallote
    • 2 years ago
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    wonder how i'll know when it happens :/

  49. NotTim
    • 2 years ago
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    possibly the molecule's attraction to the hydrogen in water makes it more soluble?

  50. lgbasallote
    • 2 years ago
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    how would i know that by llooking at the compounds?

  51. NotTim
    • 2 years ago
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    maybe not by looking at the compounds, but the periodic table?

  52. lgbasallote
    • 2 years ago
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    what do you mean?

  53. NotTim
    • 2 years ago
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    wait..that's electronegativity, charges and such...

  54. lgbasallote
    • 2 years ago
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    yeah...

  55. NotTim
    • 2 years ago
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    wait...

  56. NotTim
    • 2 years ago
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    For example, the salt's positive ions (e.g. Ag+) attract the partially negative oxygens in H2O. Likewise, the salt's negative ions (e.g. Cl−) attract the partially positive hydrogens in H2O. Note: oxygen is partially negative because it is more electronegative than hydrogen, and vice-versa (see: chemical polarity). AgCl(s) Ag+(aq) + Cl−(aq)

  57. NotTim
    • 2 years ago
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    However, there is a limit to how much salt can be dissolved in a given volume of water. This amount is given by the solubility product, Ksp. This value depends on the type of salt (AgCl vs. NaCl, for example), temperature, and the common ion effect. One can calculate the amount of AgCl that will dissolve in 1 liter of water, some algebra is required. Ksp = [Ag+] × [Cl−] (definition of solubility product) Ksp = 1.8 × 10−10 (from a table of solubility products)

  58. NotTim
    • 2 years ago
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    The result: 1 liter of water can dissolve 1.34 × 10−5 moles of AgCl(s) at room temperature. Compared with other types of salts, AgCl is poorly soluble in water. In contrast, table salt (NaCl) has a higher Ksp and is, therefore, more soluble.

  59. NotTim
    • 2 years ago
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    In relation to the points I posted: 1. Electronegativity DOEs play a role in solubility. 2. Using Ksp to find solubility. 3. Is a Ksp table provided?

  60. zbay
    • 2 years ago
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    with out looking it up i'm saying e is not soluble because it's molecular

  61. lgbasallote
    • 2 years ago
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    what do you mean molecular?

  62. zbay
    • 2 years ago
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    it's a metal bonded to a non metal

  63. lgbasallote
    • 2 years ago
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    you mean an ionic bond?

  64. lgbasallote
    • 2 years ago
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    but NaCl is ionic too...

  65. lgbasallote
    • 2 years ago
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    and wait...isnt c6h6 nonmetal + nonmetal?

  66. NotTim
    • 2 years ago
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    c6h6 is a organic compound...

  67. zbay
    • 2 years ago
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    right and it wont disolbe in water

  68. lgbasallote
    • 2 years ago
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    because it's nonmetal + nonmetal?

  69. NotTim
    • 2 years ago
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    i think so...i don't think hexane, octane, etc dissolves easily in water...it just floats on top right

  70. lgbasallote
    • 2 years ago
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    but HCl is non metal + nonmetal too...

  71. zbay
    • 2 years ago
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    hcl is a strong acid so it totaly ionizes

  72. NotTim
    • 2 years ago
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    HCl is an acid.

  73. NotTim
    • 2 years ago
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    and when added with water, loses its H, making it Cl2, and causes the water to become hydronium

  74. lgbasallote
    • 2 years ago
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    but zbay said c6h6 does not dissolve because it's metal + nonmetal but NaCl is metal + nonmetal too if it's nonmetal + nonmetal HCl is nonmetal + nonmetal too

  75. lgbasallote
    • 2 years ago
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    so what's the reason c6h6 does not dissolve?

  76. zbay
    • 2 years ago
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    i ment non metal non metal or molecular, and hcl is a strong acid making very soluble

  77. NotTim
    • 2 years ago
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    Well, for one, It's got tons of hydrogen bonding...

  78. zbay
    • 2 years ago
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    because its molecular and because of that it doesn't disolve in water.

  79. NotTim
    • 2 years ago
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    course, we may just be mixing this all up...I suggest the solubility table...

  80. lgbasallote
    • 2 years ago
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    but why does HCl dissolve in water if it's molecular too?

  81. NotTim
    • 2 years ago
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    It's simpler-less hydrogen bonds.

  82. NotTim
    • 2 years ago
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    only 1, compared to 6 in c6h6

  83. zbay
    • 2 years ago
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    Hydrogen can act as a metal or non-metal so in this case it's acting as a metal

  84. zbay
    • 2 years ago
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    hydrogen bonding is a IMF and has nothing to do with that Tim

  85. NotTim
    • 2 years ago
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    wats imf? it doesn't matter?

  86. NotTim
    • 2 years ago
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    ...it doesn't matter whether or not its metal does it? just the electronegativities?

  87. zbay
    • 2 years ago
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    an IMF is a intramolecular force and is responsible for how molecules behave around each other

  88. NotTim
    • 2 years ago
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    isn't that important for solubility, as we are looking for the chemicals' ability to be dissolved in water. Whatever affects the forces must affect the solubility too right?

  89. lgbasallote
    • 2 years ago
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    so how does IMF affect ths situation?

  90. zbay
    • 2 years ago
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    IMF has nothing to do with solubility, we are just trying to figure out if something will disolve here. So by a just remember that if the compound is molecular it doesn't disolve.

  91. NotTim
    • 2 years ago
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    Polarity?

  92. NotTim
    • 2 years ago
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    Nitrates, acetates, and ammonium though DO dissolve

  93. NotTim
    • 2 years ago
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    in water

  94. zbay
    • 2 years ago
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    look i'm not trying to debate this all night the answer to the questoin is e in my opinion. There are other exeptions to these rules but the majority of the time just find the molecular compound and assume it wont be soluble. if you want to read about all the exeptions google solubilty rules

  95. NotTim
    • 2 years ago
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    http://en.wikipedia.org/wiki/Solubility#Solubility_of_ionic_compounds_in_water

  96. NotTim
    • 2 years ago
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    (Solubility table!)

  97. Outkast3r09
    • 2 years ago
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    -_- It has to do with the bonds/the charge of the polyatomic ions of the Chemicals. If you say otherwise you don't understand what happens when you dissolve a compound.

  98. lgbasallote
    • 2 years ago
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    me? yeah i really dont

  99. Outkast3r09
    • 2 years ago
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    It has with the polarity of h2o pulling the positive ions from the compound

  100. Outkast3r09
    • 2 years ago
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    or the cations i should say

  101. Kryten
    • 2 years ago
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    i didnt read all answers but you can take guidence in this rule: similar is soluble in similar by which i mean POLARITY!!! polar molecules will dissolve in water while non polar in non polar solutes like benzene, toluene, THF(tetra hydro furane)...

  102. foodscientist
    • 2 years ago
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    like dissolves like..

  103. lgbasallote
    • 2 years ago
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    what does that mean?

  104. lgbasallote
    • 2 years ago
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    i mean "like dissolves like" and btw..is nacl polar? isnt it ionic???

  105. Kryten
    • 2 years ago
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    that means that salts like NaCl you mentioned will naturally be dissolved in water, other polar molecules like C2H5OH which have small organic groups and polar group will also dissolve in water cause in their case polarity of polar group (in this case OH) is significant, but for example fats and oils which are consisted of large organic chains will not dissolve in water (you can see that in soup where oil or fat floats on soup) but those will dissolve in nonpolar liquids (molecules) like toluene, benzene etc. because they are not polar...

  106. am01656
    • 2 years ago
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    for me, how to know the solubility are based on the BONDS. ionic compounds = soluble. covalent compounds = insoluble except in certain compounds, ex. HCl)

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