How many pi bonds does Phosphorus Pentachloride have?
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Answer is?  none... PCl5 P only has five valence electrons by which to bond with.  A pi bond is defined as a bond with no electron cloud density along the internuclear separation.  However, all five of the chlorines are bonded directly to the Phosphorus.  It has five sigma bonds.
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3 Sn(NO3)4 + 4 AlCl3 --> 4 Al(NO3)3 + 3 SnCl4
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PCl5, or phosphorus pentachloride, has a trigonal bipyramidal structure. A photo of the structure of this molecule is shown below:\n\nhttp://en.wikipedia.org/wiki/Phosphorus_pentachloride\n\nBrF5, or bromine pentafluoride, has a square pyramidal structure: a link to this molecule is shown below as well:\n\nhttp://www.chemistry.ccsu.edu/crundwell/Galleries/VSEPR/brf5.html\n\nBecause PCl5 has a trigonal bipyramidal structure, there is no net dipole moment since the molecule is symmetric around the central phosphorus atom.\n\nBrF5, on the other hand, does have a dipole moment due to the asymmetric structure. The absence of a sixth fluorine atom prevents the structure from becoming octahedral, which would be symmetrical in the structure of BrF6.\n\nSo in short, the differences between the two are as follows:\n\nPCl5=no dipole moment\nBrF5=dipole moment\n\nHope this helps!
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a) 36\nb) i just found the answer for b : it is 6 because its a p orbital
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1 - NH4OH\n2 - PbO\n3 - KBr\n4 - PCl5 (five)\n5 - Al(NO3)3\n6 - Ba3(PO4)2  (not sure)\n7 - C4H10\n8 - Sn(OH)4\n9 - NH4NO3\n10 - Li3P\n11 - Ba3ClO2   (not sure)\n12 - MgSO3
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PH3: Phosphine\nAg2SO3: Silver Phosphite\nFeCO3: Iron(II) Carbonate\nN2O4: Dinitrogen tetroxide\nPb(OH)2: Lead(II) Hydroxide
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NaCl, the bonding is stronger
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PCl3 has the same shape as NH3 (tetrahedral with P in the center, the 3 Cl at the 3 corners and a lone pair at the fourth corner) So the polar covalent bonds don't cancel out each other\n\nSO3 is planar trigonal and thus the dipole moments cancel out each other and it is non-polar\n\nCF4 has a tetrahedral shape and since all bonds are the same they cancel each others dipole moment;the molecule is nonpolar\n\nCH2F2 has the approximately the same shape as CF4, but since not all bonds are the same their angle is a bit different and the sum of the dipole moments is not zero; thus the molecule is polar\n\nSO2 is a bent molecule (because of the sulphur's lone pair), think of it in a way as water with S in the place of O and O in the place of H so it is polar.\n\nCO2 is a linear molecule (O=C=O) so the dipole moments of the two identical polar bonds cancel out each other; the molecule is nonpolar\n\nO=C=S has different polar bonds, so although they have opposite directions the result will be a slight dipole moment, so the molecule is polar.\n\nIn all your questions you have to compare a polar and a nonpolar molecule. Of course the one with the strongest dipole-dipole interactions in each case is the polar molecule.
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It seems that the tripolyphosphate hydrolises to the orthophosphate\n\nThis is the only way I could see it balance BUT I am guessing and balancing ...\n\n3Na5P3O10 + 6H20 → 5Na3PO4 + 4H3PO4
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thermodynamic factors as well as the orientation and relative energies of the pi molecular orbitals involved.
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Are you looking for Sulfur Dioxide, Carbon Tetrabromide, Phosphorus Pentachloride?
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I don't know that question.\n\nI can tell you that it's an octahedral complex. The two isomers would be CIS (Both chlorides adjacent to each other) and TRANS (both chlorines opposite each other)
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Binary: NaCl  (sodium chloride)\nPolyatomic cation:  NH4Cl  (ammonium chloride)\nPolyatomic anion:  Li2SO4  (lithium sulfate)\nPolyatomic complexed:  (NH4)3PO4  (ammonium phosphate)\nThey might be broken down differently to include inorganic and organic.  Their are also compounds called Zwitterions which contain both cation and anion.
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I'm trying to work with this info:\n\nOctet Rule - atoms want to have eight electrons in their valence shell (two for H) (most will form octets, some will not)\n\nMultiple Bonds\nSingle bond - a covalent bond in which a single pair of electrons is shared by two atoms\ndouble bond - two pairs of electrons are shared by two atoms\ntriple bond  - three pairs of electrons are shared by two atoms\n-generally form with C, N, O, S\n-------\nOkay, oxygen might attach easily to one of the Cls, leaving no spaces, but I'm not sure if there is a doule bond or something weird like that. Same with C.\nIf I remember correctly, CO2 looks like this:\nO=C=O\n------\nWait, check this out- I found the following (and no further info) somewhere on the net.\n\nE) COCl2\n      (C is the \n       central atom)\n\n----------\nWait. No.\n_______\nCl- C -Cl\n___O___\nI'm going to try that...\nI don't know. It lacks the symmetry that you normally see and it's kinda weird looking. What do you think of what I got?\n__________\nI found a pic: http://www.chem.ox.ac.uk/inorganicchemistry3/C/COCl2.html\nLooks kinda like yours.\n______\nHoly Mother of God - http://www.chem.ox.ac.uk/inorganicchemistry3/C/COCl2.html\nI found the name of the compound- phosgene- and did an image search. *exclamation of glee*\n___\nLol, better be right. Later.
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well family 13 has B and Al.  they are metaloids that are great lewis acids.  they have interesting bonding strategies that defy the normal octet rule.
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Phosphorus, (IPA: /ˈfɒsfərəs/, Greek: phôs meaning "light", and phoros meaning "bearer"), is the chemical element in the periodic table that has the symbol P and atomic number 15. A multivalent nonmetal of the nitrogen group, phosphorus is commonly found in inorganic phosphate rocks and in all living cells.\n\nPhosphorus exists in several allotropes, most commonly white, red and black. White phosphorus (P4) contains only four atoms, resulting in very high ring strain and instability. White phosphorus glows in the dark, is highly flammable and pyrophoric (self-igniting) upon contact with air as well as toxic. Red phosphorus has a network form which reduces strain and gives greater stability. Red phosphorus does not catch fire in air at temperatures below 240°C whereas white phosphorus ignites at about 40°C. Black phosphorus is amorphous and is the least reactive allotrope.\n\nRed phosphorus is formed by heating white phosphorus to 250°C (482°F) or by exposing white phosphorus to sunlight.\n\nDue to its high reactivity, phosphorus is never found as a free element in nature. It emits a faint glow upon exposure to oxygen (hence its Greek derivation and the Latin meaning 'morning star') and is an essential element for living organisms. The most important commercial use of phosphorus-based chemicals is the production of fertilizers. They are also widely used in explosives, nerve agents, friction matches, fireworks, pesticides, toothpaste, and detergents.\n\nContents [hide]\n1 Characteristics \n1.1 Glow \n2 Applications \n3 Biological role \n4 History \n5 Occurrence \n6 Precautions \n7 Isotopes \n8 Spelling \n9 Compounds \n10 References \n11 External links \n \n\n\n[edit] Characteristics\nPhosphorus, in its common form, is a waxy white (or yellowish) solid that has a characteristic, disagreeable smell similar to that of garlic. Pure forms of the element are colorless and transparent. This nonmetal is not soluble in water, but is soluble in carbon disulfide. The white allotrope ignites spontaneously in air; however both white and red phosphorus burn in air to produce phosphorus pentoxide.\n\n\n[edit] Glow\nThe glow from phosphorus was the attraction of its discovery around 1669, but the mechanism for that glow was not fully described until 1974.[1] It was known from early times that the glow would persist for a time in a stoppered jar but then cease. Robert Boyle in the 1680s ascribed it to "debilitation" of the air. In fact it is oxygen being consumed. By the 18th century it was known that in pure oxygen phosphorus does not glow at all,[2] there is only a range of partial pressure where it does, too high or too low and the reaction stops. Heat can be applied to drive the reaction at higher pressures.[3]\n\nIn 1974 the glow was explained by R. J. van Zee and A. U. Khan.[1] A reaction with oxygen takes place at the surface of the solid (or liquid) phosphorus, forming short-lived molecules HPO and P2O2 and they both emit visible light. The reaction is slow and only very little of the intermediates is required to produce the luminescence, hence the extended time the glow continues in a stoppered jar.\n\nAlthough the term phosphorescence is derived from phosphorus, the reaction is properly called luminescence (glowing by its own reaction, in this case chemoluminescence), not phosphorescence (re-emitting light that previously fell on it).\n\n\n[edit] Applications\nConcentrated phosphoric acids, which can consist of 70% to 75% P2O5 are very important to agriculture and farm production in the form of fertilizers. Global demand for fertilizers led to large increases in phosphate (PO43-) production in the second half of the 20th century. Other uses;\n\nPhosphates are utilized in the making of special glasses that are used for sodium lamps. \nBone-ash, calcium phosphate, is used in the production of fine china. \nSodium tripolyphosphate made from phosphoric acid is used in laundry detergents in sev
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atp has 3 phosphate groups (3 high energy bonds) and adp has only 2