What complex has the strongest cationic hydrogen bond and what is its binding energy?
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The Hydofluoric Acid i.e. HF has the strongest Cationic Hydrogen Bond.\nAnd I think I fogot the Binding Energy of it\nNo Problem I will tell U Later when I Read my book
130061
Yes, CN- has a triple bond, and N is slightly more EN than C, Remember that electronegativity increases up and to the left in the periodic table!
963808
The ligand will accomodate electrons from the ligands, forming dative bonds.\n\nThe sub-shell also ceases into two groups of orbitals.  One group will be at a higher energy level as compared with the other.  The difference in energy level is acounted by the strength of the ligand, in other words, by its polarising power.  The stronger the ligand, the greater is the energy difference between the two groups of orbitals.
308551
Xavier is dead wrong. NH4+ is tetrahedral. Most of his answer applies to NH3, which is trigonal pyramidal, and not the same thing as NH4+.\n\nPolar molecules have a large net electrical dipole moment. In a sense, the dipole moment tells you how close you are to becoming an ionic compound. If there is no net dipole moment, the compound is completely non-polar. On the other extreme, if it's an ionic compound, it's completely polar.\n\nLook carefully at your question. NH4+ is an ion, not a molecule, and the terms "polar" and "non-polar" don't really apply to ions. The reason is that ions must be part of an ionic compound, and the ionic compound would be considered polar by definition. For example, (NH4)Cl is an ionic compound and therefore very polar, but asking whether NH4+ is polar is no different than asking whether Cl- is polar.\n\nA couple of good textbooks for further information and examples would be "Organic Chemistry" by Solomons and "Organic Chemistry" by Peter Vollhardt.
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The bond energy is closely related to electronegativity.  It is well known in chemistry that covalent bonds involving fluorine, oxygen, and nitrogen (FON or phone) are the strongest possible bonds (in that order).  Following that within the halogens, is chlorine, bromine, and iodine.  Again, as the electronegativity is lower, the bond energy is lower and that bond is easier to break.  \n\nThis is why HI is much more reactive than HF; the bond involving iodine is weaker (lower bond energy) than that of fluorine.  \n\nSo strongest fluorine:\nF>Cl>Br>I
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If such a compound existed, it would be ionic. Calcium (IV) Chloride.\n\nBut it won't exist, particularly as an ionic compound. You're not going to be able to pull the p electrons from the calcium without a fight and chlorine isn't strong enough (or even fluorine, for that matter). Maybe you can achieve the species in the gas phase ... I don't know.\n\nIf it's covalent, what possible structure could it have? What do the bonding orbitals look like?
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Most professional papers that I read refer to it as just water ion (in its charged form).  This a water molecule with an over-all positive charge.  I do not believe that its structure is known, but I could be wrong about this.\nSee example reference below:
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No - methanol, ammonium\nYes - formic acid, sulfur troxide\nKinda - carbonate, nitrate, chlorate (all can be drawn as resonance structures, so the bonds aren't quite single and aren't quite double)
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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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Ionic compounds are basically defined as compounds where two or more ions are held next to each other by electrical attraction. One of the ions has a positive charge (called a "cation") and the other has a negative charge ("anion"). Cations are usually metal atoms, and anions are either nonmetals or polyatomic ions (ions with more than one atom).\n\nA molecular compound is made up of all non-metals. The bond that forms between the atoms is by the sharing of electrons, unlike ionic compounds, which are made by the transfer of electrons.\n\nIn the case of NaH, this is a ionic compount and this is a strong base. \n\nAcid is defined as a compound which donates a hydrogen ion (H+) to another compound (called a base). You can also see it this way: An acid is a proton donor and a base is a proton acceptor. The acid is said to be dissociated after the proton is donated.\n\nAbout naming of compounds, read the book. It's a long discussion.
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It's [Cu(NH3)6]2+ or hexaamine copper (II)
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Boiling point depends on the strength of the intermolecular forces. Following is the list of them all with their strength and when they occur. \nnetwork covalent (strongest) with only diamond or SiO2\nIonic (ionic compound, 2nd strongest) like Na-Cl etc. Gets stronger with smaller sizes. \nHydrogen bonding (N, O, F with H) 3 rd strongest. \nDipole dipole (when there is a polar molecule) 4 th strongest, gets stronger with more polarity. \nLondon dispersion weakest. Stronger with more mass. \n\na NH3of the first two. Because NH3 has hydrogen bonding (only if you have N, O, or F with hydrogen) while PH3 has regular dipole dipole (based on polarity), which is weaker than NH3. \nNow in this one its c because if you draw their Lewis diagrams out c molecule has on O----H bond while d doesn't. That hydrogen bond is strong enough to make c stronger. As other than that they only have London dispersion force, (which are found in non polar molecules, and they get stronger as atomic mass gets higher). \ne and f both have the London dispersion force that I talked about earlier cause they both are non polar. So f has greater mass so f has higher boiling point. \ng because HCl has polarity (dipole dipole forces) which are stronger than F2 which is non polar and has London dispersion forces (they are the weakest).
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Look at their conjugate bases and whichever is more stable will have the weakest acid. PKA values are also easy to prove this becuase it is a realtion of the H+ content.
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This compund has an octahedral geometry and is coordinated with 3 bidentate oxalate (C2O4) ligands.\nReaction of potassium oxalate hydrate and ferric chloride\n\n3K2C2O4ˇH2O + FeCl3 --> K3[Fe(C2O4)3]ˇ3H2O + 3KCl\n\nWater molekules do not act as ligands and potassium ions act as counter-ions
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Molecular bonding.\n\nThis is a function of the atomic weight (protons in the nuclei) and the distrobution of the electron shell.  Give me three years and I will explain it fully.
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Hydroxide Ion \nor if attached to another compound an alchohol group
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To the first answer----WHAT? What does hydrogen bonds have to do with polarity? Ever heard of dipoles? Why do the need hydrogen bonds when the electronegativity is what is causing the polarity? Please, don't answer question you have no idea about. Anyone can look up stuff and copy and paste. NaCl  doesn't form hydrogen bonds but is VERY solube.\n\nNow, to answer the question. I think what you are eluding to by using "most," is the majority of them. What it boils down to is the molecule is too big. If you have like CH3-Cl, it is a small molecule and the polarity is spread of a small place, thus making it polar. Now, if you have something like C-C-C-C-C-C-C-C-C-C-Cl, the only part that is polar is the Cl part and the rest of the molecule is not, thus will not interact in water.