which has a strong hydrogen bond in liquid & solid? h2s,hbr,sih4,hf,hci?
112370
H2S.  That's very similar to H2O (which we usually associate with H-Bonding).  HBr, HCl, and HF will ionize.  SiH4 is symmetric and Si has medium electronegavity, etc, such that it would be like methane (Si is in the same group as C).
83361
It's not really a valid question. The only diprotic strong acid is sulfuric acid (H2SO4) with the loss of its second proton being weak. Otherwise, diprotic acids are weak.\n\nIf you're asking for a comparison between something like HCl or HNO3 and H2SO4, you'd have to consult chemical literature.
290836
Solid. Most elements at standard atmospheric temperature and pressure are solids. Some of the non-metals are gases, but only Mercury and Bromine are liquids at STP.\n\nEDIT: Gloo-gal, why answer if you don't know or don't care?
874373
funny question\n\nccl4 is insoluble in water since it cannot form hydrogen bond with water\nsicl4 is soluble in water since it hydrolyse in water to give SiO2\nand HCl
1182386
Simple.\n\nH2O is liquid at room temperature because of two types of bonds it contains.  The first, between the H and O, is a polar covalent bond.  This bond is strong because of the relatively large electronegativity difference between H and O (2.2 vs 3.44).  Secondly, there are hydrogen bonds between the two hydrogens.  Both these bonds result in this peculiar property of H20.
879801
Pentane\n\nIt depends on which compound has the strongest intermolecular forces. In the case of hydrocarbons the intermolecular forces that are present are dispersion forces.\nIn such cases:\n"The more branched a molecule is, the more "spherical" it is, and the smaller surface area it will have - since dispersion forces increase with surface area, the more branched molecules will have a lower boiling point. You may notice that the trend in the melting points is rather different - this is because the longer a branch is, the more potential it has to flop around and disrupt the regular crystalline lattice of frozen pentane, giving a liquid state."
825026
what you need to do, get a SI data book, and look up their natural state. not bonded with anything else, and possibly itself.\n\nPhophorus - white: molecular (P4). red: Chain. Black: Layer\nIodine - molecular (I2)\nMagnesium - hexagonal closest-packing\nNeon - cubic closest-packing\nArsenic -grey: 3d structure - Layer formation. yellow: molecular As4\nSulfur- molecular S8\nBoron - complicated structure.\nSelenium - grey: chain, Red: molecular: Se8\nGallium - Complicated\nCesium - body-centred cubic\nOxxygen - O2, O3 molecular
481911
H2, or hydrogen gas.\n\nFor example, take magnesium metal and hydrochloric acid.\n\nMg + 2HCl -> H2 + MgCl2\n\nThis is a displacement reaction, in which a free element (Mg) breaks the bond between a compound (HCl) and then bonds to the ion with the opposite charge (Cl-) forming a new compound (MgCl2).  The ion left over (H+) loses its charge and becomes a pure element (H2).
166866
It's true that surface tension has everything to do with intermolecular forces.  Water has Hydrogen bonds, while I believe alcohol has London Dispersion Forces [LDF's]. Hydrogen bonds are much stronger than LDF's, so water is more resistant on it's surface and has a greater surface tension.
161405
The elements Hydrogen (H+) and Chlorine (Cl-) to make HCl (aka hydrochloric acid)
585856
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
445370
well this question was asked two days before.\nsearch for this question u'll get all the knowledge\nstrongest oxo-acid-- HClO4\nstrongest protonic acid--H2SO4\nstrongest lewis acid----SBF5\n btw HF is not consider very strong bcoz F is very small atom and it does not loose H+ very easily.\n\nEDIT: Question(very odd name) there has been acids with negative pH and 0 pH( 0pH is more stronger than 1)
728160
1. C, 2. Cl, 3. Se. The closer the atom is to Fluorine on the Periodic table (excluding noble gases), the stronger the electron affinity. Fluorine is the strongest.
750581
Covalent single bonds.\nYou'll find carbon - oxygen\noxygen - hydrogen\ncarbon - hydrogen\ncarbon - carbon
680519
yes, it does because fluorine, being such an electronegative elements allows one of its lone pairs to become a bonding pair for another hydrogen to attach (other than its already used up bonding pair). and like the first quote HF has some of the strongest H-bonds due to the fluorine being one of most electronegative elements.
800097
Yes 1 is correct. Oxygen and Hydrogen have very strong bonds. Also known as hydrogen bonding. That's why water, for example, has such a high surface tension. You are correct!
732674
HBr is a strong acid because of Bromine's electronegativity.