what is the Lewis dot structure for potassium bromide?
362343
8 dots around each element. this is a salt, so is realtively stable. hope that helps!
1047499
If it existed, it would be boron pentafluoride, but as far as I know, this is not a stable molecule.\n\nAre you sure you don't mean BrF5 (bromine pentafluoride), which does exist as a stable molecule?
107504
Nickel(III) Bromide and Beryllium Nitrate
797121
The answers are KCl, CaF2, and Na2O. Potassium has one electron on the outer ring while chlorine has seven. To make chlorine's ring "full" potassium gives the one electron to chlorine. They are "happy" now. :) That's what my science teacher told me. He's weird.
733447
Br+H20--->HBr+O\n\nNi(II)O+H20--->Ni+H202\n\nKO2+H2O--->KOH + H2\n\nHope that helps.
739878
I am not sure what you are asking but the answer could be a monoatomic ion. The positive being a cation and the negative being an anion.\n\nYou might ask over at http://forums.mychemistrytutor.com though.
616395
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
973000
C6H10 + Br2 ---> C6H10Br2.\n\nThe two Br atoms join at either end of the double bond.
90528
A Bronsted-Lowry acid is a species that donates an H+. So, a Bronsted-Lowry base is a species that accepts an H+.\n\nA Lewis acid is a species that accepts a pair of electrons, and a Lewis base is a species that donates a pair of electrons.
795629
Determining structure of molecules.\nIonic structures- The Alkali metal halides are ionic compounds e.g NaCl. Na has a positive charge whereas Cl has a negative charge.\n\nMolecular solids- are held by weak bonds called Van Der waals forces. \n\nMacromolecular structures or giant molecular- have covalent bonds between atoms, these bind all the atoms into a giant molecule e.g Diamond
436740
CH2Cl2\nThe molecule shape is tetraedric with the carbon in the middle
638651
An electron pair acceptor is a Lewis Acid, while a electron Pair donor is a Lewis Base. Sodium wants to give its electron away because that is the easiest way to make itself electronically more like a noble gas, therefore it is a Lewis base compared to Chlorine. Chlorine wants to accept an electron to make itself more like a noble gas, therefore it is a lewis acid compared to sodium. also see electronegativity, and electron affinity.\n\nhttp://www.abacusscience.com/electronegativity.html\n\nhttp://en.wikipedia.org/wiki/Lewis_acid
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you know its ionic because Na is a metal while Cl isnt. a metal and nonmetal almost always from an ionic bond. to draw a lewis digram, determine how many valence electons are in each and draw the diagram.. its kinda hard to explain without actually drawing it.. consult a chem bk.
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Potassium chloride, Chromium oxide, Barium chlorate, Ammonium chloride, Phosphorus trichloride
352077
Thanks NeuroProf.\n\nThe molecule AsF5 is trigonal bipyramidal in shape. First lay out all the bond pairs in that shape and then see if the 'pulling effect' of all the bonds cancel each other. Here, there are 3 bond pairs (of Cl) at the corners of the triangle, 1 bond pair at the bottom and 1 at the top. The Cl at the top pulls electrons and the pulling effect is cancelled by the one at the bottom. Considering the 3 bond pairs left in the middle, 2 are angled at 120 degress and one is at 90 degrees to the top and bottom bond pair. So the pulling effect of the 2 pairs is cancelled by the one at 90 degrees. Overall dipole cancels out and there is no charge distribution, so the molecule is non-polar.\n\nIn BrF4- (with square planar shape), the pulling effect of the lone pair at the top is cancelled by that of the lone pair at the bottom. This leaves 4 F atoms arranged at the corners of the square in the middle. The pulling effect(dipole) of 2 diagonal F atoms will cancel because they are in the same plane and are the same atoms. Hence all the 4 dipoles cancel out and that of the lone pairs too, so the molecule is non-polar.\n\nIn GaI3, the 3 I atoms are arranged in a trigonal planar manner. The dipole of the 2 I atoms at the sides will cancel, but the I atom at the top is not paired with any other atom at the bottom, so the dipole cannot cancel out. Since overall dipole moment is not equal to zero, the molecule is polar.\n\nAre you sure the molecule is SbF6- and not SeF6? If it's SbF6 then the shape will be square bipyramidal or octahedral (similar to BrF4-). The dipole of the 2 F atoms at the top and bottom will cancel and that of 2 diagonal F atoms will cancel and overall dipole will be zero, so the molecule will be non-polar.
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Be very careful:\nFirst, look at the electronegativity differences, the presence of groups like OH- or cations (like Na+ of soap)\nThen, you must know molecular geometries, it is highly important:\nFor BF3 this is a  trigonal planar compound, all differences of electronegativity B<F are canceled due to the position of the F atoms (every 120º on the same plane). It is not polar.\n[SnCl3]- this is a trigonal pyramid compound.\nCl\n I\n:Sn-Cl\n I\nCl\nAS you can see, Sn has a lone pair of electrons, making Cl atoms accommodate in the base corners of an imaginary pyramid. Even if Cl cancel each others dipolar momentum on the sides, they all point ↓. This is a polar compound.
512329
Strictly speaking, the Lewis theory is not applicable to Xenon compounds (& if XeCl3 exists at all). The proper way goes by the Valence Bond theory. In that structure, Xe forms 3 single-sigma bonds with 3 Cl. That leaves out 5 valence electrons which is 2 lone pairs & 1 unpaired. This should (if possible) thus dimerise as Xe2Cl6, each segment being an octrahedron with 2 lone pairs. there should be 2 such octahedra (parallel planes) sharing 1 bond.