Where is the highest and lowest electronegativity found?
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Ignoring the inert gases, the highest electronegativity is at the top right corner (fluorine), and the lowest is at the bottom left (francium)
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http://www-ec.njit.edu/~skawinsk/chem243/chap11/chap11.htm\nthis may help–near the bottom
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ok listen if u have a compound formed by 2 atoms u take the electronegativity of the second atom and u substract the electronegativity of the first one if the number that u get is between 0 and 0.3 its non polar covalent if its 0.4-1.7 then its polar covalent and if its 1.7 or more than it is ionic
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I think it's "a," do to the very high electronegativity of F.  I'll have to check it out...
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Acidic \n\nbelow 6 acidic above 7 basic
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No, we don't use the electronegativity chart; instead we draw the full structure of the molecule and then see which 'pulling of bonds' cancel each other. \nIn the molecule AsF3, since As has 5 outer most electrons(in group 5), each F is bonded to As with a single covalent bond. Hence, the shape of the molecule becomes trigonal pyramidal, with 3 bond pairs (with 3 F atoms) and 1 lone pair. The 3 bond pairs pull the electrons towards themselves in the lower plane, while the 1 lone pair pulls at the top. The pulling effect of the 2 F atoms at the 2 sides cancel out  because the pulling effect is the same for both F atoms; however, the pulling effect of the lone pair at the top and the 1 F bond pair at the bottom will not cancel, because it is not from the same atom/species. Hence the overall dipole moment( dipole moment = charge x distance) does not cancel out, so the molecule is polar, with some charge distribution remaining due to the unequal pulling effect.\n\nIn CF3Cl, the shape is tetrahedral, with the 3 Cl atoms and 1 F atom bonded by single covalent bonds to the central C atom. The bond pairs spread out with the 3 Cl atoms pulling at the bottom and the 1 F atom pulling at the top. The pulling effect of the 2 Cl atoms at the sides cancels out, but that of the F atom at the top and the Cl atom at the bottom does not, as the pullin effect of 2 different atoms is different. Hence, as before, overall dipole does not cancel and the molecule is hence polar.
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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!
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It's fairly easy don't worry.\n\nNo need for d level splitting diagrams to answer this since we're dealing with N and F:  use the spectrochemical series to make an assumption about the ligand.  The difference in t2g and eg levels (∆o) determines whether a complex is low or high spin.  If both ligands were the same, we would have to look at the oxidation state of the ligand in the complex.\n\nHalides <  Oxygen ligands  <  Nitrogen ligands < CN- ligands\n\n   ALWAYS HIGH SPIN    ---------------            ALWAYS LOW SPIN\n\nIf ∆o > P, then a complex is low spin.  IF ∆o < P the complex is high spin.
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a polar bond is one which the shared electron, making the bond, is closer to one atom.  A bond between two identical atoms is non-polar because the atoms have the same electronegativity.\n\nElectronegativity is the affinity for an electron.  Fluorine is the most electronegative element and Francium the least.\n\nHydrogen has an electronegativity of 2.2 and fluorine 3.98, prompting the electrons to be closer to fluorine, consequently making the hydrogen partially positive and fluorine slightly negative.
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the elements most likely to form ionic bonds have low ionization energies (such as the alkali metals and the alkaline earth metals, which form cations) or high electron affinities (such as halogens and oxygen, which form cations).
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1.  they are the outer most electrons \n2.  8 because that is a full orbital and a octet.. they want to get a noble gas notation\n3. Covalent shares electrons Ionic bonds donate electrons due to low electronegativity
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look it up on any periodic table - like the one linked below... good luck!
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Positive and Negative ends of a molecule depend upon the electornegativity of the atoms of the molecule. Lets take a simple example of water here. H2O. \n\nOxygen is water is bound to 2 Hydrogen atoms. Oxygen is highly electronegative. So, it pulls the electrons in the O - H bond towards itself partially. So, this creates a partial negative charge on it and also a partial positive charge on Hydrongen.\n\nElectronegativity actually means "the ability of an atom to pull a lone pair of electrons towards itself". Electronegativity depends on the number of electrons present in the outermost shell. \nEx: Sodium has 1 electron in the outermost shell. So, its tenedecy to release this electron and get to a stabler configuration is more than gaining electrons further. But, in case of Chlorine, there are 7 electrons. It needs just 1 more electron to attain stable configuration. So, Chlorine tends to pull electrons towards it and therefore Chlorine is highly electronegative. \n\nNow, looking at the molecules u have given...\nNitrogen is highly electronegative. It has 3 unpaired electrons in its outermost shell, but it wud still go ahead and grab a few more to get to a fully filled state. So, in NH3, N would be partially negative and H would be partially positive. \n\nSo, is the case in HCN too. Cyanide ion (CN-) is a highly electronegative ion and therefore acts as the negative end. \n\n\nHope this information helps.
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The difference in Pauling's electronegativity\ndetermine percent ionic character\ncovalent and ionic are sort of relative positions on a continuum
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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.
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electron affinity\n\nas you are changing Cl2 ->2Cl-
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d)O and Cl. They have the least difference in electronegativity, so the shared pair of electrons is not drawn particularly towards any atom. Thus the molecule shows the least ionic character. Ionic character occurs when there is polarisation of a covalent bond.