what is the meaning of electronegativity?
90178
electronegativity (ĭlĕk'trōnĕgətĭv'ətē) , in chemistry, tendency for an atom to attract a pair of electrons that it shares with another atom (see chemical bond). For example, the molecule hydrogen chloride, HCl, consists of a hydrogen atom, H, and a chlorine atom, Cl, sharing a pair of electrons. If the pair of electrons are not shared equally, i.e., if they spend more time with one atom than with the other, the favored atom is said to be more electronegative. In the case of HCl, measurements indicate that the molecule has a dipole moment, that is, the chlorine end is relatively negative and the hydrogen end is relatively positive. This means that the electron pair spends more time with the chlorine atom than with the hydrogen atom and thus chlorine is more electronegative than hydrogen. Nonmetals have much higher electronegativities than metals; of the nonmetals, fluorine is the most electronegative, followed by oxygen, nitrogen, and chlorine. The larger the difference in electronegativity between two atoms, the more polar the bond between them. In the extreme case of a bond between a metal and a nonmetal, a complete transfer of electrons takes place.\n\n\n--------------------------------------------------------------------------------
945388
density,volume,weight,number of electron and proton.
1091883
Electronegativity is a principally the ability of atomic nucleus of the element to attract electrons. Therefore, in a covalent bond, the element (for example oxygen) with a greater electronegativity which has more proton in atomic nucleus will attract more of the shared electrons, thereby creating a negative pole. The other element's ( hydrogen) which has less proton in its naked atomic nucleus has gained transiently positive charge. Its called electropositive. Water molecule is a well known dipole. It consist of electronegative oxygen and electropositive hydrogen atoms. Special bond angles help to create dipole character.
816025
b) the electronegativities of both atoms involved in the bond are identical.
253224
Larger surface area for the electrons to spread over.  In other words, the reason elements in the same family decrease in electronegativity downward is because the atoms bet larger.  For instance, Fl, the most electronegative element, is many times smaller than Cl, then Br, I.  I think you get the point.
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!
1094405
A covalent bond is a bond in which the atoms making up the resulting molecule "share" the electrons in the form of covalent bonds.\nAn ionic bond is an extremely one sided "sharing" of electrons, so one sided, one atom is said to have completely stripped of an electron from another atom.\n\nWhat determines if the bond is covalent or ionic is the difference in the electronegativities of the two atoms bonding.  If the electronegativity difference is high enough, the bond is said to be ionic.  If the difference in electronagativities is significant, but not quite to the level of a full ionic bond, the bond is said to be polar (which may or may not mean that the resulting molecule is polar, this depends on several things).\n\nLooking at a chart of [Pauling] electronegativities,\nhttp://www.psigate.ac.uk/newsite/reference/plambeck/chem1/p01244a.htm\none can see that most elements are somewhere in the 1 to 2 range, with only a few elements getting much lower or higher than this value.  Unless the difference is high enough (usually a difference of about 1.5 is considered ionic), then the bond will just be polar, or less so.\n\nSo, all elements have the potential to theoretically bond ionically, but only in certain combinations with other elements.\nFor example, you will never see an ionic bond between Carbon and Hydrogen since the difference is just .4, but an ionic bond between Lithium and Fluorine is easy to make with a huge difference of 3.0.
732674
HBr is a strong acid because of Bromine's electronegativity.
837121
Hmmm.. The one affecting the boiling point is the intermolecular force..\nAs you can see, most of the compound here is polar. \n\nTherefore all you have to do is if the compound is consisted only of 2 elements (Group 17), you'll have to calculate the electronegativity difference. The more difference between them, the boiling will increase as well.\n\nIf there is more than 2 atoms in a molecule, you'll have to see the dipole moment magnitude (a.k.a polarity). The higher the magnitude, the higher the boiling point will be.\n\n\npeace\nvixklen
741551
Covalent.\nMetallic bond (do research on the Band Theory)\nIonic.\nCovalent.\nCovalent.\nIonic.
1173986
The Inductive effect in chemistry is an experimentally observable effect of the transmission of charge through a chain of atoms in a molecule by electrostatic induction (IUPAC definition). The net polar effect exerted by a substituent is a combination of this inductive effect and the mesomeric effect.\n\nThe electron cloud in a σ-bond between two unlike atoms is not uniform and is slightly displaced towards the more electronegative of the two atoms. This causes a permanent state of bond polarization, where the more electronegative atoms has a slight negative charge(δ-) and the other atom has a slight positive charge(δ+).\n\nIf the electronegative atom is then joined to a chain of atoms, usually carbon, the positive charge is relayed to the other atoms in the chain. This is the electron-withdrawing inductive effect, also known as the -I effect.\n\nSome groups, such as the alkyl group are less electron-withdrawing than hydrogen and are therefore considered as electron-releasing. This is electron releasing character is indicated by the +I effect.\n\nAs the induced change in polarity is less than the original polarity, the inductive effect rapidly dies out, and is significant only over a short distance. The inductive effect is permanent but feeble, as it involves the shift of strongly held σ-bond electrons, and other stronger factors may overshadow this effect.\n\nThe inductive effect may caused by some molecules also. Relative inductive effects have been experimentally measured with reference to hydrogen.\n\nRelative strengths of the inductive effect of various molecules\n\n\nInductive effects can be measured through the Hammett equation.\n[edit]\n\nApplications\n\n    * (a) Aliphatic carboxylic acids\n\nThe strength of an carboxylic acid depends on the extent of its ionization-the more the ionization, the stronger is the acid. The strength of an acid is denoted by the numerical value of pKa. In aliphatic acids, the electron releasing inductive effect of the methyl group, increases the electron density on oxygen and thus hinders the breaking of the O-H bond, which consequently reduces the ionization.\n\nGreater ionization in formic acid when compared to acetic acid makes formic acid(pKa=3.75) stronger than acetic acid(pKa=4.76). Monochloroacetic acid(pKa=2.82) is stronger than formic acid since the electron-withdrawing effect of chlorine promotes ionization.\n\n    * (b) Aromatic carboxylic acids\n\nIn benzoic acid, the carbon atoms which are present in the ring are sp2 hybridised.As a result, benzoic acid(pKa=4.20) is a stronger acid than cyclohexane carboxylic acid(pKa=4.87). Also, electron-withdrawing groups substituted at the ortho and para positions, enhance the acid strength.\n\n    * (c) Dioic acids\n\nSince the carboxyl group is itself an electron-withdrawing group, the dioic acids are, in general, stronger than their monocarboxyl analogues.\n\n\nThe Polar effect or electronic effect in chemistry is the effect exerted by a substituent on modifying electrostatic forces operating on a nearby reaction center. The main contributors to the polar effect are the inductive effect, mesomeric effect and the through-space electronic field effect.\n\nAn electron withdrawing group or EWG draws electrons away from a reaction center. When this center is an electron rich carbanion or a alkoxide anion the presence of the substituent has a stabilizing effect.\n\nExamples of electron withdrawing groups are:\n\n    * halogens (F, Cl),\n    * nitriles CN,\n    * carboxylic acids COOH\n\nAn electron releasing group or ERG releases electrons into a reaction center and as such stabilizes electron deficient carbanions.\n\nExamples of electron releasing groups are:\n\n    * alkyl groups\n\n\nThe total substituent effect is the combination of the polar effect and the combined steric effects.\n\nIn Electrophilic aromatic substitution and nucleophilic aromatic substitution substituents are divided into activating groups and deactivating groups wh
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Yeah, it's the greatest electronegativity difference between the two atoms that are forming that bond.  In other words, it's the difference between how far away the two elements are from fluorine, the most electronegative element.  Diatomic molecules like Cl2 are very nonpolar because both Cl atoms are equidistant from fluorine, and HBr is more polar because Br is closer to fluorine than hydrogen.
827720
Bond polarity refers to difference of electronegativity between two atoms in a bond. \n\nMolecular polarity is the sum of all the forces\n\nThat's all I know.
525723
when an atom loses an electon from its outermost shell then it forms an electropositive ion while when an atom gains an electron it forms an electronegative elctron.\n\nfor e.g. during the formation of nacl na atom loses an elcron to the cl atom to form a +ve ionwhile the cl atom which gains that electon forms a -ve ion.
911430
Cations are positive.\nAnions are negative.
546448
this polar nature depends on electronegativity. \nIn a bond, say C-H, the most EN element gets partial -ve charge and less EN element gets partial +ve charge\nIn C-H, H is less EN and C is more EN. Thus, C gets partial +ve charge and H gets partial -ve charge.\n\nEN of C is 2.550 EN of H is 2.200\nEN of Si is 1.9 EN of Sn is 1.96\n\nIn this group EN of C is high and H is less in C-H thus, C-H is most polar. \n\nAs EN of Si and Sn is less, than H , H gets positive charge but very less +ve charge. but in C-H C is more EN and gets +ve 2.550.\nHope i was clear enough.\nAny doubts you can ask further.
224922
positive or negative charge... depending on how tightly they hold their electrons