A polar covalent bond exists when atoms with different electronegativities share electron in a covalent bond.

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From: values of essential Chemistry, 2015

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A polar covalent bond exists when atoms with different electronegativities share electrons in a covalent bond. Take into consideration the hydrogen chloride (HCl) molecule. Each atom in HCl calls for one an ext electron to form an inert gas electron configuration. Chlorine has a higher electronegativity 보다 hydrogen, yet the chlorine atom’s attraction for electrons is not enough to remove an electron native hydrogen. Consequently, the bonding electron in hydrogen chloride are mutual unequally in a polar covalent bond. The molecule is represented by the typical Lewis structure, even though the common electron pair is associated to a larger extent with chlorine than v hydrogen. The unequal sharing of the bonding pair results in a partial an adverse charge top top the chlorine atom and a partial optimistic charge top top the hydrogen atom. The price δ (Greek small letter delta) denotes this fractional charges.



The hydrogen chloride molecule has actually a dipole (two poles), which consists of a pair the opposite dues separated from every other. The dipole is presented by an arrowhead with a overcome at one end. The overcome is near the end of the molecule that is partially positive, and also the arrowhead is close to the partially negative end the the molecule.



Single or many bonds between carbon atoms room nonpolar. Hydrogen and carbon have similar electronegativity values, therefore the C—H shortcut is no normally taken into consideration a polar covalent bond. Hence ethane, ethylene, and also acetylene have actually nonpolar covalent bonds, and also the compounds are nonpolar.


Bonds in between carbon and other elements such as oxygen and also nitrogen room polar. The polarity that a bond depends on the electronegativities that the bonded atoms. Huge differences in between the electronegativities that the bonded atoms increase the polarity of bonds. The direction that the polarity of common bonds found in organic molecules is easily predicted. The usual nonmetals are much more electronegative 보다 carbon. Therefore, as soon as a carbon atom is external inspection to usual nonmetal atoms, it has actually a partial optimistic charge.



Hydrogen is also less electronegative 보다 the usual nonmetals. Therefore, once a hydrogen atom is external inspection to usual nonmetals, the resulting polar bond has actually a partial confident charge ~ above the hydrogen atom.

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The magnitude of the polarity the a shortcut is the dipole moment, (D). The dipole moment of several bond species are offered in Table 1.2. The dipole minute of a specific bond is relatively consistent from link to compound. As soon as carbon develops multiple bond to various other elements, these bonds space polar. Both the carbon-oxygen dual bond in formaldehyde (methanal) and the carbon—nitrogen triple shortcut in acetonitrile (cyanomethane) room polar.


Structural Unit1Bond moments (D)
H—C0.4
H—N1.3
H—O1.5
H—F1.7
H—S0.7
H—Cl1.1
H—Br0.8
H—I0.4
C—C0.0
C—N0.2
C—O0.7
C—F1.4
C—Cl1.5
C—Br1.4
C—I1.2
C = O2.3
C ≡ N3.5