The ability of an atom in a molecule to tempt common electrons is dubbed electronegativity. When two atoms integrate, the difference in between their electronegativities is an indication of the type of bond that will form. If the distinction between the electronegativities of the two atoms is little, neither atom deserve to take the common electrons entirely away from the other atom and also the bond will be covalent. If the difference in between the electronegativities is huge, the more electronegative atom will certainly take the bonding electrons completely amethod from the various other atom (electron deliver will certainly occur) and the bond will be ionic. This is why metals (low electronegativities) bonded with nonmetals (high electronegativities) typically produce ionic compounds.

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A bond may be so polar that an electron actually transfers from one atom to an additional, developing a true ionic bond. How execute we judge the degree of polarity? Scientists have devised a range called electronegativity, a scale for judging how much atoms of any kind of facet lure electrons. Electronegativity is a unitless number; the better the number, the even more an atom attracts electrons. A widespread range for electronegativity is presented in Figure (PageIndex1).

api/deki/files/78265/CK12_Screenshot_9-13-3.png?revision=1&size=bestfit&width=320&height=311" />Figure (PageIndex2) A nonpolar covalent bond is one in which the distribution of electron thickness in between the 2 atoms is equal.

The 2 chlorine atoms share the pair of electrons in the single covalent bond equally, and also the electron thickness surrounding the (ceCl_2) molecule is symmetrical. Also note that molecules in which the electronegativity distinction is very little (

Polar Covalent Bonds

A bond in which the electronegativity distinction in between the atoms is between 0.5 and 2.0 is called a polar covalent bond. A polar covalent bond is a covalent bond in which the atoms have an unequal attraction for electrons and so the sharing is unequal. In a polar covalent bond, occasionally ssuggest referred to as a polar bond, the distribution of electrons about the molecule is no longer symmetrical.

Figure (PageIndex3) In the polar covalent bond of (ceHF), the electron density is unevenly dispersed. There is a higher thickness (red) close to the fluorine atom, and a reduced density (blue) near the hydrogen atom.

An simple method to highlight the uneven electron distribution in a polar covalent bond is to usage the Greek letter delta (left( delta ight)).

Figure (PageIndex4) Use of (delta) to indicate partial charge.

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The atom through the higher electronegativity acquires a partial negative charge, while the atom with the lesser electronegativity acquires a partial positive charge. The delta symbol is provided to suggest that the amount of charge is less than one. A crossed arrow can additionally be offered to suggest the direction of better electron density.

what kind of bond results from an unequal sharing of electrons?