Q49E - Chemistry (OpenStax)

Question

Arrange the following in order of increasing electronegativity: \({\bf{F}};{\rm{ }}{\bf{Cl}};{\rm{ }}{\bf{O}};\)and S.

Step-by-Step Solution

Answer

The order of increasing electronegativity is \({\rm{S}} < {\rm{Cl}} < {\rm{O}} < {\rm{F}}\).

Step 1: Definition of electronegativity

Electronegativity is the tendency of atoms in an element to draw the participated brace of electrons towards itself. It principally denotes the net consequence of tittles' inclinations to attract bond-forming electrons.

Step 2: Determine the order of increasing electronegativity

• When the electronegativity of atoms is similar, an electron pair that they share is equally attracted by both atoms, making this covalent bond non-polar.

 

• The difference in the electronegativity of anytwo atoms is less than 0.5. However, when two atoms differ in their electronegativity in more than \(0.5\)but up to\(1.7\), an electron pair is closer to the one with a higher value, so this covalent bond is known as polar.

 

• When the difference in the electronegativity of atoms is greater than 2, the bond between them is considered ionic.

 

• If the difference is in a range from \(1.7 - 2\) and nonmetals are included, then the bond is a polar covalent, but if a metal is a part of a molecule, the bond is found to be ionic.

 

• Elements placed on the left lower part of the periodic table have the lowestvalues of electronegativity, while the ones onthe right upper portion have the highest values of electronegativity. 

 

On the Pauling scale of electron affinities, we can see the measured electronegativity of elements: \({\rm{F: 3}}{\rm{.98, Cl: 3}}{\rm{.16, O: 3}}{\rm{.44\;, S: 2}}{\rm{.58}}{\rm{.}}\)

 

Thus, the increasing order would be: \({\rm{S}} < {\rm{Cl}} < {\rm{O}} < {\rm{F}}\).