List the following bonds in order of increasing ionic character: the lithium- to-fluorine bond in LiF, the potassium-to-oxygen bond in \(\mathrm{K}_{2} \mathrm{O},\) the nitrogen-tonitrogen bond in \(\mathrm{N}_{2}\), the sulfur-to- oxygen bond in \(\mathrm{SO}_{2},\) the chlorine-to-fluorine bond in \(\mathrm{ClF}_{3}\).

Short Answer

Expert verified
The bonds in order of increasing ionic character are: N-N < Cl-F < S-O < K-O < Li-F

Step by step solution

01

Find the electronegativity values

Look up the electronegativity values of the atoms involved in the bonds. Electronegativity values can be found on a standard periodic table.
02

Calculate the difference in electronegativity

Subtract the electronegativity of the less electronegative atom from the electronegativity of the more electronegative atom for each bond. The result is the electronegativity difference, which is an indicator of bond polarity and hence ionic character.
03

Rank the bonds

Rank the bonds in order of increasing electronegativity difference. The bond with the smallest electronegativity difference has the least ionic character, while the bond with the largest electronegativity difference has the most ionic character.

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