Using periodic trends, place the following bonds in order of decreasing ionic character. Sb-Cl P-Cl As-Cl
A) Sb-Cl As-Cl P-Cl
B) As-Cl Sb-Cl P-Cl
C) P-Cl Sb-Cl As-Cl
D) P-Cl As-Cl Sb-Cl
E) Sb-Cl P-Cl As-Cl

Question

Using periodic trends, place the following bonds in order of decreasing ionic character. Sb-Cl P-Cl As-Cl
A) Sb-Cl > As-Cl > P-Cl
B) As-Cl > Sb-Cl > P-Cl
C) P-Cl > Sb-Cl > As-Cl
D) P-Cl > As-Cl > Sb-Cl
E) Sb-Cl > P-Cl > As-Cl

Quizplus · Accepted Answer

Ionic character increases as the electronegativity difference between atoms increases and as the size of the cation decreases. Based on periodic trends, Sb has the largest atomic radius and smallest electronegativity compared to P and As. Therefore, Sb-Cl bond will have the least ionic character. As-Cl has a smaller atomic radius and higher electronegativity than Sb-Cl, so it will have more ionic character. P-Cl has the smallest atomic radius and highest electronegativity, so it will have the most ionic character. Therefore, the correct order is Sb-Cl > As-Cl > P-Cl.

Using Periodic Trends, Place the Following Bonds in Order of Decreasing