Based on electronegativity, select the molecule with the most ionic character. Group of answer choices SBr2 OBr2 SeCl2 TeI2 SCl2

OBr₂

Explanation:

The ionic character depends on the difference of electronegativity between the elements. The higher ΔEN, the greater the ionic character.

SBr₂

ΔEN = |EN(S)-EN(Br)| = |2.5-2.8| = 0.3

OBr₂

ΔEN = |EN(O)-EN(Br)| = |3.5-2.8| = 0.7

SeCl₂

ΔEN = |EN(Se)-EN(Cl)| = |2.4-3.0| = 0.6

TeI₂

ΔEN = |EN(Te)-EN(I)| = |2.1-2.5| = 0.4

SCl₂

ΔEN = |EN(S)-EN(Cl)| = |2.5-3.0| = 0.5

OBr₂ is the molecule with the most ionic character.

- both b and d.

-since b and d are the closest coastlines then that makes it the most affected.

< 3

indium, and thallium have three electrons i think