Question

given this table of electronegativities: atom electronegativity h 2.2 c 2.6 n 3.0 o 3.4 f 4.0 s 2.6 br 3.0 cl 3.2 p 2.2 i 2.7 list the following molecules in order of increasing dipole moment: nh₃, h₂o, h₂s, hi

Explanation:

Step1: Calculate electronegativity differences

For $NH_3$: $\Delta\chi_{N - H}=3.0 - 2.2 = 0.8$
For $H_2O$: $\Delta\chi_{O - H}=3.4 - 2.2 = 1.2$
For $H_2S$: $\Delta\chi_{S - H}=2.6 - 2.2 = 0.4$
For $HI$: $\Delta\chi_{I - H}=2.7 - 2.2 = 0.5$

Step2: Consider molecular geometry and net dipole moment

All these molecules are polar. Larger electronegativity difference generally leads to larger dipole - moment. Also, molecular shape affects the net dipole moment. But in this case, considering electronegativity differences as a major factor for a quick comparison.

Answer:

$H_2S