NCl3, SiCl4, AsCl3, SCl2, PCl3 order them in terms of increasing bond polarity

NCl3<SCl2<PCl3<SiCl4<AsCl3 this
Is what I have it says "Your answer appears to contain an incorrect substance"
I don't see any incorrect substances unless I'm blind??

I don't have the same electronegativity values you have because we are using different sources but isn't SiCl4 the highest?

Yep your right I was looking at some other element for As.

Based on the order you provided (NCl3 < SCl2 < PCl3 < SiCl4 < AsCl3), it seems that you have correctly arranged the substances in terms of increasing bond polarity. The message "Your answer appears to contain an incorrect substance" might be due to a typo or an issue with the specific platform you are using. However, the order you have provided is accurate, and there are no incorrect substances in your arrangement.

I apologize for the confusion. The order of increasing bond polarity for the given compounds is actually as follows:

SCl2 < NCl3 < PCl3 < AsCl3 < SiCl4

To determine the bond polarity, we need to consider the electronegativity difference between the central atom and the surrounding atoms in each compound.

Starting with SCl2, sulfur (S) has a lower electronegativity than chlorine (Cl), resulting in a polar bond.

Moving on to NCl3, nitrogen (N) has a slightly higher electronegativity than chlorine (Cl), making the bond slightly more polar than SCl2.

Next, PCl3 has an even higher electronegativity difference between phosphorus (P) and chlorine (Cl), leading to a more polar bond than NCl3.

Then, AsCl3 has a higher electronegativity difference between arsenic (As) and chlorine (Cl), making the bond between them more polar than in PCl3.

Lastly, SiCl4 has the highest electronegativity difference between silicon (Si) and chlorine (Cl), resulting in the most polar bond among the given compounds.

It seems there was an error in your initial ordering. The correct order of increasing bond polarity is SCl2 < NCl3 < PCl3 < AsCl3 < SiCl4.