Identify the elements that undergo changes in oxidation number in the reactions:

•nai(aq)+3hocl(aq)→naio3(aq)+3hcl(a q)


3so2(g)+2hno3(aq)+2h2o(l)→3h2so4(aq )+
2no(g)

•2h2so4(aq)+2nabr(s)→br2(l)+so2(g)+
na2so4(aq)+2h2o(l)

Explanation:

1)

The iodine elements is going under oxidation in the given reaction that is from -1 to +5.

NaI

1+x=0

x=-1

In NaI , the oxidation state of iodine is -1

1+x+(3)(-2)=0

x = +5

In , the oxidation state of iodine is +5.

2)

The sulfur elements is going under oxidation in the given reaction ythat is from +4 to +6.

x+(2)(-2)=0

x = +4

In , the oxidation state of sulfur is +4.

2+x+(4)(-2)=0

x = +6

In , the oxidation state of sulfur is +6.

3)

The bromine elements is going under oxidation in the given reaction that is from -1 to 0.

NaBr

1+x=0

x=-1

in NaBr the oxidation state of bromine is -1.

2(x)=0

x = 0

In , the oxidation state of bromine is 0.

i can ! i just need to know what the paragraph is! : p

there are no statements provided but here is why:

sulfur belongs to group 16 because it can be found in nature whether it is in a free or combined state.

hope this