Answered

Assign an oxidation number to each element in the reaction.

[tex]\[ CaF_2(s) + H_2SO_4(aq) \rightarrow CaSO_4(aq) + 2 HF(g) \][/tex]

In [tex]\( CaF_2 \)[/tex], the oxidation number of [tex]\( Ca \)[/tex] is [tex]\(\square\)[/tex], and that of [tex]\( F \)[/tex] is [tex]\(\square\)[/tex].

In [tex]\( H_2SO_4 \)[/tex], the oxidation number of [tex]\( H \)[/tex] is [tex]\(\square\)[/tex], that of [tex]\( S \)[/tex] is [tex]\(\square\)[/tex], and that of [tex]\( O \)[/tex] is [tex]\(\square\)[/tex].

In [tex]\( CaSO_4 \)[/tex], the oxidation number of [tex]\( Ca \)[/tex] is [tex]\(\square\)[/tex], that of [tex]\( S \)[/tex] is [tex]\(\square\)[/tex], and that of [tex]\( O \)[/tex] is [tex]\(\square\)[/tex].

In [tex]\( HF \)[/tex], the oxidation number of [tex]\( H \)[/tex] is [tex]\(\square\)[/tex], and that of [tex]\( F \)[/tex] is [tex]\(\square\)[/tex].



Answer :

GinnyAnswer
Let's go through the compounds in the reaction and assign the oxidation numbers to each element step-by-step.

### In [tex]\( CaF_2 \)[/tex]:
- Calcium (Ca): Typically, calcium has an oxidation number of [tex]\(+2\)[/tex].
- Fluorine (F): Fluorine typically has an oxidation number of [tex]\(-1\)[/tex].

So, in [tex]\( CaF_2 \)[/tex], the oxidation numbers are:
- For [tex]\( Ca \)[/tex]: [tex]\(+2\)[/tex]
- For [tex]\( F \)[/tex]: [tex]\(-1\)[/tex]

### In [tex]\( H_2SO_4 \)[/tex]:
- Hydrogen (H): Typically, hydrogen has an oxidation number of [tex]\(+1\)[/tex].
- Oxygen (O): Oxygen typically has an oxidation number of [tex]\(-2\)[/tex].
- Sulfur (S): To determine sulfur's oxidation number, we use the fact that the sum of all oxidation numbers in a neutral molecule must be zero. The equation is:
[tex]\[ 2(+1) + S + 4(-2) = 0 \implies 2 + S - 8 = 0 \implies S - 6 = 0 \implies S = +6 \][/tex]

So, in [tex]\( H_2SO_4 \)[/tex], the oxidation numbers are:
- For [tex]\( H \)[/tex]: [tex]\(+1\)[/tex]
- For [tex]\( S \)[/tex]: [tex]\(+6\)[/tex]
- For [tex]\( O \)[/tex]: [tex]\(-2\)[/tex]

### In [tex]\( CaSO_4 \)[/tex]:
- Calcium (Ca): Typically, calcium has an oxidation number of [tex]\(+2\)[/tex].
- Oxygen (O): Oxygen typically has an oxidation number of [tex]\(-2\)[/tex].
- Sulfur (S): In sulfate (SO[tex]\(_4\)[/tex] [tex]\(^{2-}\)[/tex]), we determine sulfur's oxidation number as we did for [tex]\( H_2SO_4 \)[/tex]:
[tex]\[ S + 4(-2) = -2 \implies S - 8 = -2 \implies S - 8 + 8 = -2 + 8 \implies S = +6 \][/tex]

So, in [tex]\( CaSO_4 \)[/tex], the oxidation numbers are:
- For [tex]\( Ca \)[/tex]: [tex]\(+2\)[/tex]
- For [tex]\( S \)[/tex]: [tex]\(+6\)[/tex]
- For [tex]\( O \)[/tex]: [tex]\(-2\)[/tex]

### In [tex]\( HF \)[/tex]:
- Hydrogen (H): Typically, hydrogen has an oxidation number of [tex]\(+1\)[/tex].
- Fluorine (F): Fluorine typically has an oxidation number of [tex]\(-1\)[/tex].

So, in [tex]\( HF \)[/tex], the oxidation numbers are:
- For [tex]\( H \)[/tex]: [tex]\(+1\)[/tex]
- For [tex]\( F \)[/tex]: [tex]\(-1\)[/tex]

### Summary

In [tex]\( CaF_2 \)[/tex]:
- Oxidation number of [tex]\( Ca \)[/tex] is [tex]\( +2 \)[/tex]
- Oxidation number of [tex]\( F \)[/tex] is [tex]\( -1 \)[/tex]

In [tex]\( H_2SO_4 \)[/tex]:
- Oxidation number of [tex]\( H \)[/tex] is [tex]\( +1 \)[/tex]
- Oxidation number of [tex]\( S \)[/tex] is [tex]\( +6 \)[/tex]
- Oxidation number of [tex]\( O \)[/tex] is [tex]\( -2 \)[/tex]

In [tex]\( CaSO_4 \)[/tex]:
- Oxidation number of [tex]\( Ca \)[/tex] is [tex]\( +2 \)[/tex]
- Oxidation number of [tex]\( S \)[/tex] is [tex]\( +6 \)[/tex]
- Oxidation number of [tex]\( O \)[/tex] is [tex]\( -2 \)[/tex]

In [tex]\( HF \)[/tex]:
- Oxidation number of [tex]\( H \)[/tex] is [tex]\( +1 \)[/tex]
- Oxidation number of [tex]\( F \)[/tex] is [tex]\( -1 \)[/tex]