The student's statements contain several inaccuracies regarding oxidation numbers. While it is true that hydrogen typically has an oxidation number of +1, in the diatomic molecule H2, its oxidation number is 0, as the element is in its elemental form. Regarding iodine, while it is in Group VIIA, its oxidation number in the diatomic molecule I2 is also 0. In HI, iodine has an oxidation number of -1. Since both hydrogen and iodine change their oxidation states during the reaction (from 0 to +1 for hydrogen and from 0 to -1 for iodine), this qualifies as a redox reaction, as there is a transfer of electrons between the atoms.
answer this to where a teacher couldn't tell you wrote it
Use the chemical equation to complete the activity.
H2(g)+I2(g)→2HI(g)
A student makes the following statements:
Hydrogen always has the same oxidation number, so it has an oxidation number of +1
in both the reactant H2
and product HI
.
Iodine is in Group VIIA
, so it has an oxidation number of −1
in both the reactant I2
and product HI
.
Neither hydrogen nor iodine changes oxidation states, so the reaction is not a redox reaction.
In 3–5 sentences, describe the mistakes that the student made. Based on the oxidation numbers, is this a redox reaction? Explain your answer.
(4 points
1 answer