Which of the following ions is in the lowest oxidation state?
2 answers:
Answer:
B. Cr in
Explanation:
Let us first find the oxidation numbers in each of the following scenarios
A. The oxidation number of P in is +5
because 2H + 4O + P = -1
2(1) +4(-2) + P = -1
P = 5
B. The oxidation number of Cr in is
2Cr + 7O = -2
2Cr + 7(-2) = -2
Cr = 6
C. The oxidation number of Fe in is +3
2Fe + 3O = 0
2Fe + 3(-2) = 0
Fe = 3
The final answer is Cr
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Answer:
see explanation below
Explanation:
You are missing the reaction scheme, but in picture 1, I found a question very similar to this, and after look into some other pages, I found the same scheme reaction, so I'm gonna work on this one, to show you how to solve it. Hopefully it will be the one you are asking.
According to the reaction scheme, in the first step we have NaNH2/NH3(l). This reactant is used to substract the most acidic hydrogen in the alkine there. In this case, it will substract the hydrogen from the carbon in the triple bond leaving something like this:
R: cyclopentane
R - C ≡ C (-)
Now, in the second step, this new product will experiment a SN2 reaction, and will attack to the CH3 - I forming another alkine as follow:
R - C ≡ C - CH3
Finally in the last step, Na in NH3 are reactants to promvove the hydrogenation of alkines. In this case, it will undergo hydrogenation in the triple bond and will form an alkene:
R - CH = CH - CH3
In picture 2, you have the reaction and mechanism.
