Using the molecular orbital model, write electron configurations for the following diatomic species and calculate the bond order
s. Which ones are paramagnetic? Place the species in order of increasing bond length and bond energy.
a. CN +
b. CN
c. CN -
a. CN +
b. CN
c. CN -
1 answer:
Answer:
Bond orders
CN- =3
CN+ =2.5
CN =2
CN+ is paramagnetic
The order of increasing bond energy is CN <CN+ <CN-
The order of increasing bond length is CN- <CN+ <CN
Explanation:
The molecular orbital diagram of CN- is shown in the image attached. From that image, it is easy to deduce the bond order of the other related species. Bond length is in the reverse order as bond energy because the shorter the bond, the greater the bond energy. The specie with the highest bond order has the highest bond energy.
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Answer:
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Explanation:
The given reaction undergoes mechanism in which the nucleophile attacks the backside and it is substituted by the elimination of bromine.
Due to the backside attack of nucleophile , the inverse in stereo-chemistry is observed.
After the substitution of ethoxy group, the configuration is assigned according to the priority it shows clock wise direction(R) - configuration.
When hydrogen faces the front side , it results shows inverse configuration i.e, S- configuration.
The chemical reaction is as follows.
