Answer:
10B has 18.9%
11B has 81.1%
Explanation:Please see attachment for explanation
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.
You might be interested in
Answer:
900 K
Explanation:
Recall the ideal gas law:
Because only pressure and temperature is changing, we can rearrange the equation as follows:
The right-hand side stays constant. Therefore:
The can explodes at a pressure of 90 atm. The current temperature and pressure is 300 K and 30 atm, respectively.
Substitute and solve for <em>T</em>₂:
Hence, the temperature must be reach 900 K.