Answer: The energy of an electron in the n = 2 level of a hydrogen atom is 3.40 eV.
Explanation:
Given: n = 2
The relation between energy and
orbit of an atom is as follows.
![E = - \frac{13.6}{n^{2}} eV](https://tex.z-dn.net/?f=E%20%3D%20-%20%5Cfrac%7B13.6%7D%7Bn%5E%7B2%7D%7D%20eV)
Substitute the values into above formula as follows.
![E = - \frac{13.6}{n^{2}} eV\\= - \frac{13.6}{(2)^{2}}\\= - 3.40 eV](https://tex.z-dn.net/?f=E%20%3D%20-%20%5Cfrac%7B13.6%7D%7Bn%5E%7B2%7D%7D%20eV%5C%5C%3D%20-%20%5Cfrac%7B13.6%7D%7B%282%29%5E%7B2%7D%7D%5C%5C%3D%20-%203.40%20eV)
The negative sign indicates that energy is being released.
Thus, we can conclude that the energy of an electron in the n = 2 level of a hydrogen atom is 3.40 eV.
A) Jupiter because it has the largest mass of all the planets
Answer:
Trend in ionic character of bonds: Cs-F > Si-C > Br-Cl > Cl-Cl
(most) (least)
Explanation:
We know that, percentage ionic character of a bond is proportional to electronegativity difference between two constituting atoms.
Atom Electronegativity
Cs 0.7
F 4.0
Cl 3.0
Br 2.8
Si 1.8
C 2.5
Bond Electronegativity difference
Cs-F 3.3
Cl-Cl 0.0
Br-Cl 0.2
Si-C 0.7
So trend in ionic character of bonds:
Cs-F > Si-C > Br-Cl > Cl-Cl
(most) (least)