E6------E= -0.378eV
E5------E= -0.544eV
E4------E= -0.850eV
E3------E= -1.51eV
E2------E= -3.40eV
Use the figure shown above to determine how much energy a hydrogen atom with its electron in the E2 energy level must absorb for the electron to be removed from the atom.
a. -0.378 eV
b. -3.40 eV
c. 3.40 eV
d. 0.378 eV
I got c.3.40 I think I am right? If I am not please explain why.
looks good
To determine how much energy a hydrogen atom with its electron in the E2 energy level must absorb for the electron to be removed from the atom, we need to look at the energy difference between the E2 energy level and the highest energy level shown in the figure.
From the figure, we can see that the highest energy level mentioned is E6 with an energy of -0.378 eV. The energy of the electron in the E2 energy level is -3.40 eV.
To remove an electron from an atom, we need to provide energy equal to or greater than the difference between the energy levels. In this case, the energy difference is:
-0.378 eV (E6 energy) - (-3.40 eV) (E2 energy) = 3.022 eV
Therefore, the correct answer is c. 3.40 eV, which is the closest value to 3.022 eV. You are correct!