If potential energy of an electron in ground state is -13.6 eV. The energy of next higher state is:
a) -27.2 eV
b) -6.8 eV
c) -3.4 eV
d) none of these
please help me. Is it B?
If I understand you question, yes, B is the correct answer. The energy of the levels are negative and go to zero when the electron is at infinity; i.e., when the atom is ionized. The NEXT high level would be C after B. I hope this helps.
-3.4
Well, actually, it's none of these options! The energy of the next higher state is exactly -13.5 eV. Why? Well, you see, the energy levels in an atom are quantized, just like your ice cream servings when you're on a diet. You can only have certain specific values, and there's no room for in-between flavors! So, the energy of the next level is not exactly double the energy of the ground state. It's close, but not quite there. Don't worry, though. At least you won't have to face the agony of choosing between options A, B, or C. It's always nice to have fewer options, isn't it?
No, actually, the correct answer is A) -27.2 eV.
The potential energy of an electron in the ground state of an atom is given by -13.6 eV. In the Bohr model of the atom, the energy levels are quantized, meaning they can only have certain specific values. The energy difference between each level is given by the equation:
ΔE = -13.6 eV / n^2
where n is the principle quantum number of the level. For the ground state (n=1), the energy difference to the next higher state (n=2) would be:
ΔE = -13.6 eV / 2^2 = -13.6 eV / 4 = -3.4 eV
So, the energy of the next higher state is -3.4 eV, which corresponds to option C in the given answers. Therefore, the correct answer is C) -3.4 eV. My apologies for the previous incorrect response.
To get the answer, you need to understand the concept of electron energy levels in an atom. The energy levels of an electron in an atom are quantized, meaning they can only have certain specific values. These values are represented by negative numbers and are measured in electron volts (eV).
The ground state of an electron is the lowest energy level it can occupy. In this case, the potential energy of an electron in the ground state is given as -13.6 eV.
To find the energy of the next higher state, you need to realize that the energy levels in an atom follow a specific pattern. The energy difference between two consecutive levels is given by the Rydberg formula:
ΔE = -13.6 eV * (1/nf² - 1/ni²)
Where ΔE is the energy difference, nf is the final energy level, and ni is the initial energy level.
In this case, we are moving from the ground state (initial energy level) to the next higher state (final energy level). Substituting ni = 1 and nf = 2 into the formula, we get:
ΔE = -13.6 eV * (1/2² - 1/1²)
= -13.6 eV * (1/4 - 1/1)
= -13.6 eV * (1/4 - 4/4)
= -13.6 eV * (-3/4)
= 10.2 eV
Therefore, the energy of the next higher state is 10.2 eV. Since none of the answer options given in the question match this value, the correct answer should be "none of these."