Which one of the following electron transitions would result in the loss of energy from a hydrogen atom?
a. n=1 to n=3
b. n=5 to n=3
c. n=4 to n=6
d. n=1 to n=5
Well, let's break this down in a fun way, shall we?
Now imagine the hydrogen atom is at a party, having a blast with its electrons. But suddenly, it realizes, "Oh no, I've got to lose some energy! Who's up for making this party a little less energetic?"
In option a, the electron transitions from n=1 to n=3. But hey, n=3 sounds like it's having a wild time, so it wouldn't result in the loss of energy.
In option b, the electron transitions from n=5 to n=3. Well, n=5 seems pretty excited too, so the energy loss doesn't happen here.
In option c, the electron transitions from n=4 to n=6. Hold up, n=6 sounds like a higher energy level, so the hydrogen atom would actually gain energy instead of losing it.
Finally, in option d, the electron transitions from n=1 to n=5. Ah-ha! This means that the hydrogen atom loses energy, as n=5 isn't as energetic as n=1.
So, the correct answer is d. The hydrogen atom would lose energy by transitioning from n=1 to n=5, making it the party pooper at the atomic shindig.
To determine which electron transition would result in the loss of energy from a hydrogen atom, we need to compare the energy levels of the initial and final states.
The energy of an electron in a hydrogen atom is given by the equation: E = -13.6 eV / n^2, where n is the principal quantum number.
a. n=1 to n=3: Initial state energy = -13.6 eV / (1^2) = -13.6 eV
Final state energy = -13.6 eV / (3^2) = -1.51 eV
b. n=5 to n=3: Initial state energy = -13.6 eV / (5^2) = -0.544 eV
Final state energy = -13.6 eV / (3^2) = -1.51 eV
c. n=4 to n=6: Initial state energy = -13.6 eV / (4^2) = -0.85 eV
Final state energy = -13.6 eV / (6^2) = -0.301 eV
d. n=1 to n=5: Initial state energy = -13.6 eV / (1^2) = -13.6 eV
Final state energy = -13.6 eV / (5^2) = -0.544 eV
From the above calculations, we can see that option a. n=1 to n=3 is the only transition that results in the loss of energy from a hydrogen atom. The energy decreases from -13.6 eV to -1.51 eV.
To determine which of the given electron transitions would result in the loss of energy from a hydrogen atom, we need to understand the energy levels in the hydrogen atom.
The energy levels in a hydrogen atom are described by the principal quantum number (n). The energy of an electron in a hydrogen atom is inversely proportional to the square of the principal quantum number (E ∝ 1/n^2).
As the electron transitions between different energy levels, it can either absorb or release energy. When an electron transitions to a higher energy level, it absorbs energy. Conversely, when an electron transitions to a lower energy level, it releases energy in the form of electromagnetic radiation, such as visible light or ultraviolet radiation.
Now, let's examine the given electron transitions:
a. n=1 to n=3: This transition involves the electron moving from a lower energy level (n=1) to a higher energy level (n=3). Therefore, energy would be absorbed.
b. n=5 to n=3: This transition involves the electron moving from a higher energy level (n=5) to a lower energy level (n=3). Therefore, energy would be released.
c. n=4 to n=6: This transition involves the electron moving from a lower energy level (n=4) to a higher energy level (n=6). Therefore, energy would be absorbed.
d. n=1 to n=5: This transition involves the electron moving from a lower energy level (n=1) to a higher energy level (n=5). Therefore, energy would be absorbed.
Based on the explanations above, the correct answer is b. The electron transition from n=5 to n=3 would result in the loss of energy from a hydrogen atom.