What is the difference in energy between the two levels responsible for the ultraviolet emission line of the magnesium atom at 285.2 nm?

#### Solution:

Show me the final answer↓

We will first figure out the frequency, and use that value to calculate the difference in energy.

The first equation we will use is:

(Where v is frequency, c is speed of light, and \lambda is wavelength)

The question states that the line of emission for the magnesium atom is at 285.2 nm. We will write this value in meters.

Let us substitute the values into our equation to figure out the frequency.

(The speed of light is equal to 2.998 \times 10^8 m/s)

v\,=\,1.05 \times 10^{15} /s

We will now use the following formula to figure out the energy.

(Where E is energy, h is the Planck’s constant, and v is the frequency)

E\,=\,(6.626\times 10^{-34}\text{J}\cdot \text{s})(1.05 \times 10^{15}\text{/s})

E\,=\,6.96\times 10^{-19} J

#### Final Answer:

Wow this is great guys

Glad it helped you 🙂

This doesn’t solve the question, though. The question is asking for the difference in energy between the two levels responsible for the ultraviolet emission line of the magnesium, not just the energy of the wavelength.

I am not sure what you mean? What we found is the difference in energy levels.