1.

If the energy of a photon is 1.32 × 10^-18 J, what is its wavelength in nm?

2.

The energy of an electron in the hydrogen atom is determined by what?

Delete above response

1. To calculate the wavelength of a photon, we can use the equation:

wavelength = (speed of light) / (frequency)

First, we need to find the frequency of the photon. The energy of a photon can be calculated using the equation:

energy = Planck's constant × frequency

Therefore, rearranging the equation gives us:

frequency = energy / Planck's constant

Next, we can substitute the given energy value into the equation:

frequency = 1.32 × 10^-18 J / (6.63 × 10^-34 J·s)

Simplifying this expression gives us:

frequency = 1.99 × 10^15 Hz

Now, we can substitute this frequency value into the first equation to calculate the wavelength:

wavelength = (speed of light) / (frequency)
wavelength = (3 × 10^8 m/s) / (1.99 × 10^15 Hz)

Finally, we can convert the wavelength into nanometers (nm) by multiplying the resulting value by 10^9:

wavelength = [(3 × 10^8 m/s) / (1.99 × 10^15 Hz)] * (10^9 nm/m)

This gives us the final answer for the wavelength of the photon in nm.

2.

The energy of an electron in the hydrogen atom is determined by its energy level or orbital. It is determined using the equation:

energy = -13.6 eV / (n^2)

where "n" represents the principal quantum number or the energy level of the electron. The energy level is an integer value starting from 1 (corresponding to the ground state) and increases as the energy of the electron increases.

The equation shows that as the value of "n" increases, the energy of the electron becomes less negative (i.e., it becomes more positive and moves farther away from the nucleus). This means that electrons in higher energy levels have higher energy.

1. To find the wavelength of a photon, you can use the equation:

wavelength = (speed of light) / (frequency)

However, we can also relate the energy of a photon to its wavelength using the equation:

energy = (Planck's constant) x (speed of light) / (wavelength)

To find the wavelength, we need to rearrange the equation:

wavelength = (Planck's constant) x (speed of light) / (energy)

Given that the energy of the photon is 1.32 × 10^-18 J, we can substitute it into the equation:

wavelength = (6.626 × 10^-34 J·s) x (3.0 × 10^8 m/s) / (1.32 × 10^-18 J)

Calculating the expression, we get:

wavelength ≈ 1.5 × 10^-6 meters

To convert this to nanometers (nm), we multiply by 10^9:

wavelength ≈ 1.5 × 10^3 nm

Therefore, the wavelength of the photon is approximately 1.5 × 10^3 nm.

2. The energy of an electron in the hydrogen atom is determined by its energy level or orbital. In the hydrogen atom, the energy levels are represented by the quantum number "n." The formula for the energy of the electron in the hydrogen atom is given by:

E = -13.6 eV / n^2

Here, E represents the energy of the electron in electron volts (eV), and "n" represents the principal quantum number.

The energy levels in the hydrogen atom are discrete and quantized, meaning that only specific energy values are allowed. As the electron moves further away from the nucleus (higher values of "n"), the energy increases, and the electron becomes less tightly bound.

So, the energy of an electron in the hydrogen atom is determined by its principal quantum number "n." Each energy level corresponds to a particular orbital where the electron may reside.

1. E = hc/wavelength. Solve for wavelength in meters and convert to nm.

2. By the orbit/shell/energy level (take your pick) in which it is located.