Question 1

Which statement best describes the dual nature of light as discussed in the experiment?

Accepted Answer

Light exhibits both wave-like and particle-like properties.

Question 2

According to the Bohr model, what is the energy (in J) of the electron in the n = 1 energy level of the hydrogen atom?

Accepted Answer

$$-21.79 	imes 10$$^{-19}$$

Question 3

Which equation correctly relates the energy of a photon to its frequency?

Accepted Answer

$$E = h
u$$

Question 4

A hydrogen atom electron transitions from $$n=5 to$$ $$n=2. $$Which of the following best describes the process?

Accepted Answer

The atom emits energy and the electron moves to a lower energy level.

Question 5

Given Planck’s constant $$h = 6.626 	imes 10$$^{-34}$$ Js and the speed of light c = 3.00$$ 	imes $$10^8 m/s$$, what is the wavelength (in nm) of a photon with energy $$3.03 	imes 10$$^{-19}$$ J?

Accepted Answer

$$656 nm$$

Question 6

Which transition in the hydrogen atom produces the photon with the highest energy?

Accepted Answer

$$n=2 to$$ $$n=1$$

Question 7

If the energy difference between two levels in a hydrogen atom is $$4.09 	imes 10$$^{-19}$$ J, what is the frequency of the emitted photon?

Accepted Answer

$$6.17 	imes 10$$^{14}$$ Hz

Question 8

Which of the following best explains why the emission spectrum of hydrogen consists of discrete lines?

Accepted Answer

The energy levels of the hydrogen atom are quantized.

Question 9

A student observes a red line in the hydrogen spectrum at $$656 nm. $$Which electronic transition does this correspond to?

Accepted Answer

$$n=3 to$$ $$n=2$$

Question 10

Which of the following is true about the ground state of the hydrogen atom?

Accepted Answer

The electron is in the lowest possible energy level.

Question 11

Calculate the energy (in J) of a photon with a wavelength of $$486 nm.$$

Accepted Answer

$$4.09 	imes 10$$^{-19}$$ J

Question 12

Which of the following transitions in the hydrogen atom would emit ultraviolet light?

Accepted Answer

$$n=2 to$$ $$n=1$$

Question 13

A neon sign emits light because:

Accepted Answer

Electrons in neon atoms absorb energy and move to higher energy levels, then emit photons as they return to lower levels.

Question 14

Which formula would you use to calculate the wavelength of light emitted during an electronic transition in hydrogen?

Accepted Answer

$$\lambda = \dfrac{hc}{\Delta E}$$

Question 15

Which of the following best describes the relationship between the energy and wavelength of emitted light?

Accepted Answer

Energy is inversely proportional to wavelength.

Question 16

A student calculates the energy for $$n=4 in $$the hydrogen atom using Bohr’s equation. Which value is closest to the correct answer?

Accepted Answer

$$-1.36 	imes 10$$^{-19}$$ J

Question 17

Which of the following is NOT a possible reason for discrepancies between experimental and calculated wavelengths in the hydrogen spectrum?

Accepted Answer

The quantization of energy levels is not real.

Question 18

Which transition in the hydrogen atom corresponds to the emission of the shortest wavelength photon?

Accepted Answer

$$n=6 to$$ $$n=1$$

Question 19

Why are only certain wavelengths observed in the emission spectrum of hydrogen?

Accepted Answer

Because electrons can only occupy specific energy levels.

Question 20

Which of the following best describes the process of constructing an energy level diagram for hydrogen?

Accepted Answer

Draw horizontal lines for each energy level, label with $$n$$ and energy, indicate ground state, and show transitions as arrows labeled with wavelength and color.

Line Spectrum and Electronic Transitions in the Hydrogen Atom

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