Q: A photon has a wavelength of $$500 \ \mathrm{nm}. $$What is its frequency? (Speed of light $$c = 3.00 \times 10^8$ \ \mathrm{m/s})$$

$$6.00 \times 10$$^{14}$$ \ \mathrm{Hz}$$

Question 1

Which of the following best explains how astronomers use light to identify elements in distant nebulae, such as the Crab Nebula shown in the image?

Accepted Answer

By analyzing the emitted light wavelengths and matching them to the characteristic emission spectra of specific ions.

Question 2

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

Accepted Answer

$$E = h \, v$$

Question 3

According to the Bohr model, what happens when an electron in a hydrogen atom transitions from $$n=3 to$$ $$n=2$$?

Accepted Answer

The atom emits a photon with energy equal to the difference between the two energy levels.

Question 4

Which of the following statements about electromagnetic radiation is correct?

Accepted Answer

As the frequency of electromagnetic radiation increases, its energy increases.

Question 5

A photon has a wavelength of $$500 \ \mathrm{nm}. $$What is its frequency? (Speed of light $$c = 3.00 	imes 10^8$ \ \mathrm{m/s})$$

Accepted Answer

$$6.00 	imes 10$$^{14}$$ \ \mathrm{Hz}$$

Question 6

Which of the following best describes the trend in atomic radius across a period from left to right in the periodic table?

Accepted Answer

Atomic radius decreases due to increasing effective nuclear charge.

Question 7

Which of the following electron configurations represents a noble gas?

Accepted Answer

$$1s^2$$ \, $$2s^2$$ \, $$2p^6$$

Question 8

Which of the following best explains why the ionization energy generally increases across a period?

Accepted Answer

The effective nuclear charge increases, holding electrons more tightly.

Question 9

Which of the following is the correct order of electromagnetic radiation from lowest to highest energy?

Accepted Answer

Microwave \u003c Infrared \u003c Visible \u003c Ultraviolet \u003c X-ray

Question 10

A sodium atom emits a photon as an electron falls from a higher energy level to a lower one. Which principle explains the quantized nature of this emission?

Accepted Answer

The quantization of energy levels in atoms

Question 11

Which of the following elements has the highest first ionization energy?

Accepted Answer

Neon

Question 12

Which of the following is the correct electron configuration for phosphorus ($$Z=15$$)?

Accepted Answer

$$1s^2$$ \, $$2s^2$$ \, $$2p^6$$ \, $$3s^2$$ \, $$3p^3$$

Question 13

Which of the following statements about blackbody radiation is correct?

Accepted Answer

The peak wavelength of emission shifts to shorter wavelengths as temperature increases.

Question 14

Which of the following best describes the relationship between wavelength ($$\lambda) $$and frequency ($$v) of $$electromagnetic radiation?

Accepted Answer

$$c = \lambda v$$

Question 15

Which of the following ions is most likely responsible for the green filaments observed in the Crab Nebula image?

Accepted Answer

$$\mathrm{S}^{2+}$$

Question 16

Which of the following best explains why electrons in atoms occupy discrete energy levels?

Accepted Answer

Because the wave nature of electrons allows only certain standing wave patterns.

Question 17

A photon with energy $$3.09 \ \mathrm{eV} is $$emitted from a hydrogen atom. Which transition is most likely responsible for this emission?

Accepted Answer

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

Question 18

Which of the following best describes the trend in ionization energy down a group in the periodic table?

Accepted Answer

Ionization energy decreases due to increasing atomic radius and electron shielding.

Question 19

Which of the following is the correct order of filling for atomic orbitals according to the Aufbau principle?

Accepted Answer

$$1s \rightarrow 2s \rightarrow 2p \rightarrow 3s \rightarrow 3p \rightarrow 4s \rightarrow 3d$$

Question 20

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

Accepted Answer

Because electrons transition between quantized energy levels, emitting photons of specific energies.

Electronic Structure and Periodic Properties of Elements

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