---

Question 1:

What causes the appearance of spectral lines in a spectroscopic analysis?

A) Absorption of light by the sample
B) Emission of light by the sample
C) Scattering of light by the sample
D) Interference of light waves

Show Answer

Explanation: The correct answer is B) Emission of light by the sample. The appearance of spectral lines in a spectroscopic analysis is caused by the emission of light by the sample. When excited, atoms or molecules in the sample undergo energy transitions, emitting light at specific wavelengths corresponding to the energy differences between the involved energy levels.

---

Question 2:

What is the relationship between the energy of an energy transition and the frequency of the emitted light?

A) Directly proportional
B) Inversely proportional
C) No relationship
D) Random relationship

Show Answer

Explanation: The correct answer is A) Directly proportional. The energy of an energy transition between two energy levels in an atom or molecule is directly proportional to the frequency of the emitted light. This relationship is described by the equation E = hf, where E is the energy, h is Planck's constant, and f is the frequency of the light.

---

Question 3:

What is the term for the lowest energy level of an atom or molecule?

A) Ground state
B) Excited state
C) Ionization state
D) Discrete state

Show Answer

Explanation: The correct answer is A) Ground state. The ground state refers to the lowest energy level of an atom or molecule. When an atom or molecule is in its ground state, its electrons occupy the energy levels closest to the nucleus and are at their lowest energy state.

---

Question 4:

What is the term for the process where an electron moves from a higher energy level to a lower energy level?

A) Absorption
B) Emission
C) Excitation
D) Deexcitation

Show Answer

Explanation: The correct answer is D) Deexcitation. Deexcitation refers to the process where an electron moves from a higher energy level to a lower energy level within an atom or molecule. During this process, energy is released in the form of light, resulting in the emission of spectral lines.

---

Question 5:

What does the number of spectral lines in an emission spectrum indicate?

A) The number of energy levels in the sample
B) The chemical composition of the sample
C) The energy differences between the energy levels
D) The temperature of the sample

Show Answer

Explanation: The correct answer is C) The energy differences between the energy levels. The number of spectral lines in an emission spectrum indicates the energy differences between the energy levels in the sample. Each spectral line corresponds to a specific energy transition, and the overall pattern of spectral lines provides information about the energy level structure and electronic configuration of the atoms or molecules in the sample.