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Chapter 3: Problem 74

Passing an electrical charge through argon gas contained in a partially evacuated vessel yields which of the following? a. A line spectrum b. A continuous spectrum c. No visible change d. White light

Short Answer

Expert verified
The answer is (a) A line spectrum.

Step by step solution

01

Understanding the context

When an electrical discharge passes through an inert gas like argon in a partially evacuated vessel, the gas becomes excited, and electrons within the atoms move to higher energy levels. Upon returning to lower energy levels, these electrons will emit light.
02

Distinguishing types of spectra

A continuous spectrum shows all wavelengths of light, like a rainbow, typically produced by incandescent solids, liquids, or high-pressure gases. A line spectrum, on the other hand, consists of specific lines of color, each corresponding to a specific wavelength of light emitted by electrons in an atom transitioning between energy levels.
03

Evaluating which spectrum is produced by argon

In this scenario, argon gas, being an element, emits light at specific wavelengths when the electrical charge excites its electrons. As a result, a line spectrum consisting of distinct lines of color is produced.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Argon Gas Excitation
Argon gas excitation is a fascinating process that occurs when argon atoms receive energy from an external source, such as an electrical discharge. This energy excites the electrons in the argon atoms, pushing them to higher energy levels. Excitation is essentially the process of adding energy to the argon's electrons, which can absorb only certain amounts of energy.
  • Argon is an inert gas, meaning it typically doesn鈥檛 react chemically with other elements. However, it does have electron shells that can be excited with the right amount of energy.
  • Excitation occurs when electrical energy is introduced to the gaseous argon. This energy source, such as a spark or an electrical discharge, provides the needed boost.
Once the electrons in argon's atoms are excited, they are primed to return to their ground state, a journey that results in the emission of light.
Electrical Discharge in Gases
Electrical discharge in gases is a key method for exciting atoms in gaseous elements like argon. When you apply electrical energy to a gas, it causes the gas to conduct electricity through the excitation of its electrons.
  • Electricity flows through the gas, similar to a current through a wire, ionizing the gas and making it a conductor.
  • This ionization can energize electrons, causing them to jump to higher energy levels.
  • As gases like argon become electrically activated, they emit light at certain wavelengths because of the transitions of electrons.
This phenomena produces distinct visual outputs depending on the gas involved, often resulting in vivid colors that are visible to the naked eye.
Emission Spectra
Emission spectra occur when electrons fall back to their original, or ground, state after being excited. Each drop emits a photon, a particle of light, with an energy that corresponds to the difference between the two energy levels.
  • Every element has a unique set of energy levels for its electrons, which means each element鈥檚 emission spectrum is distinct.
  • This is why an emission spectrum appears as a series of colorful lines, where each line represents a particular transition between energy levels.
  • For argon, the emission spectrum will consist of several discrete lines, each indicative of the specific energy transitions of argon鈥檚 electrons.
The study of these spectra allows scientists to identify the elements present in a sample and to understand the atomic structure of each element.
Energy Level Transitions in Atoms
Energy level transitions in atoms are a foundational concept in understanding how line spectra are formed. These transitions occur when an electron moves between orbitals within an atom, either absorbing or emitting energy in the form of light.
  • Electrons reside in distinct energy levels or shells around an atom's nucleus. Each element has a unique arrangement of these levels.
  • When an electron absorbs energy, it transitions to a higher energy level. Conversely, when it emits energy, it falls back to a lower energy level.
  • The light emitted corresponds to the energy difference between the two levels involved in the transition, appearing as a specific spectral line.
This is why, when argon or any other element is excited, it produces a line spectrum unique to its own atomic structure. By analyzing these lines, scientists can gain insights into the electronic structure of atoms.

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Most popular questions from this chapter

The de Broglie wavelength associated with a ball of mass \(1 \mathrm{~kg}\) having a kinetic energy \(0.5 \mathrm{~J}\) is a. \(6.626 \times 10^{-34} \mathrm{~m}\) b. \(13.2 \times 10^{-34} \mathrm{~m}\) c. \(10.38 \times 10^{21} \mathrm{~m}\) d. \(6.626 \AA\)

(A): Atoms can neither be created not destroyed. ( \(\mathbf{R}\) ): Under similar conditions of temperature and pressure, equal volumes of gases do not contain equal number of atoms.

Which of the following statement(s) about spectral series is/are correct? a. Paschen series appears in the infrared region b. The lines in the Balmer series corresponds to electron transitions from energy levels higher than \(\mathrm{n}=2\) energy level. c. Transitions from higher energy levels to \(5^{\text {th }}\) energy level produce Pfund series which falls in the infrared region d. The lines of Lyman series appear in the visible region

How many moles of electrons weigh one kilogram? (mass of electron \(=9.108 \times 10^{-31} \mathrm{~kg}\), Avogadro number \(=6.023 \times 10^{23}\) ) a. \(6.023 \times 10^{23}\) b. \(1 / 9.108 \times 10^{31}\) c. \(\frac{6.023}{9.108} \times 10^{54}\) d. \(\frac{1}{9.108 \times 6.023} \times 10^{8}\)

Which of the following statement(s) is/are correct? a. Planck's study of black-body radiation led to the hypothesis that radiation is emitted in quantas of energy b. Photons of lower frequency radiation have lower energies. c. Bohr's model of the hydrogen atom showed emission of energy by atoms occurs when an electron moves to a higher orbit. d. The lowest energy state of an electron in an atom is known as the ground state
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