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Chapter 2: Problem 34

Scientists use emission spectra to confirm the presence of an element in materials of unknown composition. Why is this possible?

Short Answer

Expert verified
Scientists use emission spectra to confirm the presence of an element in materials of unknown composition because each element has a unique set of energy levels for its electrons, which results in a unique emission spectrum when its electrons are excited and then return to lower energy levels, releasing energy as light. By comparing a sample's emission spectrum to known emission spectra of various elements, scientists can identify and confirm the presence of specific elements in the material, making it a reliable method for analyzing unknown compositions.

Step by step solution

01

Understand Emission Spectra

Emission spectra are the unique patterns of wavelengths (colors) of light emitted by an energy source, such as a heated or irradiated substance. Each element has a unique set of energy levels for its electrons, and when electrons in these elements are excited (given additional energy), they jump to higher energy levels. However, the electrons aren't stable at these higher energy levels, and they return to the original, lower energy levels. In the process, they release energy in the form of light, which generates the characteristic emission spectrum for the element.
02

Generate Emission Spectra

To generate an emission spectrum from a sample, a scientist will first expose the sample to a high-energy source, such as an electric discharge or a flame. This energy source excites the electrons in the atoms of the sample, causing them to jump to higher energy levels. When the electrons return to their original energy levels, they emit light that can be analyzed with a spectroscope, which separates the light into its component wavelengths. This produces a pattern of bright lines, called the emission spectrum, unique to the element being analyzed.
03

Identify Elements by Unique Spectra

Since each element has a unique set of energy levels for its electrons, the emitted light - and thus, the emission spectrum - is characteristic of the element. This means that when a sample's emission spectrum is observed, it can be compared to known emission spectra of various elements. If the emission spectrum of the sample matches the known emission spectrum of a particular element, then that confirms the presence of the element in the material being analyzed.
04

Application to Unknown Composition Analysis

When analyzing materials of unknown composition, emission spectra can be used to determine which elements are present in the sample as well as their relative concentrations. By comparing the emission spectra of the sample to the known emission spectra of various elements, scientists can identify and confirm the presence of specific elements in the material. This method is widely used in areas such as environmental testing, forensic science, and quality control in manufacturing, to ensure the materials being used meet required specifications.

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Most popular questions from this chapter

Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of electromagnetic radiation that can completely remove (ionize) the electron from the H atom is \(1460 \mathrm{nm}\). What is the initial excited state for the electron \((n=?) ?\)

Calculate, to four significant figures, the longest and shortest wavelengths of light emitted by electrons in the hydrogen atom that begin in the \(n=5\) state and then fall to states with smaller values of \(n\).

Give the maximum number of electrons in an atom that can have these quantum numbers: a. \(n=4\) b. \(n=5, m_{\ell}=+1\) c. \(n=5, m_{s}=+\frac{1}{2}\) d. \(n=3, \ell=2\) e. \(n=2, \ell=1\)

Although no currently known elements contain electrons in \(g\) orbitals in the ground state, it is possible that these elements will be found or that electrons in excited states of known elements could be in \(g\) orbitals. For \(g\) orbitals, the value of \(\ell\) is 4 What is the lowest value of \(n\) for which \(g\) orbitals could exist? What are the possible values of \(m_{\ell} ?\) How many electrons could a set of \(g\) orbitals hold?

Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. When light hits the AgCl particles, the following reaction occurs: $$ \operatorname{AgCl} \stackrel{h v}{\longrightarrow} \mathrm{Ag}+\mathrm{Cl} $$ The silver metal that is formed causes the lenses to darken. The energy change for this reaction is \(3.10 \times 10^{2} \mathrm{kJ} / \mathrm{mol} .\) Assuming all this energy must be supplied by light, what is the maximum wavelength of light that can cause this reaction?
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