/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 17 Arrange the following kinds of e... [FREE SOLUTION] | 91Ó°ÊÓ

91Ó°ÊÓ

Arrange the following kinds of electromagnetic radiation in order of increasing wavelength: infrared, green light, red light, radio waves, X rays, ultraviolet light.

Short Answer

Expert verified
X-rays, ultraviolet light, green light, red light, infrared, radio waves.

Step by step solution

01

Understand the Electromagnetic Spectrum

The electromagnetic spectrum is the range of all types of electromagnetic radiation. Radiation is categorized by wavelength from shortest to longest. Gamma rays have the shortest wavelengths followed by X-rays, ultraviolet rays, visible light (which includes violet, indigo, blue, green, yellow, orange, and red), infrared rays, microwaves, and lastly, radio waves, which have the longest wavelengths.
02

Identify Wavelengths of Given Radiations

List the given types of electromagnetic radiation and categorize them according to their typical positions on the electromagnetic spectrum: 1. X-rays 2. Ultraviolet light 3. Green light 4. Red light 5. Infrared 6. Radio waves.
03

Arrange in Order of Increasing Wavelength

Based on the electromagnetic spectrum, order the radiation from shortest to longest wavelength: 1. X-rays (shortest) 2. Ultraviolet light 3. Green light 4. Red light 5. Infrared 6. Radio waves (longest).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91Ó°ÊÓ!

Key Concepts

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

Wavelength
Understanding wavelength is key when discussing the electromagnetic spectrum. Wavelength is the distance between two consecutive peaks of a wave. It is typically measured in meters, centimeters, or nanometers.
In the electromagnetic spectrum, different types of radiation are categorized based on their wavelength. Shorter wavelengths correspond to higher energy radiation, while longer wavelengths have lower energy.
For instance, X-rays have short wavelengths and thus carry a lot of energy. On the other hand, radio waves have long wavelengths and consequently lower energy levels.
Electromagnetic Radiation
Electromagnetic radiation is a form of energy that travels through space at the speed of light. This radiation spans a broad range, known as the electromagnetic spectrum, which encompasses different types of waves, each with varying properties.
- From the short-wavelength, high-energy gamma rays and X-rays, - To the longer-wavelength, lower-energy radio waves.
All electromagnetic waves share similar properties, such as traveling in a vacuum and being composed of oscillating electric and magnetic fields at right angles to each other. Each type of radiation interacts differently with matter, making them useful for different applications.
Understanding electromagnetic radiation allows us to harness its properties for communication, medical imaging, and other technologies.
Infrared
Infrared (IR) radiation resides just beyond the red end of the visible light spectrum. It has longer wavelengths than visible light but shorter than microwaves.
Infrared radiation is primarily known for its heat-emitting properties. Everything that generates heat gives off infrared radiation, which is why it's often used in thermal imaging.
Some common applications of infrared radiation include:
  • Remote controls for TVs and other electronic devices
  • Night vision equipment
  • Environmental and weather monitoring
Infrared's ability to project heat makes it invaluable in scientific and technological fields.
X Rays
X-rays are a type of electromagnetic radiation with very short wavelengths and high energy. Because of their high energy, X-rays can penetrate most substances, which makes them incredibly useful in medical imaging to view the inside of the human body.
Some key points about X-rays include:
  • They can be used to detect fractures in bones and other medical conditions.
  • X-rays are also used in airport security scanners.
  • However, excessive exposure to X-rays can increase the risk of cancer due to their high energy levels.
Despite the risks, the benefits of X-rays in medical diagnostics make them an essential tool in modern medicine.
Ultraviolet Light
Ultraviolet (UV) light is positioned between visible light and X-rays in the electromagnetic spectrum. It has shorter wavelengths than visible light, which gives it higher energy.
UV light is most familiar to us as a component of sunlight. It causes sunburn when one's skin is exposed for too long without protection.
Here are some important uses and effects of UV light:
  • Used in sterilizing equipment due to its ability to kill bacteria and viruses.
  • Helps the human body produce Vitamin D.
  • Overexposure can lead to skin cancer and other harmful effects.
Understanding UV light helps inform safety practices like wearing sunscreen to protect against its potential damaging effects.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The discovery of hafnium, element number \(72,\) provided a controversial episode in chemistry. G. Urbain, a French chemist, claimed in 1911 to have isolated an element number 72 from a sample of rare earth (elements \(58-71)\) compounds. However, Niels Bohr believed that hafnium was more likely to be found along with zirconium than with the rare earths. D. Coster and G. von Hevesy, working in Bohr's laboratory in Copenhagen, showed in 1922 that element 72 was present in a sample of Norwegian zircon, an ore of zirconium. (The name hafnium comes from the Latin name for Copenhagen, Hafnia). (a) How would you use electron configuration arguments to justify Bohr's prediction? (b) Zirconium, hafnium's neighbor in group \(4 \mathrm{~B}\), can be produced as a metal by reduction of solid \(\mathrm{ZrCl}_{4}\) with molten sodium metal. Write a balanced chemical equation for the reaction. Is this an oxidation- reduction reaction? If yes, what is reduced and what is oxidized? (c) Solid zirconium dioxide, \(\mathrm{ZrO}_{2}\), reacts with chlorine gas in the presence of carbon. The products of the reaction are \(\mathrm{ZrCl}_{4}\) and two gases, \(\mathrm{CO}_{2}\) and \(\mathrm{CO}\) in the ratio \(1: 2 .\) Write a balanced chemical equation for the reaction. Starting with a 55.4 -g sample of \(\mathrm{ZrO}_{2},\) calculate the mass of \(\mathrm{ZrCl}_{4}\) formed, assuming that \(\mathrm{ZrO}_{2}\) is the limiting reagent and assuming \(100 \%\) yield. (d) Using their electron configurations, account for the fact that \(\mathrm{Zr}\) and \(\mathrm{Hf}\) form chlorides \(\mathrm{MCl}_{4}\) and oxides \(\mathrm{MO}_{2}\).

Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? (a) from \(n=3\) to \(n=2\), (b) from an orbit of radius \(0.846 \mathrm{nm}\) to one of radius 0.212 \(\mathrm{nm},(\mathbf{c})\) an electron adds to the \(\mathrm{H}^{+}\) ion and ends up in the \(n=2\) shell?

If human height were quantized in 1 -cm increments, what would happen to the height of a child as she grows up: (i) the child's height would never change, (ii) the child's height would continuously increase, (iii) the child's height would increase in jumps of \(6 \mathrm{~cm},\) or (iv) the child's height would increase in "jumps" of \(1 \mathrm{~cm}\) at a time?

(a) The average distance from the nucleus of a 3 s electron in a chlorine atom is smaller than that for a \(3 p\) electron. In light of this fact, which orbital is higher in energy? (b) Would you expect it to require more or less energy to remove a \(3 s\) electron from the chlorine atom, as compared with a \(2 p\) electron?

The Lyman series of emission lines of the hydrogen atom are those for which \(n_{\mathrm{f}}=1 .\) (a) Determine the region of the electromagnetic spectrum in which the lines of the Lyman series are observed. (b) Calculate the wavelengths of the first three lines in the Lyman series-those for which \(n_{\mathrm{i}}=2,3,\) and 4 .

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.