Question

If clusters are broken up using lasers in the near-infrared to radio-frequency range of the spectrum, what frequencies could used to break a chemical bond? 1\. Far infrared 2\. Microwave 3\. Ultraviolet 4\. Red light

Short answer

The frequencies that could be used to break a chemical bond in the near-infrared to radio-frequency range are: 1. Far infrared (with a frequency range of \(10^{12}\) to \(10^{14}\) Hz) 2. Microwave (with a frequency range of \(10^9\) to \(10^{12}\) Hz) Hence, the correct answer consists of options 1 and 2.

Step-by-step solution

Understand the electromagnetic spectrum ranges and frequencies

The first step is to understand the electromagnetic spectrum and the corresponding frequencies of the given options. The electromagnetic spectrum includes various types of waves, and each has a specific frequency range.

List the frequency ranges of the given options

Now, let's list down the frequency ranges for the options mentioned in the exercise: 1. Far infrared: \(10^{12}\) to \(10^{14}\) Hz 2. Microwave: \(10^9\) to \(10^{12}\) Hz 3. Ultraviolet: \(7.5 \times 10^{14}\) to \(3 \times 10^{16}\) Hz 4. Red light: \(4 \times 10^{14}\) to \(4.8 \times 10^{14}\) Hz

Compare the frequency ranges to the breaking of chemical bonds

In general, breaking of chemical bonds requires a significant amount of energy, which translates to higher frequencies on the electromagnetic spectrum. Hence, we need to identify which of the options has a frequency in the near-infrared to the radio-frequency range that is suitable for breaking chemical bonds. After comparing the given options with their frequency ranges, the most likely frequencies that can break a chemical bond in the near-infrared to radio-frequency range would be: 1. Far infrared 2. Microwave

Determine the answer

Based on the analysis, we can conclude that the frequencies that could be used to break a chemical bond in the near-infrared to radio-frequency range are: 1. Far infrared (Option 1) 2. Microwave (Option 2) So, the correct answer consists of options 1 and 2.

Key concepts

Chemical Bonds

Chemical bonds are the connections between atoms within a molecule. They determine the stability and properties of a molecule. There are several types of chemical bonds, such as:

• Covalent Bonds: These occur when atoms share electrons to achieve stability.
• Ionic Bonds: These form when one atom donates an electron to another, resulting in positive and negative charges that hold the atoms together.
• Hydrogen Bonds: Weaker than covalent and ionic bonds, these occur between molecules when hydrogen is attracted to a more electronegative atom.

Breaking chemical bonds requires energy. This energy can be supplied in the form of high-frequency electromagnetic radiation. The strength and type of a chemical bond will determine how easily it can be broken, with stronger bonds requiring more energy to break.

Infrared Radiation

Infrared radiation lies between visible light and microwaves on the electromagnetic spectrum. It is characterized by wavelengths ranging from approximately 700 nanometers to 1 millimeter.

• Energy: Infrared radiation has less energy than visible light, but more than microwaves. Its frequency range is typically between \(10^{12}\) to \(10^{14}\) Hz.
• Applications: It is widely used in heating, night-vision devices, and remote controls, due to its heat-emitting properties.
• Interaction with Molecules: Infrared radiation can cause molecules to vibrate. This feature makes it useful in studying molecular bonds, as changes in vibration modes can indicate bond properties.

Though it has useful applications, infrared radiation does not generally possess enough energy to break strong chemical bonds on its own.

Microwave Radiation

Microwave radiation features wavelengths that range from 1 millimeter to 1 meter, placing it just above infrared radiation in the electromagnetic spectrum.

• Energy: Microwaves have a frequency range of \(10^9\) to \(10^{12}\) Hz, making them less energetic than infrared radiation.
• Uses: Widely used in cooking, communications, and radar, microwaves cause water molecules in food to vibrate, generating heat.
• Effects on Molecules: The energy from microwaves can influence molecular rotations, but it is typically insufficient for breaking chemical bonds. To break bonds, much higher frequencies, like those in the ultraviolet range, are needed.

Ultraviolet Radiation

Ultraviolet (UV) radiation spans from 10 nanometers to 400 nanometers, placing it above visible light but below X-rays in the electromagnetic spectrum.

• Energy: With a frequency range of \(7.5 \times 10^{14}\) to \(3 \times 10^{16}\) Hz, it is much more energetic compared to infrared and microwaves.
• Breaking Chemical Bonds: Due to its high energy, UV radiation is capable of breaking many chemical bonds, thus it is used in processes like disinfection and polymerization. However, this same property can make UV potentially harmful.
• Protection: The Earth's atmosphere absorbs the majority of UV radiation, protecting living organisms from its harmful effects. However, excessive exposure can lead to skin damage or other biological impacts.