Untitled Quiz

<p>The wavelength increases. (D)</p> Signup and view all the answers

<p>Visible light. (B), Microwaves. (C)</p> Signup and view all the answers

<p>They produce ionization in materials upon absorption. (B)</p> Signup and view all the answers

<p>4 eV to 300 eV (D)</p> Signup and view all the answers

<p>Ionizing radiation can have both positive and negative effects in cancer treatment. (D)</p> Signup and view all the answers

<p>It can cause skin cancer. (D)</p> Signup and view all the answers

<p>Bremsstrahlung (D)</p> Signup and view all the answers

<p>Several UV photons are required to disrupt cell reproduction. (A)</p> Signup and view all the answers

<p>They originate from atomic excitations unique to specific anode materials. (D)</p> Signup and view all the answers

<p>It has low photon energy that does not expose most films. (B)</p> Signup and view all the answers

<p>Photon energy increases with increasing frequency. (C)</p> Signup and view all the answers

<p>Dyes that absorb violet light tend to fade more quickly. (C)</p> Signup and view all the answers

<p>Cancer development (B)</p> Signup and view all the answers

<p>To help prevent bilirubin buildup. (A)</p> Signup and view all the answers

<p>Higher energy photons can lead to more severe effects on materials. (A)</p> Signup and view all the answers

<p>Its low photon energy compared to other forms of radiation. (D)</p> Signup and view all the answers

<p>The relationship between photon energy and ejected electron's kinetic energy. (C)</p> Signup and view all the answers

<p>Photons must match a precise quantized energy step for absorption. (D)</p> Signup and view all the answers

<p>They lack energy steps necessary for absorption of visible light. (D)</p> Signup and view all the answers

<p>262 nm (A)</p> Signup and view all the answers

<p>Kinetic energy will increase linearly. (D)</p> Signup and view all the answers

<p>It represents Planck's constant. (B)</p> Signup and view all the answers

<p>3.10 eV (A)</p> Signup and view all the answers

<p>BE = hc/λ (A)</p> Signup and view all the answers

<p>Photons interact individually with electrons to transfer energy. (D)</p> Signup and view all the answers

<p>Electronvolts (eV) (A)</p> Signup and view all the answers

<p>Energy changes occur in discrete steps of size ∆E = hf. (D)</p> Signup and view all the answers

<p>Energy states are always continuous. (C)</p> Signup and view all the answers

<p>Explaining the photoelectric effect. (A)</p> Signup and view all the answers

<p>Only certain wavelengths and frequencies are emitted. (A)</p> Signup and view all the answers

<p>It helps in capturing images in light meters. (D)</p> Signup and view all the answers

<p>It is a line spectrum with discrete wavelengths. (A)</p> Signup and view all the answers

<p>They initiated the development of quantum mechanics. (A)</p> Signup and view all the answers

<p>Momentum is expressed as p = γmu. (B)</p> Signup and view all the answers

<p>There is a threshold frequency below which no electrons are ejected. (D)</p> Signup and view all the answers

<p>The electron is instantly ejected. (A)</p> Signup and view all the answers

<p>It is proportional to the intensity and independent of other characteristics. (D)</p> Signup and view all the answers

<p>The maximum kinetic energy of the ejected electrons. (A)</p> Signup and view all the answers

<p>Kinetic energy equals photon energy minus binding energy. (C)</p> Signup and view all the answers

<p>Higher intensity allows for more electrons of higher energy to be ejected. (B)</p> Signup and view all the answers

<p>A single photon must impart enough energy to overcome the binding energy. (A)</p> Signup and view all the answers

<p>Photons must maintain constant energy irrespective of their intensity. (C)</p> Signup and view all the answers

The idea that energy can only exist in discrete packets called quanta, with each quantum having a specific energy value (E = h * f, where h is Planck's constant and f is the frequency).

A fundamental constant in physics that relates the energy of a quantum to its frequency. Its value is approximately 6.63 x 10^-34 joule-seconds.

The electromagnetic radiation emitted by a hypothetical ideal object that absorbs all incident radiation at all wavelengths.

The characteristic pattern of wavelengths of electromagnetic radiation emitted or absorbed by an atom or molecule.

A spectrum consisting of discrete lines, each representing a specific wavelength of emitted or absorbed radiation.

The phenomenon where electrons are emitted from a material when light shines on it.

The discrete energy states that electrons can occupy within an atom or molecule, explained by quantum mechanics.

The momentum of an object moving at speeds comparable to the speed of light, calculated using the formula: p = γ * m * u

The energy carried by a single photon of light, determined by its frequency.

The minimum frequency of light required to eject electrons from a metal surface.

The minimum energy required to remove an electron from a metal surface.

The energy of motion that the ejected electrons possess.

The number of photons per unit area per second.

Light acts as particles (photons) that directly interact with electrons in the metal. A single photon can transfer its energy to a single electron, causing it to be ejected.

The maximum kinetic energy of an ejected electron is determined by the energy of the individual photon, not the overall intensity of the light. Increasing intensity means more photons, leading to more electron emissions, but each photon's energy remains the same, resulting in the same maximum kinetic energy for the electrons.

The full range of electromagnetic radiation, categorized by wavelength, frequency, and photon energy. It includes radio waves, microwaves, infrared radiation, visible light, ultraviolet radiation, X-rays, and gamma rays.

Radiation with enough energy to remove electrons from atoms, creating ions. Examples include X-rays, gamma rays, and some UV radiation.

Radiation produced when charged particles (like electrons) are decelerated, typically by a strong electric field. It's often referred to as 'braking radiation'.

X-rays emitted when electrons transition between specific energy levels in atoms. These X-rays are unique to the type of atom from which they are emitted.

Electromagnetic radiation with frequencies lower than X-rays but higher than visible light. It can be emitted from hot solids or gases.

The highest energy form of electromagnetic radiation. They have the highest frequencies and photon energies.

UV light can cause biological effects similar to X-rays and gamma rays, like skin cancer or sterilization, but requires multiple photons. Visible light, however, has insufficient energy to ionize atoms, but triggers vitamin D production.

Using UV light to treat infantile jaundice by helping prevent the buildup of bilirubin in the blood.

Visible light photons have energies between 1.63-3.26 eV, corresponding to the energy gaps between outer electron shells in atoms and molecules, allowing absorption.

Photons can only be absorbed or emitted by atoms and molecules if the photon energy matches a specific energy transition within that atom or molecule.

Red light has insufficient energy to expose most black-and-white film, making it safe for use in darkrooms.

Violet light, with higher energy than red light, causes dyes that absorb violet light to fade faster.

Transparent materials like glass don't absorb visible light because there are no energy transitions in their atoms or molecules that match the visible light photon energies.

Infrared (IR) radiation is strongly absorbed by water because water molecules have many energy states spaced close together, allowing them to easily absorb IR photons with energies in the range of 10⁻⁵ eV to 10⁻² eV.

Microwaves are similar to IR but have lower frequencies. While IR can have a wider range of frequencies, microwaves are limited to the frequencies generated by electronic circuits.

Visible light, IR, microwaves, and lower frequencies cannot ionize atoms or molecules with a single photon. However, extremely high intensities can lead to ionization.

False. Photoelectron emission ONLY happens when the light frequency is above a certain threshold. This threshold is determined by the material and its work function.

The wavelength of the photon DECREASES after colliding with an electron. This is because the photon loses some of its energy to the electron.

KEe = hf - BE, where KEe is the maximum kinetic energy of the ejected electron, hf is the photon's energy, and BE is the binding energy of the electron to the material.

The kinetic energy of the ejected electron increases linearly with the frequency of the incident light, above the threshold frequency.

Einstein proposed that light interacts with matter as discrete packets of energy called photons. This idea explains why the photoelectric effect only occurs above a threshold frequency.

The binding energy of an electron is equal to the energy of a photon with the threshold frequency (BE = hf0).

The energy of a photon is inversely proportional to its wavelength. This means shorter wavelengths have higher energy and vice versa.