A hydrogen atom absorbs energy and an electron is excited to the n = 2 shell. When the electron relaxes back to the ground state, n = 1, it emits light. Calculate the change in energy of the electron from the excited state back to the ground state. Then, calculate the frequency of the light that was emitted. ΔΕΞ V= Identify the region on the electromagnetic spectrum where the light that was emitted is located. infrared (IR) visible x rays ultra-violet (UV) S

A hydrogen atom absorbs energy and an electron is excited to the n = 2 shell. When the electron relaxes back to the ground state, n = 1, it emits light. Calculate the change in energy of the electron from the excited state back to the ground state. Then, calculate the frequency of the light that was emitted. ΔΕΞ V= Identify the region on the electromagnetic spectrum where the light that was emitted is located. infrared (IR) visible x rays ultra-violet (UV) S

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A 359 g portion of soup is heated in a microwave oven from 25.0 °C to 90.0 °C, using radiation with…

A: Given, the mass of the soup, Msoup = 359 g Initial temperature of the Microwave Oven, ti = 25.…

Q: A certain microwave oven delivers 750 watts (J/s) of power to a coffee cup containing 35.1 g of…

A: Time taken and energy of photon is calculated for given

Q: What is the wavelength of electromagnetic radiation with a frequency of 5.00 × 1 0 12 Hz? What kind…

A: The product of frequency and wavelength of the wave is equal to the speed of light. Write the…

Q: Consider light with a wavelength of 1.25 x 10¬10 m. The energy of a single photon of this type of…

A: Photon will transfer its energy to the water molecules, and continuous bombardment of photon will…

Q: When a metal was exposed to photons at a frequency of 1.19 × 10'5 s-', electrons were emitted with a…

A: You can find the work function of the metal which is the energy required to free the electron from…

Q: None

A: Visible Spectrum TransitionsThe transitions that emit light in the visible region are part of the…

Q: DNA is one of the most important biological molecules. It is the chemical that makes up the genetic…

Q: Part C What is the kinetic energy of the emitted electrons when cesium is exposed to UV rays of…

A: Kinetic energy of cesium E = hv Where h = plank's constant = 6.626 ×10-34 J s v = frequency of…

Q: A local AM radio station broadcasts at a frequency of 592 KHz. Calculate the energy of the…

Q: Part A The energy required to dislodge electrons from rubidium metal via the photoelectric effect is…

A: We are given with the Energy required, E = hc/λ = 218 kJ/mol = 218 × 1000 J/mol Where c is velocity…

Q: Sodium metal requires a photon with a minimum energy of 4.41×10−19J to emit electrons. What is the…

A: Given data, Energy of the photon (E) in J = 4.41 x 10-19 J The frequency of the photon is to be…

Q: A mercury atom emits light at many wavelengths, two of which are at (1) 404.7 nm and (2) 435.8 nm.…

Q: Titanium metal requires a photon with a minimum energy of 6.94 x 10^-19 J to emit electrons. What is…

A: Photon is called the packet of quanta. It is basically an elementary particle. It is basic unit of…

Q: What is the frequency of the photon emitted from a Hydrogen atom's electron when it transitions from…

Q: What is the change in energy experienced by an electron in a hydrogen atom that undergoes an n = 2…

A: According to Bohr's model of an atom, electrons, having a negative charge, revolves around the…

Q: 2) Based on your knowledge of the Electromagnetic Spectrum, what are the differences between…

A: Electrons can behave as a particle as well as wave. The dual nature of electron was explained by De…

Q: The electron in an (unbound) hydrogen atom (H(g)) is excited from the ground state to the n=3 state.…

A: The electron in an (unbound) hydrogen atom (H(g)) is excited from the ground state to the n=3…

Q: Calculate the wavelength, in nanometers, for the colored line that appears in the spectrum of the…

A: Wavelength can be calculated using the equation: 1λ…

Q: 1012

A: Energy = h • v Where : h = constant = 6.626 • 10^-34 Js And v = frequency = 5.2 • 10^12 s-1

Q: The electron microscope uses the wave property of electrons to observe very small objects. A moving…

A: Kinetic energy = h22λ2m where wavelength = λ mass of electron = m Plank's constant = h

Q: For a hydrogen atom, calculate the energy of a photon in the Balmer series that results from the…

A: The energy of photon is given by the energy difference of the states between which the photon is…

Q: A few different types of electromagnetic radiation are listed in the table below. Complete the table…

A: Frequency is inversely proportional to wavelength. The waves having high wavelength will have lower…

Q: A photon with a wavelength of 1995 nm strikes a hydrogen atom. Will this photon have the correct…

A: Initial energy level n1 = 4 Final energy level n2 = 7 Wavelength of the incident radiation = 1995 nm

Q: How much energy is contained in 1 molmol of each of the following? X-ray photons with a wavelength…

Q: Calculate the energy of the red light emmitted by a neon atom with wavelength of 680 nm.

A: Energy(E) of light ray emitted from the source can be calculated by using Planck's law:

Q: A certain metal is exposed to light with increasing frequency and energy of the photons. Electrons…

A: Please find the attached images for answer

Q: A photon has the energy 2.33 × 10–20 J. What is this photon's frequency?

A: We know that , energy of a photon is related to Plank's constant as,…

Q: number of spectral lines: wavelength range from:

Q: Arrange the different types of electromagnetic radiation by wavelength. Only include the items that…

A: electromagnetic waves are the type of waves which are affected by the change of electric as well as…

Q: number of photons

Q: An electron is trapped in a is absorbed, the electron is in the n = 7 energy level. What was the…

A: The energy levels of an electron in a one-dimensional box are given by the formula: En=n2h28mL2…

Q: The work function (Φ) for a metal is 6.10×10-19 J. What is the longest wavelength of electromagnetic…

Q: An electron in the n = 2 level absorbs a photon with a wavelength of 433.9 nm. To what energy level…

Q: Consider this value: -1.6335 * 10-18 J. Based on that value, is there any 1-electron atom or ion…

A: Given: Energy = -1.6335×10-18 J Initial energy state n = 2 Final energy state n =1

Q: photons

Q: Which one of the following electromagnetic spectrum regions contains the longest wavelength? gamma…

Q: The work function (binding energy) is the energy that must be supplied to cause the release of an…

Concept explainers

Atomic Structure

The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.

Shape of the D Orbital

Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.

Question

100%

A hydrogen atom absorbs energy and an electron is excited to the n = 2 shell. When the electron relaxes back to the ground
state, n = 1, it emits light.
Calculate the change in energy of the electron from the excited state back to the ground state. Then, calculate the frequency of
the light that was emitted.
ΔΕ =
V=
Identify the region on the electromagnetic spectrum where the light that was emitted is located.
infrared (IR)
visible
x rays
ultra-violet (UV)
S
J

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1: Introduction to hydrogen

VIEW

Step 2: Rydberg equation

VIEW

Step 3: ∆E calculation

VIEW

Step 4: Frequency calculation

VIEW

Step 5: Electromagnetic Region of the transition

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 6 steps with 6 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

When a metal was exposed to photons at a frequency of 1.31 x 105 s-', electrons were emitted with a maximum kinetic energy of 3.80 × 10-19 J. Calculate the work function, D, of this metal. J/photon What is the maximum number of electrons that could be ejected from this metal by a burst of photons (at some other frequency) with a total energy of 8.97 × 10-7 J? number of electrons:
A light sample containing one mole of photons emits an energy of 1.65kj/mol. Find the frequency of one photon.
An electron absorbs a single photon with a wavelength = 127 nm. Calculate the energy of the photon.
When a metal was exposed to photons at a frequency of 1.45 x 105 s-, electrons were emitted with a maximum kinetic energy 3.80 x 10-19 J. Calculate the work function, 4, of this metal. J/photon What is the maximum number of electrons that could be ejected from this metal by a burst of photons (at some other frequency) with a total energy of 7.92 x 10-7 J? number of electrons:
Sketch a diagram of the Bohr model of a hydrogen atom, Using arrows for excitation and relaxation of electrons. Show an electron being excited from n=1 to n=5, then relaxing down to n=2. Using the equation for difference in energy levels for a hydrogen atom and the equation for the energy of a photon, calculate wavelength (in nm) of the photon emitted when the electron relaxed from n=5 to n=2. Show all our calculations.
A photon has a frequency of 4.0 × 10° Hz. What is the energy of this photon? J 1 6. C 7 8 9. +/- X 100
The photoelectric effect can be used in engineering designs for practical applications. For example, infrared goggles used in night-vision applications have materials that give an electrical signal with exposure to the relatively long wavelength of IR light. If the energy needed for signal generation is 7.6 x 10-40 J, what is the minimum wavelength? What is the frequency of light that can be detected? c = 2.998 × 10° m/s h = 6.626 x 10-34 J s m S -1
A certain microwave oven delivers 750 watts (J/s) of power to a coffee cup containing 66.6 g of water at 37.5°C. If the wavelength of microwaves in the oven is 9.75 cm, how long does it take, and how many photons must be absorbed, to make the water boil? The specific heat capacity of water is 4.18 J/ °C•g and assume only the water absorbs the energy of the microwaves. S photons
The minimum energy required to remove an electron from a certain metal is 3.7 x 10– 19 J. If the metal surface is struck by light having a wavelength of 5.00 x 102 nm, what is the kinetic energy of the electron ejected from the metal?
What frequency of electromagnetic radiation is associated with a wavelength of 100.5 nm? In what region of the spectrum is this frequency?