An electron in an atom falls from the second to the first energy level and emits a photon of green light. The same electron is re-excited and then falls from the third to the second energy level. Would the photon emitted in the second case be more likely to be yellow or blue in color? 3.

An electron in an atom falls from the second to the first energy level and emits a photon of green light. The same electron is re-excited and then falls from the third to the second energy level. Would the photon emitted in the second case be more likely to be yellow or blue in color? 3.

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter11: Modern Atomic Theory

Section11.2: The Hydrogen Atom

Problem 3RQ

See similar textbooks

Related questions

Q: Consider a piece of potassium metal which is being exposed to a stream of photons in order to eject…

Q: A When atoms of an element are emitting a certain wavelength (or color) of light, it means that 2)…

A: Given: Atoms of an element are emitting a certain wavelength or color of light.

Q: 9. How many photons are absorbed by a single atom in order for an electron to move to a higher…

A: The no of photon absorbed is the integral multiple of hv . Where v is frequency of radiation .

Q: 33. what are electrons described as in the quantum mechanical model? a. Wave Particles b.…

A: Quantum mechanical model of atom helps us find the probability of finding an electron around the…

Q: For a particular element, a photon of orange light of wavelength of 585 nm resulted when an electron…

Q: Use the information to answer the following question. Color Element Red Orange Strontium Calcium…

A: The question is based on the concept of colour of the inorganic salts. We have to identify the…

Q: An electron is promoted from a lower level (Ni) to a higher level (Nf). Which of the following…

A: When the electron makes a transition from lower energy level to higher energy level, it absorbs…

Q: a. Radiation from a sodium lamp, such as a streetlight, appears as yellow light and has a wavelength…

A: Since you have asked multiple question, we will solve the first two question for you. If you want…

Q: According to Bohr's model, Which emission results in the highest energ photon? * -shell (n=4) shell…

A: according to Bohr's model and electron would absorb energy in the form of photons to get excited to…

Q: Calculate the energy and the frequency of the red light emitted by neon atom with a wavelength of…

A: Answer :- a) The frequency of the red light emitted by neon atom with a wavelength of 680 nm = 4.41…

Q: An excited atom has an electron or electrons which are not in the lowest energy state. Excited atoms…

Q: Which form of electromagnetic radiation has photons with the lowest energy? O Radio Waves Gamma Rays…

Q: How many electrons occupy the 2p su level in an atom of boron in the ground state?

A: Boron is a group 13 element. Atomic number of boron is 5. It has total 5 electrons.

Q: How does the energy of a principal energy level depend on the value of n? Does a higher value of n…

A: There are four type of quantum numbers.They are (1) principle quantum number(n) :- it gives us idea…

Q: How many emission lines are possible, considering only the five quantum levels? photons of the…

Q: Light is given off by a sodium or mercury-containing streetlight when atoms are excited. The light…

A: Option C is correct.

Q: (8.2)Which of the following occurs as the wavelength of a photon increases? O None of the above…

A: Energy of photon = E = hc/ wavelength E = h × frequency h = plank constant

Q: Which subshell can have a maximum of 2 electrons? d Of S

A: Which orbital have maximum of 2 e-?

Q: Fill in the blanks. A photon of blue light has a frequency and a wavelength than a photon of red…

A: Frequency is inversely proportional to wavelength. So, higher is the frequency then lower is the…

Q: Consider these electron transitions in a hydrogen atom: I. n = 2 n = 1 II. n = 3 n = 1 III. n= 1n =…

A: Note - Since you have asked multiple question, we are bound to solve only the first question for…

Q: What is the total number of orbitals in the shell designated by n = 4?

Q: When a substance light, an electron undergoes a transition from the lowest-energy level to a…

A: the answer would be:

Q: the quantum numbers of 17 electrons that are placed in an atom

Q: For the photons with the following wavelengths, which of the photons possesses the least energy and…

A: The energy of a photon of electromagnetic radiation depends on the frequency of the photon.…

Q: Which of the following quantum numbers represents the greatest number of orbitals? A. n = 2 В. 5р С.…

A: The quantum numbers given are,

Q: n=2 PHOTON n=2 РHOTON n=1 n=1« FIGURE I FIGURE II Which figure correctly represents when LIGHT IS…

A: An electron jumps to a higher state when it absorbs energy or photons. An electron returns to a…

Q: 2) A sample of atomic H gas, initially in the ground state, sequentially absorbs two photons at 1874…

A: The atomic hydrogen absorbs 1874 nm wavelength radiation. Let's say that the e- will transit from…

Q: if an electron transition between energy levels 4 and 1 leads to a photon of blue light being…

A: The atoms of elements possess electrons in the valence shell along with their presence in the inner…

Q: What is the maximum number of electrons associated with any orbital? (a) 6…

A: We have one orbital in s, three in p, 5 orbitals in d and 7 orbitals in f- subshell. Orbitals is the…

Q: Indicate whether each of the following electron configurations corresponds to the ground state or to…

A: The ground state electronic configuration is the lowest energy and most stable arrangement of…

Q: 9) How many subshells are found in the 2nd energy level or shell? A) 2 B) 4 С) 3 10) What is the…

Q: The most energetic photons are gamma rays. True False

Q: Why is it more difficult to cause photons to be emitted from neon?

A: Ionization energy: Ionization energy is the minimum amount of energy required to remove the most…

Q: Consider the three electromagnetic waves shown in the image. Which wave has the longest wavelength?…

A: Wavelength is the distance between the consecutive crest and the trough. The number of waves which…

Q: This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI…

A: Given: The diagram of transition of electron from one state to another as follows:

Q: 4. Electrons must gain energy in order to move from lower energy levels to higher energy levels.…

A: As per Bohr model of atom, electrons are known to found in energy levels surrounding the nucleus.…

Q: In addition to absorption of a photon, energy can be transferred to an atom by collision. Consider a…

A: Given : Consider a hydrogen atom in its ground state. Incident on the atom are electrons having a…

Q: 3. A photon of blue light has a frequency of 7.50 × 10¹⁴ Hz. Calculate the wavelength of this photon…

Q: In the Bohr model for the hydrogen atom, which of the following transitions results in the emission…

Q: Why is light of at least a certain frequency needed to cause the photoelectric effect? O A certain…

A: Photoelectric effect :- J.J Thomson observed that when a photon of having certain frequency strikes…

Q: Describe the major concepts (Hunds, Pauli...etc.) and explain why each is a key part of the "tool…

A: Pauli exclusion principle: It states that only two electrons can be accommodated in the same…

Q: Indicate whether each of the following electron configurations corresponds to the round state or to…

A: NOTE ; Since you've posted multiple sub-parts,we'll solve only first three sub-parts for you.To get…

Q: Identify the 4 quantum numbers that can represent the last electron added to a Sr atom (use the…

Q: you made the wavelength of the light shorter and the frequency higher. What effect did this have on…

A: Energy of a light is directly proportional to frequency and inversely proportional to wavelength of…

Q: A set of photons have energy 21.8 kJ mol-1. What wavelength is associated with the photons?

Q: Because the atoms of a given element emit only certain photons of light, only certain_____ occur in…

A: We have to explain the atoms of a given element emit only certain photons of light, only…

Q: Which properties of an orbital is associated with the value of the principal quantum number?

A: Define the four quantum numbers. Determine quantum numbers for specific electrons when given…

Q: A photon of a red light has a ______ frequency and a ______ wavelength than a photon of blue light.…

A: Observe the below table with the wavelength and frequency data of VIBGYOR

Concept explainers

Quantum Chemistry

Quantum chemistry deals with the properties of chemical systems and their reactions. The branch of chemistry which is more concerned with quantum chemistry is physical chemistry. It is a more sophisticated field of theoretical physics which is concerned towards the application of physical concepts towards various chemical aspects such as, formation of atoms, chemical structure descriptions, chemical bond strength, hybridization, conjugation etc. Quantum chemistry mainly studies the various states i.e., ground state, excited state, transition states of the individual atoms or molecules taking place during any chemical reaction. The laws of motion explained by various scientists, which are termed as “classical mechanics” were not acceptable in terms of electrons, protons, atoms, light etc. Thus, a new theory named “quantum mechanics” emerged to understand the basic framework of various atomic and subatomic particles.

Question

An electron in an atom falls from the second to the first energy level and emits a
photon of green light. The same electron is re-excited and then falls from the
third to the second energy level. Would the photon emitted in the second case
be more likely to be yellow or blue in color?
3.

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

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Introduction and Principles of Quantum Theory

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

6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) lf a transition between the two higher energy states could be observed, what would be the frequency of the light?
(a) Give the complete electron configuration (1s22s22p) of aluminum in the ground state. (b) The wavelength of the radiation emitted when the outermost electron of aluminum falls from the 4s state to the ground state is about 395 nm. Calculate the energy separation (in joules) between these two states in the Al atom. (c) When the outermost electron in aluminum falls from the 3d state to the ground state, the radiation emitted has a wavelength of about 310 nm. Draw an energylevel diagram of the states and transitions discussed here and in (b). Calculate the separation (in joules) between the 3d and 4s states in aluminum. Indicate clearly which has higher energy.
An excited atom can release some or all of its excess energy by emitting a(n) and thus move to a lower energy state.
The energy of a photon of visible light emitted by an excited atom is the energy change that takes place within the atom itself.
Light with a wavelength of 614.5 nm looks orange. What is the energy, in joules, per photon of this orange light? What is the energy in eV(1eV=1.6021019J)?
6.105 When we say that the existence of atomic spectra tells us that atoms have specific energy levels, are we using deductive or inductive reasoning?
The colors of the visible spectrum and the wavelengths corresponding to the colors are given in Figure 5.2. (a) Which colors of light involve photons with less energy per photon than yellow light? (b) Which color of visible light has photons of greater energy, green or violet? (c) Which color of light has the greater frequency, blue or green?
6.28 A neon atom cmi light at many wavelengths, two of which are at 616.4 and 638.3 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) If a transition between the two higher energy states could be observed, what would be the frequency of the light?
6.27 Refer w the data and energy-Ievel diagram shown in Problem 6.26, and find the wavelength of light that would be emitted when a hydrogen atom undergoes the transition from the state labeled as n = 4 to the state labeled as n = 2. Express your answer in nm.
Consider the bright line spectrum of hydrogen shown in Fig. 11.10 . Which line in the spectrum represents photons with the highest energy? With the lowest energy?
6.18 Assume that a microwave oven operates at a frequency of 1.001011s1 . (a) What is the wavelength of this radiation in meters? (b) What is the energy in joules per photon? (c) What is the energy per mole of photons?
How many electrons in an atom can have the following quantum designation? (a) 1s (b) 4d, m l =0(c) n=5,l=2