Describe Bohr’s Model of Atomic Quantization?

Q: The emission spectrum of a hydrogen atom consists of a series of lines. Explain why this suggests…

A: Neil Bohr introduced hydrogen model in 1913. He described hydrogen model as a positively charged…

Q: What is the energy of a photon of light with a wavelength of 469 µm?

A: Interpretation: The energy of a photon of light with a wavelength of 469 μm is to be determined.…

Q: What is meant by the phrase, "the energy of an electron in a given orbital is quantized"? In…

A: The given statement means that the electrons of the given orbitals exist at a particular levels of…

Q: What is the correct order for energies of portions of the electromagnetic spectrum?

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Q: Describe how Heisenberg’s uncertainty principle challenged the Bohr model of the atom

A: Heisenberg’s uncertainty principle .how bohr model contradict the Heisenberg’s uncertainty principle…

Q: Which of the following statements best describes the Heisenberg uncertainty principle?

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Q: 6.45 What are the inadequacies of Bohr’s theory?

A: Bohr's theory of an atom defined that the negatively charged electrons revolved around the…

Q: How did the photoelectric effect lead Einstein to propose that light is quantized?

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Q: Photons of higher energy travel faster than photons of lower energy. True or False?

A: As we know that the speed of light is constant and all photons, of any energy, travel at the same…

Q: Explain Heisenberg’s uncertainty principle?

A: According to Heisenberg's uncertainty principle, exact position and momentum of a microscopic…

Q: Which kind of electromagnetic radiation contains the greatest energyper photon?a) microwavesb) gamma…

A: Correct answer is (b) gamma rays. Gamma rays are having maximum frequency and maximum energy among…

Q: What is meant by the term electromagnetic spectrum?

A: The electromagnetic spectrum is the term used in science to explain the complete range of light that…

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: 6.12 Give two everyday examples that illustrate the conceptof quantization.

A: The two everyday examples that illustrate the concept of quantization has to be given.

Q: Draw the stracture of the Bohr atom and label all the parts. Include the energy levels with their n…

A: The allowed energy state, orbit, or stationary state are basically paths around the nucleus where…

Q: Of the following transitions in the Bohr hydrogen atom, the transition results in the emission of…

A: The emission spectrum of the atomic hydrogen atom has been divided into a number of spectral series,…

Q: Use the Bohr model to calculate allowed energy levels of one-electron atoms Is there an energy level…

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Q: Describe the Bohr model for the atom. How did the Bohr model account for the emission spectra of…

A: Bohr model of hydrogen atom was given by Neil Bohr. It was based on the following postulates. 1) The…

Q: Describe electromagnetic radiation according to its wavenature.

A: Eectromagnetic radiation according to its wave nature has to be explained,

Q: Explain the consequences of Heisenberg’s uncertainty principle for measurements.

A: Electron is a negatively charged particle and it revolve around nucleus in orbits of an atom.

Q: Describe the four quantum numbers used to characterize an electron in an atom.

A: The question is based on the concept of atomic structure. We have to describe the four Quantum…

Q: A sample of excited atoms lie 3.054×10−19 J3.054×10−19 J above the ground state. Determine the…

A: The energy associated with an electromagnetic radiation is equal to hv where h is the Planck’s…

Q: How does the Bohr theory account for the observed phenomenon of the emission of discrete wavelengths…

A: Neil Bohr constructed a model of atom where electrons move in the circular orbits around the nucleus…

Q: Using the Bohr model, determine the energy in joules of the photon produced when an electron in a H…

A: To calculate the energy in joules of the photon produced when n electron oi Hydrogen moves from the…

Q: A sample of excited atoms lie 3.470×10−19 J above the ground state. Determine the emission…

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Q: A Bohr-model representation of the H atom is shown below with several electron transitions depicted…

A: The energy of H-atom during absorption and emission is given as: ∆E=-13.6 1nf2-1ni2eV When…

Q: Which of the following is an example of quantization? None of these are examples of quantization O…

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Q: Define and explain the following A. Magnetic Quantum numbers B. Spin quantum numbers

A: A. Magnetic Quantum numbers B. Spin quantum numbers

Q: In bohr’s original experiment, he expected the electrons in atoms to behave just like any other…

A: Answer - The wavelengths and frequencies of the light emitted by an atom (its emission spectrum) is…

Q: What the relationship between frequency and wavelength of electromagnetic radiation?

A: Electromagnetic radiation are those radiations which contain both electric and magnetic fields…

Q: or each of the following statements, identify which quantum number is being described or referenced.

A: The set of numbers used to describe the position and energy of the electron in an atom are called…

Q: State the relationship between the energy and thefrequency of electromagnetic radiation.

A: Electromagnetic radiation is a result of the movement of some charged particle through some matter…

Q: What is meant by saying that the energy of an electron is quantized?

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Q: Explain or define the following A. Principal Quantum numbers B. Secondary Quantum numbers C.…

A: Explain or define the following A. Principal Quantum numbers B. Secondary Quantum numbers C.…

Q: What different parts of electromagnetic radiations spectrum are used in applications of human used…

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Q: Identify the wave with the shortest wavelength

A: The question is based on the concept of electromagnetic spectrum.  Waves are arranged in order of…

Q: Calculate the energy in joules of a photon of radiation whose wavelength is 423 nm

A: Wavelength (λ) = 423 nm = 423 x 10-9 m As, 1 nm = 10-9 m Energy (E) = ?

Q: Determine the frequency and energy for yellow light with a wavelength of 584.9 nm. kJ/mol E =

A: The white light is a mixture of seven color light which have a region of a particular frequency.…

Q: The photoelectric effect was explained by Albert Einstein by assuming that: a. Light is a particle…

A: Radiant energy is emmited or absorbed discontinuously in the form of small energy bundles or energy…

Q: Suppose hydrogen atoms absorb energy so that electrons are excited to the n = 7 energy level.…

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Q: How does the emission spectra support the idea of quantized energy levels?

A: Emission spectra is observed when an e- from an excited state returns to the ground state. When an…

Q: Briefly discuss the chemistry behind the absorption of photons.

A: Photons are packets of light that are quantized. It does not have mass or charge. It is simply…

Q: How does the emission spectrum support the idea of quantized energy levels

A: Energy quantization allows electrons to move from one energy level to another rather than random…

Q: The following diagram is a shell representation of an atom. When the atom is exposed to light, the…

A: a) The outer most shell in which electron is present is known as valence shell. For ground state = K…

Q: In Bohr’s atomic theory, when an electron moves from one energy level to another energy level more…

A: Reason for the correct option:According to Bohr’s atomic theory,Electros are emits energy to moves…