9. Quantum Mechanics

Bohr Model

9. Quantum Mechanics

Bohr Model

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Bohr's Model of an Atom - Class 9 Tutorial

04:06

Bohr's Model of an Atom - Class 9 Tutorial

Emission Spectra and the Bohr Model

What Are The Different Atomic Models? Dalton, Rutherford, Bohr and Heisenberg Models Explained

Bohr Model of an Atom

Bohr Model of the Hydrogen Atom

Professor Dave Explains

Bohr’s Model of an Atom | Atoms and Molecules | Don't Memorise

Don't Memorise

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Multiple Choice

Which of the electron transitions represents absorption with the greatest frequency?

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Multiple Choice

Which of the following transitions (in a hydrogen atom) represent emission of the shortest wavelength?

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Multiple Choice

If the energy of an electron within the boron atom was calculated as –6.0556 x 10^-18 J, at what energy level would it reside?

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Multiple Choice

Which of the following statements about the Bohr model of the hydrogen atom is false?

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Textbook Question

Which arrow in the energy diagram for an atom represents the absorption of light with the shortest wavelength? (LO 5.7)

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Textbook Question

Consider the three electronic transitions in a hydrogen atom shown here, labeled A, B, and C. (a) Three electromagnetic waves, all drawn on the same scale, are also shown. Each corresponds to one of the transitions. Which electromagnetic wave (i), (ii), or (iii), is associated with electronic transition C?

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Textbook Question

Does the hydrogen atom 'expand' or 'contract' when an electron is excited from the n = 1 state to the n = 3 state?

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Textbook Question

Classify each of the following statements as either true or false: (a) A hydrogen atom in the n = 3 state can emit light at only two specific wavelengths (b) a hydrogen atom in the n = 2 state is at a lower energy than one in the n = 1 state (c) the energy of an emitted photon equals the energy difference of the two states involved in the emission.

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Textbook Question

Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? (b) from an orbit of radius 0.846 nm to one of radius 0.212 nm

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Textbook Question

Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? (a) from n = 3 to n = 2

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Textbook Question

Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from n = 2 to n = 3

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Textbook Question

(a) Using Equation 6.5, calculate the energy of an electron in the hydrogen atom when n = 3 and when n = 6. Calculate the wavelength of the radiation released when an electron moves from n = 6 to n = 3. when n = 6

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Textbook Question

Consider a transition of the electron in the hydrogen atom from n = 8 to n = 3. (b) Will the light be absorbed or emitted?

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Textbook Question

The hydrogen atom can absorb light of wavelength 1094 nm. (b) Determine the final value of n associated with this absorption.

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Textbook Question

Determine whether each transition in the hydrogen atom corresponds to absorption or emission of energy. a. n = 3¡n = 1 b. n = 2¡n = 4 c. n = 4¡n = 3

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Textbook Question

Ionization involves completely removing an electron from an atom. How much energy is required to ionize a hydrogen atom in its ground (or lowest energy) state? What wavelength of light contains enough energy in a single photon to ionize a hydrogen atom?

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Textbook Question

An atomic emission spectrum of hydrogen shows three wavelengths: 121.5 nm, 102.6 nm, and 97.23 nm. Assign these wavelengths to transitions in the hydrogen atom.

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Textbook Question

Bohr's model can be used for hydrogen-like ions—ions that have only one electron, such as He + and Li2 + . (a) Why is the Bohr model applicable to Li2+ ions but not to neutral Li atoms?

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Open Question

An atomic emission of light with a specific amount of energy from an atom confirms that

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Open Question

Consider a hydrogen atom in the ground state. What is the energy of its electron?

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Open Question

How much energy does the electron have initially in the n=4 excited state

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Open Question

How much energy does the electron have initially in the n=4 excited state?

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Open Question

Which of the following transitions (in a hydrogen atom) represent absorption of the smallest frequency photon?

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Open Question

Determine whether each of the following transitions in the hydrogen atom corresponds to absorption or emission of energy.

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Open Question

Which of the following transitions represent the emission of a photon with the largest energy?

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Open Question

Consider a hydrogen atom in the ground state. What is the energy of its electron?

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9. Quantum Mechanics

Bohr Model

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