9. Quantum Mechanics

Bohr Model

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

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

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.

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

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?

The energy of each Bohr orbit is quantized.

This statement correctly characterizes the Bohr model.

An electron in a stationary state does not emit radiation.

Transitions between stationary states that are close together require shorter wavelength that those that are spaced further apart.

When an electron jumps to a higher state, energy is absorbed.

When an electron falls to a lower state, energy is emitted.

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

Bohr Model of the Hydrogen Atom

The Bohr Atom

Which arrow in the energy diagram for an atom represents the absorption of light with the shortest wavelength? (LO 5.7)
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/4d69f7341ad079a8-1669822408652.jpg" alt="" />

Emission Spectra and the Bohr Model

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?

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?<img src="https://lightcat-files.s3.amazonaws.com/problem_images/b376e88bbbbee9c7-1664379307876.jpg" alt="" />

Bohr's Model of an Atom - Class 9 Tutorial

(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

Bohr Model of an Atom

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

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

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

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

Bohr Model Example 1

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

Order the following transitions in the hydrogen atom from
smallest to largest frequency of light absorbed: n = 3 to
n = 7, n = 4 to n = 8, n = 2 to n = 5, and n = 1 to n = 3.

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?

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

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

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

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

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10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

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15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

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23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Wavelength and Frequency

Wavelength&nbsp;is the distance from one crest of a wave to another, whereas frequency is the number of waves within a second.&nbsp;

Quantum Numbers: Spin Quantum Number

The Spin Quantum Number deals with the spin of an electron within an orbital.

Speed of Light

The Speed of Light in a vacuum is related to the wavelength and frequency of a light particle.

Bohr Equation

In the Bohr Equation, the energy and wavelength a photon is related to its energy shell transitions.

Quantum Numbers: Angular Momentum Quantum Number

The&nbsp;Angular Momentum Quantum Number&nbsp;gives the shape of the atomic orbitals.

Emission Spectrum

Emission Spectra is a series of lines formed when emitted light is focused by a slit and passed through a prism. &nbsp;

Introduction to Quantum Mechanics

The 4 Quantum Numbers provide us the coordinates to find the theoretical location of an electron.

Quantum Numbers: Nodes

A node is the region in an atom with zero electron density and where an electron is least likely to exist.

The Energy of Light

The Energy of Light&nbsp;involves the use of a new variable Planck's Constant.

Electromagnetic Spectrum

The Electromagnetic Spectrum is the different forms of radioactive energy that exists in our universe.

Heisenberg Uncertainty Principle

Heisenberg's Uncertainty Principle&nbsp;tries to explain the potential duality of an electron behaving as either a particle or wave.&nbsp;

Quantum Numbers: Number of Electrons

The Quantum Numbers can give both the quantity and location of electrons within a given atom.&nbsp;

Quantum Numbers: Principal Quantum Number

The Principal Quantum Number gives both the size and energy of an electron shell.&nbsp;

Photoelectric Effect

What happens when light strikes the surface of a metal? The Photoelectric Effect&nbsp;can help to explain that.&nbsp;

Quantum Numbers: Magnetic Quantum Number

The Magnetic Quantum Number gives the location of an electron within a specific orbital.

In the Bohr Model, electrons can move up and down to different orbitals or shells based on absorbing or releasing of energy.&nbsp;

De Broglie Wavelength

The&nbsp;De Broglie Wavelength equation relates wavelength to velocity or speed.&nbsp;