9. Quantum Mechanics

Quantum Numbers: Magnetic Quantum Number

Quantum Numbers | Principal Energy Levels | Energy Sub-levels and Orbitals

Orbitals and Quantum Numbers

Give the orbital designations of electrons with the following quantum numbers. 
(a) n = 3, l = 0, ml = 0 
(b) n = 2, l = 1, ml = -1 
(c) n = 4, l = 3, ml = -2
(d) n = 4, l = 2, ml = 0

What are the possible values of ml for each value of l?
c. 2

Select a correct set of values for an electron found within the designated 5f orbital. &nbsp;<img src="https://static.studychannel-prd.pearsonprd.tech/courses/general-chemistry/thumbnails/images/06aeb4de"class="fr-fic fr-dii">&nbsp;

What are the possible values of n, l, and ml for an electron in a 5p orbital? (LO 5.12)

What are the possible values of n, l, and ml for the orbital shown? (LO 5.13)

Quantum Numbers - Magnetic Quantum Number (ml)

Quantum Numbers: Magnetic Quantum Number Example 1

Quantum Numbers: Magnetic Quantum Example 2

What are the possible values of ml for each value of l?
b. 1

Tell which of the following combinations of quantum numbers are not allowed. Explain your answers.
(a) n = 3, l = 0, ml = -1
(b) n = 3, l = 1, ml = 1
(c) n = 4, l = 4, ml = 0

Suppose that, in an alternate universe, the possible values of
ml are the integer values including 0 ranging from -l -1 to l +1
(instead of simply -l to +l). How many orbitals exist in each
sublevel?
a. s sublevel
b. p sublevel
c. d sublevel

For the table that follows, write which orbital goes with the 
quantum numbers. Don’t worry about x, y, z subscripts. If the 
quantum numbers are not allowed, write “not allowed.” 
n l ml Orbital 
2 1 -1 2p (example) 
1 0 0 
3 -3 2 
3 2 -2 
2 0 -1 
0 0 0 
4 2 1 
5 3 0<img src="https://lightcat-files.s3.amazonaws.com/problem_images/5ba448a34310f2cf-1663007983940.jpg" alt="" />

Sketch the shape and orientation of the following types of
orbitals: (c) dx2 - y2.

Quantum Numbers, Atomic Orbitals, and Electron Configurations

Quantum Numbers

What are the possible values of ml for each value of l? 
a. 0

The Magnetic Quantum Number (mL)

Which of the following statements is false?a) A set of d orbitals contains 5 orbitals.b) A set of 4s orbitals would have more energy than a set of 3p orbitals.c) The second shell of an atom possesses d orbitals.d) A set of f orbitals contains 3 orbitals.e) The first energy level contains only s orbitals.

A certain orbital of the hydrogen atom has n = 4 and 
l = 3. (a) What are the possible values of ml for this orbital?

Which set of quantum numbers cannot occur together to specify an
orbital?
a. n = 2, l = 1, ml = -1
b. n = 3, l = 2, ml = 0
c. n = 3, l = 3, ml = 2
d. n = 4, l = 3, ml = 0

How many different values of ml are possible for a 4d set of orbitals?

Quantum Numbers | What are the 4 Quantum Numbers? Chemistry

The accompanying drawing shows a contour plot for a dyz
orbital. Consider the quantum numbers that could potentially
correspond to this orbital. (c) What is
the largest possible value of the magnetic quantum number, ml?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/0619a9f605c8ed03-1660830532114.jpg" alt="" />

Give the values for n, l, and ml for (a) each orbital in the 3p
subshell.

How many unique combinations of the quantum numbers l 
and ml are there when (b) n = 5?

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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;

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

Bohr Model

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;

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