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9. Quantum Mechanics

Quantum Numbers: Magnetic Quantum Number

9. Quantum Mechanics

Quantum Numbers: Magnetic Quantum Number

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Quantum Numbers: Magnetic Quantum Number

Quantum Numbers: Magnetic Quantum Number

Quantum Numbers: Magnetic Quantum Number Example 1

Quantum Numbers: Magnetic Quantum Number Example 1

Quantum Numbers: Magnetic Quantum Number

Quantum Numbers: Magnetic Quantum Number

Quantum Numbers: Magnetic Quantum Example 2

Quantum Numbers: Magnetic Quantum Example 2

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Quantum Numbers - Magnetic Quantum Number (ml)

Quantum Numbers - Magnetic Quantum Number (ml)

S. Michael Stewart

Orbitals and Quantum Numbers

Orbitals and Quantum Numbers

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Quantum Numbers

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Quantum Numbers | What are the 4 Quantum Numbers? Chemistry

Quantum Numbers | What are the 4 Quantum Numbers? Chemistry

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

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

Quantum Numbers, Atomic Orbitals, and Electron Configurations

Quantum Numbers, Atomic Orbitals, and Electron Configurations

Professor Dave Explains

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Practice this topic

Multiple Choice

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

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Multiple Choice

Select a correct set of values for an electron found within the designated 5d orbital.

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Multiple Choice

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.

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Multiple Choice

Which sketch could represent an orbital with the quantum numbers n = 4 and l = 2?

Textbook Question

The contour representat ion z of one of the orbitals for the n = 3 shell of a hydrogen atom is shown here. (c) In which of the following ways would you modify this sketch if the value of the magnetic quantum number, ml, were to change? (i) It would be drawn larger, (ii) the number of lobes would change, (iii) the lobes of the orbital would point in a different direction, (iv) there would be no change in the sketch.

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Textbook Question

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

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Textbook Question

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?

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

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

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Textbook Question

Suppose that in an alternate universe, the possible values of l are the integer values from 0 to n (instead of 0 to n - 1). Assuming no other differences between this imaginary universe and ours, how many orbitals would exist in each level? a. n = 1 b. n = 2 c. n = 3

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Textbook Question

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

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What are the possible values of m_ℓ for an electron in a d orbital?

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Suppose that, in an alternate universe, the possible values of ml were the integer values including 0 ranging from −l−1 to l+1 (instead of simply −l to +l). how many orbitals would exist in each of the following sublevels?

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What is the only possible value of mℓ for an electron in an s orbital?

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Which set of quantum numbers cannot specify an orbital?

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What are the possible values of ml for each of the following values of l?

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Determine the quantum numbers 𝑛 and ℓ and select all possible values for 𝑚ℓ for each subshell of the element.

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How many orbitals in an atom can have the designation

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An electron in a 3d orbital could have which of the following quantum numbers? select all that could be correct.

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What are the possible values of m_ℓ for an electron in a d orbital?

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Type in the maximum number of electrons that can be present in each shell or subshell below.

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Showing 31 of 31 practice