Question

**Question 3
Part B**:How many values of

Express your answer as an integer.

**Part C**

The quantum state of a particle can be specified by giving a
complete set of quantum numbers (*n*,*l*,
*m**l*,*m**s*). How many different
quantum states are possible if the principal quantum number is
*n* = 2?

To find the total number of allowed states, first write down the
allowed orbital quantum numbers *l*, and then write down the
number of allowed values of *m*l for each orbital quantum
number. Sum these quantities, and then multiply by 2 to account for
the two possible orientations of spin.

Express your answer as an integer.

**Part D:** Is the state *n*=3,
*l*=3, *m**l*=−2, *m**s*=1/2 an
allowable state? If not, why not?**Part D**

Is the state , , , an allowable state? If not, why not?

Yes it is an allowable state. |

No: The magnetic quantum number must equal the orbital quantum number. |

No: The magnetic quantum number cannot be negative. |

No: The orbital quantum number cannot equal the principal quantum number. |

No: The magnetic quantum number must equal the principal quantum number. |

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**Part E**

What is the maximum angular momentum *L*max that an
electron with principal quantum number *n* = 5 can have?

Express your answer in units of ℏ. (You don't need to enter the ℏ, it is in the units field for you.)

Answer #1

Part C
The quantum state of a particle can be specified by giving a
complete set of quantum numbers (n,l,
ml,ms). How many different
quantum states are possible if the principal quantum number is
n = 2?
To find the total number of allowed states, first write down the
allowed orbital quantum numbers l, and then write down the
number of allowed values of ml for each orbital quantum
number. Sum these quantities, and then multiply by 2 to account...

The quantum state of a particle can be specified by giving a
complete set of quantum numbers (n,l,
ml,ms). How many different
quantum states are possible if the principal quantum number is
n = 2?
To find the total number of allowed states, first write down the
allowed orbital quantum numbers l, and then write down the
number of allowed values of ml for each orbital quantum
number. Sum these quantities, and then multiply by 2 to account for
the...

-Calculate the magnitude of the maximum orbital angular momentum
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Express your answer in units of ℏ to three significant
figures.
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Lmax for an electron in a hydrogen atom for states with a
principal quantum number of 48.
Express your answer in units of ℏ to three significant
figures.
-Calculate the magnitude of the maximum...

Quantum numbers arise naturally from the mathematics used to
describe the possible states of an electron in an atom. The four
quantum numbers, the principal quantum number (n), the angular
momentum quantum number (ℓ), the magnetic quantum number (mℓ), and
the spin quantum number (ms) have strict rules which govern the
possible values. Identify allowable combinations of quantum numbers
for an electron. Select all that apply.
a) n=4, l=2, ml=3, ms=+1/2
b) n=6, l=6, ml= 1, ms=-1/2
c) n=3, l=1,...

Calculate the magnitude of the maximum orbital angular momentum
Lmax L m a x for an electron in a hydrogen atom for states with a
principal quantum number of 5. Express your answer in units of ℏ ℏ
to three significant figures.
Calculate the magnitude of the maximum orbital angular momentum
LmaxLmax for an electron in a hydrogen atom for states with a
principal quantum number of 21.
Express your answer in units of ℏℏ to three significant
figures.
Calculate...

For the 3d state (orbital) of the hydrogen atom, the principal
quantum number n=3. The orbital quantum number l = 2. For an
electron with these quantum numbers, what is the smallest angle (in
degrees) that an electron's spin axis (angular momentum axis) can
make with respect to an applied magnetic field?

What are the possible values of n and ml for an electron in a 3d
orbital?
A) n = 1, 2, or 3 and ml = 2
B) n = 1, 2, or 3 and ml = -2, -1, 0, +1, or +2
C) n = 3 and ml = 2
D) n = 4 and ml = -2, -1, 0, +1, +2
Each of the following sets of quantum numbers is supposed to
specify an orbital. Choose the one...

Quantum numbers arise naturally from the mathematics used to
describe the possible states of an electron in an atom. The four
quantum numbers, the principal quantum number (n), the angular
momentum quantum number (ℓ), the magnetic quantum number (mℓ), and
the spin quantum number (ms) have strict rules which govern the
possible values. Identify allowable combinations of quantum numbers
for an electron. Select all that apply.
n = 4, ℓ= 0, mℓ= 1, ms= 1/2
n = 3, ℓ= –2,...

A possible quantum combination of quantum numbers for the single
valence shell electron of K in the ground state is:
A) n = 4, l = 0, ml = 0, ms = +1/2
B) n = 5, l = 0, ml = 0, ms = +1/2
C) n = 5, l = 1, ml = 0, ms = -1/2
D) n = 5, l = 4, ml = 3, ms = -1/2
E) n = 5, l = 0, ml...

1) A quantum harmonic oscillator with frequency
ωcontains 41 electrons. What is the energy of the
highest-energy electron? Assume that the electrons are in the
lowest states possible.
2 a) An atom has a total of 18 electrons. What is the principal quantum number of the
outermost shell?
2 b) How many electrons
does the outermost shell shell contain?
3) Which of the following represents the possible range of
integer values for the magnetic quantum number?
a) 1 to l...

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