Question

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.

Answer #1

**Given**

**n = 2 as principle quantum number**

**we know that the orbital quantum number is equal to n
that from 0 to n-1 so**

**the allowed orbital quantum numbers l are , 0,(2-1)
==> 0,1**

**the number of allowed values of ml values 2l+1 , m =
2*0+1 ,2*1+1 = 1,3**

**the spin values are s = +1/2 ,-1/2**

**the total number of is N = sum of (2(2l+1)) =
2((2*0+1)+(2*1+1)) = (2((1)+(3)) = 2*4 = 8**

**that is the possible quantum states for principle
quantum number n is **

**N = 2*n^2 = 2*2^2 = 2*4 = 8**

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...

Question 3
Part B:How many values of ml are possible for an
electron with orbital quantum number l = 1?
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,
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,...

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,...

A hydrogen atom stays in the 3rd excited state (n = 4). Consider
of the quantum behavior of the electron, but ignore the quantum
behavior of the nucleus. (a) What are the possible values for the
quantum number l and what are the corresponding orbitals? Write
down the magnitude of each orbital angular momentum (in units of
ħ). (b) For each value of l, what are possible values for the
quantum number ml and the magnitude of the z component...

Which of the following statements is incorrect? a. The set of
quantum numbers n = 4, l = 3, ml = –1, ms = 0 is not permitted
because ms = 0. b. The set of quantum numbers n = 3, l = 2, ml = 3,
ms = is not permitted because ml exceeds l. c. The set of quantum
numbers n = 3, l = 2, ml = 1, ms = is permitted. d. The set of
quantum...

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?

Which of the following states of the hydrogen atom, as defined
only by the principal quantum number, orbital angular momentum
quantum number, and magnetic quantum number, is allowed?
a.
n=0, l =2,ml =1
b.
n=5, l =2,ml =3
c.
n=0, l =2,ml =2
d.
n=5, l =2,ml =0
e.
n=2, l =2,ml =0

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...

(I) What is the full ground state electron configuration for a
neutral atom with ? = 22 protons?
(II) A hydrogen atom with a principal quantum number of ? =
4.
a. write all the possible values for the other quantum
numbers.
b. calculate the total number of possible quantum states that
can exist for this principal quantum state.
(III) An excited hydrogen atom is in the 6?1 state.
a. What is the principal quantum
number of the electron?
b....

Which of the following statements is true?
1. quantum numbers n, l, and ml denote the size, shape, and
orientation, respectively, of each atomic orbital
2. the Pauli Exclusion Principle states that no two electrons in
neighboring atoms can have the same set of four quantum numbers
3. according to Bohr's model of the atom, an atomic spectrum
consists of separate lines because an atom has certain allowable
orientations in space
4.the Heisenberg Uncertainty Principle states that it is
impossible...

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