Question

what is the maximum number of electrons in the atom that can have the following quantum numbers

1). n=3 and magnetic quantum= -2

2). n =4 and l=3

3). n= 5, l=3, and magnetic quantum=2

4). n=4, l=1 and magnetic quantum=0

Answer #1

Question 1. n=3 means it contains 3 shells. Then its azimuthal quantum number will be 0 to n-1. That is 0 to 2. 0 for S, 1 for P. 2 for d orbital respectively. Then, magnetic quantum number m= -l to +l. (ie from -2,-1,0,1,2)

The magnetic quantum number here is -2. So it represent
**dxy orbital**. (five orbitals are
dxy,dyz,dxz,dx^{2}-y^{2},dz^{2}) So 2
electron can be filled dxy.

Question 2. n=4, l can be from 0 to n-1. So 0 (s),1 (p), 2 (d),
3 (f). here asked one is l=3 so **f orbital**. So
total of 14 electrons can be filled f orbitals.

Question 3. n=5, l=3, m=2 So it is an f orbital., But only one f orbital from 7 f- orbitals mentioned, so again only 2 electron can be found in m=2.

Question 4. n=4, l=1, m=0. P is orbital ( l=1) and only 3 shapes
are there in p orbitals. ie, Px, Py, and Pz. So if the m=0, then it
will be **Py orbital**. So again 2 electron can be
filled here.

What is the maximum number of electrons in an atom that can have
the following quantum numbers?
Express your answer as an integer.
part A. n = 3, ml = -2
part B. n = 4, l = 3
part C. n = 5, l = 3, ml =
2
Part D. n = 4, l = 1, ml =
0

In an atom, what is the maximum number of electrons that can
have the following quantum numbers?
(a) n = 3, ms = +1/2
(b) n = 6, l = 2
(c) n = 3, l = 2, ml = -1
(d) n = 4, l = 3, ml = +1

What is the maximum number of electrons in an atom that can have
the following quantum numbers?
(A) n=6, l=5, ml= -1
(B) n=4, l=1, ml=+1, ms=+1/2
No explanation, just answers

What is the maximum number of electrons in an atom that can have
these quantum numbers: (Remember the shortcut: n2 = #
______________________ whereas 2n2 = # ________________ where n
stands for _________________________________).
n=4 n=5, ml = +1 n=5, ms = + ½ n=3, l = 2 n=2, l = 1

What is the maximum number of electron in an atom that can have
the following quantum numbers? (a) n = 3, ml = -2; (b) n = 4, l =
3; (c) n = 5, l = 3, ml = 2; (d) n = 4, l = 1, ml = 0.

For these quantum numbers, determine the number of electrons an
atom could have.
a) n=3
b) n=4 l=2
c) n=6 l=2 ml=-1

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...

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

Suppose two electrons in an atom have quantum numbers n = 5 and
L = 4.
(a) How many states are possible for those two electrons? (Keep
in mind that the electrons are indistinguishable.)
(b) If the Pauli exclusion did not apply to the electrons, how
many states would be possible?

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?

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