Question

What are the possible values of n and ml for an electron in a 3d orbital?

A) n = 1, 2, or 3 and m_{l} = 2

B) n = 1, 2, or 3 and m_{l} = -2, -1, 0, +1, or +2

C) n = 3 and m_{l} = 2

D) n = 4 and m_{l} = -2, -1, 0, +1, +2

Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.

A) *n* = 2, *l* = 2, *ml* =+1

B) *n* = 2, *l* = 2, *ml* =0

C) *n* = 3, *l* = 2, *ml* =-3

D) *n* = 4, *l* = 3, *ml* =-2

E) *n* = 4, *l* = 2, *ml* =+4

Answer #1

Each of the following sets of quantum numbers is supposed to
specify an orbital. Choose the one set of quantum numbers that's
does NOT contain an error
A. n = 2, l = 2, m = -1
B. n = 4, l = 4, m = 2
C. n = 2, l = 2, m = 0
D. n= 4, l = 2, m = -2
E. n = 3, l = 2, m = 3

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,...

5. These sets of quantum numbers are each supposed to specify an
orbital. One set, however, is erroneous. Which one and why?
a. n = 3; l = 0; ml = 0
b. n = 2; l = 1; ml = –1
c. n = 1; l = 0; ml = 0
d. n = 4; l = 1; ml = –2

Which set of values is correct for an electron occupying a 4d
orbital? a. n = 4, l = 2, ml = 0 b. n = 4, l = 2, ml = -1/2 c. n =
3, l = 4, ml = 1 d. n = 3, l = 1, ml = 1

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?

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,...

4. Answer the following questions: (diff=3) a. For n = 4, what
are the possible values of the angular momentum quantum number, l?
b. What subshells are possible within n = 4? c. For l = 2, what are
the possible values of the magnetic quantum number, ml? d. What
orbitals do these l and ml values correspond to? e. If ml is 2,
what are the possible values for l ? f. What is the maximum number
of electrons...

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...

Which of the following are possible sets of quantum numbers for
an electron in an atom? Click the boxes with the correct
answers.
(Select all that apply.)
n = 4, l = 1, ml = -2, ms = +1/2
n = 2, l = 1, ml = -1, ms = +1/2
n = 1, l = 0, ml = 1
n = 1, l = 0, ml = 1, ms = +1/2
n = 3, l = 0, ml =...

Each electron in an atom may be described by a set of four quantum
numbers. For each of the following, write down each different set
of quantum numbers possible such that each set contains the given
value. (The answer for part (a) has been done for you below.) a. n
= 3, l = 1 b. n = 3, l = 2 c. n = 4, l = 2 d. n = 3, l = 2, ml = –2
e....

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