Question

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, m_{l} = 0, m_{s} = +1/2

B) n = 5, l = 0, m_{l} = 0, m_{s} = +1/2

C) n = 5, l = 1, m_{l} = 0, m_{s} = -1/2

D) n = 5, l = 4, m_{l} = 3, m_{s} = -1/2

E) n = 5, l = 0, m_{l} = 1, m_{s} = +1/2

Answer #1

for a given value of **n** (principal quantum
number) , **l** (azimutal quantum number) has 0 to n-1
values

for a given value of **l** there exist 2l+1 values
of **m** (magnetic quantum number)

A) if n =4, l = 0, ml has one value = 0, ms = +1/2 possible combination

B) if n = 5, l =0, ml has one value = 0, ms = +1/2 possible combination

C) if n= 5, l=1, ml has -1,0,+1 values, ms = -1/2 possible combination

D) if n=5, l=4, ml has -4,-3,-2,-2,-1,0,1,2,3,4 values , ms = -1/2 possible combination

E) if n=5,l=0,ml has one value =0, ms = +1/2 possible combination

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,...

Which of the following are permissable sets of quantum numbers
for an electron in a hydrogen atom? The atom may be in an excited
state (ie. the electron need not be in its ground state). Choose
all of the correct possibilities.
n = 5, l = 1, ml = -1, ms = -1/2
n = 4, l = 0, ml = 0, ms = -1/2
n = 5, l = -4, ml = -3, ms = -1/2
n = 5,...

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 =...

Which of the following are permissable sets of quantum numbers
for an electron in a hydrogen atom? The atom may be in an excited
state (ie. the electron need not be in its ground state). Choose
all of the correct possibilities. n = 4, l = 3, ml = -3, ms = +1/2
n = 4, l = 2, ml = -2, ms = -1/2 n = 2, l = 1, ml = 0, ms = +1/2 n
= 4,...

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...

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.
n = 4, ℓ= 0, mℓ= 1, ms= 1/2
n = 3, ℓ= –2,...

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....

1. Which of the following set of quantum numbers (ordered n, ℓ,
mℓ, ms) are possible for an electron in an atom? Check all that
apply.
a. 3, 2, 2, -1/2
b. -1, 0, 0, -1/2
c. 3, 2, 1, -1
d. 4, 3, 4, -1/2
e. 2, 2, 2, 1/2
f. 4, 3, -2, 1/2
g. 5, 2, 1, -1/2
h. 3, 1, -2, -1/2
2. How many possible combinations are there for the values of l
and ml...

Determine whether or not each set of quantum numbers shown could
correctly describe an electron in an atom. (Choose "Possible" or
"Impossible" for each statement.)
n = 4; l = 3; ml = 3; ms = 1/2
n = 3; l = 3; ml = -2; ms = 1/2
n = 3; l = 2; ml = -2; ms = 3/2
n = 3; l = 1; ml = 2; ms = 1/2
n = 3; l = 1; ml...

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