Question

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

Answer #1

option (d) is not possible

a) n=3;l=0;ml=0

for n=3, l=0, the orbital is 3s

for l=0, ml=0(1)

so 3s orbital is possible with the given quantum numbers

b) n=2; l=1 ; ml=-1

For n=2; l=1, the orbital is 2p

for l=0, ml=-1,0,+1(3)

so, 2p orbital is possible with the given quanyum numbers

c) n=1; l=0; ml=0

For n=1; l=0, the orbitsl is 1s

for l=0, ml=0(1)

1s orbital is possible with the given quantum numbers

d) n=4; l=1; ml=-2

For n=4; l=1, the orbital is 4p

for l=1, the possible orientations of ml= -1,0,+1(3)

but given ml=-2, so the orbital is not possible with the givenquantum numbers

Note: ml= 2l+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

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...

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...

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....

Which set of quantum numbers can represent a 5f orbital? My
first choice was A because ℓ is equal to n-1 but this was
incorrect. Can you please provide an explanation of of why A is
incorrect.
A) n=4, ℓ=3, mℓ = 3
B) n=5, ℓ=3, mℓ = -2
C) n=5, ℓ=2, mℓ = 0
D) n=4, ℓ=2, mℓ = -3

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 =...

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,...

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,...

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...

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