Question

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 that can occupy the 3d subshell?

Answer #1

4)

a)

for n=4, l can take values from 0, 1, 2 and 3

Answer: 0, 1, 2, 3

b)

l=0 is for s orbital

l=1 is for p orbital

l=2 is for d orbital

l=3 is for f orbital

possible subshells are 4s, 4p, 4d, 4f

Answer: 4s, 4p, 4d, 4f

c)

for l=2,

ml can be -2, -1, 0, 1, 2

Answer: -2, -1, 0, 1, 2

d)

l=2 is for d orbitals

So, it corresponds to all 5 d orbitals

e)

for ml = 2, l should be greater than or equal to 2

Answer: greater than or equal to 2

f)

3d shell has 5 subshell with ml values of -2, -1, 0, 1, 2

Each subshell can have 2 electrons

So,

number of electrons = 5*2 = 10

Answer: 10

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...

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,...

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...

a) How many values of the quantum number L (lower case cursive
L) are possible when n=7?
b) How many values of mL (again lower case cursive L) are
possible for an electron in a 6d subshell?
c) How many orbitals are there in a shell with n=3?
Please show work on how yall get the answers yall get. Thank
You!

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...

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,...

1. How many electrons could occupy a subshell with the following
quantum numbers?
a. n=2, l=1
b. n=2, l=0, ml=0
2. How many orbitals are described by each of the below
combinations of quantum numbers?
a. n=3, l=3
b. n=4, l=2, ml=2
3. How many milliliters of 0.100 M HNO3 are needed to neutralize
the following solutions?
a. 34.7 mL of 0.775 M NaOH
b. 58.5 mL of 0.0100 M Al(OH)3
4. How many milliliters of 0.100 M NaOH are...

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?

The values for the total angular momentum of single electrons
are
5/2, 7/2
3/2, 5/2
1/2, 3/2
0, 1/2
2 Possible values for the total angular momentum quantum number
of a single f-electron system are
J = 7/2, 5/2
J = ±3,2,2,0
J = ±7/2, ±5/2
J = None of these
The values for the total angular momentum of single electrons
are
5/2, 7/2
3/2, 5/2
1/2, 3/2
0, 1/2
Answer:
Possible values for the total angular momentum quantum number...

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

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