Practice: How many different values of m_{l} are possible for a 4d set of orbitals?

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The **Magnetic Quantum Number** gives the location of an electron within a specific orbital.

Example #1: Provide the identity of a set of orbitals that exist in the 4th principal level and f sublevel

Example #2: Which of the following is not a valid magnetic quantum number for the 7f set of orbitals?

Practice: How many different values of m_{l} are possible for a 4d set of orbitals?

Practice: Select a correct set of values for an electron found within the designated 5f orbital.

Practice: Which of the following statements is false?

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Concept #1: Quantum Numbers: Magnetic Quantum Number

Example #1: Quantum Numbers: Magnetic Quantum Number Example 1

Concept #2: Quantum Numbers: Magnetic Quantum Number

Example #2: Quantum Numbers: Magnetic Quantum Example 2

Practice #1: Quantum Numbers: Magnetic Quantum Practice 1

Practice #2: Quantum Numbers: Magnetic Quantum Practice 2

Practice #3: Quantum Numbers: Magnetic Quantum Practice 3

In a p x orbital, the subscript x denotes which of the following?
a. the energy of an electron
b. the spin of an electron in that orbital
c. the probability of the shell
d. the size of the orbital
e. the axis along which the orbital is aligned

Which set of quantum numbers is correct and consistent for an electron with n = 3?
a. l = 3 , m1 = – 3
b. l = 2 , m1 = + 2
c. l = 2 , m1 = + 3
d. l = 4 , m1 = – 1

What are the possible values of n and ml for an electron in a 4d orbital?
A. n = 1, 2, 3, or 4, and ml = -2, -1, 0, +1, or +2
B. n = 1, 2, 3, or 4, and ml = 2
C. n = 4 and ml = 3
D. n = 4 and ml = -2, -1, 0, +1, or +2
E. n = 5 and ml = -2, -1, 0, +1, or +2

Identify the correct values for a 4f sublevel.
a. n=3, l=1, ml=0
b. n=2, l=1, ml=-2
c. n=1, l=0, ml=0
d. n=2, l=0, ml=0
e. n=4, l=3, ml=-2

Which quantum numbers below could correctly describe the orbital to the right?
(a) n = 1, l = 0, m l = 0
(b) n = 2, l = 2, m l = 1
(c) n = 3, l = 1, m l = -1
(d) n = 3, l = 2, m l = -3
(e) n = 3, l = 2, m l = 2

There are __________ possible values for the magnetic quantum number of an electron in a 5f subshell.
A) 7
B) 3
C) 14
D) 5
E) 1

Which sketch represents an orbital with the quantum numbers n = 3, l = 0, and ml = 0?

A. How many hydrogen atom orbitals will have the following quantum numbers?
1. n = 4 __________
2. n = 4 and l = 2 __________
3. n = 4 and m l = 2 __________
4. n = 4, l = 2, and m l = 2 __________
B. The number of orbitals with n = 2 is less than / equal to / greater than (circle one) the number of orbitals with l = 2.
Explain your reasoning.

Which response lists all the true statements about the four quantum numbers?
I. n = principal quantum number, n = 0, 1, 2, 3, ...
II. l = angular momentum quantum number, l = 0, 1, 2, 3, ... ., ( n+1)
III. ml = magnetic quantum number, ml = (-l) ...., 0, .. (+l)
a) I, II, and III
b) I and III
c) I and II
d) II and III
e) III only

Provide the n, l and ml value for each of the given orbitals.
a. 22f n =
l =
m l =
b. 5d n =
l =
m l =

Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:
a) n = 3, ℓ = 2, m ℓ = 0, m s = –1/2
b) n = 3, ℓ = 1, m ℓ = –3 , m s = 1
c) n = 4, ℓ = 0, m ℓ = 0, m s = –1/2
d) n = 4, ℓ = 2, m ℓ = –3, m s = –1/2

For n = 7 and ℓ = 4, what is m ℓ ?
1. 18
2. 0, 1, 2, 3
3. 9
4. 0, 1, 2, 3, 4
5. −4, −3, −2, −1, 0, +1, +2, +3, +4

Which one of the following set of quantum numbers would not be allowed?
A) n = 3, ℓ = 2, mℓ = 1
B) n = 3, ℓ = 1, mℓ = -1
C) n = 3, ℓ = 0, mℓ = 0
D) n = 3, ℓ = 2, mℓ = -1
E) n = 3, ℓ = 3, mℓ = 1

Which is not a possible ml value for a subshell that has the following: l = 2
a. +3
b. –1
c. +2
d. 0
e. -2
f. All these are possible

Which of the following is not a valid magnetic quantum number for the 3d set of orbitals?a. 1b. 2c. 0d. -2e. -3

Set(s) of possible values of m ℓ areA) -4; -3; -2; -1; 0; +1; +2; +3; +4B) -3; -2; -1; 0; +1; +2; +3C) -2; -1; 0; +1; +2D) -1; 0; +1E) 0 Select the best choice for n = 3.1. only B, C, D, and E2. only E3. only B4. A, B, C, D, and E5. only D6. only C7. only D and E8. only C, D, and E

Which quantum numbers must be the same for the orbitals that they designate to be degenerate in a one-electron system (such as hydrogen)?a) n, l, and m lb) n and l onlyc) l and mld) ml and only e) n only

Which of the following sets of quantum numbers is not allowed?a) n = 3, l = 1, m l = +1b) n = 3, l = 0, m l = 0c) n = 4, l = 2, m l = +2d) n = 4, l = 1, m l = 0e) n = 4, l = 2, m l = +3

What type of orbital is designated when n = 4, l = 3, m l = -1?a) 3pb) 3dc) 4pd) 4de) 4f

(b) For l = 2, what are the possible values of m l?

(c) If m l is 2, what are the possible values for l?

How many possible values for l and m l are there when (a) n = 5?

Give the values for n, l, and m l for (a) each orbital in the 2p subshell

For the table that follows, write which orbital goes with the quantum numbers. Don’t worry about x, y, z subscripts. If the quantum numbers are not allowed, write “not allowed.”

Can an electron in an atom be in an energy level described by the set of quantum numbers n = 5, ℓ = 3, m ℓ = -2?1. No, because m ℓ cannot be negative.2. No, because ml must be equal to ±1.3. Yes4. No, because n cannot be as large as 5.5. No, because ℓ must be equal to n -1.

Which of the following sets of quantum numbers is possible?A. n = 3, l = 3, ml = 0B. n = 3, l = 2, ml = -3C. n = -3, l = -2, ml = -2D. n = 3, l = 1, ml = 0E. n = 3, l = 2, ml = 1/2

Which statement about quantum numbers is incorrect? Answer (e) if they are all correct or all incorrect.a. The principal quantum number cannot equal zero.b. When n = 3, the angular quantum number can be equal to 0, 1, or 2.c. For an angular quantum number equal to 1, the magnetic quantum number can be +1, 0, or -1.d. For any value of the angular quantum number (l), there are 2(2l+1) values of the magnetic quantum number.e. All the above statements are correct or all are incorrect.

Which set of quantum numbers (principal, angular and magnetic) are not valid?Set (1) 4, 2, -3Set (2) 3, 2, -2Set (3) 2, 2, +1a. Sets (1) and (2)b. Sets (2) and (3)c. Sets (1) and (3)d. all three setse. only one or none of these sets.

What are the possible values of n and m l for an electron in a 5d orbital?a) n = 1,2,3,4, or 5 and m l = 1b) n = 1,2,3,4 or 5 and m l = -2, -1, 0, +1, or +2c) n = 4 and m l = -1, 0, or ld) n = 5 and m l = 2e) n = 5 and m l = -2, -1, 0, +1 or +2

What is the only possible value of mℓ for an electron in an s orbital?

Which set of three quantum numbers does not specify an orbital in the hydrogen atom?a. n = 3; l = 3; m l = −2b. n = 2; l = 1; m l = 1c. n = 3; l = 2; m l = 2d. n = 2; l = 1; m l = 0

What are all the possible values of m l if l = 0 (an s orbital)?

How many possible values for l and m l are there when (a) n = 3?

An electron in a 3d orbital could have which of the following quantum numbers?1. n = 3; ℓ = 3; m ℓ = 12. n = 3; ℓ = 1; m ℓ = -13. n = 3; ℓ= 2; m ℓ = 04. n =3; ℓ = 0; m ℓ = 05. n = 3; ℓ = 1; m ℓ = 26. n = 3; ℓ = 2; m ℓ = -37. n = 2; ℓ = 2; m ℓ = 6

Which set of three quantum numbers does not specify an orbital in the hydrogen atom? Provide step by step explanation.a. n = 2; l = 1; m l = -1b. n = 3; l = 2; m l = 2c. n = 2; l = 0; m l = 0d. n = 3; l = 4; m l = 0

How many orbitals in an atom can have the designation 5p, 3dz 2, 4d, n = 5, n = 4?

Based on the following atomic orbital shape, which of the following set of quantum numbers is correct:a) n = 2, ℓ = 1, m ℓ = 0b) n = 3, ℓ = 2, m ℓ = –1c) n = 4, ℓ = 0, m ℓ = +1d) n = 1, ℓ = 1, m ℓ = 0

What values of ml are possible for l = 2?

What are the possible values of the magnetic quantum number m l?a. represented by the formula: m = 2k +1, where k is a positive integerb. all the non-negative integers: 0,1,2,3, etcc. all the positive integers: 1,2,3, etcd. all the integers in range from, -l to +l where l is an angular momentum quantume. number represented by the formula: m = 2l + 1, where l is an angular momentum quantum numberf. all the integer: -3,-2,-1,0,1,2,3, etc.

If mℓ = 3, what can you say about ℓ?a. ℓ = 3?b. ℓ > 3?c. ℓ ≥ 3?d. ℓ <3?e. ℓ≤ 3?

What are the possible values of mℓ for an electron in a d orbital? Express your answer numerically with sequential values separated by commas.

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