Which of the following sets of quantum numbers are not possible give reason?
Answer. a) The given set of quantum numbers is not possible because the value of the principal quantum number (n) cannot be zero.
Which of the following sets of quantum NO is possible?
(ii) n=2,l=1,ml=0,ms=-1/2. (iii) n=2,l=0,m1=3,ms=+1/2. (iv) n=3,l=1,ml=0,ms=+1/2. So , these quantum numbers are possible.
Which set of quantum numbers is not allowed?
The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on.
Which among the following sets of quantum numbers is not possible for an atom in the ground state?
Which of the following set of quantum numbers is not possible for an electron in the ground state of an atom with atomic number 19? For the s subshell, l=0and for the p subshell, l=1. Thus, the third set of quantum members is not allowed as it implies electron in a d subshell (l=2).
Which of the following quantum numbers are possible?
Answer. n = 3; l = 2 and m = +2 represents one of the 3d orbital with magnetic quantum number +2. No two orbitals have same magnetic quantum number. Hence the given quantum number is possible for only one orbital and two electrons.
For which one of the following sets of four quantum numbers an electron will have the highest energy?
Energy of electron depends on the value of (n + l). The subshell are 3d, 4d, 4p and 5s, 4d has highest energy.
Which of the following set of four quantum number is possible?
Answer. Explanation: The energy of a shell is determined by the value of n + l (Principal Quantum Number + Azimuthal Quantum Number). Hence the answer is 2nd option.
How many electrons can fit in the orbital for which N 3 and L 1?
2 electrons
Which of the following sets of quantum numbers are correct?
If n = 3, l= 0, 1,2. For l = 2, m = -2, -1, 0, +1, +2. Hence (c) is correct.
Which N and L values describe an electron in a 3d orbital?
Table of Allowed Quantum Numbers
| n | l | Orbital Name |
|---|---|---|
| 3 | 0 | 3s |
| 1 | 3p | |
| 2 | 3d | |
| 4 | 0 | 4s |
What is the P orbital shaped like?
The p orbital appears as a dumbbell – a spherical shape like the s orbital cut in half. As the atomic nucleus spins, individual protons also spin. There are two times during a rotation that three protons align – 90° and 270° (below).
Which one of the following sets of quantum number is correct for 3d orbitals?
n=3,l=2,m=−3,s=+21.
Which quantum number has only two possible values?
Answer. Answer: The spin quantum number has only two possible values of +1/2 or -1/2. If a beam of hydrogen atoms in their ground state (n = 1, ℓ = 0, mℓ = 0) or 1s is sent through a region with a spatially varying magnetic field, then the beam splits into two beams.
Which of the following can be quantum number for an orbital?
Which of the following can be the quantum numbers for an orbital? Explanation: In the given options, option c is the correct option because in this the value of l is between 0 – n-1 and value of m is between –l to +l. 10.
Which set of quantum numbers could describe an electron in a 3d orbital?
An electron in a 3d orbital could have which of the following quantum numbers? 3 refers to the principal quantum number n. d corresponds to the subsidiary quantum number ℓ = 2. Since ℓ = 2, mℓ could be −2, −1, 0, 1 or 2.
Why does 2 F Subshell not exist?
In terms of quantum numbers, the 2f subshell does not exist because the value of l must be equal to the value of n. the value of l cannot be greater than the value of n. the value of m_l must be equal to the value of l.
What is the L quantum number for a 4p orbital?
1
What is the relation between N and L?
The secondary quantum number, l, divides the shells up into smaller groups of subshells called orbitals. The value of n determines the possible values for l. For any given shell the number of subshells can be found by l = n -1.
What does each quantum number represent?
Quantum numbers are values that describe the energy or energetic state of an atom’s electron. The numbers indicate an electron’s spin, energy, magnetic moment and angular moment.
What are the values of n and l for the Subshells?
For n = 4, l can have values of 0, 1, 2, and 3. Thus, s, p, d, and f subshells are found in the n = 4 shell of an atom. For l = 0 (the s subshell), ml can only be 0. Thus, there is only one 4s orbital.
What are the values of n and l for 4d orbital?
For a 4d orbital, the value of n (principal quantum number) will always be 4 and the value of l (azimuthal quantum number) will always be equal to 2. The values of the magnetic quantum number range from -l to l, so the possible values of ml for the 4d orbital are -2, -1, 0, 1, and 2.
How do you find N and L quantum numbers?
Subshells. The number of values of the orbital angular number l can also be used to identify the number of subshells in a principal electron shell: When n = 1, l= 0 (l takes on one value and thus there can only be one subshell) When n = 2, l= 0, 1 (l takes on two values and thus there are two possible subshells)
What is quantum number and its types?
The set of numbers used to describe the position and energy of the electron in an atom are called quantum numbers. There are four quantum numbers, namely, principal, azimuthal, magnetic and spin quantum numbers. The values of the conserved quantities of a quantum system are given by quantum numbers.