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Sagot :
a correct set of quantum numbers for an electron in a 3d orbital is n = 3, l= 2, ml = -2. The correct answer is D.
There are four sets of quantum numbers that can be used to characterize electrons in orbitals. These include:
- Principle Quantum Number (n): n = 1, 2, 3,...,
Describes the size of the orbital and the energy of an electron (the distance from the nucleus of the peak in a radial probability distribution plot). The term "same shell" refers to all orbitals with the same value of n. (level). When an electron is in the n=1 orbital of a hydrogen atom, it is in its ground state; when it is in the n=2 orbital, it is in its excited state. An orbital has n² total orbitals for a given value of n.
- Angular Momentum (Secondary, Azimunthal) Quantum Number (l): l = 0, ..., n-1.
defines an orbital's form for a specific principal quantum number. The subshells are smaller groups of orbitals that are created as a result of the secondary quantum number (sublevels). To distinguish l from n, a letter code is typically used to identify it:
l 0 1 2 3 4 5 ...
Letter s p d f g h ...
The 3d subshell is the one with n=3 and l=2, The energy of the subshell is also slightly influenced by the value of l; it rises with l (s, p, d, and f).
- Magnetic Quantum Number (ml): ml = -l, ..., 0, ..., +l.
Describes how an orbital with a certain energy (n) and shape should be oriented in space (l). Each subshell has 2l+1 orbitals, which are used to separate it into separate orbitals that hold the electrons. As a result, the s subshell has a single orbital, the p subshell, three, and so on.
- Spin Quantum Number (ms): ms = +½ or -½.
defines the direction of an electron's spin axis. Only one of two possible directions can an electron spin (sometimes called up and down).
No two electrons in the same atom can have the same values for all four of their quantum numbers, according to the Pauli exclusion principle, named for Wolfgang Pauli, who won the Nobel Prize in 1945. This means that there can never be more than two electrons in a single orbital, and that they must always have opposing spins.
From 1 to infinity, the primary quantum(n) number can have positive integer values. The values of the orbital quantum number (l) range from 0 to (n - 1). The magnetic quantum number can have a value between -l and +l. The values of the spin quantum number are 1/2.
An electron's ability to spin generates a magnetic field that can be directed in one of two ways. The spins of two electrons in the same orbital must be in opposition to one another in order for them to be coupled. These compounds are referred to as diamagnetic since magnets do not attract them. Unpaired electrons are found in atoms where one electron spins more often than the other. These substances are referred to be paramagnetic because of their modest magnetic attraction.
Given these constraints and the knowledge that s p d f corresponds to 0 1 2 3, it follows that n = 5, l = 3, and ml = +1 are the appropriate quantum numbers for an electron in a 5f orbital.
from the question and explanation above we can conclude that quantum number for electron in a 3d orbital have n = 3 l= 2 and 5 orbital with the possible ml in = -2.
learn more about quantum numbers at https://brainly.com/question/16977590
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