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Why is it impossible for an electron to have the quantum numbers n3 i1?
I am checking the Wikipedia article on "quantum number", and don't find a quantum number "i" for the electron. If you mean "l", it seems that "l" can be between 0 and n-1. So, for n = 3, l can be between 0 and 2. If this is what you mean, I don't see any reason that would forbid this particular combination.
The Quantum Number that defines the probable distance an electron is from the nucleus is the quantum number.?
secondary quantum numberI don't think it is a number, but it could be referring to the Orbitals, being S, P, D, and F. Each orbital is a specific shape and the orbitals are determined in blocks on the Periodic Table. The energy, or Quantum Number would go in front, such as 4p, which means the principal quantum number or energy level is 4 and the orbital shape is p. Hope this helps
What are the possible values of the magnetic quantum number?
The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1) where l is the azimuthal, angular momentum quantum number. The magnetic quantum number ml depends on the orbital angular momentum (azimuthal) quantum number, l, which in turn depends on the principal quantum number, n. The orbital angular momentum (azimuthal) quantum number, l, runs from 0 to (n-1) where n is the principal quantum number. l= 0 is an s orbital, l= 1 is a p subshell, l= 2 is a d subshell, l=3 is an f subshell. The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1). ml "defines " the shape of the orbital and the number within the subshell. As an example for a d orbital (l=2), the values are -2, -1, 0, +1, +2, , so 5 d orbitals in total.
Who developed the quantum theory of the nuclear atom?
Heisenberg and Schrodinger developed the electron cloud model using quantum mechanical probability functions to determine the the regions, or clouds, in which electrons would most likely be found outside of the nucleus.
What determines the lenght of each period in the periodic table?
The number of elements in each period is the sum of (1) the maximum number of electrons permitted in the quantum state characterized by the same number as the number of the period and (2) the maximum number of electrons permitted in a quantum state characterized by a lower quantum than the number of the period but with an energy level for the electron that is less than the energy state of the next electron that can be added to the highest numbered quantum level of the atom with an atomic number lower by one than the atomic number of the atom concerned.A somewhat oversimplified explanation of this rather complicated rule follows:Item (2) of the rule occurs only in periods 4 and higher, because the third quantum number is the lowest one that can contain d electrons. In argon, with atomic number 18, the first three quantum levels contain all the s and p electrons that are allowed. Another electron is required to form potassium, which contains 19 protons, and it happens that a 4s electron has a lower energy than a 3d electron, so that the two allowed s electrons with quantum number 4 are added to form potassium and calcium successively. However a 4p electron has more energy than a 3d electron; therefore, the ten 3d electrons are added successively to form the elements with atomic numbers from 21 to 30, the first transition metals, before a 4d electron is added to form gallium, with atomic number 31.A similar situation arises in period 6 to form the inner transition elements. Although the fourth period is allowed to contain f electrons, their energy level is higher than that of 5s, 5p, 5d, and 6s electrons, so that no f electrons are present in atoms of the first five periods in their ground states. However, at atomic number 56, all of the s, p, and d quantum states of the first five quantum numbers have been occupied, and it happens that the energy of the first 4felectron is lower than that of the first 6p electron. Therefore, the 4f quantum level is filled with all of its electrons, from atomic numbers 57 through 71, and only then is n 6p electron added to form an atom with atomic number 72.A corresponding phenomenon occurs again in the 7th period, since the 5f orbitals have lower energies than the 7porbitals.The above explanation is oversimplified because not all f orbitals with the same quantum number have exactly the same energy, so that there can be instances in the transition and inner transition elements in which the "next" f electron has higher energy than the "next" p electron with a quantum number higher by two. Therefore, a few of the transition elements contain one or more p electrons of their highest orbital number instead of one or more of the f electrons that would be expected from the discussion above.
What is the first quantum number of a 1s2 electron in phosphorus?
The first quantum number (n) represents the energy level (shell), so for a 1s2 electron, it would have a value of 1.
What is the second quantum number of the 3p1 electron in aluminum?
The principal quantum number n = 3 and the azimuthal or orbital angular momentum quantum number would be l =1 .l = 1
What is the principal quantum number value for the highest energy electron in carbon atomic number 6?
The principal quantum number for the highest energy electron in carbon would be 2. It is easy to spot this, since carbon exists in row 2 of the period table. The row in which an element resides always shows the highest value of n, or the principal quantum number, that an electron can reside in.
What would the fourth quantum number of a 1 S 2 electron be?
Either +1/2 or -1/2; the fourth quantum number is ALWAYS either +1/2 or -1/2 and it's not generally possible to say which (other than that two electrons in the same atom which have the same first three quantum numbers will always have different values for the fourth).
Which quantum number represents the distance between an electron shell and the nucleus?
Based on Heisenberg's uncertainty principle, there is no way possible to have a quantum number for position since the electron's second quantum number already gives you an exact value for its angular momentum.Bohr calculated the most probable radius of the electron cloud (which he mistakenly thought was an actual distance) getting the number 5.29X10-11 m.What I think the asker is speaking of is the quantum number that refers to energy level, n. Though not a physical distance it may be interpreted, using the Bohr model, how "far" away an electron is from the ground state, which some would believe (incorrectly) that this is a function of distance from the nucleus.
Why is it impossible for an electron to have the quantum numbers n3 i1?
I am checking the Wikipedia article on "quantum number", and don't find a quantum number "i" for the electron. If you mean "l", it seems that "l" can be between 0 and n-1. So, for n = 3, l can be between 0 and 2. If this is what you mean, I don't see any reason that would forbid this particular combination.
How big is a quantum leap?
A quantum leap is the smallest possible change that an electron can make in an atom. It involves a discrete jump in energy levels when an electron transitions from one orbit to another. The size of a quantum leap is determined by the difference in energy levels between the initial and final states of the electron.
What are three main parts of an electron's address used in the current atomic theory that describes an electron's location?
I think you are referring to the 3 quantum numbers, n, l m; principal azimuthal and magnetic. Together with the spin quantum number they "define" an electron- but I would hesitate to call this the electrons location- Heisenbergs uncertainty principle gets in the way of a simultaneous knowledge of energy and location.
When would quantum theory change?
when data shows electron energy levels are not related to light wavelengths.
The Quantum Number that defines the probable distance an electron is from the nucleus is the quantum number.?
secondary quantum numberI don't think it is a number, but it could be referring to the Orbitals, being S, P, D, and F. Each orbital is a specific shape and the orbitals are determined in blocks on the Periodic Table. The energy, or Quantum Number would go in front, such as 4p, which means the principal quantum number or energy level is 4 and the orbital shape is p. Hope this helps
What are the possible values of the magnetic quantum number?
The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1) where l is the azimuthal, angular momentum quantum number. The magnetic quantum number ml depends on the orbital angular momentum (azimuthal) quantum number, l, which in turn depends on the principal quantum number, n. The orbital angular momentum (azimuthal) quantum number, l, runs from 0 to (n-1) where n is the principal quantum number. l= 0 is an s orbital, l= 1 is a p subshell, l= 2 is a d subshell, l=3 is an f subshell. The magnetic quantum number, ml, runs from -l to +l (sorry this font is rubbish the letter l looks like a 1). ml "defines " the shape of the orbital and the number within the subshell. As an example for a d orbital (l=2), the values are -2, -1, 0, +1, +2, , so 5 d orbitals in total.
Why do two electrons in the same orbital have to have opposite spin states?
Yes. Always. Otherwise they would break the fundamental rules of quantum mechanics, which say that no two electrons can have the same four quantum numbers -- and spin is the 4th quantum number. If two e- are in the same orbital, they share 3 quantum numbers, but the spin quantum number must then be different.
