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What is the value of the quantum number n for a spin down electron in a 2 s orbital?
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What is the only possible value of mâ„“ for an electron in an s orbital?
answer = 0
What is the relationship between n and the total number of sublevels in a main energy level?
An electron in an atom is described by four quantum numbers:n, the principal quantum numberl, the azimuthal quantum numberml, the magnetic quantum numberms, the spin angular momentum quantum numberThe principal quantum number is a positive integer: 1, 2, 3, etc.The azimuthal quantum number is a non-zero integer: 0, 1, 2, 3, etc.The relationship between n and l is that l must always be strictly less than n. So, for n=1, the only permissible l value is 0. For n=2, l can be 0 or 1. So the number of types of orbitals per level is equal to n.The relationship between l and ml is that ml is an integer between -l and +l. There are 2l+1 values of ml for any given value of l.Since each n, l, ml triple specifies an orbital, if you work it out it turns out that there are n2 orbitals with a given principal quantum number n.Each orbital can have two electrons (ms = +1/2 or -1/2), so there are twice that number of electrons.
What does the principal quantum number tell you?
The principal quantum number is the level of the most energetic electrons in an atom. It also corresponds to which period the element is in on the periodic table. For example, barium has a principal quantum number of 6 because its valence electrons are in level 6, and the element is in period 6.
What does the energy of each level n depend on?
The main principal quantum number (n) depends on the average relative distance of an electron from the nucleus. The farther away from the nucleus, the greater value for n and the greater the energy.
How many electrons have quantum numbers values n l m?
In theory, the number of electrons with each quantum number is not limited. However, for any given "main quantum number" (n), the number of electrons having the other quantum numbers is limited - but it depends on the value of "n". For more information, the Wikipedia article on "quantum number" seems to give a good overview.
What does the second quantum number (l) describe?
Which sublevel the electron is in.
What is the difference between the 2px orbital and the 2py orbital?
The px orbital has a magnetic quantum number value of -1, and the py orbital has a magnetic quantum number value of 0.
What quantum number represents the orientation of an electron orbital in space?
The quantum number that indicates the position of an orbital is the magnetic quantum number. The number of different sublevels within each energy level of an atom is equal to the value of the principle quantum number.
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.
All of the orbitals in a given electron shell have the same value of the?
Principal quantum number.
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 will be the value of magnetic quantum number if the value of azimuthal quantum number is given to you?
-l to l, so given l=2 (d orbital) the values for ml will be -2, -1, 0, +1, +2
The numerical values of the magnetic quantum number m1 depends on the?
The values of the magnetic quantum number depend on the value of the azimuthal quantum number (orbital angular momentum quantum number) and has values -l, .. 0 . ..+l l=1, p orbital, -1, 0, +1 - three p orbitals l=2 d orbital -2, -1, 0., +1,+2 five d orbitals etc.
What does the third quantum number m describe?
It refers to the orientation of the orbital on the xyz coordinate system. It is dependent on the value of "L". Possible values range from -L through +L.
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.
What is the only possible value of mâ„“ for an electron in an s orbital?
answer = 0
How many electrons can possess this set of quantum numbers... principal quantum number 4... angular quantum number 2?
10 electrons.The angular momentum quantum number is l (small L). This quantum number is dependant on the principal quantum number, and has values, 0 1,2 ..(n-1), where each value of n refers to a subshell known to chemists as followsn= 0, s orbital; n=1, p orbital; n= 2, d orbital; n= 3, f orbital.So we are looking at the d orbitals.There are five d orbitals, with magnetic quantum numbers running from -l to +l, that is -2, -1, 0, +1, +2Each of these can hold 2 electrons (with spin quantum numbers -1/2, +1/2)So we have 10 electrons that can have pricipal quantum numbers of 4 and angular monmentum quantum number of 2.
