Orbitals Definition and 236 Threads

Hello, all, I have a question about the wave functions of H atom: for p orbital, wave functions from the Schrodinger equation are p+1, p0, and p-1. In chemistry, people use the linear combination of p+1 and p-1 to generate px and py orbitals. The question is: p+1 and p-1 orbitals are...

1. We know px,py,pz are degenerate orbitals... My question is suppose in 0=[He] 2s^2 2px^2 2py^1 2pz^1 Are the px,py,pz orbitals degenerate here? 2. What is the true reason of inert pair effect? 3. What is the order of shielding effect for s,p,d,f?I just want to verify my answers...

Is there some resource on the net where I can find images of electron orbitals for dihydrogen (H2), helium (He), lithium (Li) and dilithium (Li2)? Alternatively if there is some software that can produce such images, that would be good too.

1. We know px,py,pz are degenerate orbitals... My question is suppose in 0=[He] 2s^2 2px^2 2py^1 2pz^1 Are the px,py,pz orbitals degenerate here? 2. What is the reason of inert pair effect? 3. What is the order of shielding effect for s,p,d,f?

Homework Statement Does the size of the p orbital with the lone pair change when adding electron donating groups, such as methyl? Homework Equations N/A The Attempt at a Solution I know the electron availability increases on the nitrogen's lone pair, making it a better base, but I'm...

Which one of the following orbitals is lowest in energy in a Li2+ ion? 37s 12p z 2d x^2-y^2 5f xyz 4d xz attempt on solution: n=3 l=can be n-1 ml=-l to + l Therefore the lowest energy is I suppose the answer is 12p z? since the l can be any number smaller than 3 until...

Hello all, this came up in my chemistry class when our prof. showed a graph of the size of atomic orbitals (or orbital energy) in relation to the Z number (or number of protons). He did this to show that as the z number increases the size of the orbitals also decrease (because effective nuclear...

I have observed that when the outermost orbital is half filled (like Nitrogen 1s2 2s2 2p3), the atom has a higher stability (or a lower binding energy). Why is this so? I have heard it has to do with the fact that electron spin is maximized at that point but it still does not make sense to me...

Hello, where does the energy that let electrons move inside orbitals came from and are they subject to Coulomb attraction with the nucleus ?

1. "i.e an electron is removed from one of the single electron orbitals into the vacuum." I know what orbitals are but I don't know what constitutes single-electron orbitals. I first assumed it was simply an orbital which in a given configuration only had one electron but that had to be ruled...

Are particles considered to be standing waves? Or only in certain situations such as an electron in its atomic/molecular orbital?

Hello. I'm having a problem understanding the 3d orbitals when I'm doing electron configurations. When you fill up electrons for let's say nickel, Ni, you get the configuration: [Ar]3d8 4s2, if I'm not mistaken. But what I have read, at least I think I have, the 3d orbital gets really...

(is this correct … ?) electrons "orbiting" a single atom obey the Schrodinger equation, whose solutions are linear combinations of an orthogonal basis of solutions of the form R(r)Θ(θ)Φ(φ) [SIZE="1"]where r θ and φ are the usual spherical coordinates: θ = 0 is the usual z axis these...

I know that the shape of s orbital is sphere, p orbital is dumbbell shaped and d orbital is like a doughnut but why do these orbitals have these shapes why not some other shape.

Are the orbitals circular or spherical or parabolic?? Are they 3D? Are the orbitals circular or spherical or parabolic?? Are they 3D?

Can the degeneracy of orbitals be affected in anyway?

Homework Statement Assume that you travel through space to a strange universe where the allowable values for the quantum numbers are quite different from those in our own universe. In this new universe, s orbitals may contain a total of 2 electrons, p orbitals may contain a total of 4...

I understand that electrons can be in any particular location of an orbital. However, why do they have such a large space for the electron to potentially be in? Shouldn't the electron stick to the proton?

Hey Everyone, If you have an electron with the various energy levels: -14 eV, -30 eV, -52 eV, -80 eV. And that the electron can only move between these levels. How do I go about finding the photo energy that is emitted? Do I just subtract the various levels? Ex. 14 - 30 = -16 etc?

Homework Statement Given the numerical value of a0= 5.3X10^11m in the Bohr hydrogen atom, find the radius of the first five orbitals as well as the radius for n=100. Homework Equations Rn=a0 x n^2 The Attempt at a Solution Could it be as simple as typing in for the third orbital...

I am terribly confused. I have always been hearing that in the hydrogen atom, 2s and 2p orbitals have the same energy. Similarly, the 3s, 3p and 3d orbitals have the same energies. This is also suggested by the hydrogen spectrum, my professor also believes the same, and I am unable to find...

Natural Orbitals for "Particles in a Box" Hi, Are Sine waves the natural orbitals for particles in a box when electron-electron interactions are considered? Or is it only true for non-interacting electrons?

If there is a cloud of electrons around an atom than why can't there be orbitals between 1 and 2 or between 2 and 3. I know the probability of an electron being between certain nodes decreases as they approach them but why as the probabilities go away from the perfect orbital do they not become...

Hey everyone, So I've been a little bit confused about something, and I'd like some input on this: When I look at systems like the particle in a box, or the Hydrogen Atom, it's clear that the higher energy states of comparable shape have more nodes. This seems to always be true. For any...

just thinking... the energy of an orbital depends on: a)quantum number n b)quantum number l. an orbital will be of less energy when it's more contracted. So technically, 3d should have a lower energy than 4f and hence be contracted. BUT IT'S THE OTHER WAY AROUND! help? thank you!

Homework Statement Compare the energies of the 1s, 2s, 3s and 3p orbitals for both the HE and He+. For He assume that one electron is always in the 1s orbital. State any other assumptions you have made 2. The attempt at a solution I think: He can be either 1s1 2s1 or 1s2 He+ has to be...

Homework Statement Both H and He+ atoms contain a nucleus and a single electron. Therefore He+ is often referred to as Hydrogen-like. According to the Bohr Model, the electron in He+ should orbit the nucleus in discrete orbits, much like the electron in the Hydrogen atom orbits its nucleus...

l don't quite understand the difference . as far as l see it , orbital was defined as a group of orbits so that one level of energy can contain many electrons without canceling each other . in other words one level can have exact similar electrons but in different orbits within the same...

When 2 atoms bond, do all their atomic orbitals combine, or is it just the bonding orbitals that combine? For example when sodium and chlorine bond, do all their orbitals combine or is it just sodiums 3s orbital that combines with chlorines 3p orbital?

So I usually use VESTA to make my figures, and though the new version is able to do many mad things with calculated electron density isostructures and whatnot, I can't seem to just be able to throw in some clover-leaf d or p orbitals like what was done in the image below (from this paper on...

So we've all seen the pictures of orbitals in chemistry textbooks. You know, the sphere for an s orbital, the two balloons for a p orbital, etc. But they always present these models as independent systems. No one has ever told me what the orbitals look like (and yes I know that an orbital is...

Why don't electrons move only along the surface of orbitals? Moreover, how do electrons move within orbitals, random movement or do they follow a definite path? In a p-orbital, does one lobe consist of only one electron? Why is the p-orbital dumbbell shaped and not spherical?

Hi Thinking of the structure of an atom in terms of spherical harmonics; the mathematics of which is the base of schrodinger's wave equation. If its possible to make the electrons gather at the antinodes, what are the possible applications/uses of this? (Simply a new area for research? or...

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Hi folks, Hartree Fock theory tells us, that the energy functional <\Psi|H|\Psi> where \Psi is a single Slater determinant is minimized by using spin orbitals \phi_i that fulfill the Hartree Fock equations f_i \phi_i = \epsilon_i \phi_i. Since the Fock operator f_i depends on the solution, the...

For a summer class, I’ve been trying to get the quantum picture of an atom at least in conceptual terms, no math. I understand how, if you think about an atom like a one-dimensional box, an s orbital is like the first fundamental wave, and a p-orbital is like a sine wave, and I understand how...

hi, why does one choose in Hartree Fock theory the following type of spin orbitals? spinorbital(r,s) = spacialOrbital(r)*alpha(s) or spinorbital(r,s) = spacialOrbital(r)*beta(s) where alpha(s) is the spin up function and beta(s) the spin down function. Why does one not choose the...

Just curious why chemical physicists bother with localization procedures for molecules. Because atomic orbitals become de-localized when they form molecular bonds, but then it seems people wish to come up with procedures to re-localize. I've read quite a bit on how the de-localization...

atomic orbitals, what i just know about them is they are the regions around the nucleus where the probability of finding an electron is high and that is OK with s orbital because it is spherical. but when an electron in p orbital spins the probability of finding an electron should spin...

Why electrons occupy degenerate orbitals with parallel spins? heard something of stability due to exchange pairing of electrons. someone kindly clarify this matter.

If i take any integer, x write out all integers from 0 to x - 1 write out all numbers between negative and positive values of those numbers I get x squared total values. why? what is the mathematical logoc behind this? x = 3 0 to x - 3 = 0, 1, 2 0 -1, 0, 1 -2, -1, 0, 1, 2 9...

Hi all, To my knowledge hybridization of atomc orbitals occurs only between orbitals in the same atom, with similar energies, in order to produce new atomic orbitals, identical with the same energy, to make chemical bonds with other atoms. There are sp, sp2, sp3, etc... possibilities. My...

Hi, If 2s orbital and 2p_z orbitals are near enough in energy, then they can mix together to form two sp hybrid orbitals. But how can I deal with sp^3 or sp^2 hybridization? According to MO only orbitals with the same symmetry species can overlap, so how can an s orbital overlap with a p_x...

I am studying orbitals at school. They are very interesting and strange at the same time; they seem to be very similar to a planet in orbit around a black hole. However I am not here for that. I was wondering if you knew a good and short reference in order to understand E,Shrodinger's equation...

Hello Forum, Does anyone know where I can find the slater bases for the alkali metal 'np' orbitals and the noble gas '(n+1)p' orbitals, either altogether or individually? I'm a physicist and wanted to know what the standard (or even non-standard) reference is? I know that the...

I was thinking about how you'd hybridize oxygen and nitrogen orbitals (should be pretty straightforward), but I was getting confused. It's clear to me for carbon binding to 3 atoms with a double bond on one (say C in benzene ring: electron from 2s gets promoted to 2p, then you have 3 sp2...

hey, i am concerned with landau levels and wanted to ask you whether you have a link, where one can see the orbitals- just like the orbitals for the hydrogen atom- for at least a few electron states? otherwise it would be sufficient if you could give me a hint how to calculate them. i...

I've haven't taken a chemistry course as of yet, so I'm probably getting something very wrong here, but one thing that someone said confused me. They said that when an electron changes it's orbital, it emits a photon. I like to think about orbitals (and I know that this is ONLY a useful...

It's my understanding that electron orbitals arise from the steady state solution to the Schrodinger equation. In what ways can these be deformed? Some possible solutions might be oscillating or metastable dynamic solutions. Other solutions include varying electron mass (I understand a purist...

Homework Statement What type of hybridization occurs in the orbitals of a carbon atom participating in a triple bond with another carbon atom? The Attempt at a Solution I honestly thought it would be sp3 but it turns out to be sp. Can someone explain this to me? Thanks!