21) - 21) Which one of the following sets of quantum numbers can correctly represent a 3p orbital? A) = 1 / 3 m/=3 B) = 3 = 1 m/ -1 C) =3 /=0 / 1 D) 2-3 = 1 m 2 E) =3 / 2 = 1 22) 22) The Bohr theory of the hydrogen atom predicts the energy difference (in J) between the = 3 and the state to be A) 1.55 x 10-19 J. E) the angular momentum quantum number only. D) the principal, angular momentum and magnetic quantum numbers. B) the principal and angular momentum quantum numbers (&/). E) describe regions of space in which one is most likely to find an electron 20) 20) The energy of an electron in the hydrogen atom is determined by A) the principal and magnetic quantum numbers (n&w). D) give a description of the atomic structure which is essentially the same as the Bohr model. B) describe exact paths for electron motion C) are in conflict with the Heisenberg Uncertainty Principle. These give rise to the rather unusual behavior of benzene.19) Atomic orbitals developed using quantum mechanics A) allow scientists to calculate an exact volume for the hydrogen atom. We know that benzene is pretty flat, which is the result of orbitals on either side of the ring. Having an electron pair with opposite spins is energetically beneficial, which explains how the formation of such a pair in a common orbital forms a stable bond between atoms.Įven fancier orbitals exist, in particular in benzene and similar cyclic molecules. If both atoms have orbitals with only a single unpaired electron, the common/merged orbital can hold a pair. Where two atoms approach, they may develop a common orbital. In essence, an orbital specifies where an electron pair can be (one spin up, one spin down). Basic organic chemistry depends on s- and p-orbitals overlapping to form bonds. The importance of these orbitals is critical to chemists. If you aggregate enough measurements, the uncertainties cancel out. The probability in this case is a probability for a single measurement, which is entirely uncorrelated with the same type of measurement on another atom a micrometer away. Since we must not be able to do that with enough certainty how then can we check the validity of the existence of orbitals?" It's hard to pinpoint the exact cause of your confusion.įor instance, you state that "atomic orbitals are at best a high probability region of finding certain electrons. Maybe an example will help, there is no boundation for an electron of certain energy to move in an orbital that is dumbled or double dumbled shaped! I agree with electrons having certain energies described by quantum numbers, but how can one definitively prove that an electron belonging to say 2p_x resides in a dumbled shaped orbital?Īgain, are orbitals true? Are they actually significant and not just a helpful mathematical construct? Can it be definitively proven? Google provides various links explaining the theory and listing its uses in modern chemistry but I could not find anything which properly explains the significance or even tries to explain the actual presence of something like an atomic orbital other than saying that we find so and so probability regions while working with Schrödinger equations.Īdded after answers and comments: The answers are listing the uses of the contruct only, I tried to say that I am interested in finding out whether something like an orbital is actually there or not. Overall, I am interested in learning the significance of atomic orbitals. Is it possible, that the idea of atomic orbital is now outdated in terms of modern development and only used for simplistic explanations of complex electron motions and phenomenons? Since we must not be able to do that with enough certainty how then can we check the validity of the existence of orbitals? I am not very well read in the various techniques and theories that we have developed over time, but still I think that atomic orbitals are at best a high probability region of finding certain electrons. Since, there is high degree of uncertainty when we talk about the position of merely the detection of an electron as well as the energy that we "observe" and which may pretty much not be the actual energy of the observed electron, what then is the significance of any atomic orbital? We have been taught that the atomic orbitals we read about are probability density region of finding electrons of particular energies which are designated by the various quantum numbers.
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