Atomic Orbital Size (7.3.1) Flashcards
• The wave-function solutions to Schrödinger’s equation reveal the allowed energies and location probabilities of the
electron.
• The wave-function solutions to Schrödinger’s equation reveal the allowed energies and location probabilities of the
electron.
• The 1s solution to Schrödinger’s equation indicates that the highest probability of finding the electron is 0.53 angstroms
(Å) from the nucleus.
• The 1s solution to Schrödinger’s equation indicates that the highest probability of finding the electron is 0.53 angstroms
(Å) from the nucleus.
The wave-function solutions to Schrödinger’s equation reveal
the allowed energies and location probabilities of the electron.
We cannot know the location of an electron as a consequence
of Heisenberg’s uncertainty principle. We can know
something about its energy and probability states.
The 1s solution to Schrödinger’s equation indicates that the
highest probability of finding the electron is 0.53 angstroms
(Å) from the nucleus.
At higher energy levels the most likely location for the
electron is farther from the nucleus. The 2s energy sublevel
has its highest probability outside the 1s maximum. It also
has a single node, or region with a zero probability of finding
the electron.
In the 3s energy sublevel, the highest probability of finding
the electron is beyond the 2s maximum and there are 2 nodes.
Higher s energy sublevels produce an electron probability density or “electron cloud” of a greater diameter.
The wave-function solutions to Schrödinger’s equation reveal
the allowed energies and location probabilities of the electron.
We cannot know the location of an electron as a consequence
of Heisenberg’s uncertainty principle. We can know
something about its energy and probability states.
The 1s solution to Schrödinger’s equation indicates that the
highest probability of finding the electron is 0.53 angstroms
(Å) from the nucleus.
At higher energy levels the most likely location for the
electron is farther from the nucleus. The 2s energy sublevel
has its highest probability outside the 1s maximum. It also
has a single node, or region with a zero probability of finding
the electron.
In the 3s energy sublevel, the highest probability of finding
the electron is beyond the 2s maximum and there are 2 nodes.
Higher s energy sublevels produce an electron probability
density or “electron cloud” of a greater diameter.
To which of the following is the Bohr model of an atom similar?
a planet in orbit around a sun (D)
The Bohr model used the idea of an electron in an orbit around the nucleus, much like a planet orbiting a sun, as the basis, then added restrictions to this model so that it would match observations.
The 1s, 2s, and 3s orbital solutions to Schrödinger’s equation for the hydrogen atom use only which portion of the equation?
radial (D)
The s orbitals are spherically symmetric, so the radial solutions are complete solutions for the s orbitals. This is not true for higher orbital quantum numbers.
Which of these graphs shows the distance from the hydrogen nucleus where the electron with lowest energy is most likely to be found?
(B)
The probability of finding the electron along any radius decreases with distance, but the number of regions where the electron could be increases with distance, so the maximum probability occurs at about 0.5 Å.
The Heisenberg uncertainty principle states that it is impossible to simultaneously know which two things about of an electron?
position, momentum (C)
Any attempt to measure the position of an electron disturbs its path, so its momentum cannot be measured precisely at the same time.
What information does Schrödinger’s equation combine?
kinetic energy, potential energy, and wave properties (D)
Schrödinger’s equation combines information about kinetic energy, potential energy, and wave properties, into a single equation involving the wave function of an electron.
What are the “dips” in the graphs of radial probability distribution for the 2s and 3s states called?
radial nodes (A)
They represent spherical regions where the electron is not likely to be found, similar to the nodes in a standing wave.
Which of the following explains why the Bohr model of the atom ultimately did not work?
It required knowing the position and momentum of an electron. (B)
The Bohr model pictures the electron as having a definite position and speed. The Heisenberg uncertainty principle asserts that we cannot know the position and speed of an electron.
The quantum mechanical model of the atom gives up trying to specify the location of the electron and instead shows us what?
The probability of finding the electron (C)
The quantum mechanical model enables us to calculate the probability of finding the electron in a region of space.
The Bohr model of a hydrogen atom predicts that the electron of lowest energy orbits at a distance of 0.5 Å from the nucleus. What does the quantum mechanical model predict is the most likely distance to find a 1s electron?
The same distance, 0.5Å. (B)
The quantum mechanical model predicts the maximum probability to be around 0.5Å, which is considered to be a success of the model.
In addition to information about kinetic energy and potential energy of an electron what additional information does the Schrödinger’s equation provide about an electron?
wave properties (B)
Explanation:
The wave properties of an electron are contained in Schrödinger’s “wave function” which is part of the wave equation.
