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8.3 Atomic Spectroscopy and the Bohr Model
Many of the elements' properties are dependent on their electrons.
If an electron is transferred from one atom to another, it depends on the relative energies of the two atoms.
In the following paragraphs, we describe the probability distribution maps for energy tron states in which the electron has well-defined energy but not well-defined position.
The spatial distribution of atomic electrons is important to bonding.
An operator transforms the equation for the atom of interest into the equation for the electrons in atoms.
Another mathematical function is the general form of a mathematical function.
Many possible wave functions can be achieved with the solutions to the Schrodinger Equation.
We don't examine the wave functions in detail in the book.
We have graphical representations of the orbitals that correspond to the wave functions.
The quantum numbers all have values that are in the range of integer values.
The orientation of the electron is determined by the model.
We look at each number individually.
Coulomb's law describes its interaction with the nucleus.
The shape of the orbital is determined by the angular momentum quantum number.
These shapes will be considered in Section 8.6.
The orientation of the orbital is determined by the magnetic quantum number.
The orientations will be considered in Section 8.6.
It's something of a metaphor.
The spin is a fundamental property of the electron.
One correct way to say that an electron does not have more spin than another is to say that all electrons have the same amount of inertia.
Section 9.3 begins to consider how electrons occupy orbitals when the spin quantum number becomes important.
We only look at the first three numbers.
There are two sublevels at the 2 level.
There are five orbitals, and so on.
There are nine orbitals at the 3 level.
Each set of quantum numbers is supposed to specify an orbital.
One set is incorrect.
Each set of quantum numbers is supposed to have an orbital.
One quantum number is not allowed in each set.
The quantum number that is not allowed should be replaced with one that is allowed.
The atomic spectrum of atoms is explained by quantum theory.
The electron is excited by the unstable energy level.
The electron relaxes to a lower-energy level, releasing energy in the form of radiation.
It releases a photon of light that is equal to the energy difference between the two levels.
Positive energy of a photon is carried away by the atom.
The wavelength and Frequency of the photon are determined by this energy.
There is a wavelength of .
The green is 486 nm.
Light that is higher in energy and shorter in wavelength is produced by transitions between orbitals that are closer together.
The wavelength of the emitted light was asked.
The wavelength corresponding to a photon of this energy is calculated using Equation 8.3.
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