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14 Αυγ 2024 · A total of four quantum numbers are used to describe completely the movement and trajectories of each electron within an atom. The combination of all quantum numbers of all electrons in an atom is described by a wave function that complies with the Schrödinger equation.
The quantum numbers are parameters that describe the distribution of electrons in the atom, and therefore its fundamental nature. They are: 1. PRINCIPAL QUANTUM NUMBER (n) - Represents the main energy level, or shell, occupied by an electron. It is always a positive integer, that is n = 1, 2, 3 ... 2.
The principal quantum number defines the general value of the electronic energy. The angular momentum quantum number determines the shape of the orbital. And the magnetic quantum number specifies orientation of the orbital in space, as can be seen in Figure \(\PageIndex{3}\).
Carbon has six valence electrons. We’ll start filling up the quantum numbers by following the rules above. Starting with n = 1, the only possible value of l is l = 0, since 0 ≤ l ≤ n − 1. When l = 0, m must also be 0. There are two possible spins that could go with these quantum numbers.
Describe the structure of shells and subshells in multi-electron atoms, and relate them to the observed emission spectra. Explain the Bohr-Sommerfeld model. For an electron in a given subshell, determine the quantum numbers, and explain your answer.
Upon combustion, however, oxygen is able to form two strong bonds in the combustion products CO2 and H2O. If a fossil fuel undergoes combustion (combination with oxygen) the carbon and hydrogen atoms form strong bonds already in the starting materials, just the same as in the products.
Having introduced the basics of atomic structure and quantum mechanics, we can use our understanding of quantum numbers to determine how atomic orbitals relate to one another. This allows us to determine which orbitals are occupied by electrons in each atom.
