Exploring Quantum Theory and the Atom: Electrons in Atoms and the Periodic Table
Delve into the fascinating world of quantum theory and the atom in Chapter 9, where we compare Bohr's model with the quantum mechanical model. Understand de Broglie's wave-particle duality and Heisenberg's uncertainty principle's impact on our current electron view. Discover the relationships among energy levels, sublevels, and atomic orbitals in a hydrogen atom.
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SECTION 2: QUANTUM THEORY AND THE ATOM CHAPTER 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE
Learning Goals Compare the Bohr and quantum mechanical models of the atom. Explain the impact of de Broglie s wave particle duality and the Heisenberg uncertainty principle on the current view of electrons in atoms. Identify the relationships among a hydrogen atom s energy levels, sublevels, and atomic orbitals.
Bohrs Model of the Atom Einstein s theory of light s dual nature accounted for several unexplainable phenomena, but it did not explain why atomic emission spectra of elements were discontinuous.
Bohrs Model of the Atom In 1913, Niels Bohr, a Danish physicist working in Rutherford s laboratory, proposed a quantum model for the hydrogen atom that seemed to answer this question. This model correctly predicted the frequency lines in hydrogen s atomic emission spectrum.
Bohrs Model of the Atom The lowest allowable energy state of an atom is called its ground state. When an atom gains energy, it is in an excited state.
Bohrs Model of the Atom Bohr suggested that an electron moves around the nucleus only in certain allowed circular orbits.
Bohrs Model of the Atom Each orbit was given a number, called the quantum number. Bohr orbits are like steps of a ladder, each at a specific distance from the nucleus and each at a specific energy.
Bohrs Model of the Atom Hydrogen s single electron is in the n = 1 orbit when it is in the ground state. When energy is added, the electron moves to the n = 2 orbit.
Bohrs Model of the Atom The electron releases energy as it falls back towards the ground state.
Bohrs Model of the Atom Bohr s model explained the hydrogen s spectral lines, but failed to explain any other element s lines. For this and other reasons, the Bohr model was replaced with a more sophisticated model called the quantum-mechanical or wave- mechanical model.
Quantum Mechanical Model Louis de Broglie (1892 1987) hypothesized that particles, including electrons, could also have wavelike behaviors. Electrons do not behave like particles flying through space. We cannot, in general, describe their exact paths.
Quantum Mechanical Model Heisenberg showed it is impossible to take any measurement of an object without disturbing it. The Heisenberg uncertainty principle states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time.
Quantum Mechanical Model The only quantity that can be known is the probability for an electron to occupy a certain region around the nucleus.
Quantum Mechanical Model Schr dinger treated electrons as waves in a model called the quantum mechanical model of the atom. Schr dinger s equation applied equally well to elements other than hydrogen (unlike Bohr s model).
Quantum Mechanical Model The quantum mechanical model makes no attempt to predict the path of an electron around the nucleus. Bohr orbits were replaced with quantum-mechanical orbitals.
Quantum Mechanical Model Orbitals are different from orbits in that they represent probability maps that show a statistical distribution of where the electron is likely to be found.
Quantum Mechanical Model In the quantum-mechanical model, a number and a letter specify an orbital. The lowest-energy orbital is called the 1s orbital. It is specified by the number 1 and the letter s.
Hydrogens Atomic Orbitals The number is called the Principal quantum number (n) and it indicates the relative size and energy of atomic orbitals. n specifies the atom s major energy levels, called the principal energy levels.
Hydrogens Atomic Orbitals Energy sublevels are contained within the principal energy levels.
Hydrogens Atomic Orbitals Each energy sublevel relates to orbitals of different shape. s, p, d, f s, p, d s, p s
Hydrogens Atomic Orbitals s sublevel:
Hydrogens Atomic Orbitals p sublevel:
Hydrogens Atomic Orbitals d sublevel:
Hydrogens Atomic Orbitals f sublevel:
Hydrogens Atomic Orbitals Orbitals are sometimes represented by dots, where the dot density is proportional to the probability of finding the electron. The dot density for the 1s orbital is greatest near the nucleus and decreases farther away from the nucleus. The electron is more likely to be found close to the nucleus than far away from it.
Hydrogens Atomic Orbitals At any given time, hydrogen s electron can occupy just one orbital. When hydrogen is in the ground state, the electron occupies the 1s orbital. When the atom gains a quantum of energy, the electron is excited to one of the unoccupied orbitals.
