1. Unit 4: Electrons in the Atom
Part 2: Quantum Theory and the Atom

2. Bohr’s Model of the Atom
Bohr correctly predicted the frequency lines in hydrogen’s atomic emission spectrum.
The lowest allowable energy state of an electron is called its ground state.
When an atom gains energy, it is in an excited state.
Bohr suggested that an electron moves around the nucleus only in certain allowed circular orbits.

3. Bohr’s Model of the Atom
Each orbit was given a number, called the quantum number.

4. Bohr’s Model of the Atom
Hydrogen’s single electron is in the n=1 orbit in the ground state.
When energy is added, the electron moves into the n=2 orbit.

6. Bohr’s Model of the Atom
Bohr’s model explained the hydrogen’s spectral lines, but failed to explain other element’s lines.
The behavior of electrons is still not fully understood, but it is known that they do not move around the nucleus in circular orbits.

7. The Quantum Mechanical Model of the Atom
Louis de Broglie ( ) hypothesized that particles, including electrons, could also have wavelike behaviors.
The figure below illustrates that electrons orbit the nucleus in only whole-number wavelengths.

8. The Quantum Mechanical Model of the Atom
The de Broglie equation predicts that moving particles have wave characteristics.

9. The Quantum Mechanical Model of the Atom
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.
The only quantity that can be known is the probability for an electron to occupy a certain region around the nucleus.

10. The Quantum Mechanical Model of the Atom

11. The Quantum Mechanical Model of the Atom
Schrödinger treated electrons as waves in a model called the quantum mechanical model.
Schrödinger’s equation applied equally well to elements other than hydrogen.
The wave function predicts a three-dimensional region about the nucleus called the atomic orbital.

12. Hydrogen Atomic Orbitals
Principal quantum number (n) indicates the relative size and energy of atomic orbitals.
‘n’ specifies the atom’s major energy level, called the principal energy levels.
Energy sublevels are contained within the principal energy levels.

13. Hydrogen Atomic Orbitals
Each energy sublevel relates to orbitals of different shape.

14. Hydrogen Atomic Orbitals