1. Wavelike properties of electrons help relate atomic emission spectra, energy states of atoms, and atomic orbitals. Three rules are used to determine electron arrangement in an atom. Section 2: Quantum Theory and the Atom K What I Know W What I Want to Find Out L What I Learned

2. Essential Questions How do the Bohr and quantum mechanical models of the atom compare? What is the impact of de Broglie’s wave-particle duality and the Heisenberg uncertainty principle on the current view of electrons in atoms? How do electron-dot structures represent an atom’s valence electrons? Quantum Theory and the Atom Copyright © McGraw-Hill Education

3. Review Atom electron New principal quantum number principal energy level energy sublevel electron configuration aufbau principle Pauli exclusion principle Hund’s rule valence electron electron-dot structure Quantum Theory and the Atom Copyright © McGraw-Hill Education Vocabulary New ground state quantum number de Broglie equation Heisenberg uncertainty principle quantum mechanical model of the atom atomic orbital

4. Science Rock https://media.stemscopes.com/Secondary_Science_Rock/C.6DE_ SciRock.mp4 Use your lyrics sheet for this! Quantum Theory and the Atom Copyright © McGraw-Hill Education

5. 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 atom is called its ground state. When an atom gains energy, it is in an excited state. Quantum Theory and the Atom Copyright © McGraw-Hill Education

6. Bohr’s Model of the Atom Bohr suggested that an electron moves around the nucleus only in certain allowed circular orbits. Quantum Theory and the Atom Copyright © McGraw-Hill Education

7. Bohr’s Model of the Atom Each orbit was given a number, called the quantum number. Hydrogen’s single electron is in the n = 1 orbit in the ground state. When energy is added, the electron moves to the n = 2 orbit. Quantum Theory and the Atom Copyright © McGraw-Hill Education

8. The Limits of Bohr’s Model Bohr’s model explained the hydrogen’s spectral lines, but failed to explain any other element’s lines. The behavior of electrons is still not fully understood, but substantial evidence indicates they do not move around the nucleus in circular orbits. Quantum Theory and the Atom Copyright © McGraw-Hill Education

9. The Quantum Mechanical Model of the Atom Louis de Broglie (1892–1987) hypothesized that particles, including electrons, could also have wavelike behaviors. The figure illustrates that electrons orbit the nucleus only in whole-number wavelengths. Quantum Theory and the Atom Copyright © McGraw-Hill Education

10. Hydrogen Atomic Orbitals Principal quantum number (n) indicates the relative size and energy of atomic orbitals. n specifies the atom’s major energy levels, called the principal energy levels. Energy sublevels are contained within the principal energy levels. Quantum Theory and the Atom Copyright © McGraw-Hill Education

11. Hydrogen Atomic Orbitals Each energy sublevel relates to orbitals of different shape. Quantum Theory and the Atom Copyright © McGraw-Hill Education

12. Hydrogen Atomic Orbitals Quantum Theory and the Atom Copyright © McGraw-Hill Education

13. Ground-State Electron Configuration The arrangement of electrons in the atom is called the electron configuration. The aufbau principle states that each electron occupies the lowest energy orbital available. Electron Configuration Copyright © McGraw-Hill Education

14. Ground-State Electron Configuration Electron Configuration Copyright © McGraw-Hill Education

15. Blocks on the Periodic Table

16. Ground-State Electron Configuration The Pauli exclusion principle states that a maximum of two electrons can occupy a single orbital, but only if the electrons have opposite spins. Hund’s rule states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same energy level orbitals. Electron Configuration Copyright © McGraw-Hill Education

17. Ground-State Electron Configuration The aufbau diagram can be used to write correct ground-state electron configurations for all elements up to and including Vanadium, atomic number 23. The electron configurations for certain transition metals, like chromium and copper, do not follow the aufbau diagram due to increased stability of half-filled and filled sets of s and d orbitals. Electron Configuration Copyright © McGraw-Hill Education

18. Valence Electrons Valence electrons are defined as electrons in the atom’s outermost orbitals—those associated with the atom’s highest principal energy level. Electron-dot structure consists of the element’s symbol representing the nucleus, surrounded by dots representing the element’s valence electrons. Electron Configuration Copyright © McGraw-Hill Education