* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Download Ch. 5 PPT Part 3
Bell's theorem wikipedia , lookup
Coupled cluster wikipedia , lookup
Quantum key distribution wikipedia , lookup
Relativistic quantum mechanics wikipedia , lookup
Hartree–Fock method wikipedia , lookup
Hidden variable theory wikipedia , lookup
Canonical quantization wikipedia , lookup
Quantum group wikipedia , lookup
Particle in a box wikipedia , lookup
History of quantum field theory wikipedia , lookup
X-ray fluorescence wikipedia , lookup
Wave–particle duality wikipedia , lookup
Ferromagnetism wikipedia , lookup
EPR paradox wikipedia , lookup
Quantum state wikipedia , lookup
X-ray photoelectron spectroscopy wikipedia , lookup
Symmetry in quantum mechanics wikipedia , lookup
Auger electron spectroscopy wikipedia , lookup
Quantum electrodynamics wikipedia , lookup
Theoretical and experimental justification for the Schrödinger equation wikipedia , lookup
Chemical bond wikipedia , lookup
Atomic theory wikipedia , lookup
Electron scattering wikipedia , lookup
Tight binding wikipedia , lookup
Hydrogen atom wikipedia , lookup
Molecular orbital wikipedia , lookup
Section 5.3 Quantum numbers and Atomic Orbitals • Quantum numbers are numbers that specify the properties of atomic orbitals and of the electrons in that orbital • It’s the electrons “address” Four Quantum Numbers • • • • Principal quantum number Orbital quantum number Magnetic quantum number Spin quantum number Principal quantum number • Symbol, n • Indicates the main energy levels • To this point, only 1-7 • Where do we see 7 main energy levels in this room? Orbital quantum number • Shape of an orbital • Four shapes • s, p, d, and f • Within each main energy level there are different shapes of orbitals Shapes of orbitals • s orbital p orbitals Shapes of d orbitals Examples of f-shaped orbitals Magnetic quantum number • Indicates the orientation (or position) of an orbital around the nucleus – s orbital has 1 orientation – p orbitals have 3 orientations – d orbitals have 5 orientations – f orbitals have 7 orientations • Each orbital can contain only 0, 1, or 2 electrons. Spin quantum number • Indicates the spin of the electron – +1/2 – -1/2 – So if there are two electrons in one orbital, they spin in opposite directions • *** no two electrons can have the same 4 quantum numbers*** Electron configurations (electron arrangements) • Pauli Exclusion Principle – No two electrons in the same atom will have the same set of 4 quantum numbers How to “read” orbitals • How we determine which orbital gets filled with electrons first? • Must follow the ________________: – Orbital of Lowest energy gets filled before going to the next lowest energy orbital – In other words we fill from lowest energy to highest energy – “building up” principle: electrons occupy the lowest-energy orbital that is available. – For example, Hydrogen’s electron goes into the __ orbital, because it is the lowest energy orbital Electron configurations (electron arrangements) • How do we know which orbitals are higher or lower in energy? – Read Periodic Table from Left to Right, Top to Bottom Periodic Table Sections 3 types of notation • Orbital Notation • Electron-Configuration Notation • Electron Dot Notation Orbital Notation • Unoccupied orbital • Orbital with1 e• Orbital with 2 e- __ ↑ or ↓ ↓↑ • Example: Hydrogen Example: Lithium • Example: Helium Example: Oxygen Electron configurations (electron arrangements) • Hund’s rule – Orbitals of equal energy are each occupied by 1 electron before a 2nd electron is added. – All electrons in singly occupied orbitals must have the same spin – For example, there are 3 p orbitals. If you have 3 electrons, there will be one in each orbital and all will have spin quantum number of +1/2 or -1/2 – Example N: Electron-Configuration notation • Similar to orbital notation, but uses superscripts instead of lines • Example: Hydrogen • Example: Helium • Example: Lithium Electron-Dot Notation • Uses only the Valence electrons • Valence electrons = the electrons in the highest (outermost) main energy level • H • He • K Practice Problems (orbital and dot notation) Carbon Sodium Sulfur Shorthand Notation • Use the last noble gas before your element as a “building block” • Example: Phosphorous Practice Problems (d and f orbitals) Fe Au Trick to Electron Dot Notation • Use the group number that the element is in • Hydrogen is in group 1, 1 valence electron • Oxygen is in group 6, 6 valence electrons • These 8 groups are sometimes called the 8 “main groups”