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Atomic Structure

Atomic Structure. Miha Lee California State University, Northridge. List of Content. Particles in a Atom Nucelus => Neutrons & Protons Electrons Atomic Structure Bohr => energy level of electron shell Shrodinger => orbitals & electron cloud Electron Configuration

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Atomic Structure

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  1. Atomic Structure Miha Lee California State University, Northridge

  2. List of Content • Particles in a Atom • Nucelus => Neutrons & Protons • Electrons • Atomic Structure • Bohr => energy level of electron shell • Shrodinger => orbitals & electron cloud • Electron Configuration • Rule of Elctronic Configuration • Atoms’ Electronic Configuration • Links for Self-study

  3. Electron • J.J. Thomson • Cathode-ray • The atom has a lot of tiny, negatively charged particles named electrons stuck in it.

  4. Nucelus 1 • Rutherford • α particle scattering

  5. Nucelus 2 • The atom has a small, dense, positively charged nucleus and electrons at a distance. • The vast majority of the volume of the atom is empty space.

  6. Particles in Nucleus • Proton • 1.602×10−19 C • 1.673×10−27 kg • Neutron • no net charge • 1.675×10−27 kg

  7. Atomic Structure • Bohr => elenergy level of electron shells • Schrodinger => orbitals&electron cloud

  8. Bohr’s Atomic Model 1 • Cause: Line spectrum of atoms => discrete energy levels in an atom

  9. Bohr’s Atomic Model 2 • Borh’s idea about Line spectrum • Electrons orbit around the nucleus in discret allowed energy levels (electron shells). • Electrons gain and lose energy by jumping from one orbit to another.

  10. Atomic Orbitals 1 • Schrodinger • Electrons’ motion is described as wave-function. • Probaility of finding electrons is caculated from wave function and named orbital.

  11. Atomic Orbitals 2 • Watch wave functions and orbitals • Elctron cloud: probaility of finding electron (orbital) decribed with dots

  12. Atomoic Orbitals 3 • Orbitals: area of 90~95% of probaility to find electrons s orbital p orbials d orbitals

  13. Electronic Configuration 1 • Each orbital can only contain a maximum of 2 electrons. • Elctron shells at a higher energy level have more orbitals. • Order of filling energy levels => 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

  14. Rule of Elctronic Configuration • The Aufbau Principle • The electrons occupy the lowest energy orbitals available. The “Ground State” for an atom is when every electron is in its lowest energy orbital. • The Pauli Exclusion Principle • Each orbital can be occupied by no more than two electrons. • Hund’s Rule • When more than one orbital exists of the same energy (p, d, and f orbitals), place one electron in each orbital

  15. Atoms’ Electronic Configuration

  16. Links for Electronic Configuration • Electronic Structures • Electron Configuration • Atomic electron configurations [end]

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