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QUANTUM MECHANICAL MODEL.pptx
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- 2. Lesson Objectives a.understand thedevelopment of atomic models; b.identify the energy levels, sublevels and atomic orbitals in an atom; and c. write the electron configuration of the elements.
- 3. MOST ESSENTIAL LEARNING COMPETENCIES ●Explain how the Quantum Mechanical Model of the atom describes the energies and positions of the electrons.
- 4. ENABLING COMPETENCIES ● Describehow Bohr model of the atom improved Rutherford`s atomic model.
- 5. BOHR’S ATOMIC MODEL -describesthe atom as a solar system, where he considered electrons as the particles moving around the nucleus with the specific circular paths called orbits.
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- 7. De Broglie proposed thatthe electrons (which thought as a particle) could also be taught as a wave. LOUIS VICTOR DE BROGLIE
- 8. Erwin Schrodinger -used theidea of De Broglie to develop a mathematical equation to describe the probable location of an electron around the nucleus.
- 9. Heisenberg discovered that for everysmall particle like the electron, its location cannot be exactly known. This is called the Uncertainty Principle. Werner Heisenberg
- 10. QUANTUM NUMBERS, ORBITALS ANDENERGY LEVELS
- 11. Quantum Number ORBITALS arethree- dimensional description of the most likely location of an atom. -is a value that is used when describing the energy levels available to atoms and molecules.
- 12. ENERGY LEVEL -a fixedamount of energy that a system described by quantum mechanics, such as a molecule, atom, electron, or nucleus, can have.
- 13. THE FOUR QUANTUMNUMBERS (n) l ml ms
- 14. PRINCIPAL QUANTUM NUMBER -describes theenergy level of an electron inside an atom. (n) = 1, 2, 3, 4 and so on.
- 15. PRINCIPAL QUANTUM NUMBER -each principal energylevel is also known as an electron shell. -a collection of atomic orbitals with the same principal quantum number value.
- 16. ANGULAR MOMENTUM QUANTUM NUMBER -this number describes the shape of the sublevel within an energy level. - represented by l
- 17. ORBITALS s (sharp) l =0 p(principal) l =1 d (diffuse) l =2 f (fundamental) l =3
- 18. Relationship between (n) and(l) l < n-1 n=2 l=0,1 n=1 l=0 n=3 l=0,1,2
- 19. MAGNETIC QUANTUM NUMBER -number that describes the orbitalwithin the sublevel. -represented by the symbol (ml). l ml 0 0 1 -1,0,1 2 -2,-1,0,1,2 3 -3,-2,-1,0,1,2,3
- 20. -indicates the direction the electronis spinning. -represented by the symbol ms. ELECTRON SPIN ms= ±½
- 21. ELECTRON CONFIGURATION - is away of distributing the electrons of the atom among the orbitals of the atom.
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- 23. PAULI’S EXCLUSION PRINCIPLE -states that electrons occupying the sameorbitals must have opposite spin.
- 24. AUFBAU PRINCIPLE -the available atomic orbitalswith the lowest energy levels are occupied before those with higher energy levels.
- 25. HUND’S PRINCIPLE OF MULTIPLICITY -when electronsenter a sublevel with more than one orbital, they will spread out to the available orbitals with the same spin before pairing.
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- 29. 1s22s1 s=2 electrons p=6 electrons d=10 electrons f=14 electrons
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