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Hybridization science exhibition ppt.pptx
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- 2. What do youmean by hybridization? This concept was introduced by Pauling. Orbital hybridization (or hybridization) is the concept of mixing atomic orbitals into new hybrid orbitals (with different energies, shapes, etc., than the component atomic orbitals) suitable for the pairing of electrons to form chemical bonds in valence bond theory.
- 3. Project Overview • Thisproject focuses on showing the hybridization of different atomic orbitals sp,sp2 ,sp3 ,sp3 d and sp3 d2 using balloons. The main purpose of this project is to explain people from science and non- science background that HOW HYBRIDISATION OF ATOMIC ORBITALS TAKES PLACE? • The other purpose of this project is to promote the use of toys in teaching and learning process. This would also contribute in creating interest of students in learning different concepts with the help of toys.
- 4. Types Of Hybridization sp-Hybridization •In sp hybridization , one s and p- orbitals mix and form two equivalent sp hybrid orbitals. • Each sp hybrid orbital has 50% s-character and 50% p- character. • These two sp hybrid orbitals lie along linear arrangement and therefore, it is called linear hybridization. sp2 -Hybridization • In sp2 hybridization , one s and two p-orbitals hybridize to form to form three equivalent sp2 hybrid orbitals. • Each sp2 hybrid orbital has one- third(33.3%) s-character and two-third (66.7%) p-character. These three sp2 orbitals remain in the same plane making an angle 120° with one another. • This arrangement is also called trigonal planar arrangement therefore the molecules having sp2 hybridization of the central atom will adopt trigonal planar geometry. Sp3 -Hybridization • In sp3 hybridization, one s and three p- orbitals hybridize to form four sp3 hybrid orbitals. • The four hybrid orbitals will be directed towards the four corners of a regular tetrahedral and make an angle of 109.5°. • Each sp3 hybrid orbital has one- fourth(25%) s- character and three- fourth(75%) p- character. The shape formed with the central atom is tetrahedral.
- 5. • This hybridizationinvolves the mixing of one s, three p, one d- orbitals. These five orbitals hybridize to form five sp3 d- hybrid orbitals. • These hybrid orbitals point towards the corners of a trigonal bipyramidal geometry. In this case, the three orbitals forming a plane are directed towards the corner of an equilateral triangle while the other two are perpendicular to the plane of a triangle lying above and below it. • In this case, one s, three p, two d- orbitals get hybridized to form six sp3 d2 hybrid orbitals which adopt octahedral arrangement. • The angle formed is of 90°. sp3 d-Hybridization sp3 d2 -Hybridization
- 6. • sp- Hybridization •BeCl2 Cl Be Cl 180° LINEAR GEOMETRY Be (Ground state) Be (Excited state) BeCl2 (Hybridized)
- 7. • sp2 - Hybridization •BCl3 B Cl Cl Cl 120° 120° TRIGONAL PLANAR Boron (Ground state) Boron(Excited state) BCl3(Hybridiz ed)
- 8. • sp3 - Hybridization •NH3 N H H H Lone Pair NOTE: The bond angle among the three H- atoms is 109.5° but due to the presence of lone pair the molecule gets a little distorted and the angle decreases to 107° . 107° 107° TETRAHEDRAL GEOMETRY (1s2 2s2 2px 1 2py 1 2pz 1 ) The ground state electronic configuration of nitrogen atom is (1s2 2s2 2px 1 2py 1 2pz 1 ). It contains three unpaired electrons in its ground state. Since nitrogen forms only three covalent bonds, there is no need of promotion.
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- 10. • PCl5 (Hybridization) TRIGONALBIPYRAMIDAL GEOMETRY P(Ground state) P(Excited state) PCl5 (Hybridized)
- 11. • sp3 d2 - Hybridization •SF6 S F F F F F F 90° 90° 90° OCTAHEDERAL GEOMETRY S(Ground state) S(Excited state) SF6(Hybridiz ation)
Editor's Notes
- #2 This is the question that your experiment answers