VSEPR Theory (Valence Shared Electron Pair Repulsion Theory) Syllabus: Various rules under VSEPR theory to explain molecular geometry (following examples may be taken to explain various rules- BeCl2‚ BF3‚ CH4 ‚ NH4+ ‚ PCl5 ‚ SF6‚ IF7‚ SnCl2 ‚ NH3‚ H2O‚ SF4‚ ClF3‚ ICl2‚ ICl4‚ BrF5‚ XeF6‚ SOF4‚ COF2‚ PCl3‚ PBr3‚ PI3‚ F2O‚ H2S). Limitations of VSEPR theory. How to draw VSEPR geometry? To predict the shape of a covalent molecule‚ follow these steps: Step 1: Draw the Lewis structure of molecule
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A TECHNICAL PRESENTATION ON TRANSPARENT ELECTRONICS Presented by Y.RAJESH A.LALITHA 3rd ECE 3rd ECE 09MG1A0451 09MG1A0401 Rajeshyandrathi451@gmail.com lalliatluri@gmail.com Ph no: 9494248468
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Name:____________________________ CHM 1045: Exam 4 – Chapters 9 & 10 Chapter 9: Chemical Bonding I – Lewis Theory 1. Which of the following statements is TRUE? a) A covalent bond is formed through the transfer of electrons from one atom to another. b) A pair of electrons involved in a covalent bond are sometimes referred to as "lone pairs." c) It is not possible for two atoms to share more than two electrons. e) A covalent bond has a lower potential energy than the two separate atoms. d) Single
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2670 g/cm3 Electronic Configuration: Diamond The carbon atom’s electronic configuration is believed to change from its ground state in diamond as follow: {draw:frame} Quantum-mechanical calculations indicate that greater overlap between orbitals results in a stronger covalent bond. The diamond structure represents a three-dimensional
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Chemistry: A Molecular Approach (Tro) Chapter 10 Chemical Bonding II: Molecular Shapes‚ Valance Bond Theory‚ and Molecular Orbital Theory 1) Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. A) eg=trigonal planar‚ mg=trigonal planar B) eg=tetrahedral‚ mg=trigonal planar C) eg=tetrahedral‚ mg=trigonal pyramidal D) eg=trigonal planar‚ mg=bent E) eg=trigonal bipyramidal‚ mg= trigonal bipyramidal Answer: A 2) Determine
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1. The diagram below shows the electronic structure of boron. (a) The electrons are represented by arrows. What property of the electrons do these ‘up’ and ‘down’ arrows represent? ..................................................................................................................................... (1) (b) Suggest why electrons which occupy the 2p sub-levels have a higher energy than electrons in the 2s sub-level. .....................................................
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html http://dwb4.unl.edu/chemAnime/atomic_orbits.htm http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/hybrv18.swf Salient Features Chemistry animation and videos Atomic orbital animations Hybridization animation http://jchemed.chem.wisc.edu/JCEDLib/WebWare/collection/open/JCEWWOR019/mo Molecular orbital theory animations movies.html http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/activa2.swf http://dwb4.unl.edu/chemAnime/Electro.htm Activation energy animation Electrochemistry
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HF – hydrogen fluoride is a covalent bond and shares one pair of electrons. The hydrogen end of the molecule is slightly positive and the fluorine end is slightly negative. This causes hydrogen bonding between other hydrogen fluoride molecules. KCl – potassium chloride is a metal halide salt. The bonding between potassium and chloride is an ionic bond. The potassium becomes a cation and the chloride an anion. The potassium end of the molecule becomes slightly positive and the other end slightly
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Unit 1 Key Questions Lesson 1 1. One argument against continuing research on the atom is that the cost continues to increase at an alarming rate‚ and the benefits seem to be declining. Whereas quantum chemistry experiments as early as 80 years ago were very cheap and yielded considerable practical results‚ now very few if any practical results are emerging‚ but the costs of experiments continues to increase. On the other hand
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and electrophilicity index values are comparable with the potential bioactive molecules [14‚ 16]. DOS spectrum was also simulated by convoluting the molecular orbitals with Gaussian curves of unit height. These results further validated the FMOs analysis. The green and red lines in the DOS spectrum represent the occupied and virtual orbitals‚ respectively. The simulated DOS spectrum is shown in Fig. 7b. 3.6 Local reactivity descriptors analysis The electron density based local reactivity descriptors
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