I am going to discuss the modern concept of the atom. I am going to give a brief history of the atomic model including Thomson’s atom‚ Rutherford’s atom‚ Bohr’s atom‚ and Schrödinger’s atom. I am going to include a diagram for each of these models. In 1897 physicist‚ J.J. Thomson‚ shortly after discovering electrons‚ proposed his Plum-Pudding model of the atom. He based this model on the two facts that he knew at the time: 1. atoms contain small negatively charged particles called electrons
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Chemistry A Bonding Worksheet #1: Introduction to Ionic Bonds The forces that hold matter together are called chemical bonds. There are four major types of bonds. We need to learn in detail about these bonds and how they influence the properties of matter. The four major types of bonds are: I. Ionic Bonds III. Metallic Bonds II. Covalent Bonds IV. Intermolecular (van der Waals) forces Ionic Bonds The ionic bond is formed by the attraction between oppositely charged ions.
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TUTORIAL 1: STK1503 BENZENE AND AROMATIC 1. Draw structures corresponding to the names given. a. m-fluoronitrobenzene b. p o-chlorophenol c. o-chlorophenol d. 3‚5-dimethylbenzoic acid e. 1-phenyl-3-methylpentane 2. Provide correct IUPAC names for each of the following compounds. a. NO2 CH3 b. c. CH3 d. NH2 H2N CH3 e. Ph C H3 C C CH2CH2CH3 Ph 3. For each molecule below‚ predict whether the molecule would be expected to show aromatic character or not. Explain your answer
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(mass=145g) with change in velocity of 0.11 m/s. 4. Fill in the following. | Number of orbitals | Number of electrons that can be held | n=3 | | | 4p subshell | | | 3px | | | 2f subshell | | | 5. Give the full electron configuration of the followings. For (a)‚ indicate the inner and valence electrons. (a) 14Si (b) 25Mn3+ 6. Give the condensed electron configuration and orbital diagram for 22Ti. Then determine whether the atom is paramagnetic or diamagnetic. 7. Determine
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CHEMISTRY 1. States of Matter: Solid‚ liquid and gaseous states(general characteristics)‚ Change of states‚ effect of change of temperature and pressure on states of matter‚ evaporation‚ mixture‚ solution‚ its type and its concentration(percent strength by volume and by mass)‚ separation of components from a mixture using various physical methods‚ physical and chemical changes‚ compounds 1. NCERT class IX text book (chapter 1 and 2) 2. Foundation Science(Chemistry) :Class IX A. K. Singh ( Bharati
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6. The masses and diameters of each star in the binary can be determined from eclipsing binaries. 7. If we divide the mass of a star by its volume we calculate the star’s average density. 8. Most stars on the H-R diagram are on the lower right. 9. The largest of the red stars are the super giant stars. Essay 10. Why would parallaxes be easier to observe if Earth were farther from the sun? If Earth had a further orbit it would have
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Name: __________________________________ ( ) Class: 4Q HWA CHONG INSTITUTION PRELIMINARY EXAMINATION 2010 CHEMISTRY 5072 Paper 1 Time: 1 hour INSTRUCTIONS TO CANDIDATES Do not turn the pages over until you are told to do so. Write your name and index number on the answer sheet in the spaces provided. There are forty questions on this paper. Attempt all questions. For each question‚ there are four possible answers labelled A‚ B‚ C and D. Choose the one you consider correct and
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from a metal is 5 X 1014 s-1. Will the photon of radiation having energy 3.0 X 10-19 J give photo electric effect or not? 11. A metal ‘X’ is present in chlorophyll. Identify the metal ‘X’. write the reaction of this metal with N2. 12. An orbital has n=3. What are the possible values of l and m l ? 13. Explain the hybridization of PCl5 molecule. Why PCl5 on decomposition gives PCl3 and Cl2 ? 14. Consider the chemical reaction: 2SO2 (g) + O2 (g) 2SO3 (g) +189.4 KJ. Indicate the
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s-character‚ 66% p-character sp i.e. CO2 2 regions of e- linear 180° 50% s-character‚ 50% p-character Orbitals Einstein: photoelectric effect → photons de Broglie → wave-particle duality Schrodinger → wave functions ?→ orbitals Atomic orbitals Simple Molecular Orbital Theory # MO’s = #AO’s MO’s arranged by relative E Filling follows (1: Aufbau‚ 2: Pauli) Bond Order (e- in bonding orbital - e- in antibonding) / 2 Valence Bond Theory places e- pairs between atoms problems incorrect bond
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Shapes of molecules with multiple bonds Molecular crystals of buckminsterfullerene (C60) 23.1 – 23.7 Summary 1 Examples of covalent molecules with non-octet structures are as follows: Molecule Electron diagram F BF3 B F F SF4 F Molecule Electron diagram F S F F Cl PCl5 Cl Cl P Cl Cl SF6 F F F S F F F 2 The following table summarizes the relationship between the arrangement of electron pairs around the central atom of a molecule or polyatomic ion and the shape
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