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    History of the Atom

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    Jo Adrian P. del Mundo CN 08 3S (A) August 1‚ 2013 Atomic Models The Electron Cloud Model - an atom is comprised of a nucleus made up of neutrons and protons‚ and electrons moving extremely fast around the nucleus‚ forming an electron cloud instead of moving in orbits like what Bohr’s model suggests - proposed by Erwin Schrodinger in 1926‚ when he derived this model using a mathematical equation that he himself made http://1.bp.blogspot.com

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    * Proposed that an atom was a positively charged empty sphere containing negatively charged electrons raisin scone analogy What Thompson left us with? * Atoms consist of negative electrons embedded within a positively charged sphere * Analogy of raisin bun often used Milikin’s Famous Oil Drop Experiment * Determined size and charge on electron * Discovered charge on single electron was 1.6 x 10^19 C How it worked? * Knew mass of single drop of oil‚ calculated gravity on

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    trends in periodic table

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    outermost electrons are assigned to orbitals with increasingly higher values of the principal quantum number. The underlying electrons require space so the electrons of the outer shell is farther from the nucleus. • In a period‚ going across the period‚ a proton is added to each nucleus and an electron is added to each outer shell. In each‚ the effective nuclear charge increases slightly because the effect of each additional proton is more important than the effect of an additional electron. The result

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    these modifications came in 1897 when J.J. Thomson discovered the electron. Based on the work of William Crookes and his "Crookes tube" (Cathode-ray tube)‚ Thomson discovered a negative charged particle was the cause of the light produced by the cathode-ray tube. He also discovered that these particles are present in all elements. These cathode-ray particles are now known as electrons. Soon after the discovery of electrons the proton was discovered. This led Thomson to conclude that ther

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    Magnetic Susceptability

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    NiCl2 was recorded to calculate the apparatus constant as 5.7538. cv and cm for each solution was determined in order to calculate the number of unpaired electrons for each paramagnetic complex. Fe(NH4)2(SO4)2€6(H20) had 4 unpaired electrons‚ KMnO4 had zero unpaired electrons‚ and K3[Fe(CN)6] had 1 unpaired electron. The apparent 1 unpaired electron in K3[Fe(CN)6] when there should be five according to atomic orbital calculations arises from a strong ligand field produced by CN-. Introduction: The

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    Electric Shock

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    An electric charge is a fundamental quantity that is responsible for all electrical phenomena. An electric charge can have any value. A body has a negative electric charge whenever it has an excess of electrons. Electric charges can neither be created nor destroyed. 1 2. If the two electrons of a helium atom were removed‚ what would be its charge? a. b. c. d. 1.6 × 1019 C 3.2 × 10 C − 1.6 × 1019 C −19 − 3.2 × 10 −19 C 3. Three equally-charged bodies were hung and the interaction

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    An experiment to investigate the factors which affect Resistance in a wire What is resistance? A potential difference (V) applied across a wire of length (l)‚ there is in the conductor‚ an electric field (E). In this electric field the free electrons are not however under continuous acceleration (Ee/m). This is because they repeatedly collide with the moderately massive vibrating atoms losing their kinetic energy. The vibrating atoms having gained this kinetic energy now vibrate more. The resulting

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    CHEMISTRY

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    of electron distributions in orbitals will usually result in correct molecular geometry determinations. In addition‚ the simple writing of Lewis diagrams can also provide important clues for the determination of molecular geometry. Molecular geometry‚ the bond lengths and angles‚ are determined experimentally. Lewis structures can give us an approximate measure of molecular bonding. There is a simple procedure that allows us to predict overall geometry is the VSEPR‚ Valence Shell Electron Pair

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    chemistry 2ab notes

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    consists of a lattice of positive ions surrounded by a ‘sea’ of mobile delocalised valence electrons. • Metallic bonding is the electrostatic attraction between the delocalised electrons and the positive ions in the metallic lattice. Properties of metals: Property Explanation Relatively high density The particles are very close together. This is because of high electrostatic forces between the sea of valence electrons and the positively charged nucleus. Malleability and Ductility Because metallic bonding

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    Covalent Bonding Lab

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    bond when atoms share pairs of electron to become stable. For covalent bonding‚ two or more elements must have shared electrons. Atoms become stable by filling up their outermost shell with shared electrons. An atom can only have 8 electrons and that rule came from the Octet

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