Chapter 1 Cell Theory- in the 18th century‚ two scientists came up with the cell theory. Schleiden and Schwen. 3 corollaries of the cell theory: -all cells are alike in chemical composition -all cells store and process information in the same way -all cells arise from other cell through cell division 5 types of different Microscopes 1. Light Microscope- produces 2-D image Direct descendants of Hooks scope> take two lenses to a light source> used this to magnify images up to 1‚000 fold.
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seen in all terminated surfaces that both the majority and minority are metallic. When the depth increases the majority states are still metallic and have no distinct change at the Fermi level‚ while the minority states of each atom decrease relative to those of the atoms in the surface. For the Co-Co surface is lost the half–metallic (HM) properties of the bulk system with the spin polarization about –42%. The total density of states (DOS) as well as the projected density of states (PDOS) is shown
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Chapter 4 CLO 1.A branch of chemistry dealing with compounds of Carbon. 2.Carbon’s has 4 valence electrons that can form covalent bonds with others atoms (Hydrogen‚ Nitrogen‚ Oxygen and Carbon atoms mostly) to make large‚ complex and diverse organic molecules. 3.The carbon skeleton vary in 4 areas‚ 1. Length 2. Branching 3. Double Bond Position 4. Presence of Rings. Carbon skeletons can have double bonds in different locations and also different numbers of double bonds. 4.Hydrocarbons
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electrons do atoms of each element have? a. nitrogen d. barium b. lithium e. bromine c. phosphorus f. carbon 37. Name each ion in Problem 36. Identify each as an anion or a cation. 7.2 Ionic Bonds and Ionic Compounds 38. Define an ionic bond. 39. Explain why ionic compounds are electrically 29. Write electron dot structures for each of the fol- lowing elements: a. Cl b. S c. Al d. Li neutral. *40. 30. Describe two ways that an ion forms from an atom. *
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Jeff Fry – Chemistry 11 Section Assignment 3.1: Determining Atomic Mass Instructions Perform the following calculations. Take care to give answers with the appropriate units and significant figures. Show your solution method clearly. The use of a Periodic Table will be required. 1. Element "E" (not a real symbol for an element)‚ has three naturally occurring isotopes: 60% 228E‚ 25.0% 222E‚ and 15.0% 232E. Use this information to determine the atomic mass of element "E". Atomic Mass =
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03.04 Valence Electrons and Bonding Individual neutral atoms are rarely found in nature. The noble gases are the only elements that are found as single atoms more often than they are found in compounds. Atoms are held together in compounds by electrostatic attraction between positive nuclei and negative electrons. This attraction holds atoms together in a chemical bond‚ a link between two atoms resulting from the mutual attraction of their nuclei for valence electrons. All chemical bonds involve
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second and third IE is experimental evidence for the electron shell structure of atoms • Ionization energy for the removal of the second electron is large because the second electron is removed from a much lower energy (inner) subshell • The trend across a period is rationalized by the increase in effective nuclear charge Electron Affinity • The energy of a process in which an electron is acquired by the atom (the greater the affinity‚ the more negative the value‚ exothermic reaction) • An
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achieve improvements in their effectiveness. An understanding of organic chemistry can be developed from knowledge of the structure of a carbon atom and how it can combine with other carbon atoms by forming covalent bonds. Alkanes Alkanes are hydrocarbons‚ which are molecules that contain only carbon and hydrogen. They are made up of carbon atoms linked together by only single covalent bonds and are known as saturated hydrocarbons. Many alkanes are obtained from crude oil by fractional distillation
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state into a higher energy state. This is called absorption or sometimes stimulated absorption. E2 (Absorption) E1 Spontaneous Emission: Once the atom or molecule goes in its excited state‚ there is a probability that it will emit radiation again and return to a lower energy state thus a photon is emitted. In this emission process‚ where the atoms spontaneously goes to a lower energy state through the emission of a photon is called spontaneous emission. This emission process is a random one and
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One of the easiest ways to start drawing a Lewis Structure is to make a list of each atom in the structure and next to each atom record how many valence electrons it has and how many it needs to fill its valence shell. In covalent bonding the valence electrons in the molecule come from the valence electrons in the atoms that formed the bond. a. The number of valence electrons in any main group atom is equal to its group # (I‚II‚II‚IV‚V‚VI‚VII‚ VIII or 1‚2‚3‚4‚5‚6‚7‚8) b. Compounds
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