model of the atom‚ electrons in an atom (1) travel in defined circles (3) have a positive charge (2) are most likely found in an excited state (4) are located in orbitals outside the nucleus 2. ____ What is the total charge of the nucleus of a carbon atom? (1) –6 (2) 0 (3) +6 (4) +12 3. ____ When an atom loses one or more electrons‚ this atom becomes a (1) positive ion with a radius smaller than the radius of this atom (2) positive ion with a radius larger than the radius of this atom (3) negative
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Mastering Concepts 2.1 1. Which chemical elements do organisms require in large amounts? Carbon‚ oxygen‚ hydrogen‚ nitrogen‚ sulfur‚ and phosphorus are the chemical elements that organisms require in large amounts. 2. Where in an atom are protons‚ neutrons‚ and electrons located? An atom’s protons and neutrons are in its nucleus. A cloud of electrons surrounds the nucleus. 3. What does an element’s atomic number indicate? An atom’s atomic number indicates the number of protons in its nucleus
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Gizmo Warm-up Just like students sharing markers‚ atoms sometimes share or swap electrons. By doing this‚ atoms form bonds. The Ionic Bonds Gizmo™ allows you to explore how ionic bonds form. To begin‚ check that Sodium (Na) and Chlorine (Cl) are selected from the menus at right. Click Play ([pic]) to see electrons orbiting the nucleus of each atom. (Note: These atom models are simplified and not meant to be realistic.) 1. Each atom consists of a central nucleus and several shells that contain
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Atomic structure: scientists 1. Democritus: 1st person to think of atom (500 BCE)- philosopher Atom is the smallest piece of an element that has same properties as the element. 2. Lavisier: Law of conservation of mass/ matter • Mass can’t be created or destroy; same amount of stuff 3. Joseph Proust: Law of constant composition (law of definite Proportions) • A compound is always made of the same elements in the same ratio. 4. John Dalton: English school teacher who derived the atomic theory
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UNIVERSITY OF THE GAMBIA LECTURE NOTES COURSE: PRINCIPLES OF CHEMISTRY II (ORGANIC CHEMISTRY) CODE: CHM 161 2ND SEMESTER SESSION: 2012/2013 LECTURER: ANTHONY F. ADJIVON UNIT 1 INTRODUCTION Organic chemistry started as the chemistry of life‚ when that was thought to be different from the chemistry in the laboratory. Then it became the chemistry of carbon compounds‚ especially those found in coal. Now it is both. It is the chemistry of the compounds of carbon along with other elements
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for an over view and for a reference as you work through these problems http://www.wiley.com/college/chem/spencer053872/tutorial/gramsmoles/gramsmoles1.html We can use this to do mathematical conversions to determine mass‚ volume‚ and number of atoms or molecules in a given substance. For example let’s check out this video to convert moles methane (CH4) to grams of methane. http://www.sciencegeek.net/Chemistry/Video/Unit4/GMV2.shtml Once you have finished the video let’s practice by completing
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IB Chemistry Summary- By Paul Li & Silvia Riggioni TABLE OF CONTENTS Table of Contents............................................................................................................................................................ 1 Atomic Theory................................................................................................................................................................ 3 The Electromagnetic Spectrum.............................................
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Born-Oppenheimer approximation. Along with nuclear dynamics problem‚ electronic structure problem is one of the two steps to study quantum mechanical motion of a molecular system. Except for a small number of simple problems such as hydrogen-like atoms‚ the solution of electronic structure problems require modern computers. Electronic structure problem is routinely solved with quantum chemistry computer programs. Electronic structure calculations rank among the most computationally intensive tasks
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Aristotle. Also plato was Aristotle teacher at the Acadamy at the time. It wasent untill 2000 years after no one questioned the theory of atoms‚ untill the early 1800’s. John Dalton was born in 1766 in Cumberland‚ England. Dalton made many experiment strictly to atom study even though he had no idea what is was. He is most known for the extensive research on atoms. He proposed a table of atomic weights for the number of the known element. This image is Dalton’s table of elements and the number of elemental
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hydrogen‚ oxygen‚ and carbon atoms form to form a sucrose molecule (C12H22O11). Ionic bonds form when oppositely Figure 1: The pile of white grains on the left are ordinary crystals of table salt and the grains on the right are charged atoms‚ referred to as ions‚ grains of white‚ refined sugar. Notice that the salt grains combine. Under the right conditions‚ are more cubic in shape. when individual sodium and chlorine atoms associate‚ an electron transfer will occur. The sodium atom contains a single electron
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