Introduction: According to the Bohr atomic model‚ electrons orbit the nucleus in fixed paths with specific energies. Each path is therefore often referred to as an “energy level”. Electrons possessing the lowest energy are found in the levels closest to the nucleus. Electrons of higher energy are located in progressively more distant energy levels. If an electron absorbs sufficient energy to bridge the “gap” between energy levels‚ the electron may jump to a higher level and become “excited”. Since
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simply put‚ the radius of an ion. An ion is a charged particle. Atoms become ions from the addition of electrons (giving them a negative charge) or the loss of electrons (giving them a positive charge). Ionic radius is defined as the distance between the nucleus of this charged particle (where the protons and neutrons reside) and the outermost edge of its electron cloud. Because the electron field surrounding an ion can vary‚ the ionic radius is generally measured by taking half the distance between
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combination of three nuclei and ten electrons possesses special properties that make it unique among the more than 15 million chemical species we presently know. When we stop to ponder the consequences of this‚ chemistry moves from being an arcane science to a voyage of wonder and pleasure as we learn to relate the microscopic world of the atom to the greater world in which we all live. The molecule of water A molecule is an aggregation of atomic nuclei and electrons that is sufficiently stable to possess
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occur at electrodes. Discharge the removal of electrons from negative ions to form atoms or the gain of electrons of positive ions to become atoms. Anode positive electrode connected to positive terminal of d.c. source. Oxidation occurs here. Anode loses negative charge as electrons flow towards the battery‚ leaving anode positively charged. This causes anion to discharge its electrons here to replace lost electrons and also‚ negative charge are attracted to positive
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Sample Paper – 2008 Class – Physics Class – XII Dual nature of matter Q.1. State the dependence of work function on kinetic energy of electrons emitted in a photocell. If the intensity of incident radiation is doubled‚ what changes occur in the stopping potential and photoelectric current? Q.2. How does the maximum kinetic energy of the emitted electrons vary with the work function? Q.3. the frequency of incident radiation is greater than the threshold frequency in a photocell. How will
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chem A. Electronic Structure of Atoms - The bonding behaviour of atoms depends entirely on electron configuration‚ as revealed by an atom’s position in the Periodic Table. - The "Organic Chemist’s" periodic table. Key to numbers: - upper left = atomic number = number of electrons - lower left = number of outer shell electrons (= group number) - upper right = valence = number of unpaired electrons in valence shell - lower right = electronegativity value [a full periodic table with atomic numbers
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CARBON CARBON MULTIPLE BOND PRESENTED BY: WASIQUE AZHAR MSC CHEM (2 SEM) Some basic concept Electrophile : a species with a region of positive or partial positive charge electron-poor Nucleophile: a species with a region of negative or partial negative charge electron-rich TO LERN OBJECTIVE : Elecrophilic Addition to carbon-carbon double bond Stereochemistry of Elecrophilic addition reaction Hydrogenation of double and triple bond Nucleophilic Addition to carbon-carbon double
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bonding‚ atoms attain a complete outer shell of valence electrons (stable noble gas configuration). • Atoms can form either ionic or covalent bonds to attain a complete outer shell (octet rule for second row elements). • Ionic bonds result from the transfer of electrons from one element to another. • Covalent bonds result from the sharing of electrons between two nuclei. 2 Valence Electrons • Second row elements can have no more than eight electrons around them. For neutral molecules‚ this has two
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Dense nucleus composed of neutrons (0 charge) and protons (+ charge) and surrounded by orbital electrons (- charge). Neutrons and protons firmly held in the nucleus while electrons are very loosely held and are easy to remove. When electrons are removed from the atom‚ two charged particles (ions) are produced the positively charged atom and the negative electron. Energy is absorbed to remove the electron from the atom. Atomic Notation Chemical symbols such as C for carbon‚ H for hydrogen‚ and
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400 BC Democritus: He hypothesized that all matter (plus space and time) is composed of tiny indestructible units‚ called atoms. Democritus performed no experiments. 1 .All matter consists of invisible particles called atoms. 2. Atoms are indestructible. 3. Atoms are solid but invisible. 4. Atoms are homogenous. 5. Atoms differ in size‚ shape‚ mass‚ position‚ and arrangement. ->Solids are made of small‚ pointy atoms. ->Liquids are made of large‚ round atoms. ->Oils are made of very fine
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