involves the sharing of electron pairs between two atoms. Translation: -Ionic bonding happens between a metal and a non-metal (east coast and west coast) -One atom completely donates its valence electrons to another atom -Metals become CATIONS (positive charge/oxidation state); Non-metals become ANIONS (negative charge/oxidation state) Example: Na + Cl → Na+Cl- or Mg + O → Mg2+O2- -In covalent bonding one atom completely shares its valence electrons with another atom (west
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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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Transition Metal: element of groups 3-12 * Energy level: a space with definite and fixed energy in which an electron is allowed to move * Orbit: circular/spherical path in which the electron can move around the nucleus * Electron Cloud: the region of an atom in which there is a probability that an electron exists * Quantum Mechanics: theory of the atom in which electrons are described in terms of their energies/probability patterns (model looks like smoke around a circle) * Principal
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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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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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there are two types of bonds that may form between them: Ionic bonds result from a transfer of electrons from one species (usually a metal) to another (usually a nonmetal or polyatomic ion). Covalent bonds result from a sharing of electrons by two or more atoms (usually nonmetals). Lewis theory (Gilbert Newton Lewis‚ 1875-1946) focuses on the valence electrons‚ since the outermost electrons are the ones that are highest in energy and farthest from the nucleus‚ and are therefore the ones that
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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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Explain the role of atomic number in MiniLab: Modeling Isotopes‚ p. 102 How Atoms Differ 2 sessions 1 block determining the identity of an atom. 6. Define an isotope and explain why atomic masses are not whole numbers. 7. Calculate the number of electrons‚ protons‚ and neutrons in an atom given its mass number and atomic number. Section 4.4 8. Explain the relationship between Careers Using Chemistry: Radiation Unstable Nuclei and Radioactive Decay 2 sessions 1 block unstable nuclei and radioactive
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