atom‚ a metal makes a contribution of an electron and becomes a optimistic ion‚ and when another‚ a nonmetal received an electron and becomes pessimistic ion. Metal donate electrons and non-metals receives electrons. For example is Na is positive and CL is negative. The covalent bonds share the electrons and they are normally nonpolar. The covalent bonding does not donate or gain electrons such as CH4. The ionic compounds tend to have eight electrons to keep in the highest energy level. The
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3.1 a) Valence electron: Valence electrons are the electron in the outermost electron shells of an atom. They are generally the electrons involved in chemical reactions and bonding with other atoms. b) Lewis electron: It is a structural demonstration of a molecule where you can use dots to show the position of the electron around the atoms and lines. c) Octet rule: It is referring to the principle that bonded atoms share their eight outer electrons. There rule of the octet is sometimes broken
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contact When two objects are rubbed together there is more contact between the surfaces and so more electrons are transferred Electron Affinity: Electron affinity is the tendency of a substance to hold onto electrons. Items high on the list (electrostatic/ triboelectric series) will tend to lose electrons easily (positive) Items low on the list will tend to gain electrons easily‚ or hold on to their electrons example: glass rubbed with plastic wrap glass is above plastic wrap glass will become positive
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11/19/14 Modeling Molecules Introduction: You can represent a molecule two-dimensionally‚ as a structural formula or electron dot structure. Although such models are useful in certain contexts‚ they do not accurately represent bond angles between atoms or shapes of molecules. In this activity‚ you will construct three-dimensional models of several molecules. You will use electron dot structures and structural formulas to inform how you construct the three-dimensional models. Materials: Google Microsoft
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Sharing Electrons Example~ A hydrogen atom has one electron. If it had two electrons‚ it would have the same electron configuration as a helium atom. Two hydrogen atoms can achieve a stable electron configuration by sharing their electrons and forming a Covalent bond. A covalent bond is a chemical bond in which two atoms share a pair of valence electrons. When two atoms shair one pair of electrons‚ the bond is called a singe bond. Molecules of Elements Two hydrogen atoms bonded together
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Karla Alvarez Chemistry Period One Subatomic Particle The electron is extremely small compared to all the other parts of the atom. It is negatively charged. The negative charge balances out the positive charge of the protons in the atom. Electrons are found in the electron cloud that surrounds the nucleus of an atom. The clouds are generally organized into shells. Electrons move at a quick pace‚ so you never really know where they are specifically. But after years of doing experiments‚ scientists
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Experiment 3: Electronic structure‚ bonding and shape of some simple inorganic molecules. Introduction: In quantum chemistry‚ electronic structure is the state of motion of electrons in an electrostatic field created by stationary nuclei. The term encompass both the wave functions of the electrons and the energies associated with them. Electronic structure is obtained by solving quantum mechanical equations for the aforementioned clamped-nuclei problem. Electronic structure problem arise from the
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four outer electrons (called valence electrons) with neighbouring atoms. Silicon is a poor conductor because the outer electrons in each atom are held firmly in place by the crystalline structure. Doping Doping is a method used to increase the conductivity of a semiconductor by adding tiny impurities to the crystal lattice. A very small proportional of silicon atoms are replaced with atoms of other elements. Two way of doping. N-type semiconductor Use atoms with five outer electrons (antimony
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Shell Electron Pair Repulsion) theory proposes that the geometric arrangement of terminal atoms‚ or groups of atoms about a central atom in a covalent compound‚ or charged ion‚ is determined solely by the repulsions between electron pairs present in the valence shell of the central atom. The number of electron pairs around the central atom can be determined by writing the Lewis structure for the molecule. The geometry of the molecule depends on the number of bonding groups (pairs of electrons) and
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silicon atom. Since the valency of silicon atom is 8 which means that there are 8 electrons in its outermost orbit. However in its natural state there are only 4 electrons bounded in the outermost orbit. Hence these 4 electrons are able to bond with another 4 electrons with 4 silicon atoms around it. The 4 free electrons that can move around throughout the substance. During the absence of electric potential these free electrons tend to remain close to their parent atoms so that they are at minimum energy
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