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Published byPhilip Gregory Modified over 7 years ago
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Chemical Bonding The Formation of Compounds
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Lewis Theory The attraction between electrons of one atom to the nucleus of another atom contribute to what is known as chemical bonds. G.N. Lewis (1875-1946) recognized valence electrons bond from one atom to another electron transfer resulting in ionic bonds sharing electrons resulting in covalent bonds overlapping electrons resulting in metallic bonds
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A. Why bonding? All atoms want a filled outer ring to be STABLE atoms (non-reactive) Atoms bond to fill their outer electron ring Stable=full set of valence electrons (electrons in the last ring) Atoms that already have a filled outer ring are the noble gases Bonding creates compounds like water H 2 O and glucose sugar C 6 H 22 O 11
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B. Two Types of Bonding #1 Ionic CComplete transfer of electrons from one atom to another CCreates charged particles (called ions) OOpposite charges attract OOccurs between a metal and a non-metal atom GGives a compounds a high melting/boiling point
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#2 Covalent Bonding Atoms share electrons Occurs between a non-metal and a non-metal atom
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Properties of Covalent Bonds Low melting and boiling points Brittle solids
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#3 Metallic Bonding -Electrons overlap -Occurs between two metal atoms -Gives metals their properties (malleability, ductility, conductivity)
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Lewis Dot Structures Lewis structures show the valence electrons as dots arranged around the atomic symbol. hydrogen: sodium: chlorine: Na H Cl
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The Octet Rule Atoms tend to gain, lose, or share electrons until they have eight valence electrons.
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Ionic and Molecular Compounds Formation of sodium chloride: Formation of hydrogen chloride: A metal and a nonmetal transfer electrons to form an ionic compound. Two nonmetals share electrons to form a molecular compound. Na + Na + [] Cl Cl H + Cl Cl H
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Learning Check Draw electron dot diagrams for: Hydrogen Carbon Nitrogen Oxygen These elements form life and make up cells, DNA, carbohydrates and proteins
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