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Bonding and Properties
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All Compounds Covalent Ionic Metallic Polar Nonpolar
Molecular Polymeric Network Polar Nonpolar
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WS – Bond and Property Chart
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Types of Compounds IONIC COVALENT METALLIC
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IONIC + -
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+ + + + + + + + METALLIC + + + + + + + +
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CO-VALENT + +
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IONIC COMPOUNDS
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NaCl
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NaCl
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CaCO3
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Ionic Bonds / Compounds
Oppositely charged atoms / IONS are created that attract magnetically Cation (+) attracts Anion (-) Ionic Compounds are called Salts or Ceramics
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Ionic Compounds Are Crystals
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KEY CONCEPT: Ionic Compounds are Crystals made of Alternating Positive and Negative Particles
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Ionic Compounds Are Brittle Because………..
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+ - + - - + + - + - - - + - +
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- + - + + + - - - - + + - + + - - + + -
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- + - + + + - - - - + + - + + - - + + -
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Ionic Compounds Have High Melting Points because…….
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Ionic Compounds Have Solubility in Water (Polar), but not in Oil (Nonpolar) because………
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Ionic Compounds Conduct as Liquids and When Dissolved Because…….
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e- Light e- Na+ Na+ e- Na0 e- e-
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The Electric Pickle
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Examples of Ionic Compounds (Salts)
NaCl – Flavoring and Preservative Na3PO4 – Common Preservative CuSO4 – Fungicide Na2CO3 – Leavening Agent AgNO3 – Black & White Photography
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+ + + + + + + + METALLIC + + + + + + + +
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Metallic Bonds and Compounds
A free flowing, shared pool of electrons attracted to a group of positive ions (Note: the atoms are NOT actually ionic) Loose sharing of electrons between among many metal nuclei.
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Metals like ionic compounds usually have highly ordered atomic structure (crystalline)
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Key concept of metallic compounds: Loose pool of electrons which can move between metal atoms which are in a crystalline arrangement.
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Malleability of Metals
Community pool of electrons helps cohesiveness (changing shape e.g. malleability & ductility) Bonds are electrons being shared between atoms, if no sharing then the atoms would fall apart most easily
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Bending Metals + + + + + + + + + + + + + + + + + + + + + + + + + + + +
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Bending Metals + + + + + + + + + + + + + + + + + + + + + + + + + + + +
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Bending Metals + + + + + + + + + + + + + + + + + + + + + + + + + + + +
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Community Pool of Electrons leads to conductivity of heat and electricity
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Metals typically have a high melting point because the community pool of electrons lessens the ability of metals to move freely from each other.
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Metal compounds are typically called Alloys
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Alloys Stainless Steel – Fe, Cr, Ni, Cu, etc.
Niobium-titanium Superconducting Alloy Brass – CuZn and Bronze – CuSn Lightweight Planes - AlTi Alloys Mangalloy – Strong and Tough
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Lab - Thermal Conditioning of Metals
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Annealing is a heat treating process which makes material softer and less brittle by producing uniform material properties and a higher crystalline structure. A material can be annealed by heating it to a specific temperature and then letting the material slowly cool to room temperature.
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Tempering is a heat treatment for making material harder
Tempering is a heat treatment for making material harder. The metal is heated to a specific temperature and rapidly cooled (quenched) in a bath of water, brine, oil, or air to increase its hardness. Tempering freezes atoms into a more random arrangement which makes the material stronger, but more brittle.
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Partial Annealing after Tempering will provide greater strength, but not as much brittleness
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Making Metals Strong Carbon Content and Tempering
Carbon makes steel hard. It fills open spaces making the metal have a tighter pack, but bonds are weaker between Fe and C then between Fe and Fe.
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Mangalloy
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Hardness Measures
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CO-VALENT
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COVALENT Atoms share pairs of electrons
Atoms are bonded because ELECTRONS are STRONGLY PULLED by TWO ATOMS Atoms share pairs of electrons Each pair of shared electrons creates one bond.
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H2
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Covalent Compounds Because Nonmetals have High Electronegativities a universal property of Covalent Compounds is Low Conductivity of Electricity. Otherwise, covalent compounds have a wide variety of properties including textures, hardness, malleabilities, melt points
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Why are covalent compounds so diverse?
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All Compounds Covalent Ionic Metallic Molecular Polymeric Network
Polar Nonpolar
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Key concept of Molecular Covalent: Small groups with covalently bonded atoms are called MOLECULES
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Small Covalent Compounds = Molecules
Polar Examples Water: H2O Sugar: C6H12O6 Nonpolar Examples Air: N2, O2, CO2 Wax: C25H52 H - H
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B/C Molecules are Small ……
Molecules can be all three states of matter, but they are the only type of compound that can be a gas at room temperature.
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B/C Molecules are Small ……
the lowest melt points compound will dissolve in substances of similar polarity
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Key concept of Polymeric Covalent: Polymers are LARGE and LONG chains of Covalently Bonded Atoms with a REPEATING PATTERN
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POLYethylene
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Examples are DNA, Plastics, Protein, Wood/Paper, Rubber, Cotton
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B/C Polymers are Larger they…
Are usually solids, but flexible have medium melt points Are harder to dissolve
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Key concept of Polymeric Covalent: Networks are very large covalent compounds with widespread CONTINUOUS bonding
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Covalent Network The amount of bonds makes networks very stable
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B/C Networks have SO much bonding they...
Are solids (crystalline solids) have very high melt points do not dissolve in water
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Examples of Networks Diamonds: C Graphite: C Sand: SiO2
Silicon for Computer Chips: Si NOTICE: The formula is a ratio of the elements. The formula does NOT represent the number of atoms in a network. Even my small, 9.6 g piece of silicon has 21,000,000,000,000,000,000,000 atoms.
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Basic Unit of Compounds vs. Melting Point Temperature
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Differences in Melting Point Temperatures
+ - H2O H2O H2O H2O H2O H2O H2O H2O Ionic (e.g. NaCl) Molecular Covalent C Network Covalent (diamond)
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Metallic Compounds + + + + + + + + + + + +
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Dissolving
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Dissolving Ionic Compounds
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Dissolving Sugar Molecules (C6H12O6)
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Network Covalent (diamond)
Dissolving + - H2O H2O H2O H2O H2O H2O H2O H2O Ionic (e.g. NaCl) Molecular Covalent C Network Covalent (diamond)
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END
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Potential Energy as a function of nuclear proximity
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Crystal Lattice A Lattice is an array of points repeating periodically in three dimensions. Shapes will depend on Chemical Formula
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Lattice Energy Force of attraction will influence how much energy it takes to break the ions apart Melting Point Solubility Strength of Solid
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Acids and Bases Acids and bases are small discrete units like molecules Acids and bases break down in water to form ions We will discuss acids and bases as a separate unit toward the end of the year
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Sharing of electrons (electronegativity) is a gradient
Nonpolar Ionic
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Electronegativity 0-0.3 nonpolar covalent 0.3 to 1.7 polar covalent
Above 1.7 is ionic A bond between two metals is a metallic bond
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How do we typify compounds? Bonding Lab 1
As chemists we want to relate the observable data to the microscopic structure so we can categorize, predict, engineer Does NaCl behave they way it does partly because it is made of ions and IONICALLY BONDED? Does Water H2O behave like it does because of has POLAR COVALENT Bonds? As chemists we want to relate Does Water H2O behave like it does because of has POLAR COVALENT Bonds?
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Oxidation Numbers represent when bonded and doesn’t represent anything real vs. Charge is real
Oxidation number is when as a compound and charge is when it is as an ion
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+ + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + + +
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