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Intermolecular Interaction Energy
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Ionic Structures
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A Typical Ionic Liquid Being Considered for Low- emission Manufacturing Processes, 1-methyl-3-
methylimidazolium (DMIM), is Shown in Two
Representations
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A Density Potential Plot of the Second-
Period, p-block Hydrides Shows the Greater Polarity of NH 3 , H 2 0,
and HF as Compared with CH 4
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The Strong Diapole of the OH Bond Results in a Strong Attraction of the Hydrogen End of a Water
Molecule for a Lone Pair on the Oxygen of
Another Water Molecule
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The Positively Charged Sodium Ion
Interacts with the Excess Electron Density
Around the Oxygen Atom in Water
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Surrounding a Negatively Charged Chloride Ion with Water Molecules Results in the Water
Molecules Orienting with the Hydrogen Atoms
Pointing Toward the Chloride Ion
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The Temperature Range for the Liquid Form of H 2 O is Much Larger than that for H 2 S, H 2 Se, or H 2 Te, All of Which Have the
Same Bent Structure
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The Boiling Points of Stable p-block Hydrides Show a Regular Variation Down a Group, with the Notable
Exceptions of NH 3 , H 2 O, and HF. These Three
Hydrides have Anomalously High Boiling Points
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The Intermolecular Interaction of SO 2 with Water is an Example of a Dipole -
Dipole Interaction
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Two Representations of the Interaction Between SO 2 and H 2 O. (a) The Negative End of the Water Dipole is Attracted
to the Positive End of the Sulfur Dioxide Dipole. (b) The Large Electron Density on the Oxygen Atom of Water is Attracted to the Positively Charged Region Near the Sulfur
Atom of Sulfur Dioxide
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Dipole-dipole Notation
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(a) Like All Homonuclear Diatomic Molecules, N 2 is Nonpolar.
(b) Bringing a Positive Test Charge Near the N 2
Molecules Attracts the Negatively Charged Electrons and Repels the Positively Charged Cores. (c) Due to the Dynamic Nature of the Electron Cloud, Occasionally it will
be Shifted Slightly Relative to the Atomic Cores, Giving Rise to an Instantaneous Dipole. The Positive End of the
Dipole Attracts Electrons in the Neighboring Molecule
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The Group IVA Hydrides Are All Nonpolar Molecules, Interacting Through Induced
Dipole Induced Dipole Forces
due atomi cristallo con molti atomi
banda di valenza banda di
conducibilità gap di banda
1 + 2
antilegante
legante
E
conduttori isolanti semiconduttori
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(legame ionico 100 - 350 kJ/mol)
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The Unit Cells for the Crystal Lattices of
Metallic Elements
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The Crystal Structure of the Metallic Elements;
The Semimetals Si and Ge; and the Noble Gases
in their Low-temperature, Solid Form
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A Collection of Spherical Objects Is Packed in (a) a Simple Square Array and
(b) a Close Pack Layer
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In Hexagonal Packing, Cations in the Second Layer Sit in Triangular
Hollows of the First Layer
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Comparison of Common Crystal Structures
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The Melting Point of the Metallic Elements has a Regular Variation with Position in
the Periodic Table
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Comparison of the Density of Metals in Periods 4, 5 and 6 of the Periodic Table Shows that the
Density Varies Periodically, with a Rise and Fall
Repeated in Each Period
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The Flexibility of Five Common
Elemental Wires Varies Considerably
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Bending a Wire Distorts the
Hexagonal Close Pack Layers
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There Is a Correlation Between Stiffness and Melting Point in Wires Composed of
Five Common Metallic Elements
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A Flag Pole Is Designed to Bend and
Flex in a Strong Wind
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A Typical Stress-strain Plot
Sforzo=F/A Deformazione=deltal/l
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The Elastic Modulus for Transition Metals and Calcium First Increases and Then
Decreases Across the Fourth Period
Modulo elastico=sigma/epsilon
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The Atomic-scale Result of Application of a Stretching Force. Bonds Along the Length are
Elongated, while Bonds Across the
Width are Compressed
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The Energy of a Typical Bond
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The Valence Electron Configuration of
Fourth-Metal Period
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Plastic Distortion Occurs When the Strain Becomes too Great and the Atoms Shift,
Adopting New Neighbors
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The Dark Line Represents the Variation in Energy as Two Rows of Atoms Slide over Each Other. In a Close
Pack Structure (a) the Variation Is Quite Smooth. In a Body-centered Cubic Structure (b), the Larger Spacing
Between Atoms Means that there Is a Larger Energy
Barrier to Get from One Position to the Next.
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A Close Pack Plane (FCC or HCP)
and a BCC Lattice
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Slip Planes of the BCC, FCC, and HCP
Crystal Lattices
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A Line Defect in a Simple Cubic Lattice
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It Takes a Great Deal of Effort to Pull All the Teeth of a Zipper Apart at Once, Pulling Apart a Pair of Teeth
at a Time Requires Much Less Effort
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(a) A Single Missing Atom in an Otherwise Regular Array is an Example of a Kind of Pint Defect Called a Vacancy Defect. (b) A Row of Atoms Where the Regular
Crystalline Array Is Disrupted Is a Line Defect. (c ) An Area Where Two Crystalline Arrays Meet but are out of
Register with Each Other Is a Grain Boundary
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Successive ”Snapshots" of a Line Defect
Rippling Through a Crystal Lattice
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As the Defect Ripples Through the Solid Lattice, it is Difficult for It to Cross the Gap
at the Grain Boundary
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Resistivity of First Transition Series Elements Decreases Smoothly from the Start of the Series
to the End, with the Notable Exception of Mn.
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Resistivity Shows a General Decrease
Across All Three Transition Series
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Resistivity of Transition Elements
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Selected Alloys
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Two Elements from a Substitutional Alloy over a Large Compositional Range if they are Similar in
Size, Crystal Structure, and Electronegativity
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Copper-Nickel Solutions
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The Cooling Rate Determines
the Morphology of the Solid Formed
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(a) Two Unit Cells of the Iron Lattice are Shown with the Interstitial Site Indicated. (b) In steel,
Carbon Occupies Some of the Interstitial Sites.
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Superplastic Steel Can Be Stretched to 11 times its Original Length Without Cracking or Breaking. A Piece Originally 1 in. Long, Can Be Pulled at 900 degrees C to
11 in. Long. Ordinary Steel Fails When Pulled to Twice
its Original Length
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The Nitinol Unit Cell Showing Structure of
the High-temperature Austenite Phase
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