Covalent Compounds Chapter 6 6-1 Covalent Bonds. Covalent Bond The sharing of electrons between...
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Transcript of Covalent Compounds Chapter 6 6-1 Covalent Bonds. Covalent Bond The sharing of electrons between...
![Page 1: Covalent Compounds Chapter 6 6-1 Covalent Bonds. Covalent Bond The sharing of electrons between atoms Forms a molecule To have stable (filled) orbitals.](https://reader036.fdocuments.us/reader036/viewer/2022062519/5697c0141a28abf838ccd5ac/html5/thumbnails/1.jpg)
Covalent Compounds
Chapter 66-1 Covalent Bonds
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Covalent Bond• The sharing of electrons between atoms• Forms a molecule• To have stable (filled) orbitals
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Diatomic Molecules• Formed by covalent bond between two atoms of the same element
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Molecular Orbital
• The space in which the shared electrons move
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Energy and Stability• Un-bonded atoms
(except noble gases) have low stability and high potential energy• Energy is released
when they form a bond
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Attraction and Repulsion
• When balanced, a covalent bond forms
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Bond Length
• The distance between two bonded atoms at their minimum potential energy
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Bond Energy• The energy required to
break a bond• kJ/mol
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Electronegativity and Covalent Bonding• Electronegativity - How much an atom attracts electrons• Atoms share electrons equally or unequally – depending on the
electronegativity of the atoms
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Nonpolar Covalent Bonds
• Electrons are shared equally
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Polar Covalent Bonds
• Atoms share electrons unequally• Have different
electronegativities
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Dipole Molecule• One end is partial positive and the other end is partial negative• Hydrogen and fluorine
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Polarity and Bond Strength• The greater the difference in electronegativity, the greater the polarity, and the
greater the bond strength
------------------ Bond Strength ------------------
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Determining Bond Types• Differences in Electronegativity of the atoms
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Metallic Bonds• Results from the attraction between metal atoms and the surrounding
sea of electrons
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Properties of Substances Depends on Bond Type
• Metallic – good conductors• Ionic – strong bonds, high
melting point• See table 3 page 197
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Drawing and Naming Molecules
Section 6-2
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Valence Electrons
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Lewis Electron-Dot Structures
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Octet Rule
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Lewis Structures Model Covalently Bonded Molecules
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Unshared (lone) Pairs• Not part of the bond
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Single Bond• The shared pair• Can be shown by a dash
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Lewis Structures for Polyatomic ions• Ammonia Ammonium ion
enclose in brackets w/ + charge
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Double Bonds
• Share 4 (2 pair) electrons• Carbon, oxygen, nitrogen
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Triple Bonds
• Share 6 (3 pair) electrons• Nitrogen and Carbon
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Naming Covalent Compounds
• Similar to Ionic bonds• -ide suffix
• Prefixes indicating number• On first element, only if
more than one
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Molecular ShapesSection 3
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Determining Molecular Shapes
• The shape helps determine the molecules physical and chemical properties
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Linear Shape
• “In a line”• Molecules made
of 2 atoms• H2 or CO
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VSEPR Theory
• Pronounced “vesper”• A model used to predict the shape of a molecule• Valence Shell Electron Pair Repulsion Theory• Based on the idea that valence electrons repel each other
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Linear Shape
• The shared pairs repel each other and remain as far apart as possible
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Bent Shape• Water H2O• Two shared pairs
and two unshared pairs• The unshared
pairs influence the shape
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Tetrahedral
• Methane CH4
• Four shared pairs
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Trigonal Planer
• BF3
• CH2O (Formaldehyde)• 3 shared pairs• Maximum distance apart
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Trigonal Pyramidal• 3 bonding pairs, 1 lone pair• Ammonia NH3
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Molecular Shapes Affects a Substance’s Properties
• Shape affects Polarity
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Polarity affects Properties
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