Bonding

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Chapter 3

• Bonding

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Bonding

• The interaction of atoms with each other to form
  discrete groups

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The Principles of Bonding

• There is a force of attraction between (-)
  electrons and () nuclei.
• There is a force of repulsion between electrons.
• There is a force of repulsion between nuclei.
• All chemical bonding reflects these interactions.

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The Trap of Stability

• Noble gases have stable electron electron
  arrangements, so they dont react to rearrange.
• For many other elements, chemical reactions are
  often guided by the tendency to acquire a noble
  gas electron arrangement.

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Ionic Bonding Electron Transfer
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Covalent Bonding-Electron Sharing

• water, H2O carbon dioxide, CO2

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Lewis Structures, H to He
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Some Lewis Structures, ball-and-stick,
space-filling
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More Lewis Structures, ball-and-stick,
space-filling
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Physical Properties

• Melting point the temperature at which the solid
  form of the compound becomes liquid.
• Boiling point the temperature at which the
  liquid boils and transforms into a gas.

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Electronegativity -electron-attracting ability
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Polar Covalent Bonds water as a case-study

• Each H is d
• Each O is 2 d-

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Chemical NomenclatureBinary Salts

• KBr K and Br
• potassium ion bromide ion
• Potassium bromide
• FeBr3 Fe3 and 3 Br
• iron(III) ion
  bromide ion
• iron(III) bromide

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Chemical NomenclatureBinary Covalent Compounds
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Binary Covalent Compounds

• PCl5 phosphorus pentachloride
• N2O4 dinitrogen tetroxide
• tetraphosphorus decoxide P4O10