activity series  
  bond energy
  bond lengths


  common names

  conversion factors: energy

  conversion factors: length

  conversion factors: mass

  conversion factors: pressure

  conversion factors: temp.

  conversion factors: volume

  covalent prefixes

  density solver

  diatomic elements

  e-config. chart

  element list

  gas law formulas

  Ka's of polyprotic acids

  Ka's of weak acids

  Kb's of weak bases

  metric conversion chart

  mole conversion chart

  molecular geometries

  organic prefixes

  periodic table

  periodic table (flash)

  pH/pOH converter

  polyatomic ions

  pressure converter

  SI units

  solubility chart

  solubility of salts rules

  solubility product constants

  stoichiometry chart

  temp. conversion

  temp. formulas

  thermodynamic data

  vapor pressure of water

Salts and Metals

  • Metallic bonds are formed between like metal ions. Ionic bonds are formed between a cation (usually a metal) and an anion (usually a nonmetal).
  • Both metals and salts are arranged in crystals. As a result, both metals and salts have high melting and boiling points.
  • Metals conduct electricity even as solids. Ionic compounds only conduct electricity when they are molten or dissolved in water.
  • Metals and salts have different properties because in a metal valence electrons are not attached to any one atom; in a salt they are. So, in metals, valence electrons are free to move around freely throughout the crystal. These free moving electrons are why solid metals can conduct electricity and ionic compounds cannot.
  • Metals are malleable and ductile. Ionic compounds are brittle. Although atoms in a metal are in a somewhat fixed position, they can move without breaking the attraction between atoms. This allows them to be malleable and ductile. If the atoms in an ionic compounds move, like charges line up and the repulsion between the atoms cause the ionic compound to break apart. The diagram below shows how metals respond to a force.

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