Solids Flashcards
What type of bonding is a metallic solid
Metallic bonds - the electrostatic attraction between positive metal cations and delocalized electrons.
What properties does metallic solids have?
Good conductivity, Malleable + Ductile, High melting + Boiling point, Good conductors of heat, Insoluble
Why are metallic solids not soluble?
Because to be soluble the metallic bonds must be broken but the water is not strong enough to pull the cations and electrons apart so metallic solids are insoluble.
What are the properties of Ionic solids?
Brittle, High melting + Boiling points, Soluble, Conducts electricity in molten form
Why do ionic solids conduct in molten form but not solid?
Because as molten form, the ions are free moving but when they are in solid form, the ions are in fixed positions and cannot move
What are the properties of Covalent Network?
Poor conductors with the exception of Graphite, High melting point, Insoluble, Not malleable or Ductile.
Why can Covalent Network not conduct electricity?
Because there are no charged particles. All electrons are involved in bonding not free to move. With the exception of graphite which contains delocalized electrons.
What are the properties of Covalent Molecular?
Poor conductors of electricity, Low melting point, Insoluble, Not malleable or Ductile
Why are Covalent Molecular insoluble?
Because they do not contain any charged particles - Delocalised electrons or mobile ions so Covalent Molecules cannot conduct in solid or molten form.
Where on the periodic table can the solids be found?
Metallic solids are made up of 2 metals so can be found only on the left side of PT. Ionic Solids are made up of a metal and a non-metal so can be found on both sides of PT. Covalent bonds are made up of only non-metals so can only be found on right side of PT.
Examples of Solids
Diamond - Covalent Network, Aluminum - Metallic Solid, Magnesium Chloride - Ionic Solid, Sulfur - Covalent Molecular
