Chem Metals Flashcards
What properties do metals have?
- Good conductors of heat and electricity
- High melting and boiling points
- Malleable
- Ductile
- Sonorous
- Shiny
How do metals conduct electricity?
Electrons form a ‘sea of electrons’ surrounding positive metal ions.
- Electrons are delocalised therefore they can carry charge.
Describe metallic bonding.
- Loses valence shell –> positively charged cation
- Delocalised electrons pull cations into regular formation
- Strong electrostatic attraction between electrons and cations.
Give examples of alloys.
Steel, Bronze, Brass, Stainless steel
List chemical properties of transition metals.
- Form coloured compounds
- Act as catalysts
List the properties of group 1 metals.
Malleable, Reactive, Low boiling point and density.
What is galvanising?
A way of preventing corrosion by coating a metal in zinc.
How is Iron extracted from haematite?
Coke, Haematite, Limestone in blast furnace.
Coke and air react form CO2
CO2 reacts with more coke forms CO
CO acts as a reducing agent, reduces Haematite to iron.
Limestone decomposes to calcium oxide
calcium oxide removes any more impurities forming slag
Sulphate
SO4 2-
Carbonate
CO3 2-
Hydroxide
OH -
Phosphate
PO4 3-
Nitrate
NO3 -
describe metallic bonding
Metal cations held together by delocalized electrons through strong electrostatic forces.
Saturated meaning
solution that can dissolve no more solute at a given temperature.
