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Why are pure metals malleable?
Atoms are the same size, layers not distorted and can slide over each other.
Why do pure metals have limited uses?
They are not strong.
Why are metals made into alloys?
To make them harder and stronger.
What are alloys?
Mixtures of metals or mixtures of metals and non metals.
Why are alloys examples of formulation?
They are a mixture designed as a useful product.
What is ionic bonding?
Attraction between oppositely charged ions.
Why does ionic bonding occur?
Metal atoms lose outer electrons to form +ions, non metal ions gain outer electrons to form -ions, the oppositely charged ions strongly attract eachother.
How do you describe ionic bonding?
Who transferred electrons and how many
The charge it now has
Who gained electrons and how many
What charge it now has
A reference to ‘oppositely charged ions strongly attract’
What are the limitations of dot and cross covalent diagrams?
They do not show the shape of molecule, They are 2D.
What are the limitations of ball and stick covalent diagrams?
They are not to scale, they do not show electrons.
What are the limitations of 2D ionic diagrams?
It only shows one layer of ions.
What are limitations of 3D ionic diagrams?
It is not to scale, there are large gaps between ions.
What are limitations of dot and cross ionic diagrams?
They do not show the structure of the compound or how the ions are arranged.
How do you describe the structure of any metal or metallic bonding?
A giant lattice of positive metal ions, attracted to delocalised electrons.
How do you describe metals that conduct heat?
Delocalised electrons move and transfer energy throughout the structure
How do you describe metals that conduct electricity?
Delocalised electrons move and carry charge throughout the structure.
How do you describe metals with high melting and boiling points?
Giant lattice structure, lots of energy needed to break, strong metallic bonds.
How do you describe metals with low melting and boiling points?
Simple molecule structure, little energy needed to break, weak metallic bonds.
What are the properties of diamond?
High mpt, hard, does not conduct electricity, used to drill, giant lattice of C atoms connected to 4 others by covalent bonds.
What are the properties of graphite?
High mpt, soft, conducts electricity, used as pencils, giant lattice of C atoms connected to 3 others by covalent bonds, weak forces between hexagon layers.
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