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Charge of silver ions
Ag+
Charge of copper ions
Cu 2+
Charge of iron ions
Fe 2+ or Fe 3+
Charge of lead ions
Pb 2+
Charge of zinc ions
Zn 2+
Charge of ammonium ions
NH4+
Charge of carbonate ions
CO3 2-
Charge of nitrate ions
NO3-
Charge of sulphate ions
SO4 2-
What is ionic bonding?
Bonds formed between a metal and a non metal
Metals lose electrons to form positive ions
Non-metals gain electrons to form negative ions
They are held together by their opposite charges.
Why do ionic compounds have high melting and boiling points?
Strong electrostatic forces of attraction between the oppositely charged electrons require large amounts of energy to overcome
Are ionic compounds good conductors?
They don’t conduct electricity when solid, but they do when molten and in aqueous solution.
What is covalent bonding?
Two non-metal atoms are bonded by the sharing of pair(s) of electrons.
They are held together as both nuclei have electrostatic forces
What is metallic bonding?
Bonds formed between metal elements
Metal atoms lose the electrons in their outer shell which become delocalised electrons (this is why metals are good conductors)
The metal ions are held together by the mutual electrostatic attraction towards the delocalised electrons between them
What is the main factor that affects the strength of the metallic bonding in a metal?
The size of charge on the metal ion (and the number of delocalised electrons)
Why would some ionic compounds have a higher melting point than others?
If the ions have a greater charge then the electrostatic forces between them will be stronger, requiring more energy to overcome
Note
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