# Ionic Bonds and Structures
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# Nature of the Ionic Bond
4.1.U4
The ionic bond is due to electrostatic attraction between oppositely charged ions.
4.1.U3
The number of electrons lost or gained is determined by the electron configuration of the atom.
4.1.U1
Positive ions (cations) form by metals losing valence electrons.
4.1.U2
Negative ions (anions) form by non-metals gaining electrons.
# Naming Ionic Compounds
4.1.Aims1
Aim 3: Use naming conventions to name ionic compounds.
4.1.AS1
Deduction of the formula and name of an ionic compound from its component ions, including polyatomic ions.
4.1.G1
Students should be familiar with the names of these polyatomic ions: ammonia, hydroxide, nitrate, (bi/hydrogen)carbonate, carbonate, sulphate, phosphate.
# Structure and Properties of Ionic Compounds
# Giant Ionic Lattice
4.1.NoS
Use theories to explain natural phenomena—molten ionic compounds conduct electricity but solid ionic compounds do not. The solubility and melting points of ionic compounds can be used to explain observations. (2.2)
4.1.U5
Under normal conditions, ionic compounds are usually solids with lattice structures.
4.1.AS2
Explanation of the physical properties of ionic compounds (volatility, electrical conductivity and solubility) in terms of their structure.
# Others
4.1.Uz1
Ionic liquids are efficient solvents and electrolytes used in electric power sources and green industrial processes.
# Misc
4.1.ToK1
General rules in chemistry (like the octet rule) often have exceptions. How many exceptions have to exist for a rule to cease to be useful?
4.1.ToK2
What evidence do you have for the existence of ions? What is the difference between direct and indirect evidence?
4.1.Aims2
Aim 6: Students could investigate compounds based on their bond type and properties or obtain sodium chloride by solar evaporation.