Chapter 5 - Ionic Bonding Flashcards
Give a definition of an ionic bond
The electrostatic forces of attraction between oppositely charged ions
State 4 properties of an ionic compound
-electrical conductivity - when molten or dissolved
-giant ionic lattice
-solubility - can dissolve in polar solvents such as water
-high melting and boiling points
Why do ionic compounds form giant ionic lattices?
Because the oppositely charged ions are strongly attracted in all directions
Why are the melting points higher for lattices containing ions of higher charges?
The ions have a stronger attraction between them
What two factors can affect the melting point of a lattice
The charge of the ions.
The size of the ion
What two factors are required for an ionic compound to be soluble?
- the giant ionic lattice must be broken down
- the water must be attracted to the ions and surround them
Why can’t an ionic compound conduct electricity when solid?
- the ions are fixed in position within the ionic lattice
-Does not have any ions that are free to move and carry charge
Why can an ionic compound conduct electricity when molten or dissolved?
- the ionic lattice is broken down
- the ions are free to move and carry charge
How does the polarity of water contribute to the solubility of ionic compounds?
The slightly negative charge on water is attracted to the positive ion in the giant ionic lattice. And the slightly positive charge on water is attracted to the negative ion in the giant ionic lattice. This means that the water molecules surround the ions and break the giant ionic lattice down
Why do ionic compounds have high melting and boiling points?
large amounts of energy are needed to break the many strong bonds as it is a giant ionic lattice
What states are ionic compounds usually at room temperature?
Solid at room temp
What states are ionic compounds usually at room temperature?
Solid at room temp
