Topic 2 Flashcards
Ions are formed when…
Electrons are transferred from one atom to another
Ionic bonding
Electrostatic attraction holds positive and negative ions together
Definition
An ionic bond is the strong electrostatic attraction between two oppositely charged ions
What affects the ionic bonding
Ionic charges
The greater the charge on an ion the stronger the ionic bond and therefore the higher the melting/boiling point
Ionic Radii
Small ions can pack closer together than large ions. Electrostatic attractions get weaker with distance so smaller closely packed ions have stronger ionic bonding the large ions therefore they have large melting and boiling points
Covalent bond is
Two atoms that share a pair of electrons
Dative covalent bonding
One atom donate space electrons to a bond
Shape of molecules
Molecular shade depends on electron pairs around the central atom
Electronegativity define it
The ability of an atom to attract the bonding electrons in a covalent bond
Fluorine is the most electronegative element
A polar molecule…
Has an overall dipole which is just a dipole caused by the presence of a permanent charge across the molecule
There are three types of intermolecular forces
London forces
Permanent dipole dipole bonds
Hydrogen bonding
London forces
Electrons in charge clouds are always moving really quickly. At any particular moment the electrons in an atom are likely to be more on one side than the other this means the atom would have a temporary dipole. This induces another temporary dipole in the opposite direction on a neighbouring atom
For one substance to dissolve in another all of these have to happen
Bones in the substance have to break
Bones in the solvent have to break
Newborns have to form between the substance and the solvent
Substances will only dissolve…
If the strength of the new bond formed is the same or greater than the strength of the bond that is broken
Ionic substances dissolved in
Polar solvents such as water
Alcohols dissolve in
Polar solvents like water
Nonpolar substances dissolve in
Nonpolar solvents