|Glossary of Terms|
One commonly used indicator is phenolphthalein, which is colorless in acidic and neutral solutions, but pink in basic solutions.
The strong attractions within ionic solids are responsible for their high melting points. For example, the melting point of the ionic compound sodium chloride, NaCl, is 801 oC.
Ionic bonded solids such as NaCl do not conduct electricity. This is because the electrons in an ionic compound do not move through the ionic structure like that in metallic bonding.However, ionic solids in their liquid state (i.e. when molten), and in aqueous solution conduct electricity.
The smallest unit in ionic compounds is a formula unit as ionic compounds do not exist as discrete entity but as ions.
|1 joule = 1 kg m2s-2 = 4.184 cal|
|K = oC + 273.15|
|K.E. = ½mv2|
|Element||Mass number||Most Abundant Isotope|
|Carbon (atomic mass = 12.011 amu)||
|Copper (atomic mass = 63.546 amu)||
It is the group of elements that are to the left of the diagonal line on the periodic table.
|H2 (g)||2.016 g/mole|
|One mole of an element is NA atoms.|
|One mole of a compound is NA molecules.|