7 The formation of sodium chloride (NaCl) from sodium (Na) and chlorine (Cl)
8 Note that we don’t have to draw the inner shell electrons anymore! These diagrams are called Lewis structures, Lewis dot diagrams, or electron dot diagrams
9 Name of compound: Sodium chloride Chemical formula: NaCl
10 Ions: cation and anion Ions – charged particles Cation: Metal atoms lose electrons to form positively charged ionsAnion: Non-metal atoms gain electrons to form negatively charged ionsCations (+) and anions (-) attract each other by electrostatic attraction to form ionic compound
11 Cations (+) and anions (-) attract each other by electrostatic attraction in all directions
12 The pattern grows until a giant lattice structure of ions is formed Pure ionic compounds exist as solid crystals
21 Try magnesium + fluorine Determine how many electron(s) magnesium need to lose, therefore the charge of the magnesium ionDetermine how many electron(s) fluorine need to gain, therefore the charge of the fluoride ionDetermine how many of each ions are needed to balance out the positive and negative charges
27 To obtain full outer shells, a magnesium atom must lose 2 electrons, and a fluorine atom must gain 1 electron.
28 Each magnesium atom loses two electrons to form magnesium ion Mg2+ Each fluorine atom gains one electron to form fluoride ion F-
29 Each magnesium atom reacts with two fluorine atoms to form magnesium fluoride with the chemical formular MgF2.
30 Try sodium + oxygenDetermine how many electron(s) sodium need to lose, therefore the charge of the sodium ionDetermine how many electron(s) oxygen need to gain, therefore the charge of the oxide ionDetermine how many of each ions are needed to balance out the positive and negative charges
32 Naming simple ionic compounds Write the name of the metal.Write the name of the nonmetal with the ending changed to –ide.Example:Chlorine = chloride Oxygen = oxideFluorine = fluoride Sulfur = sulfideIodine = iodide Nitrogen = nitrideBromine = bromide Phosphorous = phosphide