calcium chloride Ca Cl calcium chloride ee Ca

calcium chloride Ca Cl

calcium chloride ee- Ca Cl +2 Ca is an atom that loses 2 electrons

calcium chloride e- e- e- -1 Cl is an atom that gains 1 electron Ca Cl +2 The same amount of electrons lost by Ca has to be gained by Cl

calcium chloride e- e- -2 Ca Cl 2 +2 So two Cls are needed to accept Ca’s 2 electrons

In ALL ionic compounds, the positive charge will equal the negative charge +2 = -2 Ca. Cl 2 calcium chloride

Writing formulas is a 3 step process: Example: calcium chloride 1. Write the symbols of the elements. Ca Cl 2. Put in the charges. Ca+2 Cl-1 3. Change the amount of the ions to make the charges cancel out. Ca. Cl 2

Magnesium nitrate 0 +2 -1 Mg NO 3 3. 1. Change thein amount of each ion Write the formula of 2. Put the charges to make the charges cancel out

Magnesium nitrate +2 -1 -2 Mg(NO 3)2

Magnesium nitrate Answer: Mg(NO 3)2

iron(II)bromide +2 Fe Br 2 -2 -1 Metals that have more than one possible charge have a Roman numeral after them to let you know its positive charge.

iron(II)bromide Fe. Br 2

aluminum hydroxide +3 -1 Al OH

aluminum hydroxide +3 -1 Al(OH)3

aluminum hydroxide Al(OH)3

Example: calcium sulfide +2 -2 Ca. S

Example: calcium sulfide Ca. S

Example: potassium phosphide +1 K 3 P -3

Example: potassium phosphide K 3 P

Example: strontium nitride +6 +2 -6 -3 Sr 3 N 2

Example: strontium nitride Sr 3 N 2

Example: iron(II) oxide +2 -2 Fe. O

Example: iron(II) oxide Fe. O

Example: iron(III) oxide +6 +3 -6 -2 Fe 2 O 3

Example: iron(III) oxide Fe 2 O 3

Example: dinitrogen trioxide N 2 O 3

All ionic compounds are arrangements of ions in a 3 -D structure known as a crystal lattice. Cl- Na+ This is the Na. Cl crystal lattice