Module 5 Flashcards
(A whole lotta naming conventions)
Ions
Atoms / Groups of atoms that have gained or lost a electron (Net positive or net negative charge)
Cations (Ion)
A positively charged Ion (Lost electrons)
Anions
Negatively charged Ion (Gained electrons)
Monatomic Ions
When a single atom gained or lost a electron
Ex. Hydrogen
Binary Ionic Compound
When a metal atom combines with a nonmetal
Metal atom transfers the electron
Metals are Cations , Non-Metals are Anions
Chemical formula of Binary Ionic compounds
Must be neutral overall (Positive = Negative)
Add however many of the atom you need till they are balanced
Ex Al = -2, O = +3 , Al3O2 is the formula
Determining Ion Charges
Transition metals very in charge
Comparing it to a Known charge is the easiest way to figure it out
Ex FeCl3, Clorine has a charge -1 , Iron (Fe) would have a charge of +3 to match the amount of Chlorine
Polyatomic Ions
Bounded atoms that have a net charge (+ or -)
Most are anions
NH4^+ is one of the only cations
Chemical formulas of Ionic compounds with polyatomic ions
Use the lest amount to balance out the charges
Enclose the Polyatomic in parentheses
Write subscript outside parentheses
Ionic Compound Name
There are two ways to go about naming them based on if they are
Polyatomic (set charge) or Monatomic
(Constant / variable)
Monatomic metal cations naming (Constant)
Take the element in group 1 / 2 + ion
Hydrogen Ion etc
Monatomic metal cations with variable
Metal ions from groups 3 to 12
Use the element name + Roman numeral to indicate charge
Monatomic Anions
Groups 13 - 17, non metal. They have a constant charge
Use the element name + change ending to -ide
Polyatomic Anions Name
Blunt memorize , all In the same series have the same charge
There is 4 naming conventions
Per_ate (Halogens with 4 Oxygen),
Hypo_ite, _ate, _ite
CLO4 ^ -1
Perchlorate
CLO3 ^ -1
Chlorate
