SNC2D1
Date:__________________
Name:_____________________
L6: 5.7 Continued Names and Formulas of Multivalent Ionic Compounds
Recall: Types Of Ionic Compounds
1. _______ (2 elements): There are 2 types: ________ and ___________ metals  ‘simple’ last lesson, now ‘multivalent
2. ___________ (3 or more elements)
Also remember: group 1 elements tend to lose 1 e-  ____________
group 2 elements tend to lose 2 e-  ____ionic charge
group 13 elements tend to lose 3 e-  ____ ionic charge
group 15 elements tend to gain 3 e-  ____ionic charge
group 16 elements tend to gain 2 e-  ____ionic charge
group 17 elements tend to gain 1 e-  ____ionic charge
group 18 elements
 ____________________________
Multiple Ionic Charges / Multivalent
Some metals (transitional metals) don’t follow a pattern like the groups above. Many of these elements have been found to be stable
with _________________ ionic charge (_______________________). For example, iron ions include __________________.
See table 3 on page 198 for more. Also, look at the periodic table in your text. Look for the ionic charges on the elements (top
right). Notice some metals have more than one charge shown.
Since these elements have multiple charges, the charge must be shown in the ___________ of the ions. This is shown with _______
___________. For example, Fe2+ is written as Iron (II) and Fe3+ is written as _______________.
Writing the Chemical Formula for Multivalent Ionic Compounds
Use the cross down method to write the formula of the compound as done with simple ionic compounds.
Practice 1: Write the chemical formula for
a) lead (IV) nitride.
b) copper (II) chloride
Question: What is the charge on each compound above? Draw the compound to prove this.
Naming Multivalent Ionic Compounds
To write the names of the compound (which must include the roman numerals), use the charges and number of atoms given and set
it equal to zero. Let ‘___’ be the charge of the multivalent ion. Then solve for ____.
For example, Mn3P4 has 3 cations (of charge ‘x’) and 4 anions (of charge -3). The total charge must be zero. Setting up an equation:
Practice 2: Write the name for
a) Fe2S3
b) SnO2
Homework: Read Section 5.7, complete p.200 # 2 – 7,9 and complete worksheet Ionic Names and Formulas