Variable Charge Cations and Naming Compounds

The video lesson by Mr. Post covers the concept of variable charge cations and their naming in ionic compounds. It explains how the naming of ionic compounds changes when dealing with ions that have more than one charge, known as variable charged cations. The lesson discusses the periodic table, focusing on the d block where these cations are found, and introduces the use of Roman numerals to indicate the charge of such cations in compound names. The video also provides examples and solutions to illustrate the naming process.

What is the main focus of the lesson introduced by Mr. Post?

• Naming ionic compounds with single charge cations

• Understanding the periodic table

• Naming ionic compounds with variable charge cations

• Learning about covalent bonds

What charge does group one elements typically have on the periodic table?

• 3-

• 2+

• 1+

• 0

Why are elements in the middle of the periodic table called variable charge cations?

• They are non-metals

• They have no charge

• They have more than one possible charge

• They have a fixed charge

Which of the following is an example of a variable charge cation?

• Copper

• Helium

• Oxygen

• Sodium

How is the suffix of the non-metal changed in traditional naming of ionic compounds?

• It is replaced with 'ate'

• It is replaced with 'ide'

• It is replaced with 'ite'

• It remains unchanged

What is added to the name of a compound to indicate the charge of a variable charge cation?

• A prefix

• A suffix

• Roman numerals in parentheses

• A subscript

In the example of copper oxide, what charge does copper have when written as copper(IV) oxide?

• 2+

• 1+

• 4+

• 3+

What is the charge on phosphorus when it forms a compound with gold?

• 1-

• 4-

• 2-

• 3-

How is nickel phosphide named when nickel has a 3+ charge?

• Nickel(IV) phosphide

• Nickel(II) phosphide

• Nickel phosphide

• Nickel(III) phosphide

What is the purpose of using Roman numerals in naming compounds with variable charge cations?

• To indicate the number of atoms

• To show the type of bond

• To specify the charge of the cation

• To denote the compound's state