Understanding Ionic Compounds and Formula Mass

The video tutorial explains ionic compounds, which are made of ions, and their formation, typically from metals and non-metals. It uses sodium chloride as a primary example to illustrate the concept. The tutorial also introduces the idea of a formula unit, the simplest combination of ions in a compound, and explains formula mass, which compares the mass of a formula unit to a carbon-12 atom.

What are ionic compounds primarily composed of?

• Molecules

• Ions

• Electrons

• Atoms

Which of the following is an exception to the typical metal and non-metal composition of ionic compounds?

• Sodium chloride

• Potassium chloride

• Ammonium chloride

• Calcium chloride

What type of force holds the ions together in an ionic compound?

• Nuclear force

• Magnetic force

• Gravitational force

• Electrostatic force

In an ionic compound, what is the overall charge?

• Positive

• Negative

• Zero

• Variable

What is the simplest unit of an ionic compound called?

• Ion pair

• Atom

• Molecule

• Formula unit

How is a formula unit different from a molecule?

• It is only found in covalent compounds

• It contains more atoms than a molecule

• It is the smallest ratio of ions in an ionic compound

• It is larger than a molecule

What is the term used for the mass of a formula unit in ionic compounds?

• Molecular mass

• Atomic mass

• Formula mass

• Ionic mass

Why is the term 'formula mass' used instead of 'molecular mass' for ionic compounds?

• Because it is easier to calculate

• Because it is used for all types of compounds

• Because it is a more modern term

• Because ionic compounds do not have molecules

What is the reference atom used for comparing formula mass?

• Carbon-12

• Nitrogen-14

• Oxygen-16

• Hydrogen-1

Which of the following best describes the concept of formula mass?

• The relative mass of a formula unit compared to carbon-12

• The total mass of all ions in a compound

• The mass of a molecule

• The mass of a single atom