Nomenclature of Hydrated Salts

The video tutorial explains how to name hydrated salts, which are ionic compounds with water molecules integrated into their crystal structure. It covers the naming conventions for ionic compounds, the structure of hydrates, and how to denote the number of water molecules in both chemical formulas and verbal descriptions. Examples like cobalt(II) chloride hexahydrate and magnesium sulfate heptahydrate are provided. The video also discusses the process of efflorescence, where hydrates lose water molecules, becoming anhydrous salts.

What distinguishes a hydrated salt from a regular ionic compound?

• It contains additional cations.

• It includes water molecules in its crystal structure.

• It has a different anion.

• It is dissolved in water.

How is the chemical formula for a hydrate written?

• By listing the ionic compound followed by a dot and the number of water molecules.

• By adding the word 'hydrate' after the ionic compound.

• By listing the water molecules first, then the ionic compound.

• By using only the name of the ionic compound.

What is the correct name for a compound with the formula CoCl2·6H2O?

• Cobalt chloride hexahydrate

• Cobalt chloride dihydrate

• Cobalt(II) chloride hexahydrate

• Cobalt(II) chloride heptahydrate

What is the process called when a hydrate loses its water molecules?

• Hydration

• Dehydration

• Sublimation

• Efflorescence

Which prefix is used to indicate seven water molecules in a hydrate?

• Deca

• Octa

• Hepta

• Hexa