Relative Atomic Mass Calculations

This section explains how atomic masses are handled in chemical calculations. The relative formula mass concept is introduced for both molecular and ionic compounds.

Highlight: Relative atomic masses are used instead of actual atomic masses due to their extremely small size.

Example: For sodium chloride (NaCl), the relative formula mass is calculated by adding the relative atomic masses of sodium and chlorine.

Vocabulary: Relative formula mass - the sum of all relative atomic masses of atoms shown in a compound's formula.

Solution Concentration

The page explains the fundamental concepts of solutions and concentration calculations.

Definition: A solution is formed when a solute dissolves in a solvent.

Highlight: Concentration measures how crowded solute particles are in a solution.

Example: Concentration can be calculated using the mass of dissolved solute in grams divided by the volume of the solution.

Molar Calculations

This section introduces the concept of moles and their importance in chemical calculations.

Definition: A mole is the standard unit for measuring chemical amounts, used because actual atomic masses are too small for practical calculations.

Highlight: One mole of a substance equals its relative atomic mass (for elements) or relative formula mass (for compounds) in grams.