1. Explain relative atomic mass and average atomic mass? 2. Define a mole (in chemistry) 3. How to illustrate Avogadro’s number with examples? 4. How to determine the molar mass of elements and compounds?
Answer (1)
Answer:1. **Relative Atomic Mass**: The weighted average mass of an atom compared to carbon-12. **Average Atomic Mass**: The weighted average of all isotopes' atomic masses, reflecting their natural abundances.2. **Mole**: A unit representing \(6.022 \times 10^{23}\) particles (atoms, molecules, etc.) of a substance.3. **Avogadro’s Number**: Represents \(6.022 \times 10^{23}\) particles. For example, one mole of water contains \(6.022 \times 10^{23}\) water molecules.4. **Molar Mass**: For elements, it's the atomic mass in grams per mole. For compounds, sum the molar masses of all atoms in the formula. For example, water has a molar mass of 18 g/mol.
