1. What is Atomic Mass?

Atomic mass is the weighted average mass of all naturally occurring isotopes of an element, taking into account their relative abundances. It represents the average mass of atoms in a given sample of the element.

2. How to Calculate Atomic Mass?

The atomic mass is calculated using the formula:

Where:

• \( \text{Isotope Mass} \) — Mass of each isotope in atomic mass units (u)
• \( \% \text{Abundance} \) — Natural abundance percentage of each isotope
• \( \sum \) — Summation of all isotope contributions

Explanation: The formula calculates a weighted average where more abundant isotopes contribute more significantly to the overall atomic mass.

3. Importance of Atomic Mass Calculation

Details: Atomic mass is crucial for chemical calculations, stoichiometry, determining molecular weights, and understanding chemical reactions. It's fundamental in chemistry, physics, and materials science.

4. Using the Calculator

Tips: Enter the mass and abundance percentage for each isotope. Ensure the total abundance equals 100% for accurate results. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What is the difference between atomic mass and atomic weight?
A: Atomic mass refers to the mass of a single atom, while atomic weight is the weighted average of all naturally occurring isotopes' masses.

Q2: Why is atomic mass not a whole number?
A: Atomic mass is a weighted average of different isotopes with different masses, so it's rarely a whole number.

Q3: How many isotopes can I calculate with this calculator?
A: This calculator handles two isotopes. For more isotopes, you would need to extend the calculation manually.

Q4: What units are used for atomic mass?
A: Atomic mass is typically measured in atomic mass units (u) or daltons (Da), where 1 u = 1.66053906660 × 10⁻²⁷ kg.

Q5: Why do isotopes have different masses?
A: Isotopes have the same number of protons but different numbers of neutrons, resulting in different atomic masses.