Find the mass in atomic mass units of the following: a. 1 O atom, with a mass of 2.66 * 10^-23 g b. 1 Br atom, with a mass of 1.31 * 10^-22 g

Verified step by step guidance

1. Identify the conversion factor between grams and atomic mass units (amu). 1 amu is defined as 1/12 the mass of a carbon-12 atom, which is approximately 1.66 \times 10^{-24} g.
2. For part (a), calculate the mass of 1 O atom in amu by dividing its mass in grams by the conversion factor: $\text{mass in amu}=\frac{2.66\times {10}^{-23}\text{ g}}{1.66\times {10}^{-24}\text{ g/amu}}$.
3. For part (b), calculate the mass of 1 Br atom in amu by dividing its mass in grams by the conversion factor: $\text{mass in amu}=\frac{1.31\times {10}^{-22}\text{ g}}{1.66\times {10}^{-24}\text{ g/amu}}$.
4. Ensure that the units cancel appropriately, leaving the result in atomic mass units (amu).
5. Interpret the results to understand the relative mass of the atoms in atomic mass units, which is a more convenient unit for atomic-scale measurements.

Key Concepts

Atomic Mass Unit (amu)

An atomic mass unit (amu) is a standard unit of mass that quantifies mass on an atomic or molecular scale. It is defined as one twelfth of the mass of a carbon-12 atom, approximately 1.66 x 10^-24 grams. This unit is essential for comparing the masses of different atoms and molecules, allowing for easier calculations in chemistry.

Conversion from grams to amu

To convert the mass of an atom from grams to atomic mass units, one must use the conversion factor that 1 amu is equivalent to 1.66 x 10^-24 grams. This involves dividing the mass in grams by this conversion factor, which provides the mass in amu. This process is crucial for accurately determining the mass of individual atoms in a format commonly used in chemistry.

Mass of Elements

The mass of elements, such as oxygen (O) and bromine (Br), varies based on their atomic structure, specifically the number of protons and neutrons in their nuclei. Understanding the mass of these elements is fundamental in stoichiometry and chemical reactions, as it influences calculations involving moles, molecular weight, and the behavior of substances in reactions.