Prior to 1961, the atomic mass unit (amu) was defined as 1/16 the mass of the atomic weight of oxygen; that is, the atomic weight of oxygen was defined as exactly 16. What was the mass of a 12C atom prior to 1961 if the atomic weight of oxygen on today's scale is 15.9994?

Verified step by step guidance

1. Understand the definition of atomic mass unit (amu) prior to 1961, which was 1/16 the mass of the atomic weight of oxygen, with oxygen defined as exactly 16 amu.
2. Recognize that the atomic weight of oxygen today is 15.9994. Calculate the conversion factor between the old scale and the new scale by dividing the old atomic weight of oxygen (16 amu) by the current atomic weight (15.9994 amu).
3. Apply the conversion factor to the current atomic mass of a 12C atom, which is exactly 12 amu on today's scale, to find its mass on the old scale.
4. Multiply the current atomic mass of 12C (12 amu) by the conversion factor to adjust it to the scale used prior to 1961.
5. The result from the previous step gives the mass of a 12C atom in amu according to the old definition based on oxygen's atomic weight.

Key Concepts

Atomic Mass Unit (amu)

The 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 (12C) atom, which is approximately 1.66053906660 x 10^-27 kg. This unit allows chemists to express atomic and molecular weights in a more manageable form, facilitating comparisons between different elements and compounds.

Relative Atomic Mass

Relative atomic mass is a dimensionless quantity that represents the average mass of an atom of an element compared to 1/12 the mass of a carbon-12 atom. It reflects the weighted average of the isotopes of an element based on their natural abundance. This concept is crucial for understanding how atomic weights are determined and how they relate to the mass of individual atoms.

Historical Definition of Atomic Weight

Prior to 1961, the atomic weight of oxygen was defined as exactly 16, which established a reference point for the atomic mass unit. This historical definition influenced the calculation of atomic weights for other elements based on their mass ratios to oxygen. Understanding this context is essential for interpreting how atomic weights have evolved and how they are used in modern chemistry.