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Chapter 2: Problem 17

What fraction or percentage of carbon atoms has a mass of \(12.011\) amu?

Short Answer

Expert verified
Nearly all -- or approximately \(98.93\%\) -- of carbon atoms have a mass of \(12.011\) amu.

Step by step solution

01

Understand the Nature of Carbon Isotopes

Recognize that naturally occurring carbon is a mixture of isotopes. The most common isotope is Carbon-12, which accounts for the vast majority of all carbon found on earth.
02

Identify the Mass of the Given Isotope

Recognize that the given atomic mass unit (amu) of \(12.011\) matches the atomic mass of the most common carbon isotope, Carbon-12.
03

Calculate the Fraction

Given that Carbon-12 makes up about 98.93% of naturally occurring carbon, virtually all carbon atoms you encounter will have a mass of \(12.011\) amu. Therefore, the fraction is nearly 1 (or \(100\%\) if expressed as a percentage) of carbon atoms that have this mass.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Atomic Mass Unit
Atoms have incredibly small masses, so scientists use the atomic mass unit (amu) to express them in a more manageable way. One amu is equivalent to one-twelfth the mass of a Carbon-12 atom. This unit makes it easier to relate the masses of different atoms to one another.
  • An amu is a standard way to quantify an atom's mass.
  • It simplifies calculations that compare different atoms and isotopes.
Understanding amu is essential for grasping the scale and measurement of atomic masses in chemistry.
Carbon-12
Carbon-12 is the most prevalent isotope of carbon, comprising nearly all naturally found carbon. Its nucleus contains six protons and six neutrons.
  • This isotope serves as the benchmark for defining the atomic mass unit.
  • The atomic mass of Carbon-12 is exactly 12 amu.
The significance of Carbon-12 lies in its stability and abundance, making it a key reference point for atomic mass measurements.
Naturally Occurring Carbon
Carbon found on Earth is a mixture of isotopes, predominantly Carbon-12 and a small percentage of other isotopes like Carbon-13 and Carbon-14.
  • Carbon-12 accounts for about 98.93% of natural carbon.
  • Carbon-13 is about 1.07%, while Carbon-14 is found in trace amounts.
This natural isotopic distribution is crucial for understanding the chemical properties of carbon and its role in various environmental and biological processes.
Isotope Fractions
Isotope fractions refer to the distribution percentages of different isotopes of an element within a sample. For carbon, the fraction of each isotope is a key factor in calculating the average atomic mass.
  • Carbon-12 constitutes the majority fraction due to its abundance.
  • Knowing these fractions allows for precise measurements and predictions in chemical reactions and carbon dating processes.
The concept of isotope fractions underscores the diversity in atomic mass found even within a single element.

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Most popular questions from this chapter

If you select one carbon atom at random, the mass of that atom is most likely to be____ amu.

Describe what all isotopes of magnesium have in common and also how they are different.

Examine the periodic table and find the symbol for magnesium. a) How does the number given just below the symbol for magnesium (rounded to two decimal places) compare with the average mass (in amu) of one magnesium atom? b) How does the number given just below the symbol for magnesium (rounded to two decimal places) compare with the mass (in grams) of \(6.022 \times 10^{23}\) magnesium atoms?

For a large collection of (randomly selected) magnesium atoms: a) What is the average atomic mass of magnesium, \(\mathrm{Mg}\), in amu? b) What is the average mass of a Mg atom in grams? Show your work.

What is the mass (in amu) of a) \(1000^{12} \mathrm{C}\) atoms? b) \(1000^{13} \mathrm{C}\) atoms?
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