Domanda del libro di testo
(a) What isotope is used as the standard in establishing the atomic mass scale?
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Ch.2 - Atoms, Molecules, and Ions
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 2, Problema 34b
(b) Why is the atomic weight of carbon reported as 12.011 in the table of elements and the periodic table in the front inside cover of this text?
Guida verificata passo dopo passo1
Understand that the atomic weight of an element is a weighted average of the masses of its isotopes.
Recognize that carbon has two stable isotopes: Carbon-12 and Carbon-13.
Carbon-12 is the most abundant isotope, making up about 98.89% of carbon found in nature, while Carbon-13 makes up about 1.11%.
The atomic weight of carbon (12.011) reflects the average mass of these isotopes, weighted by their natural abundance.
The calculation involves multiplying the mass of each isotope by its relative abundance and summing these values to get the average atomic weight.
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Atomic Weight
Atomic weight, or atomic mass, is the weighted average mass of an element's isotopes, measured in atomic mass units (amu). It reflects the relative abundance of each isotope in nature, which is why it is not always a whole number. For carbon, the atomic weight of 12.011 accounts for the presence of both carbon-12 and carbon-13 isotopes.
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02:10
Atom Structure
Isotopes
Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses. For carbon, the most common isotopes are carbon-12 (with 6 neutrons) and carbon-13 (with 7 neutrons). The existence of these isotopes contributes to the average atomic weight reported in the periodic table.
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04:36Isotopes
Relative Abundance
Relative abundance refers to the proportion of each isotope of an element found in a natural sample. This concept is crucial for calculating the atomic weight, as it determines how much each isotope contributes to the overall average. For carbon, the relative abundance of carbon-12 and carbon-13 influences the reported atomic weight of 12.011.
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5:41Calculating Abundance Example
Pratica correlata
Domanda del libro di testo
(b) The atomic weight of boron is reported as 10.81, yet no atom of boron has the mass of 10.81 u. Explain.
Domanda del libro di testo
Rubidium has two naturally occurring isotopes, rubidium-85 (atomic mass = 84.9118 amu; abundance = 72.15%) and rubidium-87 (atomic mass = 86.9092 amu; abundance = 27.85%). Calculate the atomic weight of rubidium
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Domanda del libro di testo
(a) What is the mass in u of a carbon-12 atom?
Domanda del libro di testo
Only two isotopes of copper occur naturally: 63Cu (atomic mass = 62.9296 amu; abundance 69.17%) 65Cu (atomic mass = 64.9278 amu; abundance 30.83%). Calculate the atomic weight (average atomic mass) of copper.
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