Domanda del libro di testo
The element argon has three naturally occurring isotopes, with 18, 20, and 22 neutrons in the nucleus, respectively. (a) Write the full chemical symbols for these three isotopes.
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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 95
The element chromium (Cr) consists of four naturally occurring isotopes with atomic masses 49.9460, 51.9405, 52.9407, and 53.9389 u. The relative abundances of these four isotopes are 4.3, 83.8, 9.5, and 2.4%, respectively. From these data, calculate the atomic weight of chromium.
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Identify the isotopes of chromium and their respective atomic masses: 49.9460 u, 51.9405 u, 52.9407 u, and 53.9389 u.
Identify the relative abundances of each isotope: 4.3%, 83.8%, 9.5%, and 2.4%.
Convert the percentage abundances into decimal form by dividing each by 100: 0.043, 0.838, 0.095, and 0.024.
Calculate the contribution of each isotope to the atomic weight by multiplying the atomic mass of each isotope by its decimal abundance: (49.9460 u * 0.043), (51.9405 u * 0.838), (52.9407 u * 0.095), (53.9389 u * 0.024).
Sum the contributions from all isotopes to find the atomic weight of chromium.
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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 example, chromium has four isotopes, each with a unique atomic mass, which contributes to the element's average atomic weight based on their relative abundances.
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04:36
Isotopes
Relative Abundance
Relative abundance refers to the proportion of each isotope of an element present in a sample, usually expressed as a percentage. In the case of chromium, the isotopes have specific relative abundances that must be considered when calculating the weighted average atomic mass of the element.
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5:41Calculating Abundance Example
Weighted Average
The weighted average is a calculation that takes into account the different weights (or contributions) of each component in a dataset. To find the atomic weight of chromium, the atomic masses of its isotopes are multiplied by their respective relative abundances, and the results are summed and divided by 100 to yield the average atomic weight.
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02:03Average Rate of Reaction
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Domanda del libro di testo
The nucleus of 6Li is a powerful absorber of neutrons. It exists in the naturally occurring metal to the extent of 7.5%. In the era of nuclear deterrence, large quantities of lithium were processed to remove 6Li for use in hydrogen bomb production. The lithium metal remaining after removal of 6Li was sold on the market. (b) The atomic masses of 6Li and 7Li are 6.015122 and 7.016004 u, respectively. A sample of lithium depleted in the lighter isotope was found on analysis to contain 1.442% 6Li. What is the average atomic weight of this sample of the metal?
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Domanda del libro di testo
Copper (Cu) consists of two naturally occurring isotopes with masses of 62.9296 and 64.9278 u. (a) How many protons and neutrons are in the nucleus of each isotope? Write the complete atomic symbol for each, showing the atomic number and mass number. (b) The average atomic mass of Cu is 63.55 u. Calculate the abundance of each isotope.
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Domanda del libro di testo
There are two different isotopes of bromine atoms. Under normal conditions, elemental bromine consists of Br2 molecules, and the mass of a Br2 molecule is the sum of the masses of the two atoms in the molecule. The mass spectrum of Br2 consists of three peaks: Mass (u) Relative Size 157.836 0.2569 159.834 0.4999 161.832 0.2431 (a) What is the origin of each peak (of what isotopes does each consist)?
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