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What is the edge length (in cm) of a titanium cube that contains 2.55 * 1024 titanium atoms? The density of titanium is 4.50 g/cm3.
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Ch.2 - Atoms & Elements
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Capitolo 2, Problema 127
Lithium has only two naturally occurring isotopes. The mass of lithium-6 is 6.01512 amu and the mass of lithium-7 is 7.01601 amu. Calculate the relative abundances of the two isotopes.
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Identify the given masses of the isotopes: lithium-6 has a mass of 6.01512 amu, and lithium-7 has a mass of 7.01601 amu.
Let the abundance of lithium-6 be represented as x, and the abundance of lithium-7 be represented as 1-x, since the total abundance must sum to 100%.
Use the average atomic mass of lithium from the periodic table, which is approximately 6.94 amu, to set up the equation: (6.01512 * x) + (7.01601 * (1-x)) = 6.94.
Solve the equation for x to find the abundance of lithium-6. This involves simplifying the equation and isolating x.
Substitute the value of x back into the expression for the abundance of lithium-7 (1-x) to find its abundance.
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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 lithium, the two isotopes are lithium-6 and lithium-7, which have 3 protons each but differ in their neutron count (3 and 4, respectively). Understanding isotopes is crucial for calculations involving atomic mass and relative abundance.
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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. To calculate the relative abundances of isotopes, one can use the weighted average of their masses and the known average atomic mass of the element. This concept is essential for determining how much of each isotope contributes to the overall atomic mass.
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5:41Calculating Abundance Example
Weighted Average
A weighted average is a mean that takes into account the relative importance or frequency of each value in a dataset. In the context of isotopes, the weighted average of the isotopes' masses is calculated using their relative abundances. This method allows for the determination of the average atomic mass of an element, which is critical for understanding its isotopic composition.
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02:03Average Rate of Reaction
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Naturally occurring chlorine is composed of two isotopes: 75.76% Cl-35 (mass 34.9688 amu) and 24.24% Cl-37 (mass 36.9659 amu). Naturally occurring oxygen is composed of three isotopes: 99.757% O-16 (mass 15.9949 amu), 0.038% O-17 (mass 16.9991 amu), and 0.205% O-18 (mass 17.9991 amu). The compound dichlorine monoxide is composed of two chlorine atoms and one oxygen atom bonded together to form the Cl2O molecule. How many Cl2O molecules of different masses naturally exist? Give the masses of the three most abundant Cl2O molecules.
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A 67.2 g sample of a gold and palladium alloy contains 2.49×1023 atoms. What is the composition (by mass) of the alloy?
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Boron has only two naturally occurring isotopes. The mass of boron-10 is 10.01294 amu and the mass of boron-11 is 11.00931 amu. Calculate the relative abundances of the two isotopes.
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Common brass is a copper and zinc alloy containing 37.0% zinc by mass and having a density of 8.48 g/cm3. A fitting composed of common brass has a total volume of 112.5 cm3. How many atoms (copper and zinc) does the fitting contain?
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