Textbook Question
Use Rutherford's gold-foil experiment to answer each of the following:
c. How did he use the results to propose a model of the atom?
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Ch.4 Atoms and Elements
Timberlake14thChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249
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Table of contents
- Ch.1 Chemistry in Our Lives19
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy53
- Ch.4 Atoms and Elements58
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions38
- Ch.8 Gases30
- Ch.9 Solutions50
- Ch.10 Acids and Bases and Equilibrium64
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons77
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones82
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides91
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis86
- Ch.18 Metabolic Pathways and ATP Production73
Timberlake14thChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Not the one you use?Change textbook
Chapter 4, Problem 83c
Consider the following atoms in which X represents the chemical symbol of the element:
168X 169X 1810X 178X 188X
c. Which atoms have the same mass number?
Verified step by step guidance1
Step 1: Understand the concept of mass number. The mass number is the sum of protons and neutrons in the nucleus of an atom. It is represented as the superscript number before the chemical symbol (e.g., ¹¹⁵X).
Step 2: Analyze the given atoms. Each atom is represented with its mass number (superscript) and atomic number (subscript). For example, ¹¹⁵₄₉X has a mass number of 115 and an atomic number of 49.
Step 3: Compare the mass numbers of the given atoms. Look for atoms that have the same superscript value, as this indicates they have the same mass number.
Step 4: Identify the atoms with the same mass number. From the image, the atoms ¹¹⁵₄₉X, ¹¹⁵₄₆X, and ¹¹⁵₅₀X all have a mass number of 115.
Step 5: Conclude that the atoms with the same mass number are isotopes of different elements, as they have the same number of nucleons but different atomic numbers.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Mass Number
The mass number of an atom is the total number of protons and neutrons in its nucleus. It is represented as the upper left number in the atomic notation (e.g., ¹⁶ in ¹⁶₈X). Atoms with the same mass number have the same total number of nucleons, which can indicate they are isotopes of the same element.
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Mass Percent Example
Isotopes
Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons, resulting in different mass numbers. For example, the isotopes of element X in the question include ¹⁶₈X and ¹⁸₁₀X, which have different mass numbers but belong to the same element.
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Atomic Number
The atomic number of an element is the number of protons in the nucleus of an atom, which determines the element's identity. It is represented as the lower left number in the atomic notation (e.g., ₈ in ¹⁶₈X). Atoms with the same atomic number are the same element, while differing atomic numbers indicate different elements.
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Related Practice
Textbook Question
Match the subatomic particles (1 to 3) to each of the descriptions below:
1. protons
2. neutrons
3. electrons
b. surround the nucleus
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Textbook Question
Consider the following atoms in which X represents the chemical symbol of the element:
168X 169X 1810X 178X 188X
a. What atoms have the same number of protons?
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Textbook Question
Consider the following atoms in which X represents the chemical symbol of the element:
168X 169X 1810X 178X 188X
d. What atoms have the same number of neutrons?
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Textbook Question
Complete the following table for three of the naturally occurring isotopes of germanium, which is a metalloid used in semiconductor.
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Textbook Question
Complete the following table for the three naturally occurring isotopes of silicon, the major component in computer chips:
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