Textbook Question
Determine the number of protons and the number of neutrons in each isotope. a. 4019K b. 22688Ra c. 9943Tc d. 3315P
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Ch.2 - Atoms & Elements
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- 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
Chapter 2, Problem 57a
Determine the number of protons and the number of neutrons in each isotope. a. 147N
Verified step by step guidance1
Step 1: Identify the atomic number and mass number. In the isotope notation, the lower number is the atomic number (Z) and the upper number is the mass number (A). In this case, for the isotope 14 7N, 7 is the atomic number and 14 is the mass number.
Step 2: Determine the number of protons. The atomic number (Z) is equal to the number of protons in an atom. Therefore, the number of protons in this isotope is 7.
Step 3: Determine the number of neutrons. The number of neutrons in an atom can be found by subtracting the atomic number (Z) from the mass number (A). Therefore, the number of neutrons in this isotope is 14 - 7.
Step 4: Check your results. The sum of the number of protons and the number of neutrons should equal the mass number. In this case, 7 (protons) + 7 (neutrons) = 14, which is the mass number of the isotope.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Isotopes
Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This means they share the same atomic number but have different mass numbers. For example, nitrogen has several isotopes, including nitrogen-14, which has 7 protons and 7 neutrons.
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Isotopes
Atomic Number
The atomic number of an element is the number of protons found in the nucleus of its atoms. It uniquely identifies an element and determines its position in the periodic table. In the case of nitrogen (N), the atomic number is 7, indicating that all nitrogen atoms have 7 protons.
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Mass Number
The mass number of an isotope is the total number of protons and neutrons in its nucleus. It is represented as the sum of these particles and is used to distinguish between different isotopes of the same element. For nitrogen-14, the mass number is 14, which is the sum of its 7 protons and 7 neutrons.
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Related Practice
Textbook Question
Write isotopic symbols in the form AZX for each isotope. a. the nickel isotope with 32 neutrons
Textbook Question
Write isotopic symbols in the form AZX for each isotope. b. the iron isotope with 30 neutrons
Textbook Question
Write isotopic symbols in the form AZX for each isotope. c. the rubidium isotope with 45 neutrons
Textbook Question
Determine the number of protons and the number of neutrons in each isotope. d. 20882Pb
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