Textbook Question
For each representation of a nucleus A through E, write the atomic symbol and identify which are isotopes.
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Ch.4 Atoms and Elements
Timberlake14th EditionChemistry: 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
Timberlake14th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Not the one you use?Change textbook
Chapter 4, Problem 85
Complete the following table for three of the naturally occurring isotopes of germanium, which is a metalloid used in semiconductor.
Verified step by step guidance1
Step 1: Identify the atomic number of germanium (Ge) from the periodic table. The atomic number is 32, which represents the number of protons in the nucleus of the atom.
Step 2: For each isotope, note the mass number provided in the table (70, 73, and 76). The mass number is the sum of protons and neutrons in the nucleus.
Step 3: Calculate the number of neutrons for each isotope using the formula: \( \text{Number of Neutrons} = \text{Mass Number} - \text{Atomic Number} \). For example, for \( ^{70}_{32} \text{Ge} \), \( \text{Number of Neutrons} = 70 - 32 \). Repeat for \( ^{73}_{32} \text{Ge} \) and \( ^{76}_{32} \text{Ge} \).
Step 4: Determine the number of electrons for each isotope. Since germanium is neutral in its elemental form, the number of electrons equals the atomic number (32).
Step 5: Fill in the table with the calculated values for atomic number, mass number, number of protons, number of neutrons, and number of electrons for each 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 chemical element that have the same number of protons but different numbers of neutrons. This results in different mass numbers for the isotopes. For example, germanium has several isotopes, including 70Ge, 73Ge, and 76Ge, each differing in their neutron count while maintaining the same atomic number of 32.
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Isotopes
Atomic Number and Mass Number
The atomic number of an element is the number of protons in its nucleus, which determines the element's identity. The mass number is the total number of protons and neutrons in the nucleus. For germanium isotopes, the atomic number is always 32, while the mass number varies among the isotopes, reflecting their different neutron counts.
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Subatomic Particles
Subatomic particles include protons, neutrons, and electrons, which make up atoms. Protons are positively charged and found in the nucleus, neutrons are neutral and also located in the nucleus, while electrons are negatively charged and orbit the nucleus. The number of protons defines the element, while the number of neutrons affects the isotope and its stability.
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Related Practice
Textbook Question
Complete the following statements:
a. The atomic number gives the number of _____ in the nucleus.
Textbook Question
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?
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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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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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