Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

2. Atoms and the Periodic Table

Isotopes

GOB Chemistry

2. Atoms and the Periodic Table

Isotopes

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2:04 minutes

Problem 85

Textbook Question

Complete the following table for three of the naturally occurring isotopes of germanium, which is a metalloid used in semiconductor.

Verified step by step guidance

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.

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.

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.