Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Atomic Structure

Organic Chemistry

1. A Review of General Chemistry

Atomic Structure

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3:24 minutes

Problem 1a

Textbook Question

Oxygen has three isotopes, ¹⁶O, ¹⁷O, and ¹⁸O. The atomic number of oxygen is 8. How many protons and neutrons does each of the isotopes have?

Verified step by step guidance

Step 1: Recall that the atomic number of an element represents the number of protons in its nucleus. For oxygen, the atomic number is 8, so all isotopes of oxygen have 8 protons.

Step 2: Understand that the mass number of an isotope is the sum of its protons and neutrons. For example, the mass number of O¹⁶ is 16, O¹⁷ is 17, and O¹⁸ is 18.

Step 3: To calculate the number of neutrons in each isotope, subtract the atomic number (number of protons) from the mass number. Use the formula:

n = A - Z

, where

n

is the number of neutrons,

A

is the mass number, and

Z

is the atomic number.

Step 4: For O¹⁶, calculate the neutrons as

16 - 8 = 8

. For O¹⁷, calculate the neutrons as

17 - 8 = 9

. For O¹⁸, calculate the neutrons as

18 - 8 = 10

Step 5: Summarize the results: All isotopes of oxygen have 8 protons. O¹⁶ has 8 neutrons, O¹⁷ has 9 neutrons, and O¹⁸ has 10 neutrons.

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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 atomic masses for the isotopes. For example, oxygen has three isotopes: O-16, O-17, and O-18, which differ in their neutron count while maintaining the same atomic number.

Atomic Number

The atomic number of an element is defined as the number of protons found in the nucleus of its atoms. For oxygen, the atomic number is 8, meaning every oxygen atom has 8 protons. This number also determines the element's identity and its position in the periodic table.

Neutron Count

The neutron count in an atom can be calculated by subtracting the atomic number from the atomic mass number (the total number of protons and neutrons). For the isotopes of oxygen, O-16 has 8 neutrons, O-17 has 9 neutrons, and O-18 has 10 neutrons, reflecting their differing atomic masses.

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Related Practice

Textbook Question

Draw the ground-state electronic configuration for each of the following:

a. Mg

Textbook Question

Chlorine has two isotopes, ³⁵Cl and ³⁷Cl; 75.77% of chlorine is ³⁵Cl, and 24.23% is ³⁷Cl. The atomic mass of ³⁵Cl is 34.969 amu, and the atomic mass of ³⁷Cl is 36.966 amu. What is the atomic mass of chlorine?

Textbook Question

Name the element that corresponds to each electronic configuration.

a. 1s² 2s² 2p²

b. 1s² 2s² 2p⁴

c. 1s² 2s² 2p⁶ 3s² 3p³

d. 1s² 2s² 2p⁶ 3s² 3p⁵

Textbook Question

Write the ground-state electronic configuration for chlorine (atomic number 17), bromine (atomic number 35), and iodine (atomic number 53).

Textbook Question

a. How many protons do the following species have?

b. How many electrons does each have?

Na⁺
Ar
Cl^-

Textbook Question

Write the electronic configurations of the third-row elements shown in the partial periodic table in Figure 1-6.

Textbook Question

Chlorine exists as one of two isotopes with atomic masses of 34.969 amu (³⁵Cl) and 36.966 amu (³⁷Cl) . Calculate the relative abundance of ³⁵Cl and ³⁷Cl based on the average atomic mass of 35.453 amu.

Textbook Question

Bromine-79 (50.7% abundance) has an atomic mass of 78.918 amu, whereas bromine-81 (49.3% abundance) has an atomic mass of 80.916 amu. From these data, calculate the average atomic mass of bromine that you would expect to see in the periodic table.

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Oxygen has three isotopes, 16O, 17O, and 18O. The atomic number of oxygen is 8. How many protons and neutrons does each of the isotopes have?

Key Concepts

Isotopes

Atomic Number

Neutron Count

Watch next

Oxygen has three isotopes, ¹⁶O, ¹⁷O, and ¹⁸O. The atomic number of oxygen is 8. How many protons and neutrons does each of the isotopes have?