Table of contents

1. Introduction to Anatomy & Physiology5h 43m
2. Cell Chemistry & Cell Components12h 36m
3. Energy & Cell Processes10h 6m
4. Tissues & Histology10h 3m
5. Integumentary System2h 20m
6. Bones & Skeletal Tissue2h 16m
7. The Skeletal System2h 35m
8. Joints2h 17m
9. Muscle Tissue2h 33m
10. Muscles1h 11m
11. Nervous Tissue and Nervous System1h 35m
12. The Central Nervous System1h 6m
- Introduction to the Central Nervous System
  18m
- The Cerebrum
  48m
13. The Peripheral Nervous System1h 26m
14. The Autonomic Nervous System1h 38m
15. The Special Senses2h 41m
16. The Endocrine System2h 48m
17. The Blood3h 22m
18. The Heart3h 42m
19. The Blood Vessels3h 35m
20. The Lymphatic System3h 16m
21. The Immune System14h 37m
22. The Respiratory System3h 20m
23. The Digestive System2h 5m
24. Metabolism and Nutrition4h 0m
25. The Urinary System2h 39m
26. Fluid and Electrolyte Balance, Acid Base Balance37m
27. The Reproductive System2h 5m
28. Human Development1h 21m
29. Heredity3h 32m

2. Cell Chemistry & Cell Components

Covalent Bonds

Anatomy & Physiology

2. Cell Chemistry & Cell Components

Covalent Bonds

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3:29 minutes

Problem 26

Textbook Question

Explain the differences among nonpolar covalent bonds, polar covalent bonds, and ionic bonds.

Verified step by step guidance

Nonpolar covalent bonds occur when two atoms share electrons equally because they have similar electronegativity values. This results in a balanced distribution of electrical charge across the molecule. For example, in a molecule of oxygen (O₂), the two oxygen atoms share electrons equally.

Polar covalent bonds occur when two atoms share electrons unequally due to a difference in their electronegativity values. This creates a partial positive charge on one atom and a partial negative charge on the other. For instance, in a water molecule (H₂O), the oxygen atom attracts electrons more strongly than the hydrogen atoms, resulting in a polar bond.

Ionic bonds form when one atom completely transfers one or more electrons to another atom, creating ions. The atom that loses electrons becomes a positively charged cation, while the atom that gains electrons becomes a negatively charged anion. These oppositely charged ions are held together by electrostatic forces. For example, in sodium chloride (NaCl), sodium donates an electron to chlorine, forming an ionic bond.

The key difference between covalent bonds (nonpolar and polar) and ionic bonds is the method of electron interaction. Covalent bonds involve sharing electrons, while ionic bonds involve the transfer of electrons.

Nonpolar covalent bonds typically occur between identical atoms or atoms with very similar electronegativity, polar covalent bonds occur between atoms with moderate differences in electronegativity, and ionic bonds occur between atoms with large differences in electronegativity.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Nonpolar Covalent Bonds

Nonpolar covalent bonds occur when two atoms share electrons equally, resulting in a balanced distribution of electrical charge. This typically happens between identical atoms or atoms with similar electronegativities, such as in diatomic molecules like O2 or N2. Because of the equal sharing, these molecules do not have distinct positive or negative poles.

Polar Covalent Bonds

Polar covalent bonds form when two atoms share electrons unequally due to a difference in their electronegativities. The atom with higher electronegativity attracts the shared electrons more strongly, creating a partial negative charge on that atom and a partial positive charge on the other. Water (H2O) is a classic example, where the oxygen atom pulls the shared electrons closer, leading to a polar molecule.

Ionic Bonds

Ionic bonds arise when one atom donates an electron to another, resulting in the formation of charged ions. This typically occurs between metals and nonmetals, where the metal loses electrons to become a positively charged cation, and the nonmetal gains electrons to become a negatively charged anion. The electrostatic attraction between these oppositely charged ions forms a strong ionic bond, as seen in sodium chloride (NaCl).

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