Table of contents

1. Introduction to Anatomy & Physiology5h 42m
2. Cell Chemistry & Cell Components12h 37m
3. Energy & Cell Processes10h 7m
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 Heart2h 42m
19. The Blood Vessels3h 35m
20. The Lymphatic System3h 16m
21. The Immune System14h 37m
22. The Respiratory System3h 12m
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

Introduction to Chemical Bonding

Anatomy & Physiology

2. Cell Chemistry & Cell Components

Introduction to Chemical Bonding

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Problem L1.5

Textbook Question

Identify each of the following molecules or compounds as ionic, polar covalent, or nonpolar covalent.
a. H₂O _____
b. LiI _
c. C₁₀H₂₂ _
d. N₂ _
e. MgBr₂ _
f. H₂S _____

Verified step by step guidance

Step 1: Understand the types of bonds. Ionic bonds occur when electrons are transferred between atoms, typically between a metal and a nonmetal. Polar covalent bonds occur when electrons are shared unequally between atoms, leading to partial charges. Nonpolar covalent bonds occur when electrons are shared equally between atoms, usually between identical or similar nonmetals.

Step 2: Analyze each molecule or compound. For H2O, recognize that oxygen is more electronegative than hydrogen, causing an unequal sharing of electrons. This makes H2O a polar covalent molecule.

Step 3: For LiI, note that lithium is a metal and iodine is a nonmetal. The large difference in electronegativity between these elements indicates that LiI forms an ionic bond.

Step 4: For C10H22, observe that it is a hydrocarbon composed of carbon and hydrogen. The electronegativity difference between carbon and hydrogen is very small, so the bonds are nonpolar covalent, and the molecule as a whole is nonpolar.

Step 5: Repeat the analysis for the remaining compounds. For N2, the two nitrogen atoms share electrons equally, making it nonpolar covalent. For MgBr2, magnesium is a metal and bromine is a nonmetal, so it forms an ionic bond. For H2S, sulfur is more electronegative than hydrogen, leading to unequal sharing of electrons, making it polar covalent.

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Key Concepts

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

Ionic Bonds

Ionic bonds form when electrons are transferred from one atom to another, resulting in the creation of charged ions. These oppositely charged ions attract each other, leading to the formation of ionic compounds. Typically, ionic compounds consist of a metal and a non-metal, such as lithium iodide (LiI) or magnesium bromide (MgBr2), and they usually have high melting and boiling points.

Covalent Bonds

Covalent bonds occur when two atoms share electrons, allowing them to achieve a full outer electron shell. This type of bonding can be polar or nonpolar, depending on the electronegativity difference between the atoms involved. For example, water (H2O) is polar due to the significant difference in electronegativity between hydrogen and oxygen, while nitrogen gas (N2) is nonpolar as it consists of two identical nitrogen atoms sharing electrons equally.

Polarity of Molecules

Polarity in molecules refers to the distribution of electrical charge across the molecule. A polar molecule has a partial positive charge on one end and a partial negative charge on the other, often due to differences in electronegativity. Nonpolar molecules, on the other hand, have an even distribution of charge. Understanding polarity is crucial for predicting the behavior of substances in different environments, such as solubility in water.