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

Atoms- Smallest Unit of Matter

Anatomy & Physiology

2. Cell Chemistry & Cell Components

Atoms- Smallest Unit of Matter

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4:15 minutes

Problem 9

Textbook Question

DRAW IT Draw Lewis dot structures for each hypothetical molecule shown below, using the correct number of valence electrons for each atom. Determine which molecule makes sense because each atom has a complete valence shell and each bond has the correct number of electrons. Explain what makes the other molecule nonsensical, considering the number of bonds each type of atom can make. a.

Verified step by step guidance

Step 1: Identify the number of valence electrons for each atom in the molecules. For example, Carbon (C) has 4 valence electrons, Hydrogen (H) has 1 valence electron, and Oxygen (O) has 6 valence electrons.

Step 2: Draw the Lewis dot structure for each molecule by placing the valence electrons around each atom. Start by placing single bonds (pairs of electrons) between atoms to form the basic structure.

Step 3: Ensure that each atom has a complete valence shell. For Hydrogen, this means 2 electrons (1 bond), and for Carbon and Oxygen, this means 8 electrons (4 bonds for Carbon, 2 bonds and 2 lone pairs for Oxygen).

Step 4: Check if each bond has the correct number of electrons. Each single bond should have 2 electrons, each double bond should have 4 electrons, and each triple bond should have 6 electrons.

Step 5: Determine which molecule makes sense by verifying that all atoms have a complete valence shell and that the number of bonds is appropriate for each type of atom. Identify any molecule that does not meet these criteria and explain why it is nonsensical.

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Key Concepts

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

Lewis Dot Structures

Lewis dot structures are diagrams that represent the valence electrons of atoms within a molecule. Each dot corresponds to a valence electron, and the arrangement of these dots illustrates how atoms bond together. Understanding how to draw these structures is crucial for visualizing molecular geometry and predicting the behavior of molecules in chemical reactions.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are key to determining how an atom will bond with others. The number of valence electrons influences the atom's reactivity and the types of bonds it can form, whether ionic or covalent. Knowing the valence electron count for each atom involved in a molecule is essential for constructing accurate Lewis dot structures.

Octet Rule

The octet rule is a chemical principle stating that atoms tend to bond in such a way that they each have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule helps predict the types of bonds that will form between atoms and is fundamental in assessing the validity of a proposed molecular structure. Molecules that do not satisfy the octet rule may be considered nonsensical or unstable.