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

3. Ionic Compounds

Writing Formula Units of Ionic Compounds

GOB Chemistry

3. Ionic Compounds

Writing Formula Units of Ionic Compounds

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1:30 minutes

Problem 97d

Textbook Question

Consider the following Lewis symbols for elements X and Y:

d. What would be the formula of a compound of X and Y?

Verified step by step guidance

Step 1: Identify the valence electrons for elements X and Y based on their Lewis symbols. The number of dots around the element symbol represents the number of valence electrons.

Step 2: Determine the number of electrons each element needs to achieve a full octet (8 valence electrons). For example, if X has 6 valence electrons, it needs 2 more electrons, and if Y has 1 valence electron, it needs to lose 1 electron to achieve a stable configuration.

Step 3: Analyze the ratio in which X and Y will combine to satisfy the octet rule for both elements. For instance, if X needs 2 electrons and Y can donate 1 electron, the ratio of X:Y would be 1:2.

Step 4: Write the chemical formula of the compound by combining X and Y in the ratio determined in the previous step. Use subscripts to indicate the number of each type of atom in the compound.

Step 5: Verify the formula by ensuring that the total number of electrons gained and lost by the elements results in a stable configuration for both X and Y.

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Key Concepts

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

Lewis Symbols

Lewis symbols are a way to represent the valence electrons of an atom using dots around the element's symbol. Each dot corresponds to a valence electron, which plays a crucial role in chemical bonding. Understanding Lewis symbols helps predict how atoms will interact and bond with each other to form compounds.

Chemical Bonding

Chemical bonding refers to the forces that hold atoms together in a compound. The two primary types of bonds are ionic and covalent. Ionic bonds occur when electrons are transferred from one atom to another, while covalent bonds involve the sharing of electrons. The type of bond formed between elements X and Y will influence the compound's formula.

Empirical Formula

The empirical formula of a compound represents the simplest whole-number ratio of the elements present. It is derived from the number of atoms of each element in the compound. To determine the empirical formula of the compound formed by elements X and Y, one must consider their valence and the type of bond they form, which will dictate the ratio of X to Y in the compound.

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