Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

3. Chemical Reactions

Naming Ionic Compounds

General Chemistry

3. Chemical Reactions

Naming Ionic Compounds

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Multiple Choice

Which of the following is the correct method for determining the charges on the ions in an ionic compound?

By using the atomic mass of each element to determine the charge of its ion.

By using the group number of the element in the periodic table and balancing the total positive and negative charges to achieve electrical neutrality.

By assigning a charge of +1 to all metals and -1 to all nonmetals regardless of their position in the periodic table.

By counting the number of atoms in the formula and assigning charges based on the total number of atoms present.

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Verified step by step guidance

Understand that ions in ionic compounds form by atoms gaining or losing electrons to achieve a stable electron configuration, often resembling the nearest noble gas.

Recognize that the charge on an ion is related to its position (group number) in the periodic table: for main-group elements, metals tend to lose electrons equal to their group number to form positive ions, while nonmetals tend to gain electrons to complete their octet, forming negative ions.

Use the group number of the element to predict the charge of its ion. For example, elements in Group 1 typically form +1 ions, Group 2 form +2 ions, and Group 17 form -1 ions.

Balance the total positive and negative charges from the ions so that the overall ionic compound is electrically neutral. This means the sum of positive charges equals the sum of negative charges.

Write the formula of the ionic compound by combining the ions in the ratio that balances their charges, ensuring the compound has no net charge.