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 chemical formula for the ionic compound formed when calcium reacts with chlorine?

Ca_2Cl

CaCl_2

CaCl

Ca_2Cl_2

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Verified step by step guidance

Identify the charges of the ions formed by calcium and chlorine. Calcium is an alkaline earth metal in Group 2, so it forms a Ca^{2+} ion by losing two electrons. Chlorine is a halogen in Group 17, so it forms a Cl^{-} ion by gaining one electron.

Determine the ratio of ions needed to balance the overall charge of the compound. Since calcium has a +2 charge and chlorine has a -1 charge, two chloride ions are needed to balance one calcium ion.

Write the chemical formula by combining the ions in the ratio that balances the charges. This means one Ca^{2+} ion pairs with two Cl^{-} ions, giving the formula CaCl_2.

Check that the total positive charge equals the total negative charge to ensure the compound is electrically neutral. Here, +2 from calcium balances with 2 × (-1) from chlorine, resulting in zero net charge.

Confirm that the formula is written with the metal (cation) first followed by the nonmetal (anion), which is the standard convention for ionic compounds.