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

What is the correct chemical formula for the ionic compound formed between barium and bromine?

BaBr

Ba2Br2

BaBr2

Ba2Br

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Verified step by step guidance

Identify the charges of the ions formed by each element: Barium (Ba) is an alkaline earth metal in Group 2, so it forms a cation with a charge of +2, written as $\mathrm{Ba^{2+}}$.

Bromine (Br) is a halogen in Group 17 and forms an anion with a charge of -1, written as $\mathrm{Br^{-}}$.

To form a neutral ionic compound, the total positive charge must balance the total negative charge. Since barium has a +2 charge and bromine has a -1 charge, you need two bromide ions to balance one barium ion.

Write the formula by placing the cation first followed by the anion, using subscripts to indicate the number of each ion needed to balance the charges: $\mathrm{BaBr_2}$.

Confirm that the total charge is zero: $+2$ from one $\mathrm{Ba^{2+}}$ and $2 \times (-1)$ from two $\mathrm{Br^{-}}$ ions sum to zero, indicating the formula $\mathrm{BaBr_2}$ is correct.