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

2. Atoms & Elements

Periodic Table: Group Names

General Chemistry

2. Atoms & Elements

Periodic Table: Group Names

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Multiple Choice

Magnesium is classified as an alkaline earth metal. With which group of elements is magnesium most likely to react most vigorously?

Noble gases (Group 18)

Alkali metals (Group 1)

Halogens (Group 17)

Transition metals (Groups 3–12)

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Verified step by step guidance

Identify the position of magnesium in the periodic table: magnesium is an alkaline earth metal located in Group 2.

Recall that elements tend to react most vigorously with elements that have complementary electron configurations, often those that can easily gain or lose electrons to achieve a stable octet.

Understand that alkaline earth metals like magnesium tend to lose two electrons to form a +2 charge, so they react most vigorously with elements that readily gain two electrons or one electron per atom to form stable anions.

Recognize that halogens (Group 17) have seven valence electrons and need one more electron to complete their octet, making them highly reactive with metals like magnesium that can donate electrons.

Conclude that magnesium will react most vigorously with halogens (Group 17) because magnesium donates electrons and halogens accept electrons, leading to the formation of ionic compounds.