Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

9. Electrons in Atoms and the Periodic Table

Bohr Model (Simplified)

Introduction to Chemistry

9. Electrons in Atoms and the Periodic Table

Bohr Model (Simplified)

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Multiple Choice

Which of the electron transitions represents an example of absorption?

n = 5 to n = 3

n = 1 to n =3

n = 6 to n = 2

n = 7 to n = 4

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Verified step by step guidance

Understand that electron transitions involve electrons moving between energy levels in an atom. Absorption occurs when an electron absorbs energy and moves to a higher energy level.

Identify the initial and final energy levels for each transition. For example, in the transition 'n = 5 to n = 3', the electron moves from a higher energy level (n = 5) to a lower energy level (n = 3), which is an emission process.

For absorption, the electron must move from a lower energy level to a higher energy level. This means the initial energy level (n_initial) should be less than the final energy level (n_final).

Examine each given transition: 'n = 1 to n = 3' is an example of absorption because the electron moves from a lower energy level (n = 1) to a higher energy level (n = 3).

Verify the other transitions: 'n = 6 to n = 2' and 'n = 7 to n = 4' both involve electrons moving from higher to lower energy levels, indicating emission rather than absorption.