Table of contents

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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

10. Periodic Properties of the Elements

The Electron Configuration: Ions

General Chemistry

10. Periodic Properties of the Elements

The Electron Configuration: Ions

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Multiple Choice

Determine the electron configuration and electron orbital diagram for the silver ion.

[Kr] 4d¹⁰

[Kr] 4d⁸ 5p²

[Kr] 4d⁸

[Kr] 4d⁸ 5s²

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Verified step by step guidance

Identify the atomic number of silver (Ag), which is 47, and write its electron configuration in the ground state: [Kr] 4d10 5s1.

Recognize that the problem asks for the electron configuration of the silver ion. Silver commonly forms a +1 ion (Ag+), meaning it loses one electron.

Determine which electron is removed when silver forms a +1 ion. Electrons are typically removed from the outermost shell first, so the 5s electron is removed.

Write the electron configuration for the Ag+ ion after removing the 5s electron: [Kr] 4d10.

Draw the electron orbital diagram for the Ag+ ion, showing the filled 4d orbitals: 4d orbitals have 10 electrons, so all five 4d orbitals are fully filled with paired electrons.