Table of contents

1. Intro to General Chemistry(0)
2. Atoms & Elements(0)
3. Chemical Reactions(0)
4. BONUS: Lab Techniques and Procedures(0)
5. BONUS: Mathematical Operations and Functions(0)
6. Chemical Quantities & Aqueous Reactions(0)
7. Gases(0)
8. Thermochemistry(0)
9. Quantum Mechanics(0)
10. Periodic Properties of the Elements(0)
11. Bonding & Molecular Structure(0)
12. Molecular Shapes & Valence Bond Theory(0)
13. Liquids, Solids & Intermolecular Forces(0)
14. Solutions(0)
15. Chemical Kinetics(0)
16. Chemical Equilibrium(0)
17. Acid and Base Equilibrium(0)
18. Aqueous Equilibrium(0)
19. Chemical Thermodynamics(0)
20. Electrochemistry(0)
21. Nuclear Chemistry(0)
22. Organic Chemistry(0)
23. Chemistry of the Nonmetals(0)
24. Transition Metals and Coordination Compounds(0)

10. Periodic Properties of the Elements

The Electron Configurations: Exceptions

10. Periodic Properties of the Elements

The Electron Configurations: Exceptions: Videos & Practice Problems

Learn Concepts Practice Worksheet

The Electron Configurations: Exceptions Practice Problems

20 problems

1PRACTICE PROBLEM

Consider the following illustration of the periodic table. Identify which among the highlighted elements has an anomalous ground-state electron configuration. Justify your answer.

Periodic table highlighting elements A, B, and C for electron configuration anomalies.

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2PRACTICE PROBLEM

What is the electron configuration for a roentgenium atom?

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3PRACTICE PROBLEM

Palladium (Pd) has an odd electron configuration. Write the complete electron configuration of Pd in order of increasing orbital energy.

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4PRACTICE PROBLEM

Which one of the following statements is/are true?

1. Selenium (Se) has the electron configuration [Ar]4s²4d¹⁰4p³
2. Silver (Ag) has the electron configuration [Kr] 5s¹4d¹⁰
3. Chromium (Cr) has the electron configuration [Ar] 4s¹3d⁵

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5PRACTICE PROBLEM

Which is the first element in the periodic table to have a half-filled d subshell in the ground state?

Name the transition metal(s) in the second transition series that deviate(s) from the expected order of electron filling based on the Aufbau principle.

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7PRACTICE PROBLEM

Looking at its position in the periodic table, determine the number of 5d electrons present in gold (Au).

8PRACTICE PROBLEM

Looking at the position of palladium (Pd) in the periodic table, determine the number of its 4d electrons.

9PRACTICE PROBLEM

Which of the following subshells is considered more stable when it is half-filled?

10PRACTICE PROBLEM

According to Hund's rule, which of the following electron configurations is most stable for a set of p orbitals?

11PRACTICE PROBLEM

Which of the following elements has an electron configuration exception similar to chromium?

12PRACTICE PROBLEM

What is the electron configuration of chromium, considering the electron promotion exception?

13PRACTICE PROBLEM

Why does copper have an electron configuration of [Ar] 3d10 4s1 instead of [Ar] 3d9 4s2?

14PRACTICE PROBLEM

Which atomic number corresponds to an element with an electron configuration exception similar to chromium?

15PRACTICE PROBLEM

What is the primary reason for electron configuration exceptions in elements like chromium and copper?

16PRACTICE PROBLEM

What role does electron promotion from the s orbital play in stabilizing configurations in elements like copper?

17PRACTICE PROBLEM

By skipping which group in the periodic table can you identify elements with electron configuration exceptions?

18PRACTICE PROBLEM

Why do certain elements deviate from expected electron configurations, achieving symmetry and stability?

19PRACTICE PROBLEM

Which statement best explains the stability of a half-filled d subshell?

20PRACTICE PROBLEM

Using Hund's rule, what is the electron configuration for nitrogen?

Previous Topic: The Electron Configuration: Condensed Next Topic: The Electron Configuration: Ions

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