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

24. Transition Metals and Coordination Compounds

Electron Configurations of Transition Metals

General Chemistry

24. Transition Metals and Coordination Compounds

Electron Configurations of Transition Metals

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Multiple Choice

Which of the following is true about the atomic size of transition metals?

The atomic radius decreases from left to right as the number of protons increases.

The atomic radius remains relatively constant because electrons are added to an (n − 1) orbital.

The atomic radius increases from left to right as electrons are added to an outer orbital.

The atomic radius decreases from left to right as Z_eff increases.

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Verified step by step guidance

Understand the concept of atomic radius: Atomic radius is the distance from the nucleus of an atom to the outermost shell of electrons. It generally decreases across a period due to increasing nuclear charge.

Identify the role of transition metals: Transition metals are elements found in the d-block of the periodic table, where electrons are added to the (n-1)d subshell.

Analyze the effect of electron addition in transition metals: As electrons are added to the (n-1)d orbital, the increase in nuclear charge is somewhat offset by electron-electron repulsions within the d subshell, leading to a relatively constant atomic radius.

Consider the effective nuclear charge (Zeff): The effective nuclear charge is the net positive charge experienced by valence electrons. In transition metals, Zeff increases, but the added electrons in the (n-1)d orbital provide some shielding, maintaining a relatively constant atomic size.

Conclude the trend for transition metals: Unlike main group elements, the atomic radius of transition metals remains relatively constant across a period because the added electrons enter the (n-1)d orbital, which does not significantly increase the atomic size.