Electron Configurations and Transition Metals

The video tutorial discusses the stability of noble gas electron configurations and their influence on the behavior of elements in the periodic table. It explains how elements in the s and p blocks achieve stability by attaining the electron configuration of the nearest noble gas. The tutorial then explores the electron configurations of transition metals, highlighting the Aufbau principle and the concept of pseudo noble gas configurations. Using silver as an example, it illustrates how transition metals lose electrons to achieve a stable configuration, similar to noble gases, but with 18 electrons in the outermost shell. The video concludes by comparing pseudo noble gas configurations with noble gas configurations, emphasizing their role in the stability of transition metal ions.

What is the primary reason noble gases are considered stable?

• They have a full outer shell of electrons.

• They are located in the s block of the periodic table.

• They have a high atomic number.

• They can easily gain or lose electrons.

Which orbitals are filled first in the electron configurations of transition metals?

• f orbitals

• d orbitals

• s orbitals

• p orbitals

According to the Aufbau principle, why are d orbitals filled after s orbitals?

• d orbitals have a higher energy level.

• s orbitals belong to a higher principal quantum number.

• s orbitals are closer to the nucleus.

• d orbitals are spherical in shape.

When a transition metal like silver ionizes, which electrons are lost first?

• d electrons

• p electrons

• s electrons

• f electrons

What is a pseudo noble gas electron configuration?

• An electron configuration with a full outer shell of 8 electrons.

• An electron configuration with a full outer shell of 18 electrons.

• An electron configuration with unfilled d orbitals.

• An electron configuration that matches a noble gas exactly.

How does the pseudo noble gas configuration relate to the stability of transition metals?

• It results in a half-filled outer shell.

• It makes them highly reactive.

• It provides stability similar to noble gases.

• It causes them to lose all their electrons.

Which of the following is an example of a transition metal with a pseudo noble gas configuration?

• Silver

• Oxygen

• Neon

• Helium

What is the electron configuration of a silver ion after losing an electron?

• 5s1 4d9

• 5s0 4d10

• 5s2 4d9

• 5s1 4d10

Why do transition metals often lose their s electrons first?

• To achieve a full d orbital.

• To empty the valence shell with the highest principal quantum number.

• To gain additional electrons.

• To match the electron configuration of a noble gas.

What is the common oxidation state of zinc in a pseudo noble gas configuration?

• +1

• +2

• +3

• +4