Electron Configuration and Valence Electrons

These flashcards cover key concepts related to electron configuration, the Diagonal Rule, the stability of d-orbitals, and valence electrons.

What is electron configuration?

The distribution of electrons among atomic orbitals.

What is the Diagonal Rule in chemistry?

It is a guideline that explains the order in which electrons fill orbital levels based on their energy.

What does the superscript in electronic configuration represent?

The number of electrons present in the orbital.

In electronic configuration, what does the coefficient represent?

The shell number.

What is an example of electronic configuration for Sulfur (16S)?

1s² 2s² 2p⁶ 3s² 3p⁴.

In the electronic configuration 28Ni: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁸, why is 4s filled before 3d?

Because 4s is lower in energy than 3d.

What is the stability condition for d-orbitals?

An element is most stable if its d-orbital is either completely filled or half filled.

How is the electronic configuration of 24Cr adjusted for stability?

It becomes 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵ by borrowing an electron from the s-orbital.

What are valence electrons?

Valence electrons are located in the atom’s outermost orbitals and are associated with the highest principal energy level.

What does a Lewis-dot structure represent?

It shows the valence electrons surrounding the atomic symbol using dots.