Introduction to Biochemistry - Electron Orbitals and Electronic Configuration

These flashcards cover key concepts from the lecture on electron orbitals and electronic configuration, focusing on the differences between orbits and orbitals, the principles governing electron distribution, and the implications of electron configuration.

What is the main difference between 'orbits' and 'orbitals'?

Orbits are well-defined pathways for electron movement, while orbitals are 3D regions where there is a probability of finding electrons.

What does an electron orbital represent?

A 3D region with a 90% probability of containing an electron.

What are the three main principles governing electron distribution in an atom?

Aufbau principle, Hund's rule, and Pauli's exclusion principle.

How does the Aufbau principle dictate electron filling?

Electrons fill orbitals starting from the lowest energy level.

According to Hund's rule, how should electrons be distributed in orbitals of equal energy?

Each orbital should be singly occupied before any orbital is doubly occupied.

What does the Pauli exclusion principle state about electrons in an orbital?

Each orbital can hold a maximum of two electrons with opposite spins.

What is the significance of electronic orbitals in representing electrons?

They provide a more sophisticated model for visualizing electron distribution in space.

What influences the shape of an electronic orbital?

The number of electrons it contains, proximity of other orbitals, distance from the nucleus, and energy carried by the electron.

What are the shells in relation to orbitals?

Shells are numbered layers (1, 2, 3,…) that differ based on the energy required for electrons to inhabit them.

Why can the past and future location of electrons not be predicted within orbitals?

Due to the multiple pathways available that define their movement in three-dimensional space.