Introduction to Quantum Mechanics and Atomic Orbitals

These flashcards cover key concepts related to the Schrodinger equation, wave functions, and atomic orbitals discussed in the lecture.

Schrodinger equation

A key equation in quantum mechanics whose solutions describe the wave functions of electrons in atoms.

Wave function

A mathematical function that describes the quantum state of a particle and gives the probability of finding the particle at a given point in space.

Orbital

A region in an atom where there is a high probability of finding an electron.

s orbital

A spherical orbital where the angular momentum quantum number (l) is 0.

p orbital

A dumbbell-shaped orbital where the angular momentum quantum number (l) is 1.

d orbital

An orbital with complex shapes, where the angular momentum quantum number (l) is 2.

Principal quantum number (n)

A number that determines the energy level and size of an orbital.

Node

A region in an orbital where the probability of finding an electron is zero.

Degenerate orbitals

Orbitals that have the same energy level.

Aufbau principle

A principle stating that electrons occupy the lowest energy orbitals first.

Probability density plot

A graph that shows the likelihood of finding an electron in a particular region of space.

Isosurface

A 3-dimensional surface that represents points of a constant value in a wave function.

Quantum numbers

A set of numbers that describe the unique quantum state of an electron in an atom.

Electron configurations

A notation that shows the distribution of electrons among the different orbitals of an atom.

Hydrogen atom

The simplest atom, consisting of one proton and one electron, serving as a foundational example in quantum mechanics.