Chemical bonds vibrate trillions of times per second, constantly stretching and contracting like tiny springs.

In molecular physics, chemical bonds are never static. The Harmonic Oscillator model describes them best: atoms behave as masses connected by springs, vibrating at frequencies ranging from 10 to 100 terahertz—that is, 10 trillion to 100 trillion cycles per second.The frequency of each vibration depends on two factors: the mass of the atoms involved and the strength of the bond between them. A Carbon-Hydrogen (C-H) bond, for instance, typically vibrates at approximately 90 trillion times per second. Scientists measure these vibrations using Infrared Spectroscopy, which detects the specific wavelengths of light that molecules absorb when those wavelengths match their vibrational frequencies.This field of study was pioneered in the early 20th century by researchers like William Coblentz, whose work led to the development of modern molecular analysis techniques. Even at absolute zero, atoms possess what physicists call "zero-point energy," meaning they never completely stop moving. As thermal energy increases, the amplitude of vibrations grows larger until the bond reaches its dissociation energy and breaks.These atomic motions are fundamental to how heat conducts through solids and how greenhouse gases trap energy in our atmosphere. When molecules like CO₂ absorb infrared radiation from Earth, their vibrational energy increases, contributing to planetary warming. By understanding these trillions of vibrations per second, chemists can identify unknown substances and predict how they will behave under different conditions.