Related Experiment Video
Updated: Feb 10, 2026
15:04
Picometer-Precision Atomic Position Tracking through Electron Microscopy
Published on: July 3, 2021
8.4K
Atom-based vector microwave electrometry using rubidium Rydberg atoms in a vapor cell.
J A Sedlacek1, A Schwettmann, H Kübler
1Homer L. Dodge Department of Physics and Astronomy, The University of Oklahoma, 440 West Brooks Street, Norman, Oklahoma 73019, USA.
Physical Review Letters
|August 27, 2013
Summary
Rubidium atoms in a vapor cell now serve as a practical standard for measuring microwave electric field strength and polarization. This advancement utilizes Rydberg-atom electromagnetically induced transparency for precise vector electrometry.
Area of Science:
- Atomic physics
- Quantum optics
- Metrology
Background:
- Atomic standards are crucial for fundamental quantities like electromagnetic fields.
- Previous work established Rubidium (Rb) atoms in vapor cells as standards for microwave electric field strength using Rydberg states.
Purpose of the Study:
- To demonstrate the use of Rb atoms in a vapor cell for vector microwave electrometry.
- To achieve precise measurement of arbitrary microwave electric field polarization.
Main Methods:
- Utilizing Rydberg-atom electromagnetically induced transparency (Rydberg-EIT).
- Performing measurements to determine microwave electric field polarization.
- Exciting Rb atoms within a vapor cell.
Main Results:
- Demonstrated vector microwave electrometry using Rb atoms in a vapor cell for the first time.
- Achieved polarization measurements with a resolution of 0.5°.
- Experimental results showed excellent agreement with theoretical predictions.
Conclusions:
- Rb atoms in vapor cells are suitable for vector microwave electrometry.
- Rydberg-EIT provides a practical and compact method for precise electric field measurements.
- This technique advances the development of atomic standards for electromagnetic fields.
Related Concept Videos
02:44Atomic Orbitals
44.9K
An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution function indicates the total probability of finding an electron within the thin shell at a distance r from the nucleus. The atomic orbitals have distinct shapes which are determined by l, the angular momentum quantum number. The orbitals are often drawn with a boundary surface, enclosing densest regions of the cloud.
44.9K
01:33Atomic Structure
210.7K
Overview
210.7K
01:52Atomic Mass
70.4K
Atoms — and the protons, neutrons, and electrons that compose them — are extremely small. For example, a carbon atom weighs less than 2 × 10−23 g. When describing the properties of tiny objects such as atoms, we use appropriately small units of measure, such as the atomic mass unit (amu). The amu was originally defined based on hydrogen, the lightest element, then later in terms of oxygen. Since 1961, it has been defined with regard to the most abundant isotope of carbon, atoms of which...
70.4K
02:59The Atomic Theory of Matter
129.6K
The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter was composed of small, finite particles that they called atomos, meaning “indivisible.” Later, Aristotle and others came to the conclusion that matter consisted of various combinations of the four “elements” — fire, earth, air, and water — and could be infinitely divided. Interestingly, these philosophers...
129.6K
03:24Hybridization of Atomic Orbitals I
67.7K
The mathematical expression known as the wave function, ψ, contains information about each orbital and the wavelike properties of electrons in an isolated atom. When atoms are bound together in a molecule, the wave functions combine to produce new mathematical descriptions that have different shapes. This process of combining the wave functions for atomic orbitals is called hybridization and is mathematically accomplished by the linear combination of atomic orbitals. The new orbitals that...
67.7K
03:21The Energies of Atomic Orbitals
30.3K
In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are also observed. The attractive and repulsive forces are dependent on the distance between the particles, as well as the sign and magnitude of the charges on the individual particles. When the charges on the particles are opposite, they attract each other. If both particles have the same charge, they repel each other.
30.3K