Related Experiment Video
Updated: Feb 27, 2026

11:20
In Situ Visualization of the Phase Behavior of Oil Samples Under Refinery Process Conditions
Published on: February 21, 2017
7.1K
An IR investigation of solid amorphous ethanol - Spectra, properties, and phase changes
1Astrochemistry Laboratory, NASA Goddard Space Flight Center, Greenbelt, MD 20771, USA.
Summary
Infrared spectra of amorphous ethanol were analyzed at low temperatures. This research provides key data for understanding ethanol
Area of Science:
- Astrochemistry
- Spectroscopy
- Condensed Matter Physics
Background:
- Ethanol (CH3CH2OH) is a molecule of significant interest in astrochemistry.
- Understanding the physical and chemical properties of condensed ethanol is crucial for interstellar medium research.
Purpose of the Study:
- To present mid- and far-infrared spectra of condensed ethanol (CH3CH2OH) across a temperature range of 10-160K.
- To focus on amorphous ethanol, its spectral characteristics, and phase transitions.
- To provide key physical parameters of amorphous ethanol relevant to astrochemical models.
Main Methods:
- Acquisition and analysis of mid- and far-infrared spectra of condensed ethanol.
- Temperature-dependent measurements from 10K to 160K.
- Characterization of both amorphous and crystalline phases of ethanol.
Main Results:
- Detailed infrared spectra for amorphous and crystalline ethanol are presented.
- Key physical properties including refractive index at 670nm, IR band strengths, and density for amorphous ethanol at 16K are reported.
- Spectral changes near the amorphous-to-crystalline transition (155-160K) were observed.
Conclusions:
- The study provides essential spectral data for amorphous ethanol, vital for astrochemical interpretations.
- Comparison with isoelectronic ethanethiol (CH3CH2SH) aids in understanding molecular behavior in astrophysical environments.
- The findings suggest potential applications for future astrochemical studies involving ethanol ice.
Related Concept Videos
IR Spectroscopy: Molecular Vibration Overview
5.1K
When Infrared (IR) radiation passes through a covalently bonded molecule, the bonds transition from lower to higher vibrational levels. The fundamental vibrational motions that result in infrared absorption can be classified as stretching or bending vibrations.
Stretching vibrations are vibrational motions that occur along the bond line, changing the bond length or distance between two bonded atoms. They are further distinguished as symmetric or asymmetric. In symmetric stretching, the...
Stretching vibrations are vibrational motions that occur along the bond line, changing the bond length or distance between two bonded atoms. They are further distinguished as symmetric or asymmetric. In symmetric stretching, the...
5.1K
Solid–Solid Solutions
18
The temperature-composition phase diagram of two solids, A and B, which are immiscible in the solid phase but form miscible liquids, shows that when the temperature is low, these two exist as separate, pure solids (A and B). As the temperature increases, they transition into a single-phase liquid solution where A and B coexist. Moving from point a1 to a2 in the phase diagram, the composition changes such that solid B begins to separate from the solution, enriching the remaining liquid with A.
18
Physical Properties of Alcohols and Phenols
17.0K
Alcohols are organic compounds in which a hydroxy group is attached to a saturated carbon. Phenols are a class of alcohols containing a hydroxy group attached to an aromatic ring. The physical properties of the alcohols and phenols are influenced by hydrogen bonding due to the oxygen–hydrogen dipole in the hydroxy functional group and dispersion forces between alkyl or aryl regions of alcohol and phenol molecules.
Alcohols possess a higher boiling point than aliphatic hydrocarbons of similar...
Alcohols possess a higher boiling point than aliphatic hydrocarbons of similar...
17.0K
Physical Properties of Ethers
8.8K
Overview
An ether molecule has a net dipole moment due to the polarity of C–O bonds. Subsequently, boiling points of ethers are lower than those of alcohols of comparable molecular weight and slightly higher than those of hydrocarbons of comparable molecular weight (Table 1).
Ethers can act as hydrogen bond acceptors, making them more water-soluble than hydrocarbons, but since ethers cannot act as hydrogen bond donors, they are much less soluble in water than alcohols. Ethers are considered...
An ether molecule has a net dipole moment due to the polarity of C–O bonds. Subsequently, boiling points of ethers are lower than those of alcohols of comparable molecular weight and slightly higher than those of hydrocarbons of comparable molecular weight (Table 1).
Ethers can act as hydrogen bond acceptors, making them more water-soluble than hydrocarbons, but since ethers cannot act as hydrogen bond donors, they are much less soluble in water than alcohols. Ethers are considered...
8.8K
Phase Transitions: Melting and Freezing
15.4K
Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...
15.4K
¹H NMR of Labile Protons: Temporal Resolution
1.8K
Protons bonded to heteroatoms such as nitrogen and oxygen exhibit a range of chemical shift values. This is due to the varying degree of hydrogen bonding between the proton and the heteroatom in other molecules. The extent of hydrogen bonding affects the electron density around the proton, thereby giving different chemical shift values for the protons in the proton NMR spectrum.
The –OH proton in alcohols typically appears in the range of δ 2 to 5 ppm but can vary depending on the specific...
The –OH proton in alcohols typically appears in the range of δ 2 to 5 ppm but can vary depending on the specific...
1.8K

