Related Experiment Video
Updated: Feb 7, 2026
06:34
A Single-Channel and Non-Invasive Wearable Brain-Computer Interface for Industry and Healthcare
Published on: July 7, 2023
3.2K
Transition from Academia to Industry and Back
Andrea Volkamer1, Sereina Riniker2
1In silico Toxicology, Institute of Physiology , Charité-Universitätsmedizin Berlin , Charitéplatz 1 , 10117 Berlin , Germany.
Journal of Chemical Information and Modeling
|July 31, 2018
Summary
Many scientists transition between academic and industry careers. This perspective shares experiences navigating these paths, offering insights for future principal investigators (PIs) in computational chemistry.
Area of Science:
- Computational chemistry
- Career development in science
Background:
- Doctoral students and postdoctoral fellows often face a career crossroads: academia versus industry.
- Both paths present distinct advantages, disadvantages, and common stereotypes.
Purpose of the Study:
- To share personal experiences transitioning between academic and industrial research environments.
- To provide insights for early-career scientists, particularly principal investigators (PIs), considering career choices.
- To discuss the future outlook of computational chemistry.
Main Methods:
- Personal narrative and reflection on career transitions.
- Analysis of experiences as a university Ph.D. graduate, industrial postdoctoral fellow, and academic faculty member.
Main Results:
- Gained insights from an industrial postdoctoral phase.
- Motivations and challenges of returning to an academic faculty position.
- Exploration of the freedoms and burdens of establishing a principal investigator (PI) role.
Conclusions:
- Reflections on the dual nature of academic and industrial scientific careers.
- Considerations for early-career researchers in computational chemistry.
- Discussion on the future direction and challenges in computational chemistry research.
Related Concept Videos
02:31Phase Transitions
23.2K
Whether solid, liquid, or gas, a substance's state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the solid pack closely together, generally in a pattern. The particles vibrate about their fixed positions but do not move or squeeze past their neighbors. In liquids, although the particles are closely spaced, they are randomly arranged. The position of the particles are not fixed—that is, they are free to move past their neighbors to...
23.2K
02:58Properties of Transition Metals
29.9K
Transition metals are defined as those elements that have partially filled d orbitals. As shown in Figure 1, the d-block elements in groups 3–12 are transition elements. The f-block elements, also called inner transition metals (the lanthanides and actinides), also meet this criterion because the d orbital is partially occupied before the f orbitals.
29.9K
01:58Cooperative Allosteric Transitions
8.8K
Cooperative allosteric transitions can occur in multimeric proteins, where each subunit of the protein has its own ligand-binding site. When a ligand binds to any of these subunits, it triggers a conformational change that affects the binding sites in the other subunits; this can change the affinity of the other sites for their respective ligands. The ability of the protein to change the shape of its binding site is attributed to the presence of a mix of flexible and stable segments in the...
8.8K
01:58Cooperative Allosteric Transitions
2.7K
2.7K
02:39Phase Transitions: Vaporization and Condensation
21.5K
The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize (convert into vapor). The process is called vaporization—a surface phenomenon. Vaporization occurs when the thermal motion of the molecules overcome the intermolecular forces, and the molecules (at the surface) escape into the gaseous state. When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules...
21.5K
02:33Phase Transitions: Sublimation and Deposition
20.2K
Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes...
20.2K