NEET > Chemistry Class 11 > Thomson's Model of an Atom: Postulates & Drawbacks
Thomson's Model of an Atom: Postulates & Drawbacks Video Lecture - Chemistry Class 11 - NEET
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FAQs on Thomson's Model of an Atom: Postulates & Drawbacks Video Lecture - Chemistry Class 11 - NEET
| 1. What are the postulates of Thomson's model of an atom? |  |
Ans. Thomson's model of an atom, also known as the plum pudding model, had the following postulates:
1. An atom is composed of a positively charged sphere with negatively charged electrons embedded in it.
2. The positive charge is uniformly distributed throughout the atom.
3. The negative electrons are scattered uniformly within the positively charged sphere.
| 2. What are the drawbacks of Thomson's model of an atom? | |
Ans. Thomson's model had a few drawbacks, which were later addressed by subsequent atomic models:
1. It failed to explain the stability of the atom since the negatively charged electrons should have been attracted to the positively charged sphere and collapsed into it.
2. It couldn't explain the discrete energy levels observed in atomic spectra.
3. It couldn't explain the scattering of alpha particles in the famous gold foil experiment conducted by Rutherford.
4. It couldn't explain the presence of empty space in the atom.
| 3. How did Thomson's model contribute to our understanding of the atom? | |
Ans. Thomson's model of an atom was a significant step in our understanding of atomic structure. It introduced the concept of a subatomic particle, the electron, and proposed that atoms have a positive charge as well. Although the model had its drawbacks, it provided the foundation for further research and the development of more accurate atomic models.
| 4. How did Thomson's model explain the behavior of electrically charged particles? | |
Ans. Thomson's model explained the behavior of electrically charged particles by proposing that atoms contain negatively charged electrons embedded in a positively charged sphere. Due to the presence of opposite charges, the electrons were held in place within the atom and did not collapse into the positively charged region. This arrangement allowed for the stability of the atom and explained the behavior of electrically charged particles.
| 5. How did Thomson's model differ from Rutherford's atomic model? | |
Ans. Thomson's model, also known as the plum pudding model, proposed that the positive charge is uniformly distributed throughout the atom with negatively charged electrons embedded in it. On the other hand, Rutherford's atomic model, known as the nuclear model, suggested that the positive charge is concentrated in a tiny, dense nucleus at the center of the atom, while the electrons orbit around it. Rutherford's model resolved the drawbacks of Thomson's model by explaining the scattering of alpha particles and the existence of discrete energy levels.
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