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Drawback's of Rutherford's Model of Atom - Structure of Atom, Class 9, Science Video Lecture

Q: 2. What are the drawbacks of Rutherford's model of the atom?

Ans. Rutherford's model of the atom had several drawbacks:- According to classical electromagnetic theory, an accelerated charge loses energy in the form of electromagnetic radiation. Therefore, the electrons would continuously lose energy and spiral into the nucleus, resulting in the collapse of the atom.- It could not explain the stability of the atom since the electrons were in constant motion and should eventually fall into the nucleus.- It could not explain the discrete energy levels observed in the spectra emitted by atoms.- It did not account for the existence of electron clouds or the probability distribution of electrons around the nucleus.- It did not explain the phenomenon of atomic line spectra.

FAQs on Drawback's of Rutherford's Model of Atom - Structure of Atom, Class 9, Science Video Lecture

1. What is Rutherford's model of the atom?

Ans. Rutherford's model of the atom, also known as the nuclear model, proposed that the atom consists of a tiny, dense, and positively charged nucleus surrounded by negatively charged electrons that orbit around it in specific energy levels.

2. What are the drawbacks of Rutherford's model of the atom?

Ans. Rutherford's model of the atom had several drawbacks: - According to classical electromagnetic theory, an accelerated charge loses energy in the form of electromagnetic radiation. Therefore, the electrons would continuously lose energy and spiral into the nucleus, resulting in the collapse of the atom. - It could not explain the stability of the atom since the electrons were in constant motion and should eventually fall into the nucleus. - It could not explain the discrete energy levels observed in the spectra emitted by atoms. - It did not account for the existence of electron clouds or the probability distribution of electrons around the nucleus. - It did not explain the phenomenon of atomic line spectra.

3. Why did Rutherford's model of the atom fail to explain atomic stability?

Ans. Rutherford's model of the atom failed to explain atomic stability because, according to classical electromagnetic theory, the electrons in motion would continuously lose energy and spiral into the nucleus. This implied that atoms should quickly collapse, rendering them unstable. However, this contradicted the observed stability of atoms in reality.

4. How did Rutherford's model contribute to our understanding of the atom despite its drawbacks?

Ans. Although Rutherford's model of the atom had its drawbacks, it made significant contributions to our understanding of the atom. It provided evidence for the existence of a dense, positively charged nucleus at the center of the atom. Additionally, Rutherford's model paved the way for further advancements in atomic theory, leading to the development of quantum mechanics and the Bohr model, which addressed some of the limitations of Rutherford's model.

5. What advancements in atomic theory followed Rutherford's model?

Ans. Rutherford's model of the atom laid the foundation for further advancements in atomic theory. Subsequent to his model, Niels Bohr proposed the Bohr model, which introduced the concept of quantized energy levels for the electrons in an atom. This model explained the stability of atoms by suggesting that electrons occupy specific energy levels and do not emit energy while in those levels. Later, the development of quantum mechanics revolutionized atomic theory, providing a more accurate and comprehensive understanding of the behavior of atoms and subatomic particles.

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