Rutherford's Gold Foil Experiment: Unraveling Atomic Structure

The video discusses the transition from the plum pudding model to Rutherford's atomic model. It explains how Rutherford's Gold foil experiment, conducted with Geiger and Marsden, challenged the existing atomic theory. The experiment used alpha particles to bombard a thin gold foil, expecting them to pass through with minimal deflection. However, unexpected deflections and rebounds led to the conclusion that the atom has a dense nucleus, contradicting the plum pudding model. This pivotal experiment reshaped the understanding of atomic structure.

What was the main reason scientists began to question the plum pudding model?

• It was not accepted globally.

• It was too expensive to test.

• New experiments showed different results.

• It was too complex to understand.

Who were the key collaborators with Rutherford in the Gold Foil Experiment?

• Niels Bohr and Albert Einstein

• Hans Geiger and Ernest Marsden

• James Chadwick and J.J. Thomson

• Marie Curie and Pierre Curie

Why did Rutherford choose alpha particles for his experiment?

• They were the lightest particles available.

• They had high energy and mass.

• They were the cheapest option.

• They were the only particles available.

What was the reason for using a thin gold foil in the experiment?

• Gold is the most reflective metal.

• Gold is the heaviest metal.

• Gold is the least reactive metal.

• A thin foil contains fewer atoms, making it easier to study.

What was the primary purpose of the fluorescent screen in the experiment?

• To change the color of alpha particles.

• To reflect alpha particles.

• To detect and visualize the path of alpha particles.

• To absorb alpha particles.

According to the plum pudding model, how should alpha particles behave when passing through an atom?

• They should be completely absorbed.

• They should pass straight through with little deviation.

• They should change into beta particles.

• They should bounce back completely.

How did the mass of alpha particles compare to the mass of positive charges in the plum pudding model?

• Alpha particles were lighter.

• Alpha particles were heavier.

• Alpha particles had no mass.

• Alpha particles had the same mass.

What unexpected result did Rutherford observe in his experiment?

• Some alpha particles rebounded, and some were deflected.

• No alpha particles hit the detector.

• Most alpha particles were deflected at large angles.

• All alpha particles were absorbed by the foil.

What conclusion did Rutherford draw from his observations?

• Atoms are solid spheres.

• Atoms have a dense central nucleus.

• Atoms are mostly empty space.

• Atoms are made of only electrons.

What was the significance of Rutherford's experiment in the field of chemistry?

• It confirmed the plum pudding model.

• It provided a more accurate model of the atom.

• It introduced the concept of isotopes.

• It led to the discovery of the electron.