While the plum pudding model suggested that electrons in an atom are embedded in a positively charged substrate, Rutherford's experiment concluded that it is only the core of an atom that is positively charged around which the electrons move in fixed orbits.
Explanation:
J. J. Thomson's 'plum-pudding' model suggested that atoms are composed of positive and negatively charged particles. The electrons that are negatively charged are embedded (like the plums in a pudding) in a sea of positive charge.
This theory was disproved by Rutherford via his gold foil experiment in which he bombarded positively charged alpha particles onto a thin gold foil. He observed that while most of the particles passed through the foil some of them completely retraced their path. This led to two major conclusions:
- Most of the space inside the atom is empty
-The mass of the atom is concentrated in the positively charged core called the nucleus.
Thomson saw the atom to be a spherical cloud of positive proton matter with electrons dispersed throughout it. Then the gold foil experiment is when Rutherford shot alpha particles at a sheet of gold foil and when there was deflection he concluded there was a dense part in the center of an atom with he called the nucleus made up of neutrons and protons.
Strong acids and bases both denature proteins by severing disulphide bonds and at higher temperatures, can break proteins into peptides, or even individual amino acids.