atomic nucleus energy

The Nucleus - Rutherford and his co-workers, performed series of scattering experiments and concluded that the entire mass and the positive charge is concentrated in a very small region at the centre of the atom, known as nucleus. The radius of the nucleus is..

Rutherford and his co-workers, performed series of scattering experiments and concluded that the entire mass and the positive charge is concentrated in a very small region at the centre of the atom, known as nucleus. The radius of the nucleus is about 10 - 1 5 ..

It is the central core of the atom where the entire +ve charge and mass is concentrated. It is a tiny sphere of diameter ranging from 10 - 1 5 m to 10 - 1 4 m. A nucleus is made up of particles called neutrons and protons. A neutron does not carry any charge while a prot..

The value of uncertainty in velocity, D v is much higher than the velocity of light (3.0 x 10 8 ms - 1 ) and therefore, it is not possible. Hence an electron cannot be found within the atomic nucleus. In 1927, Erwin Schrodinger described the behavior of electrons around the ..

Atoms and Nuclei..

On the basis of Heisenberg's uncertainty principle, it can be shown as to why electron cannot exist within the atomic nucleus. The radius of the atomic nucleus is of the order of 10 - 1 5 m. Now, if the electron were to exist within the nucleush..

Ernest Rutherford, an energetic Scientist From New Zealand working in England, was studying the properties of particles spontaneously emitted by radioactive substances. Of particular interest was a positively charged, relatively heavy emission named alpha particle. Quantities of such particles ar..

> How do infrared and g - rays differ in their (i) wavelength and (ii) penetrating power. Suggested Answer:- (i) g - rays have much shorter wavelengths of the order of 10 - 1 3 m while the infrared have longer wavelengths of the order of 10 - 6 or more. (ii) g - rays have a much higher penetrating ..

Single electron atoms - The relative energies of various orbitals of single electrons depend on the value of the principal quantum number 'n' and is independent of the value of 'l'. This can be shown by an arrangement known as energy level diagram. The diagram given be..

As the size of the atom increases the outermost electrons are held less tightly by the nucleus (attractive force between the electron and the nucleus is inversely proportional to the distance). As a result it becomes easier to remove the electron and therefore the ion..