Nuclear Physics GCSE

Authors Avatar

Basic Information/facts about atoms:

  • All matter consists of atoms; it comes from the Greek word meaning ‘indivisible’ - they cannot be divided by chemicals.
  • Although the nucleus is generally around one ten-thousandth the size of an atom, it contains more that 99.9% of the mass!
  • Each atom is made up of electrons, protons and neutrons. Protons and neutrons are tightly packed at the centre of the atom in the nucleus, whilst the electrons orbit the nucleus in shells.
  • Electrons have a negative charge (-1), protons have a positive charge (+1) and neutrons have no charge.
  • Atoms always have the same number of electrons as protons; therefore there is overall no charge.
  • Substances made up of only one type of atom are called elements. There are approximately 117 elements known so far and the number of protons in the nucleus determines which element it is.
  • If the number of neutrons is different in the element, it is called an isotope. Not enough necessary neutrons may cause a nucleus to be unstable or lead to nuclear decay, this is because protons are positively charged (so they repel each other), and neutrons normally separate these apart.
  • The number of electrons determines how stable and reactive the atom is. Each atom has two electrons in its first shell and eight continuing on, if all is filled it is stable. Most atoms do not have a full outer shell and try to react with another through either ionic bonding or covalent bonding.
  • Protons weigh relative in size to neutrons – 1 mass; however electrons are a lot smaller weighing relatively 0.0005 of mass.

        

Discovery/Background knowledge:

  • Ernest Rutherford was fascinated by radioactivity and investigated it for twenty years, beginning at Havelock school, then Nelson College and won a scholarship to study at Canterbury College.
  • He named the easily absorbed rays ‘alpha’ and the penetrating rays ‘beta’. He began working with Hans Geiger in the University of Manchester; they observed shooting a narrow beam of alpha particles (nucleus of a helium atom) onto a thin gold foil.
  • Rutherford was amazed that some alpha particles diverted at dramatic angles instead of continuing through the thin metal foil, they seemed to ‘bounce back.’ It was noticed that an angle greater than ten degrees caused much more alpha particles to scatter than predicted.
  • As only a small proportion of particles were scattered, it seemed as though whatever caused the force had to be very small.
  • He concluded the idea of the nucleus at the centre of an atom containing protons with electrons orbiting and this is why the positively charged alpha particles reflected back.
  • He soon founded the Rutherford model (model of the atom) which suggested the past ‘plum pudding model’ was incorrect. This was where scientists believed the positively charged matter was spread out evenly in an atom with the electrons buried inside. If the ‘pudding pudding model’ was correct, it would have deflected back at a consistent level, yet through Rutherford’s test if demonstrated the protons were in the middle of the atom.
  • His ideas were accepted because it explains radioactivity and the changes that happen with an unstable nucleus, it also predicted what a neutron was.
Join now!

Radioactive decay/Background Radiation:

  • The three main types of radiation are alpha, beta and gamma.
  • Background radiation is all around us and most of it comes from natural sources or medical supplies. This includes cosmic rays, animals, rocks (which emit radon) and plants. Human activity has added to background radiation artificially through X-rays and nuclear weapons testing.
  • The reason alpha radiation decays is if the nucleus has too many protons, Helium is emitted to try reduce all the protons repulsing from each other inside the atom. Helium nuclei are continuously in collision with the walls in a nucleus, ...

This is a preview of the whole essay