• Evidence for the structure of the atom was discovered by Ernest Rutherford in the beginning of the 20th century from the study of?α-particle scattering
• The experimental setup consists of alpha particles fired at thin gold foil and a detector on the other side to detect how many particles deflected at different angles

α-particle scattering experiment set up

• α-particles are the nucleus of a helium atom and are positively charged

When α-particles are fired at thin gold foil, most of them go straight through but a small number bounce straight back

• From this experiment, Rutherford results were:
• The majority of α-particles went straight through (A)
  • This suggested the atom is mainly empty space

   

• Some α-particles deflected through small angles of < 10o?(B)
  • This suggested there is a positive nucleus at the centre (since two positive charges would repel)

   

• Only a small number of α-particles deflected straight back at angles of > 90o?(C)
  • This suggested the nucleus is extremely small and this is where the mass and charge of the atom is concentrated
  • It was therefore concluded that atoms consist of?small dense positively charged nuclei

   

• Since atoms were known to be neutral, the negative electrons were thought to be on a positive sphere of charge (plum pudding model) before the nucleus was theorised
• Now it is known that the negative electrons are orbiting the nucleus. Collectively, these make up the atom

An atom: a small positive nucleus, surrounded by negative electrons

• Note: The atom is around 100,000 times larger than the nucleus!

? ? ?ANSWER:? ?A

• The Rutherford scattering experiment directed parallel beams of α-particles at gold foil
• The observations were:
  • Most of the α-particles went straight through the foil
  • The largest value of n will therefore be at small angles
  • Some of the α-particles were deflected through small angles
  • n drops quickly with increasing angle of deflection θ

   

• These observations fit with graph?A