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Presentation on theme: "ATOMIC STRUCTURE."— Presentation transcript:


2 Models or Theories Allow scientists to communicate their ideas to others. A model should be able to explain previous observations and predict future outcomes.

3 (greek for indivisible)
HISTORY OF THE ATOM Democritus develops the idea of atoms 460 BC he pounded up materials in his pestle and mortar until he had reduced them to smaller and smaller particles which he called ATOMA (greek for indivisible)

suggested that all matter was made up of tiny spheres that were able to bounce around with perfect elasticity and called them ATOMS

5 Dalton’s Atomic Theory
All matter is made up of small particles called atoms. Atoms cannot be created, destroyed or divided into smaller particles. All atoms of the same element are identical in mass and size, but they are different in mass and size from the atoms of other elements. Compounds are created when atoms of different elements link together in definite proportions.

6 Thomson’s Experiment: Cathode Rays
Passing an electric current makes a beam appear to move from the negative to the positive end. (By adding an electric field, he was able to conclude that the particles were negative.)

7 HISTORY OF THE ATOM ELECTRON Joseph John Thompson 1898
found that atoms could sometimes eject a far smaller negative particle which he called an ELECTRON

Thompson develops the idea that an atom was made up of electrons scattered unevenly within an elastic sphere surrounded by a soup of positive charge to balance the electron's charge like plums surrounded by pudding. PLUM PUDDING MODEL

9 HISTORY OF THE ATOM Ernest Rutherford 1910
fired + particles (alpha particles) at a thin sheet of gold foil, he expected the particles to go straight though

10 HISTORY OF THE ATOM gold foil helium nuclei helium nuclei They found that while most of the positive particles passed through the foil, a small number were deflected and, to their surprise, some positive particles bounced straight back.

11 HISTORY OF THE ATOM However, this was not the end of the story.
Rutherford’s new evidence allowed him to propose a more detailed model with a central nucleus. He suggested that the there was a small, dense, positive charge in a central nucleus. With this holding the large, negative electron cloud in place by electrical attraction. However, this was not the end of the story.

12 HISTORY OF THE ATOM Niels Bohr 1913
studied under Rutherford at the Victoria University in Manchester. Bohr refined Rutherford's idea by adding that the electrons were in orbits. Rather like planets orbiting the sun. With each orbit only able to contain a set number of electrons.

13 Bohr’s Atom electrons in orbits nucleus

14 HELIUM ATOM + - + - Shell proton neutron electron
What do these particles consist of?

15 ATOMIC STRUCTURE Particle Charge Mass Found Proton +ve heavy nucleus
Neutron neutral Electron -ve light outside nucleus

16 number of electrons = number of protons
ATOMIC STRUCTURE 4 He Atomic mass the number of protons and neutrons in an atom 2 Atomic number the number of protons in an atom number of electrons = number of protons

17 ATOMIC STRUCTURE Electrons are arranged in Energy Levels or Shells around the nucleus of an atom. first shell a maximum of 2 electrons second shell a maximum of 8 electrons third shell a maximum of 8 electrons fourth shell  a maximum of 2 electrons

18 SUMMARY The Atomic Number of an atom = number of
protons in the nucleus. The Atomic Mass of an atom = number of Protons + Neutrons in the nucleus. The number of Protons = Number of Electrons. Electrons orbit the nucleus in shells. Each shell can only carry a set number of electrons.

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