Rutherford and the nucleus <ul><li>British physicist who, in 1911, proved that atoms had a small, dense, positively charge...
Rutherford’s Model of the Atom Limitation: did not specify exactly where the electrons were
Bohr and energy levels <ul><li>Danish scientist who, in 1913, proposed the “Planetary Model” of the atom </li></ul><ul><li...
<ul><li>In 1932, James Chadwick discovered the neutron. </li></ul><ul><li>The nucleus contains neutrons. </li></ul><ul><li...
Quantum Mechanical or Electron Cloud Model <ul><li>Electrons dart about within an energy level in an ever – changing path....
Electron Cloud Model n nucleus electron cloud
Seatwork: <ul><li>In size 4: start identifying the 5 suspects </li></ul><ul><li>In your SBP, draw the models of Dalton, Th...
Let us see if you got it right. 1. Dalton 2. Rutherford 3. Thomson 4. Bohr 5. Democritus
Atomic Models Dalton’s Atomic Model Rutherford’s  Atomic Model Thomson’s Atomic Model Electron Cloud Model Bohr’s Planetar...
A CLOSER LOOK ON ATOMS
ATOMS <ul><li>Potential energy and kinetic energy are present in the atom </li></ul><ul><li>Atoms are always neutral in ch...
Computation in atoms <ul><li># of protons = Atomic number </li></ul><ul><li># of electrons = Atomic number </li></ul><ul><...
Element Mass Number Atomic Number Number of Protons Number of Electrons Number of Neutrons Li Cu Cl Ag Pb
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1 k 0106f_particles of matter

  1. 1. Rutherford and the nucleus <ul><li>British physicist who, in 1911, proved that atoms had a small, dense, positively charged nucleus. </li></ul><ul><li>Rutherford’s Model </li></ul><ul><ul><li>Protons ( the positively charged sub-atomic particles ) are concentrated in a small area at the center of the atom. </li></ul></ul><ul><ul><li>He called this area the nucleus. </li></ul></ul><ul><ul><li>An atom is mostly empty space. </li></ul></ul><ul><ul><li>The nucleus is tiny compared to the whole atom, but it contains nearly all the atom’s mass. </li></ul></ul>
  2. 2. Rutherford’s Model of the Atom Limitation: did not specify exactly where the electrons were
  3. 3. Bohr and energy levels <ul><li>Danish scientist who, in 1913, proposed the “Planetary Model” of the atom </li></ul><ul><li>The energy levels occupied by electrons are like the orbits of planet at different distances from the sun. </li></ul><ul><li>Bohr compares electrons to the planets and nucleus to the sun. </li></ul>
  4. 4. <ul><li>In 1932, James Chadwick discovered the neutron. </li></ul><ul><li>The nucleus contains neutrons. </li></ul><ul><li>A neutron has about the same mass as a proton but has no electrical charge. </li></ul>Chadwick and the neutron Jimmy neutron walked into a bar and  asked how much for a drink.  The bartender replied,  &quot;for you, no charge.&quot;  -Jaime - Internet Chemistry Jokes
  5. 5. Quantum Mechanical or Electron Cloud Model <ul><li>Electrons dart about within an energy level in an ever – changing path. </li></ul><ul><li>Their rapid motion creates a “ cloud” of negative electricity around the nucleus. </li></ul><ul><li>The electron cloud gives an atom its size and shape. </li></ul>
  6. 6. Electron Cloud Model n nucleus electron cloud
  7. 7. Seatwork: <ul><li>In size 4: start identifying the 5 suspects </li></ul><ul><li>In your SBP, draw the models of Dalton, Thomson, Rutherford, Bohr and the Quantum model. Label and write a short description about the model. </li></ul>
  8. 8. Let us see if you got it right. 1. Dalton 2. Rutherford 3. Thomson 4. Bohr 5. Democritus
  9. 9. Atomic Models Dalton’s Atomic Model Rutherford’s Atomic Model Thomson’s Atomic Model Electron Cloud Model Bohr’s Planetary Atomic Model
  10. 10. A CLOSER LOOK ON ATOMS
  11. 11.
  12. 12.
  13. 13.
  14. 14. ATOMS <ul><li>Potential energy and kinetic energy are present in the atom </li></ul><ul><li>Atoms are always neutral in charge </li></ul><ul><li>In an atom, no. of protons = no. of electrons </li></ul><ul><li>Atomic number: </li></ul><ul><ul><li>Lower in amount than mass number </li></ul></ul><ul><ul><li>Number of protons in an atom </li></ul></ul><ul><ul><li>Tells you the identity of the element </li></ul></ul><ul><li>Mass number/ Atomic weight/Atomic mass: </li></ul><ul><ul><li>Higher in amount than atomic munber </li></ul></ul><ul><ul><li>Number of protons and neutrons in an atom </li></ul></ul>
  15. 15. Computation in atoms <ul><li># of protons = Atomic number </li></ul><ul><li># of electrons = Atomic number </li></ul><ul><li># of neutrons = Mass number– Atomic number </li></ul><ul><li>Mass number = # of protons + # of neutrons </li></ul>
  16. 16. Element Mass Number Atomic Number Number of Protons Number of Electrons Number of Neutrons Li Cu Cl Ag Pb

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