1. Atomic Structure
What is an atom?

2. Atom
An atom is the smallest physical particle of an element that still retains the properties of that element.

3. Atomic Theory First scientist to suggest atoms: Democritus
“Everything that is must be eternal.”
Democritus believed that there were basic things that always exist, but can be rearranged; he called these “atomos”.

4. Atomic Theory John Dalton exceptionally bright Quaker
put in charge of the local school at age 12
Color blind (was once called Daltonism)
First scientist to create a modern definition of “atom”

5. Atomic Theory
“We might as well attempt to annihilate [a planet], as to create or destroy a particle of hydrogen.”
Determined relative weights of known elements by breaking apart compounds consisting of them.

6. Atomic Theory All elements are composed of atoms.
Atoms of the same element are identical. Atoms of different elements are always different.
Atoms of different elements can chemically combine in fixed ratios to form compounds.

7. Atomic Theory
Chemical reactions occur when atoms are joined, separated, or rearranged. Atoms of one element are NEVER changed into another during a chemical reaction.

8. Review of Atoms? All atoms of the same element are identical.
Chemical reactions occur when atoms of one element are changed into atoms of another element.

9. What does an atom look like?
Atomic Structure
What does an atom look like?

10. Proof of Atoms
Three scientists that made contributions to atomic structure – J.J. Thompson, Ernest Rutherford, and Neils Bohr.

11. John Dalton’s Atom
Atoms are solid and indivisible.

12. J. J. Thompson’s Atom
Thompson passed electric current through gases in a glass tube. The result was a glowing beam flowing from the negative side to the positive side.

13. J. J. Thompson’s Atom
Glowing ray (cathode ray) was attracted to a positive magnet on the side of the tube.
Beam must be negatively charged.

14. J. J. Thompson’s Atom
Thompson hypothesized that all atoms had such negative charges within. (plum pudding model)
Later, scientists proved that atoms contained both positive and negative charges (which balance each other out).

15. Electrons and Protons
Electrons – negatively charged portion of an atom
Protons – positively charged portion of an atom

16. James Chadwick’s Atom
Chadwick found that the mass of an atom is greater than the mass of protons plus electrons.
Neutrons – portion of an atom with no charge
Protons, neutrons, and electrons are called subatomic particles.

17. Ernest Rutherford’s Atom
Born in New Zealand.
Terrible at mathematics.
Diligent problem solver.
Did most of his work at McGill in Montreal

18. Ernest Rutherford’s Atom
Shot radioactive particles through a sheet of gold foil.
Most went straight through, but others were knocked off course or bounced back.
“Like shooting a fifteen-inch shell at a sheet of paper and having it bounce off.”

19. Ernest Rutherford’s Atom

20. Ernest Rutherford’s Atom
Nucleus – compact center of the atom where protons and neutrons are located
Nucleus has very little of the atom’s volume, but contains most of the atom’s mass.

21. Niels Bohr’s Atom
Electrons orbit the nucleus in orbits, like a solar system.
Planetary Model

22. Atomic Properties
How do atoms differ?

23. Atomic Number Atoms of different elements have different structures.
Elements differ because their atoms contain different numbers of protons!
Atomic Number – number of protons in the atom

24. Mass Number
Electrons have negligible mass compared to protons and neutrons.
Mass of a neutron is approximately equal to mass of a proton.
Mass Number - number of protons plus number of neutrons in an atom.

25. Names and Symbols Gold – 118 neutrons Beryllium – 5 neutrons
Mass Number = ?
Beryllium – 5 neutrons
Mass Number – ?
Sodium – 12 neutrons

26. Isotopes Atoms of the same element with different number of neutrons
Chemically equivalent
Most elements occur as a mixture of isotopes

27. Isotopes of Hydrogen

28. Calculating Atomic Mass
Mass of a proton is more than 1800 times the mass of an electron
Spectrometer used to find masses of atoms
Masses of subatomic particles too small to work with, so a reference isotope is used

29. Calculating Atomic Mass
One amu (atomic mass unit) is defined as 1/12 the mass of a Carbon-12 atom
1 amu is approx. equal to the mass of a proton or neutron

30. Self Quiz, Part 1 What is an atom? What is the symbol for… Calcium?
Phosphorus?
Potassium?
Copper?
Silver?
Tin?
Mercury?

31. Self Quiz, Part 2 What is the atomic number of…
Lithium?
Lead?
Gold?
Neon?
Describe Dalton’s atomic model.
Name the four premises of Dalton’s atomic theory.

32. Self Quiz, Part 3 Explain the difference between atoms and molecules.
Describe Thompson’s experiments and his atomic model.
Describe Rutherford’s experiments and his atomic model.
What is an atomic number?

33. Self Quiz, Part 4
Compare and contrast protons, neutrons, and electrons.
Chlorine-35?
Mass Number?
Number of Protons?
Number of Electrons?