1. Chapter 4 Atomic Structure

2. Democritus Greek philosopher Tried to define matter more than 2400 years ago. – Could matter be divided into smaller and smaller pieces forever, or was there a limit to the number of times a piece of matter could be divided?

3. Atomos He theorized that matter could not be divided into smaller and smaller pieces forever, eventually the smallest possible piece would be obtained. He named the smallest piece of matter atomos, meaning “indivisible.”

4. Atomos  Atoms were small, hard particles  All made of the same material  Different shapes and sizes  Infinite in number  Always moving and capable of joining together

5. Why was this theory ignored and forgotten for more than 2000 years? …something was missing

6. John Dalton Early 1800s, English Chemist Experimentation- led to the acceptance of the idea of atoms Studied ratios of elements in rxns.

7. Dalton’s Atomic Theory 1. All elements are composed of atoms. Atoms are indivisible and indestructible particles. 2. Atoms of the same element are exactly alike, but different from those of any other element.

8. Dalton’s Atomic Theory 3. Compounds are formed by the joining of atoms of two or more elements in simple whole-number ratios. 4. Chemical reactions occur when atoms are separated, joined, or rearranged. The atoms of one element are never changed into atoms of another element.

10. This theory became one of the foundations of modern chemistry.

11. The Men behind Atomic Theory Their quest for knowledge about the nature of the universe helped define our views.

12. Exit Ticket 1.Identify two points of Dalton’s Atomic Theory. 2.Describe the structure of the atom, including subatomic particles, their charge and location.

13. Just how small is an atom? 100,000,000 copper atoms = 1 cm

14. Thomson’s Plum Pudding Model In 1897, the English scientist J.J. Thomson provided the first hint that an atom is made of even smaller particles.

15. Thomson studied the passage of an electric current through a gas. As the current passed through the gas, it gave off rays of negatively charged particles.

16. Thomson concluded that the negative charges came from within the atom. A particle smaller than an atom had to exist. The atom was divisible!

17. Thomson called the negatively charged particles “corpuscles,” today known as electrons. Since the gas was known to be neutral, having no charge, he reasoned that there must be positively charged particles in the atom. But he could never find them.

18. To test his hypothesis… Measured the ratio of the charge of an electron to its mass Ratio was constant Ratio did not depend on the kind of gas in CRT or metal electrodes used Therefore, electrons are part of atoms of all elements

19. Rutherford’s Gold Foil Experiment In 1908, the English physicist Ernest Rutherford conducted an experiment that involved firing a stream of tiny positively charged particles at a thin sheet of gold foil

20. Most of the positively charged “bullets” passed right through the gold atoms in the sheet of gold foil. Some of the positively charged “bullets,” bounced away from the gold sheet. He knew that positive charges repel positive charges.

22. Rutherford reasoned that all of an atom’s positively charged particles were contained in the nucleus. The negatively charged particles were scattered outside the nucleus around the atom’s edge.

23. He concluded…the gold atoms in the sheet were mostly open space, not a pudding filled with a positively charged material. Rutherford concluded that an atom had a small, dense, positively charged center that repelled his positively charged “bullets.” He called the center of the atom the nucleus. The nucleus is tiny compared to the atom as a whole.

24. Eugen Goldstein In 1886 found rays traveling in the opposite direction to that of the cathode rays Composed of positive particles, which were later named protons Mass is about 1840 times that of an electron

25. James Chadwick 1932 confirmed the existence of the neutron No charge Mass is equal to the proton’s mass

26. Robert A. Millikan Calculated the mass of the electron in 1916 An electron carries one unit of negative charge An electron’s mass is 1/1840 the mass of a hydrogen atom

27. Bohr Model In 1913, the Danish scientist Niels Bohr proposed an improvement. In his model, he placed each electron in a specific energy level.

28. Bohr Model According to Bohr’s atomic model, electrons move in definite orbits around the nucleus, much like planets circle the sun. These orbits, or energy levels, are located at certain distances from the nucleus.

29. The Wave Model Today’s atomic model is based on the principles of wave mechanics. According to the theory of wave mechanics, electrons do not move about an atom in a definite path, like the planets around the sun.

30. MODELIndivisibleElectronsNucleusOrbitElectron Cloud Greek X Dalton X Thomson X RutherfordXX Bohr XXX Wave XXX